Single `N-N` bond is weaker than the single `P-P` bond. This is because of `:`

Options

A. larger `N-N` bodn length in comparison to `P-P` bond length.
B. high interelectronic repulsion of the non`-` bondioni electrons, owing to the small `N-N` bond length in comparison to that in that in `P-P` single bond.
C. Higher electronegativity of N in comparison to P.
D. smaller atomic size of N as compared to that of P.

Explanation

To solve the question regarding why a single N-N bond is weaker than a single P-P bond, we can break it down into the following steps:

### Step 1: Understanding the Bonds
- **N-N Bond**: This bond is formed between two nitrogen atoms.
- **P-P Bond**: This bond is formed between two phosphorus atoms.

### Step 2: Analyzing the Nature of Non-bonding Orbitals
- In nitrogen, the non-bonding orbitals (lone pairs) are closer together due to the smaller atomic size compared to phosphorus. This proximity leads to increased repulsion between the non-bonding electrons.

### Step 3: Effect of Electron Repulsion
- The increased repulsion between the non-bonding electrons in the N-N bond weakens the bond. This is because the repulsion counteracts the attractive forces that hold the bond together.

### Step 4: Bond Length Consideration
- The bond length of the N-N bond is smaller than that of the P-P bond. A smaller bond length typically indicates a stronger bond; however, in this case, the repulsion effects in the N-N bond dominate, making it weaker despite the shorter bond length.

### Step 5: Conclusion
- Therefore, the reason the N-N bond is weaker than the P-P bond is due to the high inter-electronic repulsion of the non-bonding electrons in nitrogen, which is exacerbated by the smaller atomic size of nitrogen compared to phosphorus.

### Final Answer
The correct explanation for why a single N-N bond is weaker than a single P-P bond is: "High inter-electronic repulsion of the non-bonding electrons owing to small end-to-end bond length in comparison to that in P-P single bond."

---