complete the table below by writing the symbols for the cation and anion that make up each ionic compound…

Explanation:

Step1: Analyze MnS

Manganese (Mn) forms a cation with a charge of +2 in this compound and sulfur (S) forms an anion with a charge of - 2. So the cation is $Mn^{2 + }$ and the anion is $S^{2-}$.

Step2: Analyze $NH_{4}Br$

The ammonium ion $NH_{4}^{+}$ is the cation and bromide ion $Br^{-}$ is the anion.

Step3: Analyze $Fe(NO_{3})_{3}$

Iron (Fe) has a charge of +3 in this compound and the nitrate ion $NO_{3}^{-}$ is the anion. So the cation is $Fe^{3+}$ and the anion is $NO_{3}^{-}$.

Step4: Analyze $CrCl_{4}$

Chromium (Cr) has a charge of +4 in this compound and chloride ion $Cl^{-}$ is the anion. So the cation is $Cr^{4+}$ and the anion is $Cl^{-}$.

Answer:

ionic compound	cation	anion
MnS	$Mn^{2 + }$	$S^{2-}$
$NH_{4}Br$	$NH_{4}^{+}$	$Br^{-}$
$Fe(NO_{3})_{3}$	$Fe^{3+}$	$NO_{3}^{-}$
$CrCl_{4}$	$Cr^{4+}$	$Cl^{-}$