Which of the following compounds has the samallest bond angle in its molecule ?

Options

A. `OH_(2)`
B. `SH_(2)`
C. `NH_(3)`
D. `SO_(2)`

Answer

To determine which of the given compounds has the smallest bond angle, we will analyze each compound one by one:

### Step 1: Analyze Water (H2O)
- **Structure**: Water has a bent shape due to the presence of two lone pairs on the oxygen atom.
- **Hybridization**: The hybridization of water is sp³.
- **Bond Angle**: The bond angle in water is approximately 104.5°.

### Step 2: Analyze Hydrogen Sulfide (H2S)
- **Structure**: Hydrogen sulfide also has a bent shape, similar to water, but with a larger bond angle due to the larger size of sulfur compared to oxygen.
- **Hybridization**: The hybridization of hydrogen sulfide is also sp³.
- **Bond Angle**: The bond angle in hydrogen sulfide is approximately 92.5° (close to 90°).

### Step 3: Analyze Ammonia (NH3)
- **Structure**: Ammonia has a trigonal pyramidal shape due to the presence of one lone pair on nitrogen.
- **Hybridization**: The hybridization of ammonia is sp³.
- **Bond Angle**: The bond angle in ammonia is approximately 106.5°.

### Step 4: Analyze Sulfur Dioxide (SO2)
- **Structure**: Sulfur dioxide has a bent shape with one lone pair on sulfur.
- **Hybridization**: The hybridization of sulfur dioxide is sp².
- **Bond Angle**: The bond angle in sulfur dioxide is approximately 119°.

### Conclusion:
Now, we compare the bond angles:
- Water (H2O): 104.5°
- Hydrogen Sulfide (H2S): 92.5°
- Ammonia (NH3): 106.5°
- Sulfur Dioxide (SO2): 119°

The compound with the smallest bond angle is **Hydrogen Sulfide (H2S)** with a bond angle of approximately 92.5°.

### Final Answer:
**Hydrogen Sulfide (H2S) has the smallest bond angle.**

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