Which of the following statemnet is wrong ?

Options

A. The stablility of hydrides increase from `NH_(3)` to `BiH_(3)` in group 15 of the periodic table.
B. Nitrogen cannot form `dpi-ppi` bond.
C. Single N-N bond is weaker than the single P-P bond.
D. `N_(2)O_(4)` has resonance structure.

Explanation

To determine which statement is wrong regarding the hydrides of the nitrogen family, we will analyze each statement one by one.

### Step 1: Analyze the first statement
**Statement:** The stability of hydride increases from ammonia (NH3) to bismuthine (BiH3).

- **Analysis:** The stability of hydrides in the nitrogen family decreases as we move down the group from NH3 to BiH3. This is due to the increase in atomic size, which leads to a decrease in bond dissociation enthalpy. As the central atom's size increases, the bond becomes weaker and easier to break. Thus, BiH3 is less stable than NH3.

**Conclusion:** This statement is incorrect.

### Step 2: Analyze the second statement
**Statement:** Nitrogen cannot form dπ-pπ bonds.

- **Analysis:** Nitrogen has an atomic number of 7, with an electronic configuration of 1s² 2s² 2p³. Since nitrogen does not have d orbitals in the second shell, it cannot form dπ-pπ bonds. Therefore, this statement is correct.

### Step 3: Analyze the third statement
**Statement:** A single N-N bond is weaker than a single P-P bond.

- **Analysis:** The N-N bond is indeed weaker than the P-P bond. This is because nitrogen is smaller in size compared to phosphorus, leading to greater lone pair-lone pair repulsion in nitrogen. In phosphorus, the larger size results in less repulsion, making the P-P bond stronger. Thus, this statement is also correct.

### Step 4: Analyze the fourth statement
**Statement:** N2O4 has resonance structures.

- **Analysis:** N2O4 does have resonance structures. The different arrangements of electrons in the molecule lead to various valid Lewis structures, confirming the presence of resonance. Therefore, this statement is correct.

### Final Conclusion
After analyzing all the statements, we find that:

- The first statement is incorrect.
- The second, third, and fourth statements are correct.

Thus, the answer to the question is that the first statement is wrong.