Question

part 3 of 3
iron(ii) sulfate (containing the fe²⁺ ion and so₄²⁻ ion)
name
empirical formula

Explanation:

Step1: Determine ion charges

The iron(II) ion has a charge of + 2 ($Fe^{2+}$) and the sulfate ion has a charge of - 2 ($SO_{4}^{2 - }$).

Step2: Balance charges

To balance the charges in an ionic compound, the ratio of cations to anions should result in a net - charge of zero. Since the magnitudes of the charges of $Fe^{2+}$ and $SO_{4}^{2 - }$ are equal, the ratio of $Fe^{2+}$ to $SO_{4}^{2 - }$ is 1:1.

Answer:

$FeSO_{4}$