Final answer:
In methanol, CH3OH, all C—H bonds are formed from C sp³ and H 1s orbitals, the C—O bond is formed from C sp³ and O sp³, and the O—H bond is from O sp³ and H 1s orbitals.
Step-by-step explanation:
The bonds in methanol, CH3OH, are formed by the overlap of different hybridized orbitals between carbon, oxygen, and hydrogen atoms.
All C—H bonds are formed from C sp³ — H1s. The C—O bond is formed from C sp³ — Osp³. The O—H bond is formed from Osp³ — H1s.
In a methane molecule, which has a similar carbon-hydrogen bonding to methanol, the 1s orbital of each of the four hydrogen atoms overlaps with one of the four sp³ orbitals of the carbon atom to form a sigma (o) bond, producing strong, equivalent covalent bonds. For the C—O and O—H bonds in methanol, the carbon and oxygen both use sp³ hybrid orbitals to form sigma bonds, while the hydrogen uses its 1s orbital.
Methanol also has the ability to form intermolecular hydrogen bonds due to the presence of the hydroxyl (-OH) group, but this aspect involves interactions between different methanol molecules, not the intramolecular bonding within a single molecule.