Illustrate by taking examples of transition elements and non-transition elements that oxidation states of elements are largely based on electronic configuration.

Answer

A

Explanation

Oxidation state of an element depends upon the electrons present in the outermost shell or eight minus the number of valence shell electrons (outermost shell electrons). E.g.
Alkalli metals (Group 1 elements) General valence shell electronic configuration `-ns^(-1)`, Oxidation states =`+1`.
Alkaline earth metals, (Group 2 elements) General valence shell electronic configuration -`ns^(2)`, Oxidation state =`+2`
Alkali metals and alkaline earth metals belong to s-block elements and elements of group of 13 to group 18 are known as p-block elements.
Group 13 elements: General valence shell electronic configuration `-ns^(2), np^(1)`. Oxidation states =`+3` and `+1`.
Group 14 elements: General valence shell electronic configuration `-ns^(2) np^(2)`, Oxidation states `=+4` and `+2`.
Group 15 elements: General valence shell electronic configuration`-ns^(2) np^(3)`, Oxidation states `=-3, +3` and `+5`. Nitrogen shows `+1,+2, +4` oxdiation states also.
Oxidation 16 elements. General valence shell electronic configuration `-ns^(2), np^(4)`, Oxidation states =`-2,+2, +4` and `+6`.
Group 17 elements: General valence shell electronic configuration -`ns^(2) np^(5)`, Oxidation states =`-1` , Cl, Br and I also show `+1, +3, +5` and `+7` oxidation states.
Group 18 elements: General valence shell configuration `-ns^(2) np^(6)`. Oxidation state = zero.
Transition elements or d-block elements: General electronic configuration `-(n-1)d^(1-10) ns^(1-2)`. These elements show variable oxidation states due to involvement of not only ns electrons but d or f-electrons (inner-transitioin elements) as well. Their most common oxidation states are `+2` and `+3`.