Shape of `PCl_5` molecule is

Options

A. Octahedron
B. Square pyramid
C. Trigonal bipyramid
D. Pyramidal

Explanation

To determine the shape of the PCl₅ molecule, we can follow these steps:

### Step 1: Identify the central atom and its valence electrons
- The central atom in PCl₅ is phosphorus (P). Phosphorus is in group 15 of the periodic table and has 5 valence electrons.

### Step 2: Count the number of surrounding atoms
- PCl₅ has 5 chlorine (Cl) atoms surrounding the phosphorus atom.

### Step 3: Determine the total number of electron pairs
- Each P-Cl bond involves one pair of electrons. Therefore, with 5 P-Cl bonds, we have 5 bonding pairs of electrons and no lone pairs on the phosphorus atom.

### Step 4: Determine the hybridization of the central atom
- To accommodate 5 bonding pairs, phosphorus undergoes hybridization. The hybridization that accommodates 5 pairs of electrons is sp³d. This involves the mixing of one s orbital, three p orbitals, and one d orbital.

### Step 5: Determine the molecular geometry based on hybridization
- The geometry associated with sp³d hybridization is trigonal bipyramidal. In this arrangement, there are three equatorial positions in one plane and two axial positions above and below this plane.

### Step 6: Visualize the shape
- In the trigonal bipyramidal shape, the three chlorine atoms in the equatorial plane are 120 degrees apart, while the two axial chlorine atoms are positioned 90 degrees to the equatorial plane.

### Conclusion
- Therefore, the shape of the PCl₅ molecule is trigonal bipyramidal.

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