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. of P

Answer

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

### Step-by-Step Solution:

1. **Identify the Group of Elements**:
- Phosphorus (P) belongs to Group 15 (or Group V) of the periodic table.
- Chlorine (Cl) belongs to Group 17 (or Group VII) of the periodic table.

2. **Understand the Trend in Atomic Size**:
- As we move from left to right across a period in the periodic table, the atomic size (or covalent radius) decreases. This is due to the increase in nuclear charge, which pulls the electrons closer to the nucleus.
- As we move down a group, the atomic size increases due to the addition of electron shells.

3. **Compare the Elements**:
- Since phosphorus is in Group 15 and chlorine is in Group 17, chlorine is further to the right in the periodic table compared to phosphorus.
- Therefore, we can conclude that the covalent radius of chlorine will be smaller than that of phosphorus.

4. **Given Data**:
- The single covalent radius of phosphorus (P) is given as 0.11 nm.

5. **Conclusion**:
- Since chlorine is smaller than phosphorus, we can conclude that the single covalent radius of chlorine will be less than 0.11 nm.

6. **Final Answer**:
- The single covalent radius of chlorine is expected to be less than 0.11 nm.