Question

Identify the correct statement about \(ClF_3\).

• A. It has T-shaped geometry with three lone pairs on Cl atom.
• B. It has planar trigonal geometry with two lone pairs on Cl atom.
• C. It has T-shaped geometry with two lone pairs on Cl atom.
• D. It has trigonal pyramidal geometry with two lone pairs on Cl atom.

Hint:

\(ClF_3\) has \(3\) bond pairs and \(2\) lone pairs, so its molecular geometry is T-shaped.

Answer 1

The Correct Option is C

Step 1: Count valence electrons of central atom.
In \(ClF_3\), chlorine is the central atom. Chlorine has: \[ 7 \] valence electrons.

Step 2: Count bond pairs.
Chlorine forms three bonds with three fluorine atoms. So number of bond pairs is: \[ 3 \]

Step 3: Count lone pairs on chlorine.
Out of \(7\) valence electrons of chlorine, \(3\) electrons are used for bonding. Remaining electrons: \[ 7-3=4 \] These \(4\) electrons form: \[ 2 \] lone pairs.

Step 4: Determine electron pair geometry.
Total electron pairs around chlorine: \[ 3+2=5 \] Five electron pairs give trigonal bipyramidal electron pair arrangement.

Step 5: Determine molecular shape.
In \(ClF_3\), two lone pairs occupy equatorial positions to reduce repulsion. The remaining three bond pairs form a T-shaped structure. Therefore: \[ ClF_3 \] has: \[ \text{T-shaped geometry with two lone pairs on chlorine}. \]