http://205.166.159.208/wiki/index.php?action=history&feed=atom&title=Gen_Chem_Ch9_Lec_1 2026-04-07T03:17:41Z Revision history for this page on the wiki MediaWiki 1.35.5 http://205.166.159.208/wiki/index.php?title=Gen_Chem_Ch9_Lec_1&diff=14227&oldid=prev 2020-05-04T21:04:53Z

<p><span dir="auto"><span class="autocomment">Chapter 9: Chemical Bonding</span></span></p> <table class="diff diff-contentalign-left diff-editfont-monospace" data-mw="interface"> <col class="diff-marker" /> <col class="diff-content" /> <col class="diff-marker" /> <col class="diff-content" /> <tr class="diff-title" lang="en"> <td colspan="2" style="background-color: #fff; color: #202122; text-align: center;">← Older revision</td> <td colspan="2" style="background-color: #fff; color: #202122; text-align: center;">Revision as of 21:04, 4 May 2020</td> </tr><tr><td colspan="2" class="diff-lineno" id="mw-diff-left-l8" >Line 8:</td> <td colspan="2" class="diff-lineno">Line 8:</td></tr> <tr><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><div>The most stable elements in the periodic table are the nobel gases, He, Ne, Ar, Kr, Xe, Rn. Why? '''''The answer is that they have a full shell of electrons.'''</div></td><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><div>The most stable elements in the periodic table are the nobel gases, He, Ne, Ar, Kr, Xe, Rn. Why? '''''The answer is that they have a full shell of electrons.'''</div></td></tr> <tr><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><div>::- He --&gt; full 1s (this one is a bit different and is why it sometimes shows up in the periodic table over near H)</div></td><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><div>::- He --&gt; full 1s (this one is a bit different and is why it sometimes shows up in the periodic table over near H)</div></td></tr> <tr><td class='diff-marker'>−</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div>::- Ne --&gt; full 2p</div></td><td class='diff-marker'>+</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div>::- Ne --&gt; full <ins class="diffchange diffchange-inline">2s and </ins>2p</div></td></tr> <tr><td class='diff-marker'>−</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div>::- Ar --&gt; full 3p</div></td><td class='diff-marker'>+</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div>::- Ar --&gt; full <ins class="diffchange diffchange-inline">3s and </ins>3p</div></td></tr> <tr><td class='diff-marker'>−</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div>::- Kr --&gt; full 4p</div></td><td class='diff-marker'>+</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div>::- Kr --&gt; full <ins class="diffchange diffchange-inline">4s and </ins>4p</div></td></tr> <tr><td class='diff-marker'>−</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div>::- Xe --&gt; full 5p  </div></td><td class='diff-marker'>+</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div>::- Xe --&gt; full <ins class="diffchange diffchange-inline">5s and </ins>5p  </div></td></tr> <tr><td class='diff-marker'>−</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #ffe49c; vertical-align: top; white-space: pre-wrap;"><div>::- Rn --&gt; full 6p</div></td><td class='diff-marker'>+</td><td style="color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #a3d3ff; vertical-align: top; white-space: pre-wrap;"><div>::- Rn --&gt; full <ins class="diffchange diffchange-inline">6s and </ins>6p</div></td></tr> <tr><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"></td><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"></td></tr> <tr><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><div>===Ionic Bonding (Sec 9.2)===</div></td><td class='diff-marker'> </td><td style="background-color: #f8f9fa; color: #202122; font-size: 88%; border-style: solid; border-width: 1px 1px 1px 4px; border-radius: 0.33em; border-color: #eaecf0; vertical-align: top; white-space: pre-wrap;"><div>===Ionic Bonding (Sec 9.2)===</div></td></tr> </table>

Bes http://205.166.159.208/wiki/index.php?title=Gen_Chem_Ch9_Lec_1&diff=14226&oldid=prev 2020-05-04T21:03:47Z

<p>Created page with &quot;(5/4/20, bes) Sorry i am so late...got caught up in grading. ==Chapter 9: Chemical Bonding== As we are all aware, elements in the periodic table form associations with other...&quot;</p> <p><b>New page</b></p><div>(5/4/20, bes)<br /> <br /> Sorry i am so late...got caught up in grading.<br /> <br /> ==Chapter 9: Chemical Bonding==<br /> As we are all aware, elements in the periodic table form associations with other elements...the question is why? I am going to answer this for your in the following discussion.<br /> <br /> The most stable elements in the periodic table are the nobel gases, He, Ne, Ar, Kr, Xe, Rn. Why? '''''The answer is that they have a full shell of electrons.'''<br /> ::- He --&gt; full 1s (this one is a bit different and is why it sometimes shows up in the periodic table over near H)<br /> ::- Ne --&gt; full 2p<br /> ::- Ar --&gt; full 3p<br /> ::- Kr --&gt; full 4p<br /> ::- Xe --&gt; full 5p <br /> ::- Rn --&gt; full 6p<br /> <br /> ===Ionic Bonding (Sec 9.2)===<br /> So one of the most common ionic compound we discussed was NaCl...why is this so stable...<br /> :- Na 1s2 2s2 2p6 3s1... if it loses 1 electron then it has the electron configuration of Ne.<br /> :- Cl 1s2 2s2 2p6 3s2 3p5... if it gains 1 electron then it has the electron configuration of Ar.<br /> ::So, NaCl is sort of like NeAr, but since Na+ is a cation and Cl- is an anion, they strongly associate with each other forming a strong ionic bond.<br /> <br /> '''''The above discussion holds for all of the alkali metals and halogens.'''''<br /> <br /> The same goes for all of the alkaline earth metals...except these lose 2 electrons from the &quot;s-orbital&quot; and hence associate with 2 halogen anions, ex. CaCl&lt;sub&gt;2&lt;/sub&gt;.<br /> <br /> Please look over this book section...end of this short lecture :)</div>

Bes