Why HClO2 is stronger acis than H2SO4?
Answers
In both, the oxygens bonded to the chlorine but not to the hydrogen draw the electrons in the O—H bond towards the chlorine and the oxygen, making the O—H bond more polar. ... This results in a stronger acid, as the hydrogen will more readily dissociate in a more polar bond.
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Explanation:
ClO2 is not an acid, or not a Bronsted acid anyway. Note the lack of hydrogen. ClO2 is a radical, although like NO a rather stable one,
A more interesting question is why HClO3 is a stronger acid than HClO2. It is in fact usually the case that when the parent element is the same, the higher oxidation state gives the stronger acid. There is an explanation for this.
Structurally HClO3 is [O2Cl]OH and HClO2 is [OCl]OH. Both ionize to give conjugate bases, ClO3(-) which is [O2Cl]O-, and ClO2(-) which is [OCl]O-. In both cases, the O- is directly attached to Cl. But if we accept oxidation number as an atomic charge, we are comparing Cl(+5)—O(-2) with Cl(+3)—O(-2). The former has a greater electrostatic attraction between the Cl and O, and hence the stronger bond. This stabilizes ClO3(-) more than ClO2(-), and contributes to making ClO3(-) the weaker conjugate base, and hence HClO3 is the stronger acid.
There is another factor stabilizing ClO3(-) over ClO2(-). These are both resonance hybrids (look if you don’t understand this term). Resonance makes the three oxygen atoms in ClO3(-) equal, so that each oxygen atom has -1/3 charge. Similarly, resonance gives each oxygen atom in ClO2(-) a -1/2 charge. Since the negative charge is more spread out in ClO3(-) than in ClO2(-), this also makes ClO3(-) a weaker conjugate base, and thus HClO3 the stronger acid
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