Give the systematic names for the formulas or the formulas for the names:

a. $\mathbf{Sn}{\mathbf{\left(}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\right)}}_{\mathbf{2}}$

b. potassium dichromate;

c. ${\mathbf{FeCO}}_{\mathbf{3}\mathbf{;}}$

d. Copper(II) nitrate.

The compound is an ionic compound. Tin ion can have many forms so the charge should be known for naming it. The subscripts will just interchange as charges of these elements.

$\mathbf{Sn}{\mathbf{\left(}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\right)}}_{\mathbf{2}}\mathbf{\to }{\mathbf{Sn}}^{4+}{\mathbf{SO}}_{\mathbf{3}}^{\mathbf{2}\mathbf{-}}$

The cation is tin (IV) and the anion is sulfite. So it is tin(IV) sulfite.

Dichromate is a polyatomic ion with a charge of -2 and potassium has a charge of +1. The charges will just interchange as the subscripts of these elements.

${\mathbf{K}}^{\mathbf{1}\mathbf{+}}{\mathbf{Cr}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{7}}^{\mathbf{2}}\mathbf{\to }\mathbf{\to }{\mathbf{K}}_{\mathbf{2}}{\mathbf{Cr}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{7}}$

The compound is an ionic compound. The name does not depend on the number of elements. Iron ions can have many forms so the charge should be known.

${\mathbf{CO}}_{\mathbf{3}}$is a polyatomic ion with charge -2. So Fe must be in +2 charge.

The cation is iron (II) and the anion is carbonate. So it is iron (II) carbonate

The charge of copper is +2 and the polyatomic ion nitrate has a charge of -1.

The charges will just interchange as the subscripts of these elements.

${\mathbf{Cu}}^{\mathbf{2}\mathbf{+}}{\mathbf{NO}}_{\mathbf{3}}^{\mathbf{1}\mathbf{-}}\mathbf{\to }\mathbf{Cu}{\left({\mathrm{NO}}_3\right)}_{\mathbf{2}}$