Given the structure of ${\mathrm{CH}}_3\mathrm{CH}{\mathrm{CH}}_2\mathrm{OH}$ (1-propanol), what is the hybridization of the carbon atom bonded directly to the hydroxyl group?

• A. ${\mathrm{sp}}^3$
• B. ${\mathrm{sp}}^1$
• C. ${\mathrm{sp}}^2$ and ${\mathrm{sp}}^3$ (both)
• D. ${\mathrm{sp}}^2$

Answer: (A)

Verified step by step guidance

1. Identify the carbon atom bonded directly to the hydroxyl group (-OH) in 1-propanol. This is the carbon in the -CH2OH group at the end of the chain.
2. Recall that the hybridization of a carbon atom depends on the number of regions of electron density (bonds and lone pairs) around it. Count the sigma bonds and lone pairs on this carbon.
3. The carbon bonded to the hydroxyl group forms four sigma bonds: two to hydrogen atoms, one to the adjacent carbon atom, and one to the oxygen atom of the hydroxyl group.
4. Since this carbon has four sigma bonds and no lone pairs, it has four regions of electron density, which corresponds to an \(sp^{3}\) hybridization.
5. Conclude that the carbon bonded directly to the hydroxyl group in 1-propanol is \(sp^{3}\) hybridized.