http://205.166.159.208/wiki/api.php?action=feedcontributions&feedformat=atom&user=ShounsveMC Chem Wiki - User contributions [en]2026-06-26T06:00:43ZUser contributionsMediaWiki 1.35.5http://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8890SAHounsve Spring 20182018-05-11T00:08:44Z<p>Shounsve: /* Results and Discussion */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Different proportions of solvents such as 0.1% TFA as eluent B and acetonitrile as eluent A were used for the separation. The multiple gradient used for the chromatographic separation consisted of different proportions of eluent A/B (0:100 for 1-15 mins, 80:20 for 15-25 min, and 0:100 for 25-30 min). The mobile phase flow rte was 1.0 mL/min, the sample injection volume 10 μL, and the chromatograph was monitored at 280 nm. <br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
[[File:eug_trails_only_a.png|400px|thumb|left|Figure 2: HPLC chromatograph of 1 mM eugenol standard and oxidation mixtures. The eugenol standard is present at 13 minutes, at 9 minutes there is a small peak that is unknown at what is present here. At 16 minutes, there is a peak that could be a possible radical product.]]<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
[[File:eug_trial_c.png|400px|thumb|left|Figure 3: HPLC chromatograph with product highlights and kinetic graph. Kinetic graph shows relationship between eugenol and H<sub>2</sub>O<sub>2</sub>.]]<br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===References===<br />
<br />
1. Hakkim, Lukmanul F., C. Gowri Shankar, and S. Girija. Chemical Composition and Antioxidant Property of Holy Basil (Ocimum sanctum L.) Leaves, Stems, and Inflorescence and Their in Vitro Callus Cultures. J. Agric. Food Chem., 2007, 55, 9109-9117. <br />
<br />
2. Mastelić, Josip, et al. Comparative Study on the Antioxidant and Biological Activities of Carvacrol, Thymol, and Eugenol Derivatives. J. Agric. Food Chem., 2008, 56, 3989-3996. <br />
<br />
3. Sipe, H. J., Lardinois, O. M., & Mason, R. P. Free Radical Metabolism of Methyleugenol and Related Compounds. Chemical Research in Toxicology, 2014, 27(4), 483–489.<br />
<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=File:Eug_trial_c.png&diff=8889File:Eug trial c.png2018-05-11T00:06:54Z<p>Shounsve: File uploaded with MsUpload</p>
<hr />
<div>File uploaded with MsUpload</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8887SAHounsve Spring 20182018-05-11T00:05:27Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Different proportions of solvents such as 0.1% TFA as eluent B and acetonitrile as eluent A were used for the separation. The multiple gradient used for the chromatographic separation consisted of different proportions of eluent A/B (0:100 for 1-15 mins, 80:20 for 15-25 min, and 0:100 for 25-30 min). The mobile phase flow rte was 1.0 mL/min, the sample injection volume 10 μL, and the chromatograph was monitored at 280 nm. <br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
[[File:eug_trails_only_a.png|400px|thumb|left|Figure 2: Chromatograph of 1 mM eugenol standard and oxidation mixtures. The eugenol standard is present at 13 minutes, at 9 minutes there is a small peak that is unknown at what is present here. At 16 minutes, there is a peak that could be a possible radical product.]]<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===References===<br />
<br />
1. Hakkim, Lukmanul F., C. Gowri Shankar, and S. Girija. Chemical Composition and Antioxidant Property of Holy Basil (Ocimum sanctum L.) Leaves, Stems, and Inflorescence and Their in Vitro Callus Cultures. J. Agric. Food Chem., 2007, 55, 9109-9117. <br />
<br />
2. Mastelić, Josip, et al. Comparative Study on the Antioxidant and Biological Activities of Carvacrol, Thymol, and Eugenol Derivatives. J. Agric. Food Chem., 2008, 56, 3989-3996. <br />
<br />
3. Sipe, H. J., Lardinois, O. M., & Mason, R. P. Free Radical Metabolism of Methyleugenol and Related Compounds. Chemical Research in Toxicology, 2014, 27(4), 483–489.<br />
<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8884SAHounsve Spring 20182018-05-10T23:56:32Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Different proportions of solvents such as 0.1% TFA as eluent B and acetonitrile as eluent A were used for the separation. The multiple gradient used for the chromatographic separation consisted of different proportions of eluent A/B (0:100 for 1-15 mins, 80:20 for 15-25 min, and 0:100 for 25-30 min). The mobile phase flow rte was 1.0 mL/min, the sample injection volume 10 μL, and the chromatograph was monitored at 280 nm. <br />
<br />
<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
[[File:eug_trails_only_a.png|400px|thumb|left|Figure 2: Chromatograph of 1 mM eugenol standard and oxidation mixtures. The eugenol standard is present at 13 minutes, at 9 minutes there is a small peak that is unknown at what is present here. At 16 minutes, there is a peak that could be a possible radical product.]]<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===References===<br />
<br />
1. Hakkim, Lukmanul F., C. Gowri Shankar, and S. Girija. Chemical Composition and Antioxidant Property of Holy Basil (Ocimum sanctum L.) Leaves, Stems, and Inflorescence and Their in Vitro Callus Cultures. J. Agric. Food Chem., 2007, 55, 9109-9117. <br />
<br />
2. Mastelić, Josip, et al. Comparative Study on the Antioxidant and Biological Activities of Carvacrol, Thymol, and Eugenol Derivatives. J. Agric. Food Chem., 2008, 56, 3989-3996. <br />
<br />
