For the properties mentioned, the correct trend for the different species is :

inert pair effect -

A l > G a > I n

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first ionization enthalpy -

B > A l > T l

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strength as Lewis acid -

B {C l}_{3} > A l {C l}_{3} > G a {C l}_{3}

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oxidising property -

{A l}^{+ 3} > {I n}^{+ 3} > {T l}^{+ 3}

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Solution

The correct option is C strength as Lewis acid - $B {C l}_{3} > A l {C l}_{3} > G a {C l}_{3}$
On moving down in group tendency to accept lone pair decreases. Therefore, lewis acid strength decreases $B C l_{3} > A l C l_{3} > G a C l_{3}$

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Similar questions

G a, A l, T l, P b, S n, G e

E^{o}

A l^{3 +} / A l

T l^{3 +} / T l

- 1.66 V

+ 1.26 V

The first ionization enthalpy values (in kJmol^–1) of group 13 elements are :

B	Al	Ga	In	Tl
801	577	579	558	589

How would you explain this deviation from the general trend?

The order of ionization enthalpy for B, Al and Ga is:

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