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Describe the general trends in the following properties of the elements in Groups-13 Oxidation states |
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Answer» Solution :Oxidation states: In the electronic configurations of elements of group-13 they have two electrons in s-type orbital and one electron in p-type orbitals, so total three electrons in outermost orbital, hence it possesses +3 oxidation state. The oxidation state of boron and aluminium is +3 while Ga, In and TL have both +1 and +3 oxidation states. As the atomic number is increasing the stability of +3 oxidation state decreases and stability of +1 oxidation state INCREASES because on going down the group as the atomic number is increasing the tendency of s-electron to PARTICIPATE in bond FORMATION decreases which means `ns^2` electron of Ga, In and Tl remain paired because of INTERVENING of d and f-orbitals. The screening effect of `ns^2` orbitals becomes poor and inert pair effect becomes more predominant as atomic number increases and so the `ns^2` orbital electrons are more strongly attracted towards the nucleus and therefore, it is difficult to remove that electron, so the stability of oxidation state +1 increases and that of +3 oxidation state decreases. |
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