3. Sipe, H. J., Lardinois, O. M., & Mason, R. P. Free Radical Metabolism of Methyleugenol and Related Compounds. Chemical Research in Toxicology, 2014, 27(4), 483–489.<br />
<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8883SAHounsve Spring 20182018-05-10T23:51:21Z<p>Shounsve: /* References */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
[[File:eug_trails_only_a.png|400px|thumb|left|Figure 2: Chromatograph of 1 mM eugenol standard and oxidation mixtures. The eugenol standard is present at 13 minutes, at 9 minutes there is a small peak that is unknown at what is present here. At 16 minutes, there is a peak that could be a possible radical product.]]<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===References===<br />
<br />
1. Hakkim, Lukmanul F., C. Gowri Shankar, and S. Girija. Chemical Composition and Antioxidant Property of Holy Basil (Ocimum sanctum L.) Leaves, Stems, and Inflorescence and Their in Vitro Callus Cultures. J. Agric. Food Chem., 2007, 55, 9109-9117. <br />
<br />
2. Mastelić, Josip, et al. Comparative Study on the Antioxidant and Biological Activities of Carvacrol, Thymol, and Eugenol Derivatives. J. Agric. Food Chem., 2008, 56, 3989-3996. <br />
<br />
3. Sipe, H. J., Lardinois, O. M., & Mason, R. P. Free Radical Metabolism of Methyleugenol and Related Compounds. Chemical Research in Toxicology, 2014, 27(4), 483–489.<br />
<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8882SAHounsve Spring 20182018-05-10T23:51:03Z<p>Shounsve: /* Conclusion */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
[[File:eug_trails_only_a.png|400px|thumb|left|Figure 2: Chromatograph of 1 mM eugenol standard and oxidation mixtures. The eugenol standard is present at 13 minutes, at 9 minutes there is a small peak that is unknown at what is present here. At 16 minutes, there is a peak that could be a possible radical product.]]<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8881SAHounsve Spring 20182018-05-10T23:50:54Z<p>Shounsve: /* Discussion */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
[[File:eug_trails_only_a.png|400px|thumb|left|Figure 2: Chromatograph of 1 mM eugenol standard and oxidation mixtures. The eugenol standard is present at 13 minutes, at 9 minutes there is a small peak that is unknown at what is present here. At 16 minutes, there is a peak that could be a possible radical product.]]<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8880SAHounsve Spring 20182018-05-10T23:50:47Z<p>Shounsve: /* Results and Discussion */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
[[File:eug_trails_only_a.png|400px|thumb|left|Figure 2: Chromatograph of 1 mM eugenol standard and oxidation mixtures. The eugenol standard is present at 13 minutes, at 9 minutes there is a small peak that is unknown at what is present here. At 16 minutes, there is a peak that could be a possible radical product.]]<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=File:Eug_trails_only_a.png&diff=8879File:Eug trails only a.png2018-05-10T23:49:13Z<p>Shounsve: File uploaded with MsUpload</p>
<hr />
<div>File uploaded with MsUpload</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8878SAHounsve Spring 20182018-05-10T23:48:49Z<p>Shounsve: /* Results */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results and Discussion===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8877SAHounsve Spring 20182018-05-10T23:48:32Z<p>Shounsve: /* Results */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.There is a peak at 16 minutes that could be a possible radical product. As the concentration of H<sub>2</sub>O<sub>2</sub> increases, the eugenol peak decreases and the possible radical product at 16 minutes increases, indicating that this could a possible radical product. <br />
<br />
To further investigate if this is a radical product from eugenol is to implement Flash Chromatography and Electron Paramagnetic Resonance (EPR). By utilizing Flash Chromatography, the sample can be injected in the instrument where the mixture is separated into fractions. The specific fractions that contained either the peak at 9 minutes or 16 minutes can be used on either Gas Chromatography –Mass Spectrometry (GC-MS) or Nuclear Magnetic Resonance (NMR) to determine the structure of the radical product. Once the structure of the product is determined, we need to know how this product is related to eugenol. To do so, we would use EPR to determine if it is a free radical and where the unpaired electron is on the product’s structure.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8875SAHounsve Spring 20182018-05-10T23:46:55Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
Table 1: Series of mixtures made to oxidize eugenol. Eugenol and HRP had the same amount in each trial, Where H<sub>2</sub>O<sub>2</sub> had varying amounts.<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8874SAHounsve Spring 20182018-05-10T23:46:08Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8873SAHounsve Spring 20182018-05-10T23:45:58Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8872SAHounsve Spring 20182018-05-10T23:45:23Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
2. 0.25 M H<sub>2</sub>O<sub>2</sub> Stock<br />
3. HRP Stock<br />
{| class="wikitable"<br />
|-<br />
! Trial !! Eugenol (1 mM) !! H<sub>2</sub>O<sub>2</sub> (0.25 M) !! HRP<br />
|-<br />
| 1 || 5μL || 10μL || 10μL<br />
|-<br />
| 2 || 5μL || 5μL || 10μL<br />
|-<br />
| 3 || 5μL || 2.5μL || 10μL<br />
|-<br />
| 4 || 5μL || 0μL || 10μL<br />
|}<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8871SAHounsve Spring 20182018-05-10T23:42:11Z<p>Shounsve: /* Introduction */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]]<br />
