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
vi₅
nh₄f
v(oh)₃
mn(no₃)₃

Explanation:

Step1: Analyze $VI_5$

In $VI_5$, vanadium has a charge of $V^{5 +}$ (since there are 5 iodine atoms and iodine has a - 1 charge in ionic compounds) and iodine has a charge of $I^{-}$.

Step2: Analyze $NH_4F$

In $NH_4F$, the ammonium ion is $NH_4^{+}$ and the fluoride ion is $F^{-}$.

Step3: Analyze $V(OH)_3$

In $V(OH)_3$, vanadium has a charge of $V^{3+}$ (because there are 3 hydroxide ions and each hydroxide ion has a - 1 charge) and the hydroxide ion is $OH^{-}$.

Step4: Analyze $Mn(NO_3)_3$

In $Mn(NO_3)_3$, manganese has a charge of $Mn^{3+}$ (due to 3 nitrate ions and each nitrate ion has a - 1 charge) and the nitrate ion is $NO_3^{-}$.

Answer:

Ionic compound	Cation	Anion
$NH_4F$	$NH_4^{+}$	$F^{-}$
$V(OH)_3$	$V^{3+}$	$OH^{-}$
$Mn(NO_3)_3$	$Mn^{3+}$	$NO_3^{-}$