In methanol (CH3OH), which hybrid orbitals are used by the central carbon atom to form its bonds?

• A. sp hybrid orbitals
• B. sp3 hybrid orbitals
• C. Only unhybridized p orbitals
• D. sp2 hybrid orbitals

Answer: (B)

Verified step by step guidance

1. Identify the central atom in methanol (CH3OH), which is the carbon atom bonded to three hydrogen atoms and one oxygen atom.
2. Determine the number of regions of electron density (bonding and lone pairs) around the carbon atom. In methanol, carbon forms four single bonds: three with hydrogen and one with oxygen.
3. Recall that the hybridization of an atom depends on the number of electron regions around it: 4 regions correspond to sp3 hybridization, 3 regions to sp2, and 2 regions to sp.
4. Since carbon in methanol has four single bonds (four regions of electron density), it uses sp3 hybrid orbitals to form these bonds.
5. Conclude that the carbon atom in methanol uses sp3 hybrid orbitals to form its bonds, which explains the tetrahedral geometry around the carbon.