Question

copper nitrate ionic equation

Answer 1

Chemical and Ionic Equations

Consider the reaction between copper metal and silver nitrate solution to form copper nitrate solution and silver metal.
            copper + silver nitrate → copper(II) nitrate + silver               
              Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)      ---------      Equation 1      
This is called a chemical equation, which shows all the reactants and products in a chemical reaction.
Silver nitrate is soluble in water. Its aqueous solution contains Ag+(aq) and NO3–(aq) ions. 
Similarly an aqueous solution of copper(II) nitrate contains Cu2+(aq) and NO3–(aq) ions. 
We can rewrite the chemical equation in the following form:
             Cu(s) + 2Ag+(aq) + 2NO3–(aq) → Cu2+(aq) + 2NO3–(aq) + 2Ag(s)
2NO3–(aq) appear on both sides of the chemical equation. They undergo no changes in the reaction,
i.e. they do not participate in the reaction. They are called spectator ions and we can cancel them.
             Cu(s) + 2Ag+(aq) + 2NO3–(aq) → Cu2+(aq) + 2NO3–(aq) + 2Ag(s)
or                                 Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)      ---------      Equation 2     
   
This is called an ionic equation, which shows only the species that participate in the reaction.
 
No. of atoms
Total charges
 LHS of equation
Cu = 1  Ag = 2
0 + (+2) = +2
 RHS of equation
Cu = 1  Ag = 2
(+2) + 0 = +2
 
For a balanced ionic equation,

No. of each type of atoms on the LHS = No. of each type of atoms on the RHS

Total charges on the LHS = Total charges on the RHS

Although equation 1 does not look the same as equation 2, they in fact represent the same chemical reaction. Hence
they are equivalent.
Ionic equations, rather than chemical equations, are sometimes employed for reactions involving ionic compounds.
It is because ionic equations

are simpler than the corresponding chemical equations;

show exactly the species that are involved in the reactions. 

Soluble ionic compounds
Many ionic compounds are soluble in water. When dissolved in water, the ions dissociate from each other. They are 
assigned the aqueous state (aq) after their formulae.  
e.g. K+(aq) and SO42–(aq).
.
Insoluble ionic compounds 
Some ionic compounds are insoluble, e.g. CaCO3, PbSO4 and Cu(OH)2. Their solubilities can only be tested by
performing experiments and cannot be predicted from their names or formulae. Their ions do not dissociate in 
water. When writing chemical equations, they are assigned the solid states (s) after their formulae, e.g. Cu(OH)2(s). ;
 
 

Answer 2

CuN is the copper nitrates valence ions of equation