It is well known that natural antioxidants extracted from herbs and spices have vast antioxidant activity and are used in numerous food applications.<sup>1</sup> Most of the antioxidant potential of herbs and spices is due to the redox properties of their phenolic compounds, which permits them to act as reducing agents, hydrogen donors, and singlet oxygen quenchers.<sup>1</sup> Phenols are able to donate hydrogen atoms of phenol hydroxyl groups in reaction with peroxyl radicals that can produce stabilized phenoxyl radicals, thus terminating lipid peroxidation chain reactions.<sup>2</sup><br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP Stock<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8870SAHounsve Spring 20182018-05-10T23:38:50Z<p>Shounsve: /* Proposed Research Project */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Introduction===<br />
Eugenol is a phenolic derivative that can be extracted from spices and herbs like cinnamon, nutmeg, basil, cloves, and some natural oils. Eugenol is a yellow oily liquid with the characteristic fragrance of cloves. The phenol belongs to the most active natural antioxidants found in essential oils. <br />
[[File:eug_structure.png|400px|thumb|left|Figure 1: Chemical structure of eugenol]] <br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP Stock<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=File:Eug_structure.png&diff=8869File:Eug structure.png2018-05-10T23:38:18Z<p>Shounsve: File uploaded with MsUpload</p>
<hr />
<div>File uploaded with MsUpload</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8868SAHounsve Spring 20182018-05-10T23:34:25Z<p>Shounsve: /* Results */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP Stock<br />
<br />
===Results===<br />
Eugenol oxidized by HRP activated by hydrogen peroxide in solution is seen in Figure 2. <br />
The eugenol peak is at 13 minutes, with the top being the 1 mM eugenol standard only. The following peaks below the eugenol standard are increasing amounts of hydrogen peroxide. As the concentration of hydrogen peroxide increases, the eugenol peak decreases. This means that eugenol is being oxidized. <br />
As eugenol is being oxidized, the peak at 16 minutes could be a possible radical product because this peak increases in height as eugenol decreases.<br />
There is another peaks at 9 minutes, however we do not know what this peak is at this time.<br />
<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8867SAHounsve Spring 20182018-05-10T23:30:40Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. 1 mM Eugenol stock substrate of pH 7.4 PBS with 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP Stock<br />
<br />
===Results===<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8866SAHounsve Spring 20182018-05-10T23:29:48Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. Eugenol stock substrate of 1.0 mM PBS pH 7.4 and 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP Stock<br />
<br />
===Results===<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8864SAHounsve Spring 20182018-05-10T23:29:15Z<p>Shounsve: /* Instruments to be used */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC and UV-Vis<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. Eugenol stock subtrate of 1.0 mM PBS pH 7.4 and 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP stock<br />
<br />
===Results===<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8863SAHounsve Spring 20182018-05-10T23:28:58Z<p>Shounsve: /* Proposal */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
The purpose of the experiment is to report the observation of radical products of eugenol produced by horseradish peroxidase (HRP) and hydrogen peroxide by using HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. Eugenol stock subtrate of 1.0 mM PBS pH 7.4 and 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP stock<br />
<br />
===Results===<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8860SAHounsve Spring 20182018-05-10T23:25:06Z<p>Shounsve: /* Project Title */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
Enzymatic Metabolism of Eugenol<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
To understand the oxidation properties of eugenol by utilizing HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. Eugenol stock subtrate of 1.0 mM PBS pH 7.4 and 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP stock<br />
<br />
===Results===<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8663SAHounsve Spring 20182018-03-22T14:13:02Z<p>Shounsve: /* Experimental */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
To understand the oxidation properties of eugenol by utilizing HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC<br />
<br />
===Experimental===<br />
Eugenol standard for HPLC:<br />
15.5 ul of eugenol in 0.1 mM PBS with 10% ethanol, pH 7.4 and 1% tween. Used method "eugenol_SH_020918_b".<br />
<br />
Oxidation reaction:<br />
1. Eugenol stock subtrate of 1.0 mM PBS pH 7.4 and 10% ethanol<br />
2. 0.25 M H2O2 Stock<br />
3. HRP stock<br />
<br />
===Results===<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=SAHounsve_Spring_2018&diff=8662SAHounsve Spring 20182018-03-22T14:06:09Z<p>Shounsve: /* Proposal */</p>
<hr />
<div><P ALIGN="left"> Chemistry/Biochemistry Research 430 </P><br />
<P ALIGN="left"> Spring 2018 </P><br />
<P ALIGN="left"> Selene Hounsve </P><br />
<P ALIGN="left"> Senior Biochemistry Major </P><br />
==Research Times==<br />
Wed: 11AM-2PM<br />
<br />
Fri: 4-5 PM<br />
<br />
==Proposed Research Project==<br />
