12.51 comparing strengths of acids

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Michele Shi 1K
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Joined: Thu Jul 27, 2017 3:00 am

12.51 comparing strengths of acids

Postby Michele Shi 1K » Sat Dec 09, 2017 9:14 pm

Problem 12.51 part (a) asks to compare strengths of HF and HCL. HCL is stronger because Cl has a larger atomic radius. However, for part (c), HBrO2 vs HClO2, HClO2 is stronger than HBrO2 because Cl is more electronegative.

Why isn't HBrO2 stronger? In the case of HF and HCl, atomic radius was considered first. I thought you would use this same procedure for part (c) but electronegativity was considered over the atomic radius. Thank you!

Sabah Islam 1G
Posts: 50
Joined: Sat Jul 22, 2017 3:01 am

Re: 12.51 comparing strengths of acids

Postby Sabah Islam 1G » Sat Dec 09, 2017 9:31 pm

HClO2 is a stronger acid than HBrO2 because since Cl has a higher electronegativity, the resulting ClO2- is more stable than the resulting BrO2-. Since there are oxygens bonded to each of the central atoms in the instances of HBrO2 and HCl2, we need to take in account the formal charges present throughout the atoms to determine the stability, whereas, in HCl and HBr, the only thing bonded to the Br and Cl is H+, which is where we would take in account the size of each atom.

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