# Question #69d7d

Mar 23, 2017

$3 {\text{Mg"_ ((s)) + "N"_ (2(g)) -> "Mg"_ 3"N}}_{2 \left(s\right)}$

#### Explanation:

Magnesium will react with nitrogen gas to produce magnesium nitride, ${\text{Mg"_3"N}}_{2}$, and ionic compound that consists of magnesium cations, ${\text{Mg}}^{2 +}$, and nitride anions, ${\text{N}}^{3 -}$.

The unbalanced chemical equation looks like this

${\text{Mg"_ ((s)) + "N"_ (2(g)) -> "Mg"_ 3"N}}_{2 \left(s\right)}$

Notice that all you need to do in order to balance this chemical equation is multiply magnesium metal by $3$. This will give you a total of $3$ atoms of magnesium and $2$ atoms of nitrogen on both sides of the equation.

$3 {\text{Mg"_ ((s)) + "N"_ (2(g)) -> "Mg"_ 3"N}}_{2 \left(s\right)}$

This reaction is an example of a redox reaction. Here magnesium is being oxidized and nitrogen gas is being reduced.