# Question bd2d0

Mar 1, 2017

"Be"("NO"_3)_2#

#### Explanation:

Start with the fact that beryllium, $\text{Be}$, is located in group 2 of the Periodic Table of Elements, which suggests that it has $2$ valence electrons.

In order to become stable, it donates these electrons to form $2 +$ cations. This means that the beryllium cation will carry a $2 +$ charge.

${\text{Be}}^{2 +} \to$ the beryllium cation

The nitrate anion is actually a polyatomic ion that carries a $1 -$ charge.

${\text{NO}}_{3}^{-} \to$ the nitrate anion

Since beryllium nitrate is a neutral compound, the overall positive charge coming from the cations must be balanced by the overall negative charge coming from the anions.

This means that you will need two nitrate anions in order to balance the $2 +$ charge coming from one beryllium cation.

Therefore, you will have

${\left[{\text{Be"]^(2+) + 2 xx ["NO"_ 3]^(-) -> "Be"("NO}}_{3}\right)}_{2}$