<br />
===Project Title===<br />
<br />
===General Information===<br />
Advisor: Dr. Bradley E. Sturgeon<br />
===Proposal===<br />
To understand the oxidation properties of eugenol by utilizing HPLC.<br />
<br />
===Instruments to be used===<br />
HPLC<br />
<br />
===Experimental===<br />
===Results===<br />
===Discussion===<br />
===Conclusion===<br />
===References===<br />
===Research pledge===<br />
I, Selene Hounsve, have read the Chem/Bioc 430 course syllabus and understand the general structure and expectations of the research program. The above material was prepared after consultation, and in conjunction with my research advisor.</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8523Photochromic Lenses2018-02-08T18:20:23Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|none|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|none|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|none|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
[[File:lenses_uv_3.png|400px|frame|none|Figure 4: A dental curing device was used to emit UV rays to polycarbonate lenses to darken over a time period of 40 seconds. The red graph is the dental curing device exposed to the probe. The blue graph is the dental curing device exposed to the lenses and probe.]]<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8522Photochromic Lenses2018-02-08T18:18:52Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|none|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|none|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|none|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
[[File:lenses_uv_3.png|400px|frame|none|Figure 4:]]<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=File:Lenses_uv_3.png&diff=8521File:Lenses uv 3.png2018-02-08T18:18:30Z<p>Shounsve: File uploaded with MsUpload</p>
<hr />
<div>File uploaded with MsUpload</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=File:Lenses_uv_2.png&diff=8520File:Lenses uv 2.png2018-02-08T18:17:14Z<p>Shounsve: File uploaded with MsUpload</p>
<hr />
<div>File uploaded with MsUpload</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8519Photochromic Lenses2018-02-08T18:15:17Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|none|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|none|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|none|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
[[File:lenses_uv.png|400px|frame|none|Figure 4:]]<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=File:Lenses_uv.png&diff=8518File:Lenses uv.png2018-02-08T18:14:37Z<p>Shounsve: File uploaded with MsUpload</p>
<hr />
<div>File uploaded with MsUpload</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8509Photochromic Lenses2018-02-02T17:51:17Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|none|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|none|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|none|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8508Photochromic Lenses2018-02-02T17:49:30Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|block|400px|frame|left|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|block|400px|frame|left|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|center|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8507Photochromic Lenses2018-02-02T17:49:14Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|block|400px|frame|center|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|block|400px|frame|center|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|center|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8506Photochromic Lenses2018-02-02T17:46:29Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|center|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|center|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|center|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8505Photochromic Lenses2018-02-02T17:46:03Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|right|block|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|right|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|right|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8504Photochromic Lenses2018-02-02T17:45:19Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|right|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|right|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|right|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8503Photochromic Lenses2018-02-02T17:45:00Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|right|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|center|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|center|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8502Photochromic Lenses2018-02-02T17:44:35Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|frame|center|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|frame|center|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|frame|center|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8501Photochromic Lenses2018-02-02T17:40:44Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|thumb|left|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
*https://pubs.acs.org/cen/science/87/8715sci5.html<br />
*https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111<br />
*http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8500Photochromic Lenses2018-02-02T17:39:35Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|thumb|left|Figure 2: Benzoxazine is composed of an oxazine ring, a heterocyclic aromatic six-membered ring with oxygen and nitrogen, attached to a benzene ring.]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/<br />
