QuestionMay 9, 2025

Exercise 2.14 Describe the hybridization of the central atoms N and S in molecules and the molecular geometry of: a. NO_(2) b. SO_(3)

Exercise 2.14 Describe the hybridization of the central atoms N and S in molecules and the molecular geometry of: a. NO_(2) b. SO_(3)
Exercise 2.14 Describe the hybridization of the central atoms N and S in molecules and the molecular geometry of: a. NO_(2) b. SO_(3)

Solution
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Answer

a. In NO_2, the nitrogen atom is sp^2 hybridized, and the molecular geometry is bent (angular). ### b. In SO_3, the sulfur atom is sp^2 hybridized, and the molecular geometry is trigonal planar. Explanation 1. Determine the hybridization of the central atom in NO_2 The nitrogen atom in NO_2 has 5 valence electrons. In NO_2, it forms two sigma bonds with oxygen atoms and has one unpaired electron, resulting in a total of three regions of electron density. This corresponds to sp^2 hybridization. 2. Determine the molecular geometry of NO_2 With sp^2 hybridization, the molecular geometry is bent or angular due to the presence of an unpaired electron, which affects the bond angles. 3. Determine the hybridization of the central atom in SO_3 The sulfur atom in SO_3 has 6 valence electrons. It forms three sigma bonds with oxygen atoms, resulting in three regions of electron density. This corresponds to sp^2 hybridization. 4. Determine the molecular geometry of SO_3 With sp^2 hybridization and no lone pairs on the sulfur atom, the molecular geometry is trigonal planar.

Explanation

1. Determine the hybridization of the central atom in $NO_2$<br /> The nitrogen atom in $NO_2$ has 5 valence electrons. In $NO_2$, it forms two sigma bonds with oxygen atoms and has one unpaired electron, resulting in a total of three regions of electron density. This corresponds to $sp^2$ hybridization.<br />2. Determine the molecular geometry of $NO_2$<br /> With $sp^2$ hybridization, the molecular geometry is bent or angular due to the presence of an unpaired electron, which affects the bond angles.<br />3. Determine the hybridization of the central atom in $SO_3$<br /> The sulfur atom in $SO_3$ has 6 valence electrons. It forms three sigma bonds with oxygen atoms, resulting in three regions of electron density. This corresponds to $sp^2$ hybridization.<br />4. Determine the molecular geometry of $SO_3$<br /> With $sp^2$ hybridization and no lone pairs on the sulfur atom, the molecular geometry is trigonal planar.
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