In the oxyacids of phosphorous the hybridisation of phosphorous is

Options

A. `sp^(3)`
B. `sp^(2)`
C. `sp`
D. `dsp^(2)`

Answer

To determine the hybridization of phosphorus in the oxyacids of phosphorus, we can follow these steps:

### Step 1: Identify the Oxyacid
The most common oxyacid of phosphorus is phosphoric acid, which has the chemical formula H₃PO₄.

### Step 2: Draw the Lewis Structure
To understand the hybridization, we need to draw the Lewis structure of H₃PO₄. The structure can be represented as follows:

- Phosphorus (P) is the central atom.
- It forms a double bond with one oxygen (O).
- It forms single bonds with three hydroxyl groups (OH).

The Lewis structure can be depicted as:
```
O
||
H - P - O - H
|
O - H
```

### Step 3: Count the Bonds
In the structure:
- There is 1 double bond (P=O).
- There are 3 single bonds (P-OH).

This results in a total of 4 bonds around the phosphorus atom.

### Step 4: Determine the Hybridization
To find the hybridization, we can use the formula:
- Hybridization = Number of sigma bonds + Number of lone pairs.

In H₃PO₄:
- There are 4 sigma bonds (3 from P-OH and 1 from P=O).
- There are no lone pairs on phosphorus.

Thus, the hybridization can be calculated as:
- Hybridization = 4 (sigma bonds) + 0 (lone pairs) = 4.

Since the hybridization number is 4, the hybridization type is sp³.

### Step 5: Determine the Geometry
The geometry of the molecule can be determined based on the hybridization:
- sp³ hybridization corresponds to a tetrahedral geometry.

### Conclusion
The hybridization of phosphorus in the oxyacids of phosphorus (specifically in H₃PO₄) is **sp³**.