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Question
Illustrate by taking examples of transition elements and non-transition elements that oxidation states of elements are largely based on electronic configuration.
Solution
The electronic configuration of \[\ce{Cr}\] = 1s2 2s2 2p6 3s2 3p6 4s1 3d10
The electronic configuration of \[\ce{Cr}\] after losing one electron= 1s2 2s2 2p6 3s2 3p6 3d10
The electronic configuration of \[\ce{F}\] = 1s2 2s2 2p6 3s2 3p5
The electronic configuration of \[\ce{F}\] after gaining one electron= 1s2 2s2 2p6 3s2 3p6
From the above electronic configuration we can see that chromium will achieve stable electronic configuration after losing one 4s electron and fluorine will achieve stable electronic configuration after gaining one electron. So, the oxidation of chromium will be +1 and that of fluorine will be –1.
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