Which of the following bond is non-polar

Options

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

Answer

To determine which of the given bonds is non-polar, we need to analyze the electronegativity of the atoms involved in each bond. Here’s the step-by-step solution:

### Step 1: Understand Non-Polar Bonds
Non-polar bonds are formed between two atoms that have the same or very similar electronegativity. In such cases, the electrons are shared equally between the two atoms, resulting in no dipole moment.

### Step 2: Analyze Each Option
We will evaluate each of the given options to determine their polarity based on the electronegativity of the atoms involved.

- **Option A: NH (Nitrogen-Hydrogen Bond)**
- Nitrogen (N) has an electronegativity of about 3.0, while Hydrogen (H) has an electronegativity of about 2.1.
- Since there is a difference in electronegativity, this bond is polar.

- **Option B: BCH (Boron-Chlorine Bond)**
- Boron (B) has an electronegativity of about 2.0, and Chlorine (Cl) has an electronegativity of about 3.0.
- The difference in electronegativity indicates that this bond is also polar.

- **Option C: FF (Fluorine-Fluorine Bond)**
- Both Fluorine (F) atoms have the same electronegativity of about 4.0.
- Since the electronegativities are equal, the bond is non-polar.

- **Option D: OH (Oxygen-Hydrogen Bond)**
- Oxygen (O) has an electronegativity of about 3.5, while Hydrogen (H) has an electronegativity of about 2.1.
- This difference indicates that this bond is polar.

### Step 3: Conclusion
Based on the analysis, the bond that is non-polar among the options is **Option C: FF (Fluorine-Fluorine Bond)**.

### Summary of the Solution
- Non-polar bonds occur between atoms with the same electronegativity.
- Analyzed each bond:
- NH: Polar
- BCH: Polar
- FF: Non-polar
- OH: Polar
- Therefore, the non-polar bond is **FF**.