Question:
Identify the shape of \(\text{IF}_5\) molecule from the following options.
Identify the shape of \(\text{IF}_5\) molecule from the following options.
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Count bond pairs and lone pairs on iodine: 5 bond pairs and 1 lone pair.
Updated On: Oct 1, 2026
- Trigonal bipyramidal
- Square planar
- Hexagonal
- Square pyramidal
Show Solution
Verified By Collegedunia
The Correct Option is D
Solution and Explanation
Step 1: Count electron pairs on iodine
Iodine has \(7\) valence electrons. Five are used in bonds with fluorine, leaving \(2\) electrons, which is one lone pair.
So there are \(5\) bond pairs and \(1\) lone pair, \(6\) pairs in total.
Step 2: Find the geometry
Six electron pairs give an octahedral arrangement (\(sp^3d^2\) hybridisation).
The lone pair takes one octahedral position, leaving five atoms in a square pyramid shape.
Step 3: Other options
Trigonal bipyramidal needs \(5\) pairs in all. Square planar is the shape of XeF\(_4\) (4 bonds, 2 lone pairs). Hexagonal does not occur for such molecules.
Final Answer:
IF\(_5\) is square pyramidal, option (D). \[ \boxed{\text{(D) Square pyramidal}} \]
Iodine has \(7\) valence electrons. Five are used in bonds with fluorine, leaving \(2\) electrons, which is one lone pair.
So there are \(5\) bond pairs and \(1\) lone pair, \(6\) pairs in total.
Step 2: Find the geometry
Six electron pairs give an octahedral arrangement (\(sp^3d^2\) hybridisation).
The lone pair takes one octahedral position, leaving five atoms in a square pyramid shape.
Step 3: Other options
Trigonal bipyramidal needs \(5\) pairs in all. Square planar is the shape of XeF\(_4\) (4 bonds, 2 lone pairs). Hexagonal does not occur for such molecules.
Final Answer:
IF\(_5\) is square pyramidal, option (D). \[ \boxed{\text{(D) Square pyramidal}} \]
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