Question

The shapes of the compounds ClF\(_3\), XeOF\(_2\), N\(_3^-\) and XeO\(_3\)F\(_2\) respectively, are:

• A. T-shape, T-shape, linear and trigonal bipyramidal
• B. trigonal planar, T-shape, V-shape and square pyramidal
• C. T-shape, trigonal planar, linear and square pyramidal
• D. trigonal planar, trigonal planar, V-shape and trigonal bipyramidal

Hint:

Use the VSEPR theory to predict the shapes of molecules based on the number of bonding pairs and lone pairs.

Answer 1

The Correct Option is A

Step 1: Analyze the Molecular Geometries.
- ClF\(_3\): Chlorine trifluoride has three bonding pairs and two lone pairs, resulting in a T-shape geometry.
- XeOF\(_2\): Xenon oxyfluoride has two bonding pairs of fluorine and one bonding pair of oxygen, giving it a T-shape geometry.
- N\(_3^-\): The azide ion has a linear structure due to the bonding between nitrogen atoms.
- XeO\(_3\)F\(_2\): Xenon trioxide difluoride has five bonding pairs (three oxygen and two fluorine), giving it a trigonal bipyramidal geometry.

Step 2: Conclusion.
The correct geometries for these compounds are T-shape, T-shape, linear, and trigonal bipyramidal, respectively.

Final Answer: \[ \text{T-shape, T-shape, linear and trigonal bipyramidal.} \]