# How do you balance Ni + C_4H_8N_2O_2 -> Ni(C_4H_8N_2O_2)_2?

Jan 28, 2016

$N i + 2 {C}_{4} {H}_{8} {N}_{2} {O}_{2} \to N i {\left({C}_{4} {H}_{8} {N}_{2} {O}_{2}\right)}_{2}$

#### Explanation:

$N i + {C}_{4} {H}_{8} {N}_{2} {O}_{2} \to N i {\left({C}_{4} {H}_{8} {N}_{2} {O}_{2}\right)}_{2}$
as there are 1 molecule nickel, 4 molecules of carbon, 8 molecules of hydrogen, 2 molecules of nitrogen, and 2 molecules of oxygen in left hand side
but 1 molecule of nickel, 8 molecules of carbon, 16 molecules of hydrogen, 4 molecules of nitrogen, and 4 molecules of oxygen
so, by multiplying ${C}_{4} {H}_{8} {N}_{2} {O}_{2}$ by $2$ the equation will be balanced.

Jan 28, 2016

${\text{Ni"_text((aq])^(2+) + 2"C"_4"H"_8"N"_2"O"_text(2(aq]) -> "Ni"("C"_4"H"_7"N"_2"O"_2)_text(2(s]) darr + 2"H}}_{\textrm{\left(a q\right]}}^{+}$

#### Explanation:

The starting chemical equation given to you is actually incorrect.

This reaction takes place in aqueous solution and it involves the nickel(II) cation, ${\text{Ni}}^{2 +}$, not nickel metal, $\text{Ni}$.

Reacting nickel(II) cations with dimethylglyoxime, ${\text{C"_4"H"_8"N"_2"O}}_{2}$, will produce an insolube solid called nickel dimethylglyoxime, "Ni"("C"_4"H"_8"N"_2"O"_2)_2, which will precipitate out of solution.

The nickel(II) cations can be delivered to the solution by a soluble salt like nickel(II) nitrate, "Ni"("NO"_3)_2.

The actual balanced chemical equation for this reaction can be written like this

${\text{Ni"_text((aq])^(2+) + 2"C"_4"H"_8"N"_2"O"_text(2(aq]) -> "Ni"("C"_4"H"_7"N"_2"O"_2)_text(2(s]) darr + 2"H}}_{\textrm{\left(a q\right]}}^{+}$

The reaction involves two dimethylglyoxime molecules acting as chelating agents to form the nickel dymethylglyoxime complex. When the nickel(II) cations are delivered via nickel(II) nitrate, the reaction will produce

${\text{Ni"("NO"_3)_text(2(aq]) + 2"C"_4"H"_8"N"_2"O"_text(2(aq]) -> "Ni"("C"_4"H"_7"N"_2"O"_2)_text(2(s]) darr + 2"HNO}}_{\textrm{3 \left(a q\right]}}$

The nitrate anions, ${\text{NO}}_{3}^{-}$, are spectator ions in the reaction, meaning that they can be found on both sides of the chemical equation.

This reaction is used as a confirmation test for the presence of nickel(II) cations. Nickel dymethylglyoxime is a red precipitate. 