Which of the following bonds will be most polar?

Options

A. N-Cl
B. O-F
C. N-F
D. N-N.

Explanation

To determine which bond is the most polar among the given options (N-F, N-N, O-F, N-Cl), we need to analyze the electronegativity values of the elements involved in each bond. The polarity of a bond is influenced by the difference in electronegativity between the two atoms forming the bond.

### Step-by-Step Solution:

1. **Identify the Elements and Their Electronegativity Values:**
- Fluorine (F) has an electronegativity of approximately 4.0.
- Oxygen (O) has an electronegativity of approximately 3.5.
- Nitrogen (N) has an electronegativity of approximately 3.0.
- Chlorine (Cl) has an electronegativity of approximately 3.0.

2. **Calculate the Electronegativity Differences:**
- For N-F: |3.0 - 4.0| = 1.0
- For N-N: |3.0 - 3.0| = 0.0
- For O-F: |3.5 - 4.0| = 0.5
- For N-Cl: |3.0 - 3.0| = 0.0

3. **Rank the Bonds Based on Electronegativity Differences:**
- N-N: 0.0 (non-polar)
- N-Cl: 0.0 (non-polar)
- O-F: 0.5 (polar)
- N-F: 1.0 (most polar)

4. **Conclusion:**
The bond with the highest electronegativity difference is N-F, making it the most polar bond among the options given.

### Final Answer:
The bond that is most polar is **N-F**.

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