Which of the following element does not show `-3` oxidation state.

Options

A. `Bi`
B. `N`
C. `As`
D. None of these

Answer

To determine which of the following elements does not show a -3 oxidation state, we will analyze the oxidation states of the elements provided: bismuth (Bi), nitrogen (N), and arsenic (As). All these elements belong to Group 15 of the periodic table, also known as the nitrogen family.

### Step-by-Step Solution:

1. **Identify the Elements**: The elements in question are bismuth (Bi), nitrogen (N), and arsenic (As).

2. **Understand Group 15 Elements**: All elements in Group 15 have 5 valence electrons. Their electronic configuration can be represented as \( ns^2 np^3 \). They tend to gain 3 electrons to achieve a stable noble gas configuration.

3. **Oxidation States in Group 15**:
- **Nitrogen (N)**: Nitrogen can form a nitride ion (N³⁻) by gaining 3 electrons, thus showing a -3 oxidation state.
- **Arsenic (As)**: Arsenic can also exhibit a -3 oxidation state in compounds such as Na₃As.
- **Bismuth (Bi)**: Bismuth, while it can theoretically show a -3 oxidation state, does not commonly do so due to its larger atomic size and the energy required to gain 3 electrons. Instead, it typically shows positive oxidation states (+3, +5).

4. **Conclusion**: Among the elements listed, bismuth (Bi) does not show a -3 oxidation state in practice, while nitrogen and arsenic do.

### Final Answer:
**Bismuth (Bi)** does not show a -3 oxidation state.