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)`

Explanation

To determine which of the given compounds has the smallest bond angle, we will analyze the molecular structures and bond angles of each compound: H2O, H2S, NH3, and SO2.

### Step 1: Analyze H2O (Water)
- **Molecular Geometry**: The molecular geometry of water is bent due to the presence of two lone pairs on the oxygen atom.
- **Bond Angle**: The bond angle in H2O is approximately **104.5 degrees**.

### Step 2: Analyze H2S (Hydrogen Sulfide)
- **Molecular Geometry**: Similar to water, H2S also has a bent shape. However, sulfur is less electronegative than oxygen, which affects the repulsion between lone pairs and bond pairs.
- **Bond Angle**: The bond angle in H2S is approximately **92.5 degrees**.

### Step 3: Analyze NH3 (Ammonia)
- **Molecular Geometry**: Ammonia has a trigonal pyramidal shape due to one lone pair on the nitrogen atom.
- **Bond Angle**: The bond angle in NH3 is approximately **106.5 degrees**.

### Step 4: Analyze SO2 (Sulfur Dioxide)
- **Molecular Geometry**: SO2 has a bent shape with one lone pair on the sulfur atom and two double bonds with oxygen.
- **Bond Angle**: The bond angle in SO2 is approximately **119.5 degrees**.

### Step 5: Compare the Bond Angles
- H2O: 104.5 degrees
- H2S: 92.5 degrees
- NH3: 106.5 degrees
- SO2: 119.5 degrees

### Conclusion
The compound with the smallest bond angle is **H2S**, with a bond angle of 92.5 degrees.

### Final Answer
**H2S** has the smallest bond angle among the given compounds.

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