The shapes of nitrite and nitrile respectively are:

Options

A. Lineat and angular
B. Angular and linear
C. Both angular
D. Both linear

Answer

To determine the shapes of nitrite (NO2⁻) and nitrile (CN), we can follow these steps:

### Step 1: Determine the Valence Electrons
- For nitrite (NO2⁻):
- Nitrogen (N) has 5 valence electrons.
- Each Oxygen (O) has 6 valence electrons, and there are two Oxygens.
- There is one additional electron due to the negative charge.

Calculation:
\[ \text{Total valence electrons} = 5 + (6 \times 2) + 1 = 18 \]

- For nitrile (CN):
- Carbon (C) has 4 valence electrons.
- Nitrogen (N) has 5 valence electrons.

Calculation:
\[ \text{Total valence electrons} = 4 + 5 = 9 \]

### Step 2: Calculate Bond Pairs and Lone Pairs
- For nitrite (NO2⁻):
- Divide the total valence electrons by 8 to find bond pairs:
\[ \text{Bond pairs} = \frac{18}{8} = 2 \text{ (with a remainder of 2)} \]
- Divide the remainder by 2 to find lone pairs:
\[ \text{Lone pairs} = \frac{2}{2} = 1 \]

- For nitrile (CN):
- Divide the total valence electrons by 8:
\[ \text{Bond pairs} = \frac{9}{8} = 1 \text{ (with a remainder of 1)} \]
- Divide the remainder by 2:
\[ \text{Lone pairs} = \frac{1}{2} = 0 \]

### Step 3: Draw the Lewis Structures
- For nitrite (NO2⁻):
- The structure consists of one nitrogen atom bonded to two oxygen atoms, with one lone pair on the nitrogen. The shape is bent (angular) due to the presence of the lone pair.

- For nitrile (CN):
- The structure consists of a carbon atom triple-bonded to a nitrogen atom. There are no lone pairs on the carbon, resulting in a linear shape.

### Step 4: Conclusion
- The shape of nitrite (NO2⁻) is **bent (angular)**.
- The shape of nitrile (CN) is **linear**.

### Final Answer:
The shapes of nitrite and nitrile respectively are: **bent (angular) and linear**.

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