Question

the order of relative stability of 1 oxidation state for heavior elements is

Answer 1

The boron family contains elements in group 13 of the periodic talbe and include the semi-metal boron (B) and the metals aluminum (Al), gallium (Ga), indium (In), and thallium (Tl). Aluminum, gallium, indium, and thallium have three electrons in their outermost shell (a full s orbital and one electron in the p orbital) with the valence electron configuration ns2np1. The elments of the boron family adopts oxidation states +3 or +1. The +3 oxidation states are favorable except for the heavier elements, such as Tl, which prefer the +1 oxidation state due to its stability; this is known as the inert pair effect.

Answer 2

Answer:

Al < Ga < In < Ti

Explanation:

Oxidation state of boron family -

Boron show +3 covalence, this tendency decreases down the group, other members have +3 oxidation state form ionic compounds.

- wherein

Lower elements also show +1 ionic state due to inert pair effect. E.g. Tl+, Ga+

Inert pair effect -

The phenomenon in which outer shell s electrons (ns2) penetrate to (n-1) d-electrons and thus become closer to nucleus and are more effectively pulled by the nucleus

- wherein

This results in less availability of ns2 electrons pair for bonding or ns2 electron pair becomes inert.

Due to inert pair effect as we move down the group in 13th group lower oxidation state becomes more stable.

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