Predict the geometric structures of (a) \(\mathrm{BrF}_{3} ;\) (b) IF \(_{5}\); (c) \(\mathrm{Cl}_{3} \mathrm{IF}^{-}\). (Central atom underlined.).

Short Answer

Expert verified
The geometric structures of the molecules are: (a) \(\mathrm{BrF}_{3}\) - T-shaped, (b) IF\(_{5}\) - square pyramidal, (c) \(\mathrm{Cl}_{3} \mathrm{IF}^{-}\) - T-shaped

Step by step solution

01

Lewis Structure

Firstly, draw the Lewis structure for each molecule. The Lewis structure is a graphical representation of the molecule that shows how the electrons are arranged around individual atoms in the molecule.
02

Count electron regions

Using the Lewis structure, identify the regions where electrons are found. These include both bonding (shared) and nonbonding (unshared) electrons. Each bond, single, double or triple, counts as one region. The number of these regions helps determine the electron geometry.
03

Identify the molecular geometry

From the number of electron regions, use the VSEPR theory to predict the molecular geometry. If there are nonbonding electrons, it will affect the final molecular geometry.
04

Apply for each molecule

Repeat steps from 1 to 3 for each molecule. The Lewis structure, electron geometry, and molecular geometry for each are,\n (a) \(\mathrm{BrF}_{3}\): According to the VSEPR model, it exhibits a ‘T-shaped’ geometry. (b) IF \(_{5}\): The molecule adopts a square pyramidal geometry. (c) \(\mathrm{Cl}_{3} \mathrm{IF}^{-}\): The molecular geometry of \(\mathrm{Cl}_{3} \mathrm{IF}^{-}\) is T-shaped.

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