The compound having highest boiling point :

Options

A. `CH_(4)`
B. `CH_(3)OH`
C. `CH_(3)Br `
D. `CH_3Cl`

Explanation

To determine which compound has the highest boiling point among the given options (CH4, CH3OH, CH3Br, and CH3Cl), we need to analyze the types of intermolecular forces present in each compound.

### Step-by-Step Solution:

1. **Identify the Compounds and Their Intermolecular Forces:**
- **CH4 (Methane)**: This compound exhibits only Van der Waals forces (dispersion forces).
- **CH3OH (Methanol)**: This compound can form hydrogen bonds due to the presence of an -OH group.
- **CH3Br (Bromomethane)**: This compound exhibits Van der Waals forces, and since it has a larger molecular mass than CH4, it will have stronger dispersion forces.
- **CH3Cl (Chloromethane)**: This compound also exhibits Van der Waals forces, and like CH3Br, it has a larger molecular mass than CH4, resulting in stronger dispersion forces than CH4.

2. **Compare the Strength of Intermolecular Forces:**
- **Hydrogen Bonding**: This is the strongest type of intermolecular force present in CH3OH. Hydrogen bonds occur when hydrogen is bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine.
- **Van der Waals Forces**: These are weaker than hydrogen bonds and depend on the size and mass of the molecules. Larger molecules with greater mass will have stronger Van der Waals forces.

3. **Rank the Compounds Based on Boiling Points:**
- **CH4**: Weakest intermolecular forces (lowest boiling point).
- **CH3Cl**: Stronger Van der Waals forces than CH4.
- **CH3Br**: Stronger Van der Waals forces than CH3Cl due to higher molecular mass.
- **CH3OH**: Strongest intermolecular forces due to hydrogen bonding (highest boiling point).

4. **Conclusion:**
- Among the compounds, CH3OH has the highest boiling point due to the presence of hydrogen bonding, which is significantly stronger than the Van der Waals forces present in the other compounds.

### Final Answer:
The compound with the highest boiling point is **CH3OH (Methanol)**.

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