`PCl_5` has trigonal pyramidal geometry with `sp^3 d` hybridisation in gases and liquid state but in solid state it exist as ionic compound.
The hyridisation of `P` and shape of `POCl_3` are.

Options

A. `sp^3`, tetrahedral
B. `sp^3 d`, distorted tetrahedral
C. `sp^3 d`, square planar
D. `sp^3`, pyramidal

Explanation

To determine the hybridization and shape of POCl₃, we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
- The central atom in POCl₃ is phosphorus (P).
- Phosphorus is in group 15 of the periodic table and has 5 valence electrons.

### Step 2: Count the number of attached atoms
- In POCl₃, phosphorus is bonded to one oxygen (O) and three chlorine (Cl) atoms.
- Oxygen is a divalent atom, but we will focus on the monovalent atoms for our calculation.
- There are 3 chlorine atoms, each contributing 1 bond.

### Step 3: Calculate the steric number
- The steric number (SN) can be calculated using the formula:
\[ \text{Steric Number} = \frac{1}{2} \left( V + M + C \right) \]
where:
- \( V \) = number of valence electrons of the central atom (5 for P)
- \( M \) = number of monovalent atoms attached (3 for Cl)
- \( C \) = charge (0 for neutral compounds)

- Plugging in the values:
\[ \text{Steric Number} = \frac{1}{2} \left( 5 + 3 + 0 \right) = \frac{8}{2} = 4 \]

### Step 4: Determine the hybridization
- A steric number of 4 corresponds to \( sp^3 \) hybridization.

### Step 5: Determine the shape of the molecule
- With a steric number of 4 and no lone pairs on the central atom, the shape of the molecule is tetrahedral.

### Conclusion
- The hybridization of phosphorus in POCl₃ is \( sp^3 \).
- The shape of POCl₃ is tetrahedral.

### Summary
- **Hybridization**: \( sp^3 \)
- **Shape**: Tetrahedral