example 14.1

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Miya Eberlein 1J
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Joined: Fri Sep 25, 2015 3:00 am

example 14.1

Postby Miya Eberlein 1J » Mon Feb 01, 2016 11:03 pm

can someone explain the oxidation half-reaction part of this example? I'm just confused about why C2 has an oxidation number of +3 when C usually has an oxidation number of 4.

thank you

Jana Sandhu 3J
Posts: 25
Joined: Fri Sep 25, 2015 3:00 am

Re: example 14.1

Postby Jana Sandhu 3J » Tue Feb 02, 2016 12:37 am

The molecule is C2H2O4. We know H is almost always +1, and O is almost always -2. The overall charge of the compound is 0. For hydrogen, 2x1 is +2, and for oxygen, 4x(-2) is -8. Adding these together gives -6. So we know that the total charge of the carbons must be +6 for the molecule's charge to equal 0. There are 2 carbons, so 6/2 is 3, therefore carbon has a charge of +3


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