Ch7 lec 2 - Revision history

Bes at 13:11, 22 April 2020

2020-04-22T13:11:30Z

Bes: /* Electronic Structure Worksheets */

2020-04-22T13:09:56Z

Electronic Structure Worksheets

Bes: /* Electronic Structure Worksheets */

2020-04-22T13:09:32Z

Electronic Structure Worksheets

Bes: /* Sec 7.3: Bohr's Theory of the Hydrogen Atom */

2020-04-22T13:09:03Z

Sec 7.3: Bohr's Theory of the Hydrogen Atom

Bes: /* Sec 7.3: Bohr's Theory of the Hydrogen Atom */

2020-04-22T13:05:59Z

Sec 7.3: Bohr's Theory of the Hydrogen Atom

Bes: /* Sec 7.3: Bohr's Theory of the Hydrogen Atom */

2020-04-22T13:03:22Z

Sec 7.3: Bohr's Theory of the Hydrogen Atom

Bes: /* Sec 7.3: Bohr's Theory of the Hydrogen Atom */

2020-04-22T13:02:28Z

Sec 7.3: Bohr's Theory of the Hydrogen Atom

Bes: /* Sec 7.3: Bohr's Theory of the Hydrogen Atom */

2020-04-22T12:42:21Z

Sec 7.3: Bohr's Theory of the Hydrogen Atom

Bes: /* Sec 7.3: Bohr's Theory of the Hydrogen Atom */

2020-04-22T12:35:38Z

Sec 7.3: Bohr's Theory of the Hydrogen Atom

Bes: /* Sec 7.3: Bohr's Theory of the Hydrogen Atom */

2020-04-22T12:14:52Z

Sec 7.3: Bohr's Theory of the Hydrogen Atom

← Older revision		Revision as of 13:11, 22 April 2020
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−	(4/21/20, bes)	+	(4/22/20, bes)

	==Additional Light Lab Info==		==Additional Light Lab Info==

@@ Line 54: / Line 54: @@
 ====Electronic Structure Worksheets====
-(''These worksheets will not be collected. A similar WA will be generated shortly by Friday)''
+(''These worksheets will not be collected. A similar WA will be generated by Friday)''
 :# [[Media:Electronic Structure Worksheet I.docx|Electronic Worksheet I]]
 :# [[Media:Electronic Structure Worksheet II.docx|Electronic Worksheet II]]

@@ Line 54: / Line 54: @@
 ====Electronic Structure Worksheets====
-::(''These worksheets will not be collected. A similar WA will be generated shortly by Friday)''
+(''These worksheets will not be collected. A similar WA will be generated shortly by Friday)''
 :# [[Media:Electronic Structure Worksheet I.docx|Electronic Worksheet I]]
 :# [[Media:Electronic Structure Worksheet II.docx|Electronic Worksheet II]]

@@ Line 53: / Line 53: @@
 :::- ''R<sub>H</sub>'' = 13.6 eV <-- electron-volt
-===Worksheets===
+====Electronic Structure Worksheets====
 ==Sec 7.4: The Dual Nature of the Electron==

@@ Line 49: / Line 49: @@
 :where ''R = R<sub>H</sub>'' = Rydberg constant and is given in many different units (but they are all the same number)...
 :::- ''R<sub>H</sub>'' = 2.18e-18 J
-:::- ''R<sub>H</sub>'' = 1099,677.581 1/cm
+:::- ''R<sub>H</sub>'' = 109,677.581 1/cm
 :::- ''R<sub>H</sub>'' = 13.6 eV <-- electron-volt

@@ Line 44: / Line 44: @@
 An equation called the Rydberg Equation was concurrently (? <-- i need to explore this history) developed (see eq. 7.6)...and it is shown in a few different ways:
-[[File:Screen Shot 2020-04-22 at 7.55.28 AM.png|400px]]
 :where ''R = R<sub>H</sub>'' = Rydberg constant and is given in many different units (but they are all the same number)...
 :::- ''R<sub>H</sub>'' = 2.18e-18 J

@@ Line 35: / Line 35: @@
 :- If the electron is ''excited'' to a higher energy state/level, then when it relaxes back down to its original state/level it give off energy (''E'') in the form of light (''λ'').
 :- Since the H-atom has 4 emission lines (410, 434, 486, 656 nm) then there must be at least 5 energy levels (in the diagram below, n=2, n=3, n=4, n=5, and n=6). '''''STUDY THIS FIGURE'''''
-:[[File:Balmer_energy_levels.png|400px]]
+<div align="center">[[File:Balmer_energy_levels.png|400px]]</div>
 ==Sec 7.4: The Dual Nature of the Electron==

