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Electronegativity and Bonding Between Atoms - Revision history
2026-06-08T13:07:52Z
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Cmditradmin at 19:27, 29 December 2009
2009-12-29T19:27:25Z
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Cmditradmin
http://cleanenergywiki.org/index.php?title=Electronegativity_and_Bonding_Between_Atoms&diff=5839&oldid=prev
Cmditradmin at 00:15, 22 December 2009
2009-12-22T00:15:11Z
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Cmditradmin
http://cleanenergywiki.org/index.php?title=Electronegativity_and_Bonding_Between_Atoms&diff=4442&oldid=prev
Nsylvain at 00:49, 27 August 2009
2009-08-27T00:49:50Z
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Nsylvain
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Cmditradmin at 23:17, 26 August 2009
2009-08-26T23:17:57Z
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<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;"><br/></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;"><br/></td></tr>
<tr><td class="diff-marker" data-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>[[Image:Ionization_pot.jpg|thumb|300px|Energy level diagram showing the relation between electron affinity (EA), ionization potential (IP) to the vacuum level and the valence band]]</div></td><td class="diff-marker" data-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>[[Image:Ionization_pot.jpg|thumb|300px|Energy level diagram showing the relation between <ins style="font-weight: bold; text-decoration: none;">electronegativity (&chi;), </ins>electron affinity (EA), ionization potential (IP) to the vacuum level and the valence band]]</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>Electronegativity describes how much an atom hold its electrons tightly. An atom that is less electronegative will be more likely to give up its electrons. The electronegativity of atoms determines the degree that electrons are transferred between molecules or shared between bonding atoms. </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>Electronegativity describes how much an atom hold its electrons tightly. An atom that is less electronegative will be more likely to give up its electrons. The electronegativity of atoms determines the degree that electrons are transferred between molecules or shared between bonding atoms. </div></td></tr>
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Cmditradmin
http://cleanenergywiki.org/index.php?title=Electronegativity_and_Bonding_Between_Atoms&diff=4434&oldid=prev
Cmditradmin at 23:17, 26 August 2009
2009-08-26T23:17:10Z
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<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>[[Image:Ionization_pot.jpg|thumb|300px|Energy level diagram showing the relation between electron affinity (EA), ionization potential (IP) to the vacuum level and the valence band]]</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>[[Image:Ionization_pot.jpg|thumb|300px|Energy level diagram showing the relation between electron affinity (EA), ionization potential (IP) to the vacuum level and the valence band]]</div></td></tr>
<tr><td class="diff-marker" data-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>Electronegativity describes how much an atom hold its electrons tightly. An atom that is less electronegative will be more likely to give up its electrons. The electronegativity of atoms determines the degree that electrons are transferred between molecules or shared between bonding atoms. </div></td><td class="diff-marker" data-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>Electronegativity <ins style="font-weight: bold; text-decoration: none;"> </ins>describes how much an atom hold its electrons tightly. An atom that is less electronegative will be more likely to give up its electrons. The electronegativity of atoms determines the degree that electrons are transferred between molecules or shared between bonding atoms. </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;"><br/></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;"><br/></td></tr>
<tr><td class="diff-marker" data-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>Mulliken presents a useful definition of electronegativity as the average of the ionization potential (IP) and the electron affinity (EA).</div></td><td class="diff-marker" data-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>Mulliken presents a useful definition of electronegativity <ins style="font-weight: bold; text-decoration: none;">(&chi;) </ins>as the average of the ionization potential (IP) and the electron affinity (EA).</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;"><br/></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;"><br/></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>:<math>\chi = \frac{IP + EA}{ 2}\,\!</math></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>:<math>\chi = \frac{IP + EA}{ 2}\,\!</math></div></td></tr>
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<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>Note that the ionization potential is the energy required to remove an electron from an atom (to vacuum) and the electron affinity is the energy released when an atom captures an electron (into the lowest unfilled orbital).</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>Note that the ionization potential is the energy required to remove an electron from an atom (to vacuum) and the electron affinity is the energy released when an atom captures an electron (into the lowest unfilled orbital).</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;"><br/></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;"><br/></td></tr>
<tr><td class="diff-marker" data-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>The more electronegative the atom is the lower the energy of the orbital within a given row. <del style="font-weight: bold; text-decoration: none;">As you move </del>to the right on the periodic table across a row the electronegativity increases because the number of protons increases which increases the pull on the electrons. When the difference in electronegativity is great, as in Na<sup>+</sup> and Cl<sup>-</sup>, the electron is transferred from the electropositive species to the more electronegative species. These ionic compounds are held together by electrostatic forces and form a salt. In pure covalent bonds between like atoms each of the bonding electrons are shared equally. The electron density is highest between the atoms an there is no dipole moment. When there is slight difference in electronegativities for example in in C-F bond, the fluorine holds the electrons closer, the carbon less so. The whole bond has a polarity with unequal distribution of electrons..</div></td><td class="diff-marker" data-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>The more electronegative the atom is the lower the energy of the orbital within a given row. <ins style="font-weight: bold; text-decoration: none;">Moving </ins>to the right on the periodic table across a row the electronegativity increases because the number of protons increases which increases the pull on the electrons. When the difference in electronegativity is great, as in Na<sup>+</sup> and Cl<sup>-</sup>, the electron is transferred from the electropositive species to the more electronegative species. These ionic compounds are held together by electrostatic forces and form a salt. In pure covalent bonds between like atoms each of the bonding electrons are shared equally. The electron density is highest between the atoms an there is no dipole moment. When there is slight difference in electronegativities for example in in C-F bond, the fluorine holds the electrons closer, the carbon less so. The whole bond has a polarity with unequal distribution 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;"><br/></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;"><br/></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>Here is a summary of the different kinds of bonds.</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>Here is a summary of the different kinds of bonds.</div></td></tr>
</table>
Cmditradmin
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Cmditradmin at 22:15, 25 August 2009
2009-08-25T22:15:02Z
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Cmditradmin
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Cmditradmin at 22:14, 25 August 2009
2009-08-25T22:14:38Z
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Cmditradmin
http://cleanenergywiki.org/index.php?title=Electronegativity_and_Bonding_Between_Atoms&diff=4325&oldid=prev
Cmditradmin at 22:14, 25 August 2009
2009-08-25T22:14:15Z
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Cmditradmin
http://cleanenergywiki.org/index.php?title=Electronegativity_and_Bonding_Between_Atoms&diff=4324&oldid=prev
Cmditradmin at 22:12, 25 August 2009
2009-08-25T22:12:23Z
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Cmditradmin
http://cleanenergywiki.org/index.php?title=Electronegativity_and_Bonding_Between_Atoms&diff=4323&oldid=prev
Cmditradmin at 22:12, 25 August 2009
2009-08-25T22:12:04Z
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