Which of the following statements is/are wrong?

Options

A. Van der waals' radius of iodine is more than its covalent radius
B. all isoelectronic ions belong to same period of the peridic table
C. `I.E_(1)` of N is higher than that of O while `I.E_(2)` of O is higher than that of N
D. The electron affinity N is almost zero while that of P is 74.3 kJ `mol^(-1)`

Explanation

To determine which of the statements provided is wrong, we will analyze each statement one by one.

### Step 1: Analyze the first statement
**Statement 1:** "Van der Waals radius of iodine is more than the covalent radius."

- The Van der Waals radius is indeed larger than the covalent radius for any element. This is because the Van der Waals radius accounts for the distance between non-bonded atoms, while the covalent radius considers the distance when atoms are bonded and overlapping occurs. Therefore, this statement is **correct**.

### Step 2: Analyze the second statement
**Statement 2:** "All the isoelectronic ions belong to the same period of the periodic table."

- Isoelectronic ions are ions that have the same number of electrons. However, they can belong to different periods of the periodic table. For example, the ions \( \text{Li}^+ \) (from period 2) and \( \text{Ne} \) (from period 2) are isoelectronic, but \( \text{Na}^+ \) (from period 3) is also isoelectronic with \( \text{Ne} \). Thus, this statement is **incorrect**.

### Step 3: Analyze the third statement
**Statement 3:** "Ionization energy of nitrogen is higher than oxygen while second ionization energy of oxygen is higher than nitrogen."

- The ionization energy of nitrogen is indeed higher than that of oxygen due to nitrogen having a half-filled \( 2p \) subshell, which is more stable. The second ionization energy of oxygen is higher than that of nitrogen because removing an electron from oxygen results in a stable noble gas configuration. Therefore, this statement is **correct**.

### Step 4: Analyze the fourth statement
**Statement 4:** "Electron affinity of nitrogen is almost zero."

- The electron affinity of nitrogen is low (close to zero) because nitrogen has a half-filled \( 2p \) subshell, which is stable. The small size of nitrogen also contributes to its low electron affinity as the lone pair electrons repel incoming electrons. Therefore, this statement is **correct**.

### Conclusion
After analyzing all four statements, we find that:
- **Statement 1:** Correct
- **Statement 2:** Incorrect
- **Statement 3:** Correct
- **Statement 4:** Correct

Thus, the only wrong statement is **Statement 2**.