Chapter 3: Problem 25

Discuss the geometry of the following molecules: (a) \(\mathrm{ClF}_{3}\) (b) \(\mathrm{XeF}_{2}\) (c) IF, (d) \(\mathrm{PCl}\),

Short Answer

Expert verified

The geometries of molecules are as follows: \n(a) ClF3 - T-Shaped \n(b) XeF2 - Linear \n(c) IF - Bent \n(d) PCl - Bent

Step by step solution

Determine the Lewis structure and VSEPR structure of ClF3

Start by drwaing the Lewis structure of ClF3. Cl is in the center with F atoms surrounding it and extra lone pairs on Cl. From this, we find that there are 3 bonding pairs and 2 lone pairs of electrons. According to VSEPR theory, this leads to a T-Shaped structure.

Determine the Lewis structure and VSEPR structure of XeF2

For XeF2, Xe is in center with F atoms and 3 lone pairs around it. There are 2 bonding pairs and 3 lone pairs of electrons. According to VSEPR theory, this leads to a Linear structure.

Determine the Lewis structure and VSEPR structure of IF

For IF, draw I in the center with F atom and along with three lone pairs around it. This shows that there are 1 bonding pair and 3 lone pairs of electrons. According to VSEPR theory, this would lead to a Bent structure.

Determine the Lewis structure and VSEPR structure of PCl

In PCl, P is in the center with Cl atom and a lone pair around it. This indicates 1 bonding pair and 1 lone pair of electrons. According to VSEPR theory, this would lead to a Bent structure.

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Discuss the geometry of the following molecules: (a) \(\mathrm{ClF}_{3}\) (b) \(\mathrm{XeF}_{2}\) (c) IF, (d) \(\mathrm{PCl}\),

Short Answer

Step by step solution

Determine the Lewis structure and VSEPR structure of ClF3

Determine the Lewis structure and VSEPR structure of XeF2

Determine the Lewis structure and VSEPR structure of IF

Determine the Lewis structure and VSEPR structure of PCl

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