@@ Line 28: / Line 28: @@
 :[[File:Hydrogen_spectrum.001.png|400px]]
-'''''So why is the emission spectrum of the hydrogen atom look like it does?''''' The rest of this section tries to explain this complex answer...read carefully...
+'''''So why is the emission spectrum of the hydrogen atom look like it does?''''' The rest of this section explains this complex answer...read carefully...
-The observation of a single emission line, like the 656 nm emission line, implies that light with an energy of 3.03e-19 J is emitted ''(you can do this nm --> energy clac)''. In physics we learned about the conservation of energy, so if 3.03e-19 J of energy is given off, then something had to lose this energy. After much refinement of experiments and data analysis the following Bohr' model (theory) fo the hydrogen atom was proposed.
+The observation of a single emission line, like the 656 nm emission line, implies that light with an energy of 3.03e-19 J is emitted ''(you can do this nm --> energy clac)''. In physics we learned about the conservation of energy, so if 3.03e-19 J of energy is given off, then something had to lose this energy. After much refinement of experiments and data analysis the following Bohr' model (theory) for the hydrogen atom was proposed.
-:- This model/theory has been called the "planetary model" since it look a bit like the planets in out solar system.
+:- This model/theory has been called the "planetary model" since it look a bit like the planets in our solar system.
-:- The single electron in a H-atom must exist in an energy state (or at an energy level).
+:- The single electron in a H-atom must exist in an '''energy state''' (or at an '''energy level''' <--these mean the same thing).
-:- If the electron is excited to a higher state, then when it relaxes back down to its original state it give off energy (''E'') in the form of light (''λ'').
+:- If the electron is ''excited'' to a higher energy state/level, then when it relaxes back down to its original state/level it give off energy (''E'') in the form of light (''λ'').
-:- Since the H-atom has 4 emission lines then there must be at least 5 energy levels
+:- Since the H-atom has 4 emission lines (410, 434, 486, 656 nm) then there must be at least 5 energy levels (in the diagram below, n=2, n=3, n=4, n=5, and n=6). '''''STUDY THIS FIGURE'''''
 :[[File:Balmer_energy_levels.png|400px]]

@@ Line 25: / Line 25: @@
 ==Sec 7.3: Bohr's Theory of the Hydrogen Atom==
-An experiment i would have done with you in the lab would have involved the experimental setup shown in Figure 7.6 of your text. The light source would have been a  similar to a fluorescent tube, but the gas inside of the tube would have been hydrogen gas (H<sub>2</sub>) (see Figure 7.7). Now you don't really need to know this level of detail, but when a high voltage is applied across the "discharge tube" the H<sub>2</sub> gas breaks into individual H-atoms that then produce the "emission spectrum"...show in a "line spectrum" in Figure 7.6. The real emission spectrum would look like this...with emission lines at 410 nm (very small), 434 nm (small), 486 nm (medium), and 656 nm (largest):
+An experiment i would have done with you in the lab would have involved the experimental setup shown in Figure 7.6 of your text. The light source would have been a  similar to a small fluorescent tube, but the gas inside of the tube would have been hydrogen gas (H<sub>2</sub>) (see Figure 7.7). Now you don't really need to know this level of detail, but when a high voltage is applied across the "discharge tube" the H<sub>2</sub> gas breaks into individual H-atoms that then produce the "emission spectrum"...show in a "line spectrum" in Figure 7.6. The real emission spectrum would look like this...with emission lines at 410 nm (very small), 434 nm (small), 486 nm (medium), and 656 nm (largest):
 :[[File:Hydrogen_spectrum.001.png|400px]]
 ==Sec 7.4: The Dual Nature of the Electron==

← Older revision		Revision as of 12:14, 22 April 2020
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	==Sec 7.3: Bohr's Theory of the Hydrogen Atom==		==Sec 7.3: Bohr's Theory of the Hydrogen Atom==
		+	An experiment i would have done with you in the lab would have involved the experimental setup shown in Figure 7.6 of your text. The light source would have been a similar to a fluorescent tube, but the gas inside of the tube would have been hydrogen gas (H<sub>2</sub>) (see Figure 7.7). Now you don't really need to know this level of detail, but when a high voltage is applied across the "discharge tube" the H<sub>2</sub> gas breaks into individual H-atoms that then produce the "emission spectrum"...show in a "line spectrum" in Figure 7.6. The real emission spectrum would look like this...with emission lines at 410 nm (very small), 434 nm (small), 486 nm (medium), and 656 nm (largest):
		+	:[[File:Hydrogen_spectrum.001.png\|400px]]

	==Sec 7.4: The Dual Nature of the Electron==		==Sec 7.4: The Dual Nature of the Electron==