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2 months ago

For each group of compounds listed, which is the strongest acid? I. HIO2, HIO3, HIO4 II. H2Se, H2S, H3As III. HPO2, HClO2, HBrO2

Chemistry

1 answer:

Anarel [2.9K]2 months ago

7 0

Answer:

In group I, the most potent acid is $HIO_4$ .

For group II, the strongest acid is $H_2Se$ .

In group III, the strongest acid identified is $HClO_2$ .

Explanation:

Group I:

The strength of an acid is influenced by the stability of the conjugate base formed after H+ ion loss.

From the acids provided, the following conjugate bases result upon H+ release:

$HIO_2 \rightarrow H^+ + IO_2^-\\HIO_3 \rightarrow H^+ + IO_3^-\\HIO_4 \rightarrow H^+ + IO_4^-$

In $IO_4^-$ , the negative charge is spread across three electronegative oxygen atoms, rendering it more stable compared to the other two conjugate bases.

Thus, $HIO_4$ becomes the strongest acid in this group.

Group II:

The H-Se bond is less robust than H-S bonds, making it more acidic since breaking the H-Se bond more easily releases H+.

For $H_3As$ , arsenic (As) has lower electronegativity than selenium (Se). Due to the higher electronegativity of Se, it attracts the electrons of the H-Se bond, facilitating the removal of H+.

Consequently, $H_2Se$ is the strongest acid in this grouping.

Group III:

Acidity is also impacted by the distance between bonds and the central atom's electronegativity.

In this scenario, electronegativity takes precedence over bond distance.

Among the elements listed, chlorine (Cl) exhibits the highest electronegativity. This significant electronegativity causes the electrons to be pulled toward Cl, making the release of H+ easier compared to the other two.

Therefore, $HClO_2$ is the strongest acid in this set.

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