The hybridisation of the carbon atom in carbon dioxide is
Correct answer: C. sp
- A. sp3
- B. sp2
- C. sp
- D. unhybridised
Explanation
The carbon has only two regions of electron density, since each double bond counts as one region, so two sp hybrid orbitals point in opposite directions and the molecule is linear. The two remaining unhybridised p orbitals form the pi bonds. Counting regions rather than bonds is what makes this quick.
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About Hybridization
Hybridization explains bonding by combining atomic orbitals to form equivalent hybrid orbitals with definite geometries. Coverage includes sp, sp², sp³, sp³d and sp³d² hybridization, their shapes and bond angles, and the relation of sigma and pi bonds to molecular structure.
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