Question

fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table.
some ionic compounds
cation anion empirical formula name of compound
$rb^{+}$ $p^{3 -}$
$sn^{2+}$ $i^{-}$
$sn^{4+}$ $f^{-}$
$mg^{2+}$ $s^{2 -}$

Explanation:

Step1: Combine $Rb^+$ and $P^{3 -}$

To form a neutral ionic compound, we need 3 $Rb^+$ ions for every 1 $P^{3 -}$ ion. The empirical formula is $Rb_3P$ and the name is rubidium phosphide.

Step2: Combine $Sn^{2+}$ and $I^-$

We need 2 $I^-$ ions for every 1 $Sn^{2+}$ ion. The empirical formula is $SnI_2$ and the name is tin(II) iodide.

Step3: Combine $Sn^{4+}$ and $F^-$

We need 4 $F^-$ ions for every 1 $Sn^{4+}$ ion. The empirical formula is $SnF_4$ and the name is tin(IV) fluoride.

Step4: Combine $Mg^{2+}$ and $S^{2 -}$

The ratio is 1:1. The empirical formula is $MgS$ and the name is magnesium sulfide.

Answer:

cation	anion	empirical formula	name of compound
$Sn^{2+}$	$I^-$	$SnI_2$	tin(II) iodide
$Sn^{4+}$	$F^-$	$SnF_4$	tin(IV) fluoride
$Mg^{2+}$	$S^{2 -}$	$MgS$	magnesium sulfide