Multiple bond can exist in :

Options

A. `CH_(4)` molecule
B. `NH_(3)` molecule
C. `Cl_(2)` molecule
D. `N_(2)` molecule

Answer

To determine where multiple bonds can exist, we need to analyze the given compounds: CH4, NH3, Cl2, and N2.

### Step-by-Step Solution:

1. **Analyze CH4 (Methane)**:
- CH4 has a carbon atom bonded to four hydrogen atoms.
- The bonds formed between carbon and hydrogen are all **single bonds**.
- Therefore, CH4 does not contain any multiple bonds.

**Hint**: Look for the types of bonds formed between the atoms in the molecule.

2. **Analyze NH3 (Ammonia)**:
- NH3 consists of a nitrogen atom bonded to three hydrogen atoms.
- The bonds between nitrogen and hydrogen are also **single bonds**.
- Thus, NH3 does not contain any multiple bonds.

**Hint**: Count the number of bonds between the central atom and surrounding atoms.

3. **Analyze Cl2 (Chlorine)**:
- Cl2 is a diatomic molecule consisting of two chlorine atoms.
- The bond formed between the two chlorine atoms is a **single bond**.
- Hence, Cl2 does not have multiple bonds.

**Hint**: Remember that diatomic molecules often have single bonds unless specified otherwise.

4. **Analyze N2 (Nitrogen)**:
- N2 consists of two nitrogen atoms.
- Each nitrogen atom has five valence electrons and shares three of them to form a **triple bond** with the other nitrogen atom.
- Therefore, N2 contains a multiple bond (specifically, a triple bond).

**Hint**: Check the valence electrons and how they are shared between atoms to identify multiple bonds.

### Conclusion:
The only compound among the given options that contains multiple bonds is **N2 (Nitrogen)**, which has a triple bond.

### Final Answer:
**N2 (Nitrogen molecule)** contains multiple bonds.