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oxidation state on homonuclear molecules or elemental species = 0
Oxygen = -2 always
you can figure out the rest by balancing the charges
Alright, so for a i got 0, b -3, c -2, d 1, e 2, f -2 and g 0. Are these right?
Let me see if I get this right: You suggest that hydrogen in water have the oxidation number -3?
I believe so
Okay. We need an additional rule: "The sum of oxidations numbers most equal to total charge of the molecule." So when we look at water it have no charge... sense oxygen always get -2 each hydrogen most be what?
-5? And in that equation, which element was reduced and which was oxidized?
And can verify my answers please?
Best you get some training, so I'm gonna start with water and we take them each by each. H2O we take notice: Total charge = 0 oxygen always -2 Hydrogen always +1 This also make sense we should say: 0=-2+2*x <-> x=+1
aluminum is right. again it does not have charge and is an elemental species.
Both hydrogens are positive one as well?
Yes. it is 2 times +1
Alright, so what about for e through g?
Sorry I was thinking. both e and g are wrong.
The oxidation state of oxygen is -2 the oxidation state of hydrogen is +1: so we get: Al(OH)4 -1 -1 = -8+4+x Here is x the oxidation state of Al.. What is x?
So aluminum was reduced, so which was oxidized?
which one are you working on?
I need the answer for g and then: In the equation above, which element was reduced and which element was oxidized?
The H on the compound is part of the hydroxide ion, which is OH^- since O is -2 and theres a -1 charge on ion, H is +1
Awesome. so then which was oxidized and which was reduced?
they're both 0 when not part of a molecule, if one gains e then we say its reduced because it became more negative, the opposite is for oxidized.
I mean for all of the elements in the equations, it seems like aluminum gained electrons
we already did everything in the equation