Question
Identify the correct statement about $ClF_3$ from the following options :
This question was previously asked in
NEET UG Re-Exam 2026 Question Paper (21-Jun-2026)
The correct answer is
It has T-shaped geometry with two lone pairs on Cl atom.
Analyzing $ClF_3$ Structure
To determine the correct statement about $ClF_3$, we need to find its molecular geometry and the number of lone pairs on the central chlorine (Cl) atom using VSEPR theory.
1. Valence Electron Count
- Chlorine (Cl) is in Group 17, contributing 7 valence electrons.
- Fluorine (F) is in Group 17, contributing 7 valence electrons each.
- Total valence electrons = 7 (Cl) + 3 \times 7 (F) = 7 + 21 = 28 electrons.
2. Lewis Structure and Lone Pairs
- Cl is the central atom, bonded to three F atoms (3 single bonds). This uses 6 electrons.
- Each F atom needs 6 electrons to complete its octet (3 lone pairs per F). This uses 18 electrons.
- Total electrons used so far = 6 + 18 = 24 electrons.
- Remaining electrons = 28 - 24 = 4 electrons.
- These 4 electrons are placed on the central Cl atom as lone pairs.
- So, the Cl atom has 3 bonding pairs and 2 lone pairs.
3. Electron and Molecular Geometry
- The central Cl atom has 5 electron domains (3 bonding + 2 lone pairs).
- The electron geometry for 5 domains is trigonal bipyramidal.
- In trigonal bipyramidal geometry, lone pairs occupy equatorial positions to minimize repulsion.
- The 2 lone pairs will occupy two equatorial positions, and the 3 F atoms will occupy the remaining one equatorial and two axial positions.
- This arrangement results in a T-shaped molecular geometry.
4. Evaluating Options
- Option 1 is incorrect: $ClF_3$ has 2 lone pairs, not 3.
- Option 2 is incorrect: The geometry is T-shaped, not planar trigonal.
- Option 3 is correct: It has a T-shaped geometry with two lone pairs on the Cl atom.
- Option 4 is incorrect: The geometry is T-shaped, not trigonal pyramidal.
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