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Wize University Chemistry Textbook > Valence Bond Theory (Hybridization)

Detailed Look at Hybridization

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sp3 Hybridization

  • Consider a CH4 molecule. Based on VSEPR Theory, we expect a tetrahedral geometry. Based on the structure and based on experimental data, we expect all four covalent bonds to be equal in energy (i.e., identical); however, based on their atomic orbitals, we expect 3 x 1s-2p orbitals and 1 x 1s-2s orbitals between the hydrogen and carbon atoms. Therefore, we need a new bonding model →\rightarrow Valence Bond (Hybridization) Theory.













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sp3 Hybridization - Example Problem

Ex) Determine the hybridization of H2O.


The oxygen atom bonds with the 2 hydrogen atoms with two sp3 hybridized orbitals. The two lone pairs sit in unbonded sp3 hybridized orbitals. See video for explanation.
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sp2 Hybridization

  • Consider a BH3 molecule. Like with sp3 hybridization, the atomic orbitals of B will hybridize one s orbital and two p orbitals to form 3 identical sp2 hybridized orbitals.











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sp2 Hybridization - Example Problem

Ex) Determine the hybridization of NH2+.


The nitrogen atom bonds with two hydrogen atoms with two sp2 hybridized orbitals. The lone pair on the nitrogen sits in the remaining hybridized sp2 orbital. See video for explanation.
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sp Hybridization

  • Consider a BeH2 molecule. Similar to sp3 and sp2 hybridization, the atomic orbitals of Be will hybridize one s orbital and one p orbitals to form 2 identical sp hybridized orbitals to bond with the two H atoms.










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sp Hybridization - Example Problem

Ex) Determine the hybridization of CO.


The carbon atom bonds with the oxygen atom using one hybridized sp orbital. The lone pair on the carbon atom will sit in the other sp hybridized orbital. The oxygen atom is also sp hybridized.
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Unhybridized p Orbitals

  • In Valence Bond Theory, the unhybridized orbitals (often unhybridized p orbitals) can still participate in bonding to form π\pi bonds.

Ex) C2H4 and C2H2









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Unhybridized p Orbitals - Example Problem

Ex) Determine the hybridization of the C and O atoms in CO2. What are the orbitals responsible for all σ\sigma and π\pi bonds in the molecule?


C: sp
O: sp2
sigma bonds: C (sp) - O (sp2)
pi bonds: C (2p) - O (2p)
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dsp3 and d2sp3 Hybridization

Thus far, we have looked at the hybridization of linear (sp), trigonal planar (sp2) and tetrahedral (sp3) structures. What would be the hybridization of trigonal bipyramidal and octahedral structures?

Ex) PF5 and SF6










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dsp3 Hybridization - Example Problem

Ex) Describe all the orbitals involved in σ\sigma bonds, π\pi bonds and lone pairs in the structure of SeF4.


There are 4 σ\sigma bonds between Se and the 4 F atoms, which are bonded through dsp3-sp3 hybridized orbitals. There are no π\pi bonds. The lone pair on Se is in a dsp3 hybridized orbital, and the lone pairs on F are in sp3 hybridized orbitals.
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d2sp3 Hybridization - Example Problem

Ex) Describe all the orbitals involved in σ\sigma bonds, π\pi bonds and lone pairs in the structure of ICl5.


There are five σ\sigma bonds between the I atom and the 5 Cl atoms, which are bonded through d2sp3-sp3 hybridized orbitals. There are no π\pi bonds. The lone pair on the I atom is in a d2sp3 hybridized orbital. The lone pairs on the Cl atoms are in sp3 hybridized orbitals.

Practice Question: Hybridization with d Orbitals

Draw the Lewis structure of XeOCl4 to answer the following questions.