The electronegativities of `H,Cl,N,O and F are 2.1,3.0,3.2,3.5 and 4.0 respectively. The strongest bond is formed between

Options

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

Answer

To determine which bond is the strongest based on the given electronegativities of hydrogen (H), chlorine (Cl), nitrogen (N), oxygen (O), and fluorine (F), we can follow these steps:

### Step 1: List the Electronegativity Values
We start by listing the electronegativities of the elements:
- H: 2.1
- Cl: 3.0
- N: 3.2
- O: 3.5
- F: 4.0

### Step 2: Calculate the Electronegativity Differences
Next, we calculate the electronegativity differences (ΔEN) for each possible bond formed between these elements. The electronegativity difference is calculated by subtracting the electronegativity of one atom from that of the other atom in the bond.

1. H - Cl: |2.1 - 3.0| = 0.9
2. H - N: |2.1 - 3.2| = 1.1
3. H - O: |2.1 - 3.5| = 1.4
4. H - F: |2.1 - 4.0| = 1.9
5. Cl - N: |3.0 - 3.2| = 0.2
6. Cl - O: |3.0 - 3.5| = 0.5
7. Cl - F: |3.0 - 4.0| = 1.0
8. N - O: |3.2 - 3.5| = 0.3
9. N - F: |3.2 - 4.0| = 0.8
10. O - F: |3.5 - 4.0| = 0.5

### Step 3: Identify the Maximum Electronegativity Difference
Now, we need to identify the maximum electronegativity difference from the calculated values. The maximum ΔEN is:

- H - F: 1.9

### Step 4: Conclusion
The bond with the maximum electronegativity difference indicates the strongest bond. Therefore, the strongest bond is formed between hydrogen (H) and fluorine (F).

### Final Answer
The strongest bond is formed between H and F.

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