Which of the following bonds will be most polar?

Options

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

Explanation

To determine which of the given bonds is the most polar, we will follow these steps:

### Step 1: Identify the bonds and their components
The bonds we need to analyze are:
1. Nitrogen-Fluorine (N-F)
2. Nitrogen-Oxygen (N-O)
3. Fluorine-Nitrogen (F-N)
4. Nitrogen-Chlorine (N-Cl)

### Step 2: Understand the concept of polarity
Polarity in a bond arises due to the difference in electronegativity between the two atoms involved in the bond. The greater the difference in electronegativity, the more polar the bond.

### Step 3: Determine the electronegativity values
The electronegativity values (on the Pauling scale) for the relevant elements are approximately:
- Fluorine (F): 4.0
- Oxygen (O): 3.5
- Nitrogen (N): 3.0
- Chlorine (Cl): 3.0

### Step 4: Calculate the electronegativity differences for each bond
1. **N-F**: |4.0 - 3.0| = 1.0
2. **N-O**: |3.5 - 3.0| = 0.5
3. **F-N**: |4.0 - 3.0| = 1.0 (same as N-F)
4. **N-Cl**: |3.0 - 3.0| = 0.0

### Step 5: Compare the electronegativity differences
- N-F: 1.0
- N-O: 0.5
- F-N: 1.0
- N-Cl: 0.0

### Step 6: Determine which bond is the most polar
The bond with the highest electronegativity difference is the most polar. Both N-F and F-N have the highest difference of 1.0, indicating they are the most polar bonds.

### Conclusion
Thus, the most polar bond among the given options is the Nitrogen-Fluorine (N-F) bond.

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

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