All possible bond angles in anionic part of `PCl_(5)` are

Options

A. `109^(@) 28'` only
B. `90^(@),180^(@)`
C. `90^(@), 120^(@),180^(@)`
D. `72^(@),90^(@),180^(@)`

Answer

To determine the possible bond angles in the anionic part of PCl5, we will follow these steps:

### Step 1: Identify the Anionic Part
PCl5 can dissociate into PCl4+ (cation) and PCl6- (anion). We will focus on the PCl6- part for our analysis.

### Step 2: Determine the Hybridization
To find the hybridization, we can use the formula:
\[ x = \frac{1}{2} \left( \text{Valence electrons of central atom} + \text{Monovalent atoms} - \text{Charge on cation} + \text{Charge on anion} \right) \]

For PCl6-:
- Valence electrons of phosphorus (P) = 5 (since it is in group 15)
- Monovalent atoms (Cl) = 6 (there are 6 Cl atoms)
- Charge on cation (PCl4+) = +1
- Charge on anion (PCl6-) = -1

Plugging in these values:
\[ x = \frac{1}{2} \left( 5 + 6 - 1 + 1 \right) = \frac{1}{2} \left( 11 \right) = 6 \]

### Step 3: Identify the Hybridization Type
Since \( x = 6 \), the hybridization is \( sp^3d^2 \).

### Step 4: Determine the Shape of the Molecule
The shape corresponding to \( sp^3d^2 \) hybridization is octahedral.

### Step 5: Identify the Bond Angles
In an octahedral structure, there are two types of bond angles:
- The bond angles between the axial and equatorial positions are 90 degrees.
- The bond angles between the axial positions are 180 degrees.

### Conclusion
Thus, the possible bond angles in the anionic part of PCl5 (PCl6-) are:
- 90 degrees
- 180 degrees

### Final Answer
The possible bond angles in the anionic part of PCl5 are 90 degrees and 180 degrees.

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