Question

Elements of group 14 exhibit oxidation state of:
A) +4 only
B) +2 and +4 only
C) +1 and +3 only
D) +2 only

Answer 1

Hint: The answer to this question is based on the concept of inert pair effect and here the calculation of oxidation state denotes the valence electrons of the element.

Complete answer:
We have studied the facts about various effects which also includes inert pair effects and about calculation of oxidation states. We have also come across the calculation of oxidation states which is based on the formation of those atoms with compounds that leads to the change in oxidation numbers.
- In group 14, the elements have four valence electrons. Therefore, the oxidation for this group is +4 and also there are several oxidation states which are stable for those particular atoms when it combines with other atoms.
- Some of the oxidation states are also unstable for the atoms present in their respective group and some of the atoms have more than one stable oxidation state.
- This is due to the inert pair effect which is basically defined as the tendency of the two electrons present in the outermost atomic s orbital that remains unshared in the compounds of post transition metals.
This results in the most tightly held electrons of ns shells towards the nucleus and thus participates in less bond formation or even no bond formation.
- Therefore, considering all these facts we can say that the group 14 elements have +4 oxidation states but due to the inert pair effect, the more stable oxidation state will be the lower ones and less stable oxidation states will be higher ones.

Thus, this group exhibits both +4 and +2 oxidation states and the correct answer is option B).

Note: To know the oxidation state of a particular group you must know the valence electrons present and even know that elements with same valence electrons are placed in that same particular group.