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
$ce{mncl2}$	$square$	$square$
$ce{mn2s3}$	$square$	$square$
$ce{vf2}$	$square$	$square$
$ce{nio}$	$square$	$square$

Explanation:

Step1: Analyze \( \ce{MnCl2} \)

In \( \ce{MnCl2} \), the anion is \( \ce{Cl^-} \) (from the first example, chloride ion). For the cation, since there are 2 chloride ions (each with -1 charge), the manganese cation must have a +2 charge to balance the charge (total negative charge is \( 2\times(-1) = -2 \), so positive charge must be +2). So cation is \( \ce{Mn^{2+}} \), anion is \( \ce{Cl^-} \).

Step2: Analyze \( \ce{Mn2S3} \)

In \( \ce{Mn2S3} \), let the charge of \( \ce{Mn} \) be \( x \) and \( \ce{S} \) be \( y \). We know that for sulfide, the common charge is -2 (so \( y = -2 \)). There are 2 Mn and 3 S. Total charge: \( 2x + 3y = 0 \). Substituting \( y = -2 \): \( 2x + 3\times(-2) = 0 \) → \( 2x - 6 = 0 \) → \( 2x = 6 \) → \( x = +3 \). So cation is \( \ce{Mn^{3+}} \), anion is \( \ce{S^{2-}} \) (sulfide ion).

Step3: Analyze \( \ce{VF2} \)

In \( \ce{VF2} \), anion is \( \ce{F^-} \) (fluoride ion, charge -1). There are 2 F ions, so total negative charge is \( 2\times(-1) = -2 \). Thus, vanadium cation must have +2 charge to balance. So cation is \( \ce{V^{2+}} \), anion is \( \ce{F^-} \).

Step4: Analyze \( \ce{NiO} \)

In \( \ce{NiO} \), anion is \( \ce{O^{2-}} \) (oxide ion, charge -2). To balance, nickel cation must have +2 charge (since 1 Ni and 1 O: \( x + (-2) = 0 \) → \( x = +2 \)). So cation is \( \ce{Ni^{2+}} \), anion is \( \ce{O^{2-}} \).

Answer:

Ionic Compound	Cation	Anion
\( \ce{MnCl2} \)	\( \ce{Mn^{2+}} \)	\( \ce{Cl^-} \)
\( \ce{Mn2S3} \)	\( \ce{Mn^{3+}} \)	\( \ce{S^{2-}} \)
\( \ce{VF2} \)	\( \ce{V^{2+}} \)	\( \ce{F^-} \)
\( \ce{NiO} \)	\( \ce{Ni^{2+}} \)	\( \ce{O^{2-}} \)

(For the table cells:

• \( \ce{MnCl2} \): cation \( \ce{Mn^{2+}} \), anion \( \ce{Cl^-} \)
• \( \ce{Mn2S3} \): cation \( \ce{Mn^{3+}} \), anion \( \ce{S^{2-}} \)
• \( \ce{VF2} \): cation \( \ce{V^{2+}} \), anion \( \ce{F^-} \)
• \( \ce{NiO} \): cation \( \ce{Ni^{2+}} \), anion \( \ce{O^{2-}} \))