# Magnesium reacts with titanium(4) chloride to produce magnesium chloride and titanium metal. How do you write a balanced equation for this reaction?

Dec 18, 2016

$2 M g + T i C {l}_{4} \rightarrow 2 M g C {l}_{2} + T i$

#### Explanation:

Because the magnesium ion has a +2 charge, the formula for magnesium chloride is $M g C {l}_{2}$.

To balance the four Cl ions in titanium (IV) chloride, the reaction must produce 2 units of $M g C {l}_{2}$

Dec 18, 2016

$T i C {l}_{4} + 2 M g \rightarrow T i + 2 M g C {l}_{2}$

#### Explanation:

We could do this by individual redox steps:

$T i C {l}_{4} + 4 {e}^{-} \rightarrow T i + 4 C {l}^{-}$ $\left(i\right)$

$M g \rightarrow M {g}^{2 +} + 2 {e}^{-}$ $\left(i i\right)$

$\left(i\right) + 2 \times \left(i i\right) =$ $T i C {l}_{4} + 2 M g \rightarrow T i + 2 M g C {l}_{2}$

With all chemical reactions, 2 conditions must be absolutely satisfied: (i) mass must be balanced; and (ii) charge must be balanced. Well, is they?

Note that just because I can write the reaction, there is no likelihood that the reaction can be performed. Should I attempt to reduce the chloride with magnesium metal I would likely get a mess. Titanic chloride is unstable with respect to water and dioxygen.