Which one of the group 16 elements given below hardly show -2 oxidation state ?

Options

A. Selenium
B. Tellurium
C. Polonium
D. Oxygen

Answer

To determine which group 16 element hardly shows a -2 oxidation state, we can analyze the properties of the elements in this group. The group 16 elements include oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po).

### Step-by-Step Solution:

1. **Identify the Group 16 Elements**:
The elements in group 16 are:
- Oxygen (O)
- Sulfur (S)
- Selenium (Se)
- Tellurium (Te)
- Polonium (Po)

2. **Understand Oxidation States**:
- The -2 oxidation state is commonly exhibited by nonmetals in this group, particularly oxygen and sulfur.
- As we move down the group, the tendency to gain electrons (and thus exhibit a -2 oxidation state) generally decreases.

3. **Analyze the Trend in Electronegativity**:
- Electronegativity decreases as we move down the group.
- Oxygen has the highest electronegativity, followed by sulfur, selenium, tellurium, and finally polonium.

4. **Consider the Metallic Character**:
- Metallic character increases down the group. This means that elements become more likely to lose electrons rather than gain them.
- Polonium, being the heaviest and most metallic element in this group, is more inclined to lose electrons.

5. **Conclusion**:
- Since polonium (Po) is more metallic and has a lower tendency to gain electrons, it hardly shows a -2 oxidation state compared to the other elements in the group.

### Final Answer:
The group 16 element that hardly shows a -2 oxidation state is **Polonium (Po)**.