Question

complete the table below by writing the symbols for the cation and anion that make up each ionic compound. the first has been completed for you.

ionic compound	cation	anion
mns
nh₄br
fe(no₃)₃
crcl₄

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
$NH_{4}Br$	$NH_{4}^{+}$	$Br^{-}$
$Fe(NO_{3})_{3}$	$Fe^{3+}$	$NO_{3}^{-}$
$CrCl_{4}$	$Cr^{4+}$	$Cl^{-}$