How would you account the lower atomic radius of $G a$ as compared to $A l$ .

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Solution

The lower atomic radius of Ga as compared to Al can be explained on the basis of the presence of 3d series of transition metals. The size of d orbitals is larger than that of p orbitals. This results in poor shielding in d block elements. Hence, the effective nuclear charge of Ga is lower than the expected value. This results in lower atomic radius.

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G a

A l

(a) How would you account for the following:

(i) The chemistry of actinoids is more complicated as compared to lanthanoids.

(ii) Transition metals form complex compounds.

(b) Complete the following equation:

$2 {M n O_{4}}^{-} + 6 H^{+} + {S O_{3}}^{2 -} \to$

2 {M n O_{4}}^{-} + 6 H^{+} + S {O_{3}}^{2 -} ⟶

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