Shape of molecule having 4-bond pair and one lone pair is :-

Options

A. Trigonal bipyramidal
B. T-Shape
C. See saw
D. Square planar

Explanation

To determine the shape of a molecule with 4 bond pairs and 1 lone pair, we can use the VSEPR (Valence Shell Electron Pair Repulsion) theory. Here’s a step-by-step solution:

### Step 1: Identify the number of bond pairs and lone pairs
- We have 4 bond pairs and 1 lone pair in the molecule.

### Step 2: Determine the total number of electron pairs
- Total electron pairs = Bond pairs + Lone pairs = 4 + 1 = 5.

### Step 3: Determine the basic geometry
- With 5 electron pairs, the basic geometry is **trigonal bipyramidal**.

### Step 4: Consider the effect of lone pairs
- In a trigonal bipyramidal arrangement, lone pairs occupy equatorial positions to minimize repulsion. Therefore, one of the equatorial positions will be occupied by the lone pair.

### Step 5: Determine the molecular shape
- With 4 bond pairs and 1 lone pair, the resulting molecular shape is **seesaw** (also referred to as "K shape").

### Conclusion
- The shape of the molecule having 4 bond pairs and 1 lone pair is **seesaw**.

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