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.

C. 1s22s22p63s23p43d104s24p5

Product should she record in last row of the table

rosa was looking for patterns to predict the products of chemical reactions. she recorded three similar decomposition reactions in the table.she should record 2licl + 3o2.

in the last row of the table. it is the thermal decomposition of chlorate lithium, hence, she should record these products as: lithium chloride ( 2licl ) and oxygen ( 3o2 )   2 > 2 licl + 3o2.