The single covalent radius of P is 0.11 nm. The single covalent radius of Cl will be:

Options

A. smaller than P
B. greater than P
C. same as P
D. none of these

Answer

To determine the single covalent radius of chlorine (Cl) based on the given single covalent radius of phosphorus (P), we follow these steps:

### Step-by-Step Solution:

1. **Identify the Period and Group of Elements**:
- Phosphorus (P) and Chlorine (Cl) are both located in the third period of the periodic table.
- Phosphorus is in Group 15, while Chlorine is in Group 17.

2. **Understand the Trend in Atomic Size**:
- As we move from left to right across a period in the periodic table, the atomic radius decreases. This is due to the increase in the effective nuclear charge (Z effective) as protons are added to the nucleus while the number of electron shells remains constant.

3. **Relate the Covalent Radius of P to Cl**:
- Given that the single covalent radius of phosphorus is 0.11 nm, we can infer that the single covalent radius of chlorine will be smaller than that of phosphorus.
- The reason for this decrease is the increased nuclear charge in chlorine, which pulls the electrons closer to the nucleus, resulting in a smaller atomic size.

4. **Estimate the Covalent Radius of Cl**:
- While the exact value isn't provided, we can estimate that the single covalent radius of chlorine is typically around 0.099 nm, which is smaller than that of phosphorus.

5. **Conclusion**:
- Therefore, the single covalent radius of chlorine (Cl) is approximately 0.099 nm.

### Final Answer:
The single covalent radius of Cl is approximately 0.099 nm.

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