### 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 compound . The electronic configuration pf group 16 is ns2 np4 . So they can loose 6 electrons and attain a oxidation state or +6 according to rules . But due to inert pair effect s electrons remain unshared and hence maximum oxidation state attained by group 16 is +4 . Thus s electrons do not participate in bond formation . The reason of this inert pair effect is s orbital is very close to nucleus and hence more energy is required to extract electrons from s orbital due to which +6 oxidation state become less stable and +4 oxidation state become more stable . Example include - sn2+ , Sb3+ , pb2+, Bi3+ etc . These elements of group 16 maintain at its lower oxidation state .

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

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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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