The bond angle between hybrid orbitals in methane CH3 is___________?
Correct answer: B. 109.5°
- A. 115.5°
- B. 109.5°
- C. 105. 7°
- D. 180°
Explanation
In methane, each carbon atom is sp3 hybridised and the four bonding orbitals point towards the corners of a tetrahedron. The angle between these equivalent hybrid orbitals is 109.5°. The likely distractor is 180°, option d, which belongs to linear sp hybridisation rather than tetrahedral sp3 hybridisation.
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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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