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Question

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

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Solution

Oxidation state of an element, depends upon the electrons present in the outermost shell or eight minus the number of valence shell electrons (outernost shell electrons) .
Alkali metals (Group 1 elements) General valence shell electronic configuration - ns1;
oxidation state = +1.
Alkallne earth metals( Group 2 elements ) General valence shell electronic configuration - ns2 oxidation state = +2
Alkali metals and alkaline earth metalks belong to s - block elements and elements of group 13 to group 18 are known as p - block elements.
Group 13 elements General valence shell electronic configuration ns2np1 Oxidation
States = +3 and +1
Group 14 element General valence shell electronic configuration - ns2np2; Oxidation states =+4and+2.
Group 15 elements General valence shell electronic configuration ns^2 np^3; Oxidation
States =3+3and+5, Nitrogen shows+1,+2,+4 oxidation states also,
Group 16 elements
General valence shell electronic configuration ns2np4 oxidation staes =2,+2,+4and+6
Group 17 elements General valence shell electronic configuration - ns^2 np^6; Oxidation states = - 1, Cl Br and I also show +1, 3, +5 and +7 oxidation states,
Group 18 elements
General valence shell configuration ns2np6. Oxidation states = zero.
Transition elements or d - lock elements General electronic configuration - (n1)d110ns12 . these elements show variable oxidation states due to involvement of not only ns electrons but d or f - electrons (inner - transition elements) as well . Their most common oxidation states are +2 and +3


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