Which statement is not correct for nitrogen?

Options

A. It has a small size
B. It does not readily react with `O_(2)`
C. It is a typical non-metal
D. d-orbitals are available for bonding

Answer

To determine which statement about nitrogen is not correct, we need to analyze the properties and characteristics of nitrogen based on its atomic structure and behavior.

### Step-by-Step Solution:

1. **Identify Nitrogen's Atomic Number and Configuration:**
- Nitrogen has an atomic number of 7.
- Its electronic configuration is 1s² 2s² 2p³, which can also be represented as 2, 5 (indicating 2 electrons in the first shell and 5 in the second shell).

**Hint:** Remember that the atomic number indicates the number of protons and electrons in a neutral atom.

2. **Evaluate Nitrogen's Size:**
- Due to its electronic configuration, nitrogen has a small atomic size. The presence of only two electron shells contributes to this small size.

**Hint:** Smaller atomic size is often associated with fewer electron shells and a higher effective nuclear charge.

3. **Reactivity with O₂:**
- Nitrogen does not readily react with O₂ (oxygen) because it requires three additional electrons to achieve a stable noble gas configuration (similar to neon). Oxygen is a stable diatomic molecule, and nitrogen's triple bond makes it less reactive under normal conditions.

**Hint:** Consider the stability of molecules and the number of electrons needed for bonding.

4. **Classification as a Non-Metal:**
- Nitrogen is classified as a typical non-metal. It exists as a gas at room temperature and is essential for life, making it a non-metallic element.

**Hint:** Non-metals are typically poor conductors of heat and electricity and can exist in various states at room temperature.

5. **Availability of d Orbitals for Bonding:**
- Nitrogen's electronic configuration shows that it has no d orbitals available for bonding (only s and p orbitals are present). This means that any statement claiming the availability of d orbitals for bonding in nitrogen is incorrect.

**Hint:** Recall that d orbitals start to appear in elements from the third period onward in the periodic table.

### Conclusion:
The statement that is not correct for nitrogen is the one claiming that "d orbitals are available for bonding." Therefore, the correct answer is the statement indicating the availability of d orbitals.

### Final Answer:
The incorrect statement about nitrogen is that "d orbitals are available for bonding."