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
$pb^{2 + }$	$po_{4}^{3 - }$
$k^{+}$	$bro_{4}^{-}$
$ca^{2 + }$	$io^{-}$
$pb^{4 + }$	$so_{4}^{2 - }$

Explanation:

Step1: Determine formula for $Pb^{2 +}$ and $PO_{4}^{3 -}$

To form a neutral compound, we need to balance the charges. The least - common multiple of 2 and 3 is 6. So we need 3 $Pb^{2+}$ ions and 2 $PO_{4}^{3 -}$ ions. The empirical formula is $Pb_{3}(PO_{4})_{2}$, and the name is lead(II) phosphate.

Step2: Determine formula for $K^{+}$ and $BrO_{4}^{-}$

Since the charges are + 1 and - 1 respectively, the empirical formula is $KBrO_{4}$, and the name is potassium perbromate.

Step3: Determine formula for $Ca^{2+}$ and $IO^{-}$

To balance the + 2 charge of $Ca^{2+}$, we need 2 $IO^{-}$ ions. The empirical formula is $Ca(IO)_{2}$, and the name is calcium hypoiodite.

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

The least - common multiple of 4 and 2 is 4. We need 1 $Pb^{4+}$ ion and 2 $SO_{4}^{2 -}$ ions. The empirical formula is $Pb(SO_{4})_{2}$, and the name is lead(IV) sulfate.

Answer:

cation	anion	empirical formula	name of compound
$K^{+}$	$BrO_{4}^{-}$	$KBrO_{4}$	potassium perbromate
$Ca^{2+}$	$IO^{-}$	$Ca(IO)_{2}$	calcium hypoiodite
$Pb^{4+}$	$SO_{4}^{2 -}$	$Pb(SO_{4})_{2}$	lead(IV) sulfate