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moongazer Group TitleBest ResponseYou've already chosen the best response.0
I already know the rules in finding the oxidation number I just don't know how to get it in this one.
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
Sulfate has a charge of 2
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
Thus we can conclude that Magnesium would have a charge of +2
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
I would assume
 2 years ago

moongazer Group TitleBest ResponseYou've already chosen the best response.0
It is from KMnO4 + KCl + H2SO4 = K2SO4 + MnSO4+Cl2+H2O I already determined the other oxidation number from this except for MnSO4
 2 years ago

moongazer Group TitleBest ResponseYou've already chosen the best response.0
How about for oxygen? isn't it it should have an oxidation number of 2 ?
 2 years ago

shubham.bagrecha Group TitleBest ResponseYou've already chosen the best response.0
MnSO4 +H2O > Mn^(2+) + SO4^(2)
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
Oxygen, 2, 2, 2, 2 Sulpher is a less electronegative element so it will give up its electrons more readily S has +6 6 2 2 2  2 = 2 charge total
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
I could be wrong, as I'm going off what I have read on Wikipedia and my knowledge of chemistry
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
I'm basing this on the fact in Oxygen Diflouride OF2 Oxygen has a charge of +2 instead of 2 because fluoride is more electronegative than oxygen
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
and since PO4 is a polyatomic anion, I would expect it to maintain its integrity while bonded to manganese, although this is speculation on my part I hope it is helpful.
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
If you have any questions feel free to ask
 2 years ago

moongazer Group TitleBest ResponseYou've already chosen the best response.0
So the oxidation numbers will be Mn(+2)S(+6)O4(2) I based in your statement "Sulfate has a charge of 2 Thus we can conclude that Magnesium would have a charge of +2"
 2 years ago

moongazer Group TitleBest ResponseYou've already chosen the best response.0
Is it correct?
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
O4 should probably have a charge of 8 if S has a charge of +6
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
but your conclusion seems correct other wise, Remember Oxygen can attract and hold electrons better than sulfer, so sulfer basically becomes an electron source for the oxygen so they can be more like Neon, making Sulfer more like Neon as well instead of what it usually wants to be like Argon
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
I'm pretty sure the 2 charge is just distributed through out all the oxygen atoms until manganese comes along and donates 2 of its electrons
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
wait you are probably correct if it is asking for the charge of each individual atom separately :)
 2 years ago

moongazer Group TitleBest ResponseYou've already chosen the best response.0
I am getting all the oxidation numbers separately for balancing. Thanks :)
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
To be honest with you I have never had to answer a question like this I dont think
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
But I have taken a lot of chemistry courses in my life so I dont know that has to count for something
 2 years ago

moongazer Group TitleBest ResponseYou've already chosen the best response.0
Did you mean you haven't balanced a reaction using the oxidation state change method ?
 2 years ago

moongazer Group TitleBest ResponseYou've already chosen the best response.0
anyway, thanks for the help :)
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
yeah
 2 years ago

Australopithecus Group TitleBest ResponseYou've already chosen the best response.1
I had some other method when I did these problems that I cannot remember, but yeah no problem thanks for the question chemistry problems subside the insanity for me :)
 2 years ago
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