Fall 2010 Final Exam Question 5

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Hailey Donaldson 1E
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Joined: Fri Sep 25, 2015 3:00 am

Fall 2010 Final Exam Question 5

Postby Hailey Donaldson 1E » Thu Dec 03, 2015 9:15 am

On page 223 of the course reader, the question reads "Draw the most stable Lewis Structure for the following Bronsted acids and list them from least acidic to most acidic: HClO3;HCLO; HCLO2;HCLO4. Explain their trend in increasing stability. Why is HClO4 the most acidic?

Jake Ney lecture 1 discussion 1F
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Joined: Fri Sep 25, 2015 3:00 am

Re: Fall 2010 Final Exam Question 5

Postby Jake Ney lecture 1 discussion 1F » Thu Dec 03, 2015 11:27 am

HCLO:

Cl-O-H

HCLO2:

O
ll
Cl-O-H

HClO3:

O
ll
Cl-O-H
ll
O

HClO4:

O
ll
O=Cl-O-H
ll
O

As these acids have an increasing number of Oxygens bonded to the central Cl, these Oxygens which are highly electronegative withdraw e- density from the Oxygen attached to the hydrogen atom. Thus as there are more oxygen atoms, the oxygen atom bonded to the hydrogen becomes less electronegative as in unable to bond with the Hydrogen atom as strongly. HCO4 is the most acidic because it releases its Hydrogen atom with the most ease.


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