Orbital hybridisation: Difference between revisions
Jump to navigation
Jump to search
imported>Robert Tito mNo edit summary |
imported>Petréa Mitchell m (Big Cleanup) |
||
| Line 1: | Line 1: | ||
<!-- This article uses -ise spelling(i.e. ...i*s*ation instead of i*z*ation) because it was originally written that way. Please do not change the spellings to the -ize variant. | <!-- This article uses -ise spelling(i.e. ...i*s*ation instead of i*z*ation) because it was originally written that way. Please do not change the spellings to the -ize variant. | ||
In [[chemistry]], '''hybridisation''' or '''hybridization''' (see also [[spelling differences]]) is the concept of mixing [[atomic orbital]]s to form new ''hybrid orbitals'' suitable for the qualitative description of atomic bonding properties. Hybridised orbitals are very useful in the explanation of the shape of [[molecular orbital]]s for [[molecule]]s. It is an integral part of [[valence bond theory]] and the [[VSEPR|valence shell electron-pair repulsion (VSEPR) theory]] <ref>Clayden, Greeves, Warren, Wothers. ''Organic Chemistry.'' Oxford University Press (2001), ISBN 0-19-850346-6.</ref> <ref>''Organic chemistry'' John McMurry 2nd Ed. ISBN 0534079687</ref>. | In [[chemistry]], '''hybridisation''' or '''hybridization''' (see also [[spelling differences]]) is the concept of mixing [[atomic orbital]]s to form new ''hybrid orbitals'' suitable for the qualitative description of atomic bonding properties. Hybridised orbitals are very useful in the explanation of the shape of [[molecular orbital]]s for [[molecule]]s. It is an integral part of [[valence bond theory]] and the [[VSEPR|valence shell electron-pair repulsion (VSEPR) theory]] <ref>Clayden, Greeves, Warren, Wothers. ''Organic Chemistry.'' Oxford University Press (2001), ISBN 0-19-850346-6.</ref> <ref>''Organic chemistry'' John McMurry 2nd Ed. ISBN 0534079687</ref>. | ||
| Line 79: | Line 77: | ||
== sp<sup>2</sup> hybrids == | == sp<sup>2</sup> hybrids == | ||
Other carbon based compounds and other molecules may be explained in a similar way as methane, take for example [[ethene]] (C<sub>2</sub>H<sub>4</sub>). Ethene has a double bond between the carbons. The Lewis structure looks like this: | Other carbon based compounds and other molecules may be explained in a similar way as methane, take for example [[ethene]] (C<sub>2</sub>H<sub>4</sub>). Ethene has a double bond between the carbons. The Lewis structure looks like this: | ||
Carbon will sp<sup>2</sup> hybridise, because hybrid orbitals will form only sigma bonds and one [[pi bond]] is required for the [[covalent bond|double bond]] between the carbons. The hydrogen-carbon bonds are all of equal strength and length, which agrees with experimental data. | Carbon will sp<sup>2</sup> hybridise, because hybrid orbitals will form only sigma bonds and one [[pi bond]] is required for the [[covalent bond|double bond]] between the carbons. The hydrogen-carbon bonds are all of equal strength and length, which agrees with experimental data. | ||
| Line 137: | Line 133: | ||
* [http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/hybrv18.swf Hybridisation flash movie] | * [http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/hybrv18.swf Hybridisation flash movie] | ||
[[Category:Chemistry Workgroup]] | [[Category:Chemistry Workgroup]] | ||