Multiple covalent bonds exist in a molecule of

Options

A. Option 1. `F_(2)`
B. Option 2. `N_(2)`
C. Option 3. `CH_(4)`
D. Option 4. `H_(2)`

Answer

To determine which molecule contains a multiple covalent bond, we need to analyze the bonding in each of the given molecules. Let's go through them step by step.

### Step 1: Analyze the first molecule (F2)
- **Valence Electrons**: Each fluorine atom has 7 valence electrons.
- **Bond Formation**: To achieve a full octet, each fluorine atom shares one electron with the other, forming a single covalent bond.
- **Conclusion**: F2 has a single bond. No multiple bond exists here.

### Step 2: Analyze the second molecule (N2)
- **Valence Electrons**: Each nitrogen atom has 5 valence electrons.
- **Bond Formation**: To complete their octets, the two nitrogen atoms share three pairs of electrons, resulting in a triple bond.
- **Conclusion**: N2 has a triple bond, which is a type of multiple covalent bond.

### Step 3: Analyze the third molecule (CH4)
- **Valence Electrons**: Carbon has 4 valence electrons, and each hydrogen has 1 valence electron.
- **Bond Formation**: Carbon shares one electron with each of the four hydrogen atoms, forming four single covalent bonds.
- **Conclusion**: CH4 has only single bonds. No multiple bond exists here.

### Step 4: Analyze the fourth molecule (H2)
- **Valence Electrons**: Each hydrogen atom has 1 valence electron.
- **Bond Formation**: The two hydrogen atoms share one pair of electrons, forming a single covalent bond.
- **Conclusion**: H2 has a single bond. No multiple bond exists here.

### Final Conclusion
Among the given options, only the nitrogen molecule (N2) contains a multiple covalent bond (triple bond).

### Answer
**N2 has a multiple covalent bond.**

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