Question

The correct statement(s) about the oxoacids, \[HCl{O_4}\]and \[HClO\], is(are):
This question has multiple correct options
A. The central atom in both \[HCl{O_4}\] and \[HClO\] is \[s{p^3}\] hybridized
B. The conjugate base of \[HCl{O_4}\] is weaker base than\[\;{H_2}O\]
C. \[HCl{O_4}\] is formed in the reaction between\[C{l_2}\] and \[\;{H_2}O\]
D. \[HCl{O_4}\] is more stable than \[HClO\] because of the resonance stabilization of its anion.

Answer 1

Hint: We know that oxoacids are the acids that have oxygen atoms in it. They are different from hydrochloric acid. Oxoacid may contain sulphur, carbon and nitrogen elements from p-block.

Complete answer:
Option (A) The central atom in both \[HCl{O_4}\]and \[HClO\] is \[s{p^3}\] hybridized. The central \[Cl\] atom in \[HCl{O_4}\] has \[4\] bonding domains and zero lone pairs of electrons. The oxygen atom in \[HClO\] has two bonding domains and two lone pairs of electrons.
Option (B) The conjugate base of \[HCl{O_4}\] is weaker than water. This is because \[HCl{O_4}\] is stronger acid than water. A stronger acid has weaker conjugate base and vice versa.
Option (D)\[HCl{O_4}\] is more acidic than \[HClO\] because of the resonance stabilization of its anion. Greater is the extent of delocalisation, greater is the stabilisation of negative charge and higher is the acidity. In \[HCl{O_4}\], negative charge is delocalised over four oxygen atoms.
Hence, the above statements (A), (B) and (D) are correct.
Now, let’s talk about the statement (C).
(C) \[HCl{O_4}\] is formed in the reaction between \[C{l_2}\] and \[{H_2}O\]. This is not the correct statement. Instead, the following methods are used.
\[NaCl{O_4} + HCl \to NaCl + HCl{O_4}\]

Hence, the answer is (A)(B) and (D).

Note:
Here the halogen can be any halogen from the halogen group of p-block.

Here as shown in the figure the chlorine will have a different oxidation state. The change in oxidation state will be as per the bonding of the atoms with chlorine and hybridisation will be dependent on that.