Following are configuration of 4 atom :-
`P=(Ne)3s^(2)3p^(3)`
`Q=(Ar)3d^(10)4s^(2)4p^(3)`
`R=(He)2s^(2)2p^(5)`
`S=(Ne)3s^(1)`
Incorrect statement is :-

Options

A. `EA:QgtR` (EA=electron affinity)
B. `EN:RgtP` (EN=electro negativity)
C. `IP:PgtS` (IP=Ionisation potential)
D. Atomic radius `: SgtR`

Explanation

To solve the question, we need to analyze the electronic configurations of the given atoms and determine which statement is incorrect based on their properties.

### Step 1: Determine the Atomic Numbers
1. **Atom P**: Configuration is \( (Ne) 3s^2 3p^3 \)
- Neon (Ne) has an atomic number of 10.
- Therefore, \( 10 + 2 + 3 = 15 \) (Atomic number of P is 15).

2. **Atom Q**: Configuration is \( (Ar) 3d^{10} 4s^2 4p^3 \)
- Argon (Ar) has an atomic number of 18.
- Therefore, \( 18 + 10 + 2 + 3 = 33 \) (Atomic number of Q is 33).

3. **Atom R**: Configuration is \( (He) 2s^2 2p^5 \)
- Helium (He) has an atomic number of 2.
- Therefore, \( 2 + 2 + 5 = 9 \) (Atomic number of R is 9).

4. **Atom S**: Configuration is \( (Ne) 3s^1 \)
- Neon (Ne) has an atomic number of 10.
- Therefore, \( 10 + 1 = 11 \) (Atomic number of S is 11).

### Step 2: Analyze the Statements
1. **Statement 1**: Electron affinity of Q is greater than electron affinity of R.
- **Analysis**: Q has a half-filled configuration in the 4p subshell, while R has a 2p subshell with 5 electrons. Typically, atoms with half-filled or fully filled subshells have lower electron affinities compared to those that can easily accept an electron. Thus, this statement is likely incorrect.

2. **Statement 2**: Electronegativity of R is greater than electronegativity of P.
- **Analysis**: R has a 2p subshell (closer to the nucleus), while P has a 3p subshell. Electronegativity decreases as we move down a group. Therefore, this statement is correct.

3. **Statement 3**: Ionization potential of P is greater than ionization potential of S.
- **Analysis**: P has a half-filled stable configuration (3s² 3p³), which requires more energy to remove an electron compared to S (3s¹). Therefore, this statement is correct.

4. **Statement 4**: Atomic radius of S is greater than R.
- **Analysis**: S (3s¹) has its outermost electron in the 3rd shell, while R (2p⁵) has its outermost electron in the 2nd shell. Atomic radius increases down a group, so this statement is also correct.

### Conclusion
The incorrect statement is:
**Electron affinity of Q is greater than electron affinity of R.**