Concept:Hybridization is determined by counting the number of electron domains (sigma bonds and lone pairs) around an atom.
Solution:- In the formyl group (\( -CHO \)), the central carbon atom is double-bonded to an oxygen atom and single-bonded to a hydrogen atom and the rest of the R-group.
- This gives the carbon atom three electron domains (three regions of electron density).
- To accommodate three domains, one s-orbital mixes with two p-orbitals to form three \( sp^2 \) hybridized orbitals, leaving one unhybridized p-orbital to form the \( \pi \) bond with oxygen.
- The geometry is trigonal planar with bond angles of approximately 120°.
Why other options are incorrect:\( sp^3 \) hybridization occurs in single-bonded carbons (tetrahedral). \( sp \) hybridization occurs with triple bonds or two consecutive double bonds (linear).
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