Given a molecule in which the antimony atom forms three sigma bonds and has one lone pair, what is the hybridization of the antimony atom?

• A. sp3
• B. dsp3
• C. sp2
• D. sp

Answer: (A)

Verified step by step guidance

1. Identify the number of regions of electron density around the antimony atom. Each sigma bond and lone pair counts as one region. Here, there are three sigma bonds and one lone pair, totaling four regions of electron density.
2. Recall that the hybridization of an atom depends on the number of electron regions around it. The general rule is: 2 regions correspond to sp, 3 regions to sp2, 4 regions to sp3, 5 regions to dsp3, and 6 regions to d2sp3 hybridization.
3. Since the antimony atom has four regions of electron density (3 bonds + 1 lone pair), the hybridization corresponds to sp3.
4. Understand that the presence of a lone pair affects the molecular geometry but does not change the count of electron regions used to determine hybridization.
5. Conclude that the antimony atom's hybridization is sp3 based on the total number of electron regions around it.