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Chemistry 9 Online
OpenStudy (anonymous):

Say I have the compound: Pb(C2H3O2)3. How do I determine the oxidation states? I know I split it up into ions: (C2H3O2)1- According to the rulings, OX[H] = +1 OX[O] = -2 So then: 2x + 3(+1) + 2(-2) = -1 2x + 3 -4 = -1 2x - 1 = -1 2x = 0 x = 0? Where x represents OX[C]. Is it by all means possible to have an oxidation number of 0?

OpenStudy (anonymous):

Also, is the oxidation state of PB3+: OX[Pb] = +3?

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