What is the hybridization of the oxygen atom in $C_2{H}_{6}O$ (dimethyl ether, ${\mathrm{CH}}_{3}O{\mathrm{CH}}_3$)?

• A. $\mathrm{sp}$
• B. The oxygen atom is unhybridized
• C. $\mathrm{sp}{2}^{}$
• D. $\mathrm{sp}{3}^{}$

Answer: (D)

Verified step by step guidance

1. Identify the central atom of interest, which is the oxygen atom in dimethyl ether (CH3-O-CH3).
2. Determine the number of regions of electron density around the oxygen atom. These include both bonding pairs (to the two carbon atoms) and lone pairs on oxygen.
3. Recall that oxygen typically has two lone pairs and forms two single bonds in ethers, giving a total of four regions of electron density around it.
4. Use the steric number (number of regions of electron density) to determine hybridization: a steric number of 4 corresponds to sp\^3 hybridization.
5. Conclude that the oxygen atom in dimethyl ether is sp\^3 hybridized because it has four electron density regions (two bonds and two lone pairs).