Writing net ionic equation: a solution of diamminesilver(i) chloride is treated with dilute nitric acid. so what i did was.. [ag(nh3)2]cl(aq) + hno3(aq) -> the answer is [ag(nh3)2]+ + cl- + 2h+ -> agcl + 2nh4+ i would guess that the oxidation #s for diamminesilver(i) chloride would be: ag +1 nh3 0 cl -1 can someone show me the steps in between? i don't really know how to break the [ag(nh3)2]cl apart and predict/form the products.

The net ionic equation is:
[Ag(NH₃)₂]⁺ + Cl⁻ + 2H⁺ → AgCl + 2 NH₄⁺ 
As i can see that you balanced it correctly also you calculated the charge of each part correctly but you need to know more details about complexes:
complex is formed between Metal cations  as Ag⁺, Cu⁺², Fe⁺³ and ligands which may be neutral as NH₃ or H₂O or negatively charged as CN⁻ or halide 
The number of ligands attached to metal is the co-ordination number, in our case Ag has coordination number = 2 so it must attached to two ligands which are NH₃ here (neutral ligands) 
- The charge of complex is the sum of metal and ligand charges +1 for Ag and 0 for NH₃ so the overall charge of complex is +1
 so the complex must be attracted to negatively charged anion which is Cl⁻ here and both react with H⁺ from acid (HNO₃) to give AgCl precipitate and NH₄⁺ ion.