14.1 (b)

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Ilan Shavolian 1K
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Joined: Fri Sep 29, 2017 7:03 am

14.1 (b)

Postby Ilan Shavolian 1K » Thu Feb 22, 2018 2:19 am

pretty basic question but can someone help me understand how to find the oxidation numbers of the atoms in the C2H5OH and C2H4O?

Alyssa Parry Disc 1H
Posts: 53
Joined: Sat Jul 22, 2017 3:01 am

Re: 14.1 (b)

Postby Alyssa Parry Disc 1H » Thu Feb 22, 2018 9:54 am

You have to look at the other molecules and their typical oxidation states like in this one you would look at the oxidation states of H and O, Usually +1 and -2 respectively and then look at the total charge of both molecules, I think in this case its 0 for both and then you just do algebra. Like for the first one there are 6 H and 1 O so 6(+1) +1(-2) + 2X = 0, and then you would get X=-2 so thats the oxidation state for that carbon in that molecule C2H5OH. Then you do the same for the others.

Grace Han 2K
Posts: 33
Joined: Tue Nov 15, 2016 3:00 am

Re: 14.1 (b)

Postby Grace Han 2K » Thu Feb 22, 2018 10:05 am

Oxygen is going to have an ON (Oxidation number) of -2 unless its in a peroxide.
Hydrogen is going to have an ON of +1 if its with nonmetals.
Now we have to solve for Carbon's ON
When adding up all of the ON for C2H5OH, it should equal zero.

____/2 (Carbon)+ 6x +1(Hydrogen) + -2(Oxygen)= O
Then ON of carbon is -2

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