[Kelth]

     Hey all, first post! ^.-.^ pleasure to be aboard. Unfortunatly my first post is one asking for clarification.
Ok First off, here is the chemically equation, Unbalenced mind you (please excuse poor MSpaint representation):                                                                                                                                                                             






Now, what i can not figure out is that....shouldn't the charges equal out? I mean shouldn't it neutral? no charge? or...what am I forgetting?
Thanks for the *delete me*

[Borek]

what am I forgetting?

To balance the equation.

[Kelth]

eeh that only makes the charges worse:

2K₃PO₄ + 3Sr(NO₃)₂ --produces--> 6KNO₃ + Sr₃(PO₄)₂


still the charges are not neutral.

6KNO₃ now has
K: 6(+1) = +6     N: 6(-3) = -18   O: (6*3)(-2) = -36

 +6 != -56

[DrCMS]

KN0₃ is a neutral species. 

Look up the structure of nitrates, try here

http://en.wikipedia.org/wiki/Nitrate

[Alexander]

eeh that only makes the charges worse:

6KNO₃ now has
K: 6(+1) = +6     N: 6(-3) = -18   O: (6*3)(-2) = -36

 +6 != -56

here is a mistake:
N: 6(+5)=+30  not "-3" and "-18"

[xiankai]

try not to figure out the oxidation numbers of individual atoms, but that of the ions instead.

that is to say, you know PO₄ has a valency of -3, dont try to find out the valency of P and O separately, its too much trouble and proves nothing (you got the valency of P wrong btw, its +5), since the overall ion will remain the same.

[AWK]

For double exchange reaction use charges for anions and cations, not for individual atoms