Which of the following element does not show an oxidation state of +4 ?

Options

A. Oxygen
B. Sulphur
C. Seleium
D. Tellurium

Answer

To determine which of the following elements does not show an oxidation state of +4, we will analyze each element: oxygen, sulfur, selenium, and tellurium.

### Step-by-Step Solution:

1. **Identify the Elements**: The elements in question are oxygen (O), sulfur (S), selenium (Se), and tellurium (Te). All of these elements belong to Group 16 of the periodic table, also known as the oxygen family.

2. **Understand Oxidation States**: The common oxidation states for these elements include -2, 0, +2, +4, and +6. However, not all elements in this group can exhibit all these oxidation states.

3. **Analyze Each Element**:
- **Oxygen (O)**: Oxygen typically shows an oxidation state of -2 in compounds. It can only exhibit a +2 oxidation state due to the absence of d orbitals. Therefore, it does not show a +4 oxidation state.
- **Sulfur (S)**: Sulfur can show oxidation states of +4 and +6 by promoting electrons from the 3p orbital to the 3d orbital.
- **Selenium (Se)**: Selenium can also exhibit +4 and +6 oxidation states by promoting electrons from the 4p orbital to the 4d orbital.
- **Tellurium (Te)**: Tellurium can similarly show +4 and +6 oxidation states by promoting electrons from the 5p orbital to the 5d orbital.

4. **Conclusion**: Based on the analysis, oxygen is the only element among the four that does not show an oxidation state of +4.

### Final Answer:
**Oxygen (O)** does not show an oxidation state of +4.