Hybridisation: Difference between revisions
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A hybrid orbital results from the mixing of different atomic orbitals on the same [[ | A hybrid orbital results from the mixing of different atomic orbitals on the same [[Atom|atom]]. The atom can form stronger [[Covalent bonds|covalent bonds]] using these hybrid orbitals. When [[Atomic orbitals|atomic orbitals]] overlap they form two types of [[Covalent bonds|covalent bonds]]: sigma and pi. | ||
[[Sigma bond|Sigma bonds]] occur when two atomic orbitals overlap along the bond axis and this bond always forms in a single covalent bond. [[Pi-bonding|Pi bonds]] occur when two pi orbitals overlap sideways and they only form within a double or triple bond. A double bond contains one sigma bond and one pi bond, whereas a triple bond contains one sigma bond and two pi bonds. | [[Sigma bond|Sigma bonds]] occur when two atomic orbitals overlap along the bond axis and this bond always forms in a single covalent bond. [[Pi-bonding|Pi bonds]] occur when two pi orbitals overlap sideways and they only form within a double or triple bond. A double bond contains one sigma bond and one pi bond, whereas a triple bond contains one sigma bond and two pi bonds. | ||
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There are three types of hybridization: sp<sup>3</sup>, sp<sup>2</sup> and sp. | There are three types of hybridization: sp<sup>3</sup>, sp<sup>2</sup> and sp. | ||
Sp<sup>3</sup> hybridization forms a tetrahedral structure with 109.5° between the orbitals. [[Carbon|Carbon]] undergoes sp<sup>3</sup> hybridization when it forms four single bonds and produces four equal orbitals. An example of sp<sup>3</sup> hybridization is [[ | Sp<sup>3</sup> hybridization forms a tetrahedral structure with 109.5° between the orbitals. [[Carbon|Carbon]] undergoes sp<sup>3</sup> hybridization when it forms four single bonds and produces four equal orbitals. An example of sp<sup>3</sup> hybridization is [[Methane|methane]], CH<sub>4 </sub><ref name="orb">ORBITAL PICTURE OF BONDING: ORBITAL COMBINATIONS, HYBRIDIZATION THEORY, and MOLECULAR ORBITALS, https://www.utdallas.edu/~scortes/ochem/OChem1_Lecture/Class_Materials/05_orbitals_hybrid_geom.pdf</ref>. | ||
Sp<sup>2</sup> hybridization forms a triangular planar shape with 120° between the orbitals. Carbon undergoes sp<sup>2</sup> hybridization when it forms a double bond, producing three equal orbitals. An example of sp<sup>2 </sup>hybridization is [[ | Sp<sup>2</sup> hybridization forms a triangular planar shape with 120° between the orbitals. Carbon undergoes sp<sup>2</sup> hybridization when it forms a double bond, producing three equal orbitals. An example of sp<sup>2 </sup>hybridization is [[Ethene|ethene]], C<sub>2</sub>H<sub>4</sub>. | ||
Sp hybridization forms a linear structure with 180° between the orbitals. Carbon undergoes sp hybridization when it forms a triple bond, creating two equal orbitals. An example of sp hybridization is ethyne, C<sub>2</sub>H<sub>2</sub>. | Sp hybridization forms a linear structure with 180° between the orbitals. Carbon undergoes sp hybridization when it forms a triple bond, creating two equal orbitals. An example of sp hybridization is ethyne, C<sub>2</sub>H<sub>2</sub>. | ||
=== References === | === References === | ||
<references /> | <references /> | ||
Revision as of 12:09, 5 December 2017
A hybrid orbital results from the mixing of different atomic orbitals on the same atom. The atom can form stronger covalent bonds using these hybrid orbitals. When atomic orbitals overlap they form two types of covalent bonds: sigma and pi.
Sigma bonds occur when two atomic orbitals overlap along the bond axis and this bond always forms in a single covalent bond. Pi bonds occur when two pi orbitals overlap sideways and they only form within a double or triple bond. A double bond contains one sigma bond and one pi bond, whereas a triple bond contains one sigma bond and two pi bonds.
There are three types of hybridization: sp3, sp2 and sp.
Sp3 hybridization forms a tetrahedral structure with 109.5° between the orbitals. Carbon undergoes sp3 hybridization when it forms four single bonds and produces four equal orbitals. An example of sp3 hybridization is methane, CH4 [1].
Sp2 hybridization forms a triangular planar shape with 120° between the orbitals. Carbon undergoes sp2 hybridization when it forms a double bond, producing three equal orbitals. An example of sp2 hybridization is ethene, C2H4.
Sp hybridization forms a linear structure with 180° between the orbitals. Carbon undergoes sp hybridization when it forms a triple bond, creating two equal orbitals. An example of sp hybridization is ethyne, C2H2.
References
- ↑ ORBITAL PICTURE OF BONDING: ORBITAL COMBINATIONS, HYBRIDIZATION THEORY, and MOLECULAR ORBITALS, https://www.utdallas.edu/~scortes/ochem/OChem1_Lecture/Class_Materials/05_orbitals_hybrid_geom.pdf