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Assign reasons for each of the following : (i) + 1 gallium undergoes disproportionation reactions. (ii) Unlike In^(+), Ti^(+) is more stable with respect to disproportionation. (ii) InCl undergoes disproportionationbut TlCl does not. (iv) In (III)is more stablethan In (I) aqueous solution. |
Answer» Solution :(i) Due to inert pair effect, galliumshowsboth +1 and +3 oxidationstates butits +3 oxidationstate is more stable than `+1` oxidationstate.In other words +1 oxidation state. Inother words `+1` gallium is less stable than +3 gallium and hence undergoes disproportionation (self oxidation -reduction) to form gallium metal and the more stable+3 gallium IONS in aqueoussolutionas shownbelow : (ii) Althroughboth In and TI can show oxidationstates of +1 and +3 , but inert pair effect is more prominent in Tl than in In. Therefore,+1 oxidationstate of Tl is more stablethan its +3 oxidation state while +3 oxiationstate ofln is more stablethan its + 1 oxidationstate.Consequently in aqueous solution, less stable`ln^(+)`undergoesdisproportionation to form more state `In^(3+)` but `+1`thalliumbeing more stabledoes not undergo disproportionationto form +3 THALLIUM. `3In^(+) (aq) overset("Disproportionation")rarr 2In(s) + In^(3+) (aq)`  (iii) As statedabove, `+3` oxidationstate of In is more stable than its +1 oxidationstate, therefore, `InCl` undergoesdisproportionation in aqueoussolution. `3In Cl(aq) rarr 2In (s) + In^(3+) (aq) + 3Cl^(-) (aq)` Since +1 oxidationstate of Tl is morestablethan its +3 oxidationstate,therefore,`TlCl` does notundergo disproportional in aqeuoussolution.  (iv) Same as explained in ANSWER (ii) above. |
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