Question

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

ionic compound	cation	anion
$ce{vbr3}$	$square$	$square$
$ce{crf3}$	$square$	$square$
$ce{coi2}$	$square$	$square$
$ce{mno}$	$square$	$square$

Explanation:

Step1: Analyze \(VBr_3\)

In ionic compound \(VBr_3\), the cation is \(V^{3+}\) (since the formula has 3 \(Br^-\) ions, and to balance charge, \(V\) has +3 charge) and anion is \(Br^-\).

Step2: Analyze \(CrF_3\)

For \(CrF_3\), the cation is \(Cr^{3+}\) (3 \(F^-\) ions, so \(Cr\) has +3 charge) and anion is \(F^-\).

Step3: Analyze \(CoI_2\)

In \(CoI_2\), the cation is \(Co^{2+}\) (2 \(I^-\) ions, so \(Co\) has +2 charge) and anion is \(I^-\).

Step4: Analyze \(MnO\)

For \(MnO\), the cation is \(Mn^{2+}\) (1 \(O^{2-}\) ion, so \(Mn\) has +2 charge) and anion is \(O^{2-}\).

Answer:

Ionic Compound	Cation	Anion
\(VBr_3\)	\(V^{3+}\)	\(Br^-\)
\(CrF_3\)	\(Cr^{3+}\)	\(F^-\)
\(CoI_2\)	\(Co^{2+}\)	\(I^-\)
\(MnO\)	\(Mn^{2+}\)	\(O^{2-}\)