In `NO_(2)` molecule N atom undergoes in :

Options

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

Answer

To determine the hybridization of the nitrogen atom in the NO₂ molecule, we can follow these steps:

### Step 1: Determine the Valence Electrons of Nitrogen
Nitrogen (N) has an atomic number of 7, which means it has 7 electrons. The electron configuration of nitrogen is 1s² 2s² 2p³. The valence shell (2s and 2p) contains 5 electrons (2 from 2s and 3 from 2p).

### Step 2: Analyze the Bonding in NO₂
In the NO₂ molecule, nitrogen forms bonds with two oxygen atoms. Each oxygen atom typically forms a double bond with nitrogen. Therefore, nitrogen will share electrons with both oxygen atoms.

### Step 3: Count Bond Pairs and Lone Pairs
- Nitrogen forms two double bonds with the two oxygen atoms. This accounts for 2 bond pairs.
- In the NO₂ molecule, nitrogen has one unpaired electron, which can be considered a free radical. This means there is one lone pair of electrons on nitrogen.

### Step 4: Calculate the Hybridization
Hybridization can be determined using the formula:
\[ \text{Hybridization} = \text{Number of Bond Pairs} + \text{Number of Lone Pairs} \]

From the previous steps:
- Number of Bond Pairs = 2 (from the two double bonds)
- Number of Lone Pairs = 1 (the unpaired electron)

So, we have:
\[ \text{Hybridization} = 2 + 1 = 3 \]

### Step 5: Identify the Hybridization Type
The hybridization state of 3 corresponds to sp² hybridization. This means that the nitrogen atom in the NO₂ molecule undergoes sp² hybridization.

### Conclusion
The nitrogen atom in the NO₂ molecule undergoes sp² hybridization.

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