The hybridisation of nitrogen in `R_(2)NH` is :

Options

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

Explanation

To determine the hybridization of nitrogen in R₂NH, we can follow these steps:

### Step 1: Identify the structure of R₂NH
R₂NH is a type of amine where R represents alkyl or aryl groups. The nitrogen atom is bonded to two R groups and one hydrogen atom.

### Step 2: Count the valence electrons of nitrogen
Nitrogen has 5 valence electrons. In R₂NH, nitrogen is bonded to two R groups (which are typically single-bonded) and one hydrogen atom.

### Step 3: Determine the number of bonding pairs and lone pairs
- Nitrogen is bonded to 2 R groups and 1 hydrogen atom, which accounts for 3 bonding pairs.
- Since nitrogen has 5 valence electrons and it uses 3 for bonding, it will have 2 remaining electrons, which form 1 lone pair.

### Step 4: Calculate the hybridization
To find the hybridization, we use the formula:
\[ \text{Hybridization} = \frac{1}{2} \times (\text{Number of valence electrons} + \text{Number of monovalent atoms} + \text{Charge}) \]

In this case:
- Number of valence electrons = 5 (from nitrogen)
- Number of monovalent atoms = 3 (2 from R groups and 1 from hydrogen)
- Charge = 0

So, substituting these values:
\[ \text{Hybridization} = \frac{1}{2} \times (5 + 3 + 0) = \frac{1}{2} \times 8 = 4 \]

### Step 5: Identify the hybridization type
A hybridization number of 4 corresponds to sp³ hybridization.

### Conclusion
Thus, the hybridization of nitrogen in R₂NH is **sp³**.

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