Oxidation States

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Vanessa Romero-Campos 2B
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Oxidation States

Postby Vanessa Romero-Campos 2B » Sun Feb 05, 2017 10:52 pm

How do you determine which elements are undergoing changes in oxidation states?

Ex: H(+) + Cr2O7 (2-) + C2H5OH ----> Cr(3+) + C2H4O +H20

I know that Cr is one of the elements, but how is Carbon also undergoing changes?

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Re: Oxidation States

Postby Kyle_Nakahira_1B » Sun Feb 05, 2017 11:00 pm

If the element undergoes a change in its charge, then there is a change in its oxidation state.

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Re: Oxidation States

Postby Terry1A » Sun Feb 05, 2017 11:27 pm

In that example you can see that C appears in two different compounds in the reactant and product (C2H5OH and C2H4O). You can calculate the charge of the C in C2H5OH because the charge for H is +1 and O is -2, so in order to neutralize the overall charge, C is -1. Then you do the same for the C in C2H4O and find that its charge is -1. Because the charge of C changed from -2 to -1 from reactant to product, you know that C is oxidized.

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Re: Oxidation States

Postby Cayla_Brooks_1I » Sun Feb 05, 2017 11:31 pm

When solving a two part problem asking you to balance a reaction under basic conditions (part a) then to balance the same reaction under acidic conditions (part b) how are you to navigate between adding H2O and OH-

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