https://www.sigmaaldrich.com/chemistry/chemistry-products.html?TablePage=16267111</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8499Photochromic Lenses2018-02-02T17:36:14Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
[[File:pyridobenzoaxine.png|400px|thumb|left|Figure 2:]]<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 3:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=File:Pyridobenzoaxine.png&diff=8498File:Pyridobenzoaxine.png2018-02-02T17:35:50Z<p>Shounsve: File uploaded with MsUpload</p>
<hr />
<div>File uploaded with MsUpload</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8497Photochromic Lenses2018-02-02T17:31:30Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 2:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8489Photochromic Lenses2018-02-01T23:07:10Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.<br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.<br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.<br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 2:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8488Photochromic Lenses2018-02-01T23:06:39Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<P ALIGN="left">Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear.</P><br />
<br />
<P ALIGN="left">Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken.</P><br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
<br />
<P ALIGN="left">Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes.</P><br />
<br />
<P ALIGN="left">Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.</P><br />
<br />
<P ALIGN="left">Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.</P><br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 2:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8483Photochromic Lenses2018-02-01T23:05:14Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear. <br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken. <br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes. <br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 2:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8481Photochromic Lenses2018-02-01T23:05:02Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear. <br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken. <br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes. <br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 2:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsvehttp://205.166.159.208/wiki/index.php?title=Photochromic_Lenses&diff=8475Photochromic Lenses2018-02-01T23:02:30Z<p>Shounsve: </p>
<hr />
<div>By Selene Hounsve<br />
<br />
Photochromic lenses are clear indoors and darken when exposed to sunlight. The first photochromic lenses were made of glass in the 1960s and glass photochromic lenses contain silver halide crystals embedded in a glass substrate. In the presence of UV light (320-400 nm), electrons from the glass combines with the colorless silver cations to form elemental silver. Elemental silver is visible which we see when the lenses darken. In absent of UV rays, the reaction is reversed. The silver returns to its original ionic state, and the lenses become clear. <br />
<br />
Glass photochromic lenses are still manufactured but are less popular than plastic photochromic lenses. The plastic photochromic lenses are completely different from the glass lenses. The first generation of plastic lenses were made of a family of organic dyes known as blue pyridobenzoxazines. Subsequent generations used naphthopyrans, and today lenses are made with indenonaphthopyrans. <br />
When a photochromic dye is exposed to UV radiation, a chemical bond is broken. The molecules then rearranges into a specific species that absorbs at longer wavelengths in the visible region, causing lenses to darken. <br />
<br />
[[File:photochromic_reaction.gif|400px|thumb|left|Figure 1:]]<br />
<br />
Improvements in the dyes over the years have led to faster activation and clearing, as well as longer lifetimes. For example, fusion of a bicyclic hydrocarbon group, called an indene group, to one of the benzene rings in a naphthopyran dye to make indenonaphthopyrans helps protect the dye from breaking down over time.<br />
The lenses material is important to support the layer of photochromic dyes, which affects how fast the lens darken and fades. Photochromic dyes do not work well in common plastic lenses, so companies developed special monomers that are compatible with the dyes. <br />
<br />
Thinner plastic lens materials used for strong prescriptions, such as polycarbonate and thiourea, are also not readily amenable to the photochromic dyes. For example, thioureas can attack the photochromic dyes, breaking them down fairly quickly. To get around those issues, Transitions has developed a process in which the photochromic dyes are sandwiched between multiple coatings of polyurethane on the surface of polycarbonate and thiourea lenses.<br />
<br />
Glass photochromic lenses offer better resistance to scratches and can faithfully switch between dark or clear for longer than their plastic lens counterparts. This is because glass lenses employ durable inorganic silver, whereas plastic lenses employ less robust organic dye molecules.<br />
<br />
[[File:img_1.jpg|400px|thumb|left|Figure 2:Transition of photochromic lenses exposed to UV radiation]]<br />
<br />
===Sources===<br />
https://pubs.acs.org/cen/science/87/8715sci5.html<br />
http://www.seiko-opt.co.jp/en/lens/pc/transitions_s/</div>Shounsve