### Understanding the Inert Pair Effect in Group 16 Elements**3. Predict how the inert pair effect would manifest itself in Group 16.**The inert pair effect refers to the reluctance of the s-electrons in the outermost electron shell to participate in bonding as we move down a group in the periodic table. In Group 16, which includes elements like oxygen, sulfur, selenium, tellurium, and polonium, this effect becomes more pronounced.### Explanation:1. **Oxygen and Sulfur:** - These lighter elements in Group 16 do not experience the inert pair effect significantly. They typically exhibit oxidation states of -2 due to their tendency to gain electrons and achieve a stable electron configuration.2. **Selenium and Tellurium:** - As we move down to selenium and tellurium, the reluctance of the s-electrons to participate in bonding becomes more evident. These elements often show +4 oxidation states, in addition to their common -2 states.3. **Polonium:** - For polonium, the heaviest element in this group, the inert pair effect is quite strong. It predominantly exhibits a +2 oxidation state, resulting from the non-participation of the 6s electrons in bonding, instead of the expected higher oxidation states.Understanding this effect is crucial for predicting the chemical behavior and bonding characteristics of these elements, particularly in complex compounds where differing oxidation states play a significant role.

Solution- Inert pair effect is tendency of two electrons in s orbital to remain unshared in a…

Answered: 3. Predict how the inert pair effect…

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3. Predict how the inert pair effect would manifest itself in Group 16.

Chemistry

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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### Understanding the Inert Pair Effect in Group 16 Elements

**3. Predict how the inert pair effect would manifest itself in Group 16.**

The inert pair effect refers to the reluctance of the s-electrons in the outermost electron shell to participate in bonding as we move down a group in the periodic table. In Group 16, which includes elements like oxygen, sulfur, selenium, tellurium, and polonium, this effect becomes more pronounced.

### Explanation:

1. **Oxygen and Sulfur:**
- These lighter elements in Group 16 do not experience the inert pair effect significantly. They typically exhibit oxidation states of -2 due to their tendency to gain electrons and achieve a stable electron configuration.

2. **Selenium and Tellurium:**
- As we move down to selenium and tellurium, the reluctance of the s-electrons to participate in bonding becomes more evident. These elements often show +4 oxidation states, in addition to their common -2 states.

3. **Polonium:**
- For polonium, the heaviest element in this group, the inert pair effect is quite strong. It predominantly exhibits a +2 oxidation state, resulting from the non-participation of the 6s electrons in bonding, instead of the expected higher oxidation states.

Understanding this effect is crucial for predicting the chemical behavior and bonding characteristics of these elements, particularly in complex compounds where differing oxidation states play a significant role.

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