The bond in molecular nitrogen (`N_(2)` ) is difficult to break, because it is a

Options

A. twisted configuration
B. quadruple hydrogen bond
C. triple covalent bond
D. triple lonic bond

Answer

To answer the question regarding why the bond in molecular nitrogen (N₂) is difficult to break, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Molecular Nitrogen (N₂)**:
- Molecular nitrogen consists of two nitrogen atoms bonded together. Each nitrogen atom has five electrons in its outer shell.

2. **Bond Formation**:
- In N₂, each nitrogen atom shares three of its five outer electrons with the other nitrogen atom. This sharing of electrons leads to the formation of a bond.

3. **Type of Bond**:
- The bond formed between the two nitrogen atoms is known as a **triple covalent bond**. This means that three pairs of electrons are shared between the two nitrogen atoms.

4. **Stability of the Bond**:
- The triple covalent bond is very strong and stable because it involves the sharing of six electrons (three pairs). This strong bond requires a significant amount of energy to break.

5. **Conclusion**:
- Therefore, the bond in molecular nitrogen (N₂) is difficult to break due to the presence of a **triple covalent bond**.

### Final Answer:
The bond in molecular nitrogen (N₂) is difficult to break because it is a **triple covalent bond**.

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