Redox half reactions

we are doing redox half reactions in chem
we need to write a balabced net ionic equation
the oxidation half-reaction
the reduction half-reaction

this is what i got for
2Na+FeCl2->2NaCl+Fe

net:2Na->2NaCl->2Fe+L
oxidation:2Na->2Na-+2e-
reduction:Fe+2 +2e-->Fe

now i cant figure this one out
AgNo3+Cu->CuNo3+Ag
need net ionic,oxidation, reduction
thanks

SYMBOLS:
e- = electron
(s)/(aq) = physical state
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WORK:
I'm assuming that the Copper is of the (I) form.

**Oxidation**: Cu(s) --> Cu+(aq) + e-

**Reduction**: Ag+(aq) + e- --> Ag(s)

**Net ionic**: Ag+(aq) + Cu(s) + e- --> Ag(s) + Cu+(aq) + e-
You may then cross out the electrons, ie:
Ag+(aq) + Cu(s) --> Ag(s) + Cu+(aq)


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Note: NO3-(aq) is a spectator ion, and is hence irrelevant in the answer required. The reason it is a spectator ion is that it is in aqueous form throughout the whole equation.

AgNO3 + Cu ----> CuNO3 +Ag (net ionic, already balanced!)
(Ag=+1, Cu=0) (Cu=+1, Ag=0) these are oxidation numbers of the elements.

oxidation half reaction: Cu ---> CuNO3 + e-

reduction half reaction: AgNO3 +e- ----> Ag