Sodium ordinarily does not show an oxidation state of `+2`, because of its

Options

A. High first ionisation potential
B. High second ionization potential
C. large ionic radius
D. high electronegativity

Answer

To determine why sodium does not ordinarily show an oxidation state of +2, we need to analyze its electronic configuration and the implications of ionization potentials.

### Step-by-Step Solution:

1. **Identify the Electronic Configuration of Sodium**:
- Sodium (Na) has an atomic number of 11. Its electronic configuration is:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^1 \]
- This means sodium has one electron in its outermost shell (3s orbital).

**Hint**: Remember that the outermost electrons are crucial for determining oxidation states.

2. **Understand the Concept of Ionization Energy**:
- Ionization energy is the energy required to remove an electron from an atom.
- Sodium can easily lose its one outermost electron to achieve a stable electronic configuration (like neon), resulting in a +1 oxidation state.

**Hint**: The first ionization potential is typically lower for elements that readily lose electrons.

3. **Consider the First and Second Ionization Energies**:
- The first ionization potential (to remove the first electron) is relatively low for sodium, allowing it to easily form Na⁺.
- However, removing the second electron (to achieve a +2 oxidation state) would require overcoming the stability of the filled second shell (2s² 2p⁶), which is much more difficult.

**Hint**: The stability of filled electron shells plays a significant role in determining ionization energies.

4. **Evaluate the Ionization Energies**:
- The second ionization potential is significantly higher than the first because after losing the first electron, sodium achieves a stable noble gas configuration. Thus, removing a second electron from a stable configuration requires much more energy.

**Hint**: Higher ionization energy indicates difficulty in removing an electron.

5. **Conclusion**:
- Since sodium has a high second ionization potential, it does not ordinarily show an oxidation state of +2. Instead, it prefers to lose just one electron, resulting in a +1 oxidation state.

**Final Answer**: Sodium ordinarily does not show an oxidation state of +2 because of its **high second ionization potential**.

### Summary of Options:
- **Option A**: High first ionization potential - Incorrect.
- **Option B**: High second ionization potential - Correct.
- **Option C**: Large atomic radius - Incorrect.
- **Option D**: High electronegativity - Incorrect.