The correct statement(s) about the oxoacids, $\mathrm{HClO}_4$ and HClO, is(are)

(A) The central atom in both $\mathrm{HClO}_4$ and HClO is $sp^3$ hybridized; (B) $\mathrm{HClO}_4$ is more acidic than HClO because of the resonance stabilization of its anion; (D) The conjugate base of $\mathrm{HClO}_4$ is weaker base than $\mathrm{H}_2\mathrm{O}$

(C) $\mathrm{HClO}_4$ is formed in the reaction between $\mathrm{Cl}_2$ and $\mathrm{H}_2\mathrm{O}$

JEE Advanced · 2017 · 21 May 2017 · Paper 1 · p-Block Elements

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The correct statement(s) about the oxoacids,

HClO_{4}

and HClO, is(are)

(A)The central atom in both $HClO_{4}$ and HClO is $s p^{3}$ hybridized✓ Correct
(B) $HClO_{4}$ is more acidic than HClO because of the resonance stabilization of its anion✓ Correct
(C) $HClO_{4}$ is formed in the reaction between $Cl_{2}$ and $H_{2} O$
(D)The conjugate base of $HClO_{4}$ is weaker base than $H_{2} O$ ✓ Correct

Answer: (A), (B), (D)

Solution

Option A: In

HClO_{4}

, Cl has 4 oxygen atoms around it (tetrahedral,

s p^{3}

). In HClO, Cl has 2 lone pairs and 1 oxygen (bent,

s p^{3}

).

Option B:

ClO_{4}^{-}

has four resonance structures, making it very stable, so

HClO_{4}

is a stronger acid than HClO.

Option C:

Cl_{2} + H_{2} O

gives HClO and HCl (disproportionation), not

HClO_{4}

.

Option D:

HClO_{4}

is a very strong acid (stronger than

H_{3} O^{+}

), so its conjugate base

ClO_{4}^{-}

is weaker than

H_{2} O

.

Correct answers: A, B, D

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JEE Advanced · 2017 · 21 May 2017 · Paper 1 · p-Block Elements

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