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Chapter 3: Problem 26

Discuss the geometry of the following ions: (a) \(\mathrm{ClO}_{3}^{-}\) (b) \(\mathrm{SO}_{4}^{2-}\) (c) \(\mathrm{NO}_{3}^{-}\)

Short Answer

Expert verified
The geometry of the following ions: (a) \(\mathrm{ClO}_{3}^{-}\) is trigonal pyramidal, (b) \(\mathrm{SO}_{4}^{2-}\) is tetrahedral, and (c) \(\mathrm{NO}_{3}^{-}\) is trigonal planar.

Step by step solution

01

Determine the Lewis Structure

Draw Lewis structure for each ion, showing all valence electrons around each atom. Make sure the atoms obey the octet rule, meaning each atom should be surrounded by eight electrons.
02

Determine the Electron Pair Geometry

Use the VSEPR theory to predict the electron pair geometry around the central atom. Count the number of bonding pairs (shared electrons) and non-bonding pairs (lone pairs) around the central atom.
03

Determine Molecular Geometry

The molecular geometry is determined by considering only the bonding pairs around the central atom. Ignore the lone pairs.
04

Discuss the Geometry of the Ions

(a) For \(\mathrm{ClO}_{3}^{-}\), the electron pair geometry is tetrahedral, and the molecular geometry is trigonal pyramidal. (b) For \(\mathrm{SO}_{4}^{2-}\), the electron pair geometry and molecular geometry are both tetrahedral. (c) For the \(\mathrm{NO}_{3}^{-}\), since there are no ester pairs on the nitrogen atom, the electron pair geometry and molecular geometry are both trigonal planar.

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