Question

13 multiple choice 1 point fe(so₄) iron (ii) sulfate iron (ii) sulfide iron (i) sulfate iron (i) sulfide

Explanation:

• The sulfate ion has the formula \(SO_{4}^{2 -}\).
• Iron (II) has a charge of \(+ 2\).
• When naming ionic compounds, we use the name of the cation (Iron (II)) followed by the name of the anion (sulfate).
• Sulfide ion is \(S^{2 -}\), which is not present in \(FeSO_{4}\).
• Iron (I) has a charge of \(+1\), which does not balance with the sulfate ion (\(SO_{4}^{2 -}\)) to form \(FeSO_{4}\) (\(+2+( - 2)=0\) for \(Fe^{2 +}\) and \(SO_{4}^{2 -}\), while for \(Fe^{+}\) and \(SO_{4}^{2 -}\), the charge balance would require \(Fe_{2}SO_{4}\)).

Answer:

Iron (II) Sulfate