Question

fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table:

cation	anion	empirical formula	name of compound
k⁺	clo⁻
pb²⁺	po₃³⁻
pb⁴⁺	so₃²⁻

Explanation:

Step1: Determine formula for $Ca^{2 +}$ and $BrO_{3}^{-}$

To balance charges, we need 2 $BrO_{3}^{-}$ for 1 $Ca^{2+}$. The empirical formula is $Ca(BrO_{3})_{2}$ and the name is calcium bromate.

Step2: Determine formula for $K^{+}$ and $ClO^{-}$

The charges balance in a 1:1 ratio. The empirical formula is $KClO$ and the name is potassium hypochlorite.

Step3: Determine formula for $Pb^{2+}$ and $PO_{3}^{3 -}$

To balance charges, we need 3 $Pb^{2+}$ and 2 $PO_{3}^{3-}$. The empirical formula is $Pb_{3}(PO_{3})_{2}$ and the name is lead(II) phosphite.

Step4: Determine formula for $Pb^{4+}$ and $SO_{3}^{2 -}$

To balance charges, we need 1 $Pb^{4+}$ and 2 $SO_{3}^{2-}$. The empirical formula is $Pb(SO_{3})_{2}$ and the name is lead(IV) sulfite.

Answer:

cation	anion	empirical formula	name of compound
$K^{+}$	$ClO^{-}$	$KClO$	potassium hypochlorite
$Pb^{2+}$	$PO_{3}^{3 -}$	$Pb_{3}(PO_{3})_{2}$	lead(II) phosphite
$Pb^{4+}$	$SO_{3}^{2 -}$	$Pb(SO_{3})_{2}$	lead(IV) sulfite