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
$pb^{4 + }$	$oh^{-}$
$mg^{2+}$	$po_{4}^{3 - }$

Explanation:

Step1: Determine formula for $Na^+$ and $NO_3^-$

Charge - balance to get $NaNO_3$.

Step2: Name the compound for $Na^+$ and $NO_3^-$

Sodium is the cation and nitrate is the anion, so it's sodium nitrate.

Step3: Determine formula for $Pb^{4 +}$ and $OH^-$

To balance charges ($+4$ from lead and $- 1$ from hydroxide), we need 4 $OH^-$ ions, so the formula is $Pb(OH)_4$.

Step4: Name the compound for $Pb^{4 +}$ and $OH^-$

Lead(IV) is the cation and hydroxide is the anion, so it's lead(IV) hydroxide.

Step5: Determine formula for $Mg^{2+}$ and $PO_4^{3 -}$

To balance charges ($+2$ from magnesium and $-3$ from phosphate), we need 3 magnesium ions and 2 phosphate ions, so the formula is $Mg_3(PO_4)_2$.

Step6: Name the compound for $Mg^{2+}$ and $PO_4^{3 -}$

Magnesium is the cation and phosphate is the anion, so it's magnesium phosphate.

Answer:

cation	anion	empirical formula	name of compound
$Pb^{4+}$	$OH^-$	$Pb(OH)_4$	lead(IV) hydroxide
$Mg^{2+}$	$PO_4^{3 -}$	$Mg_3(PO_4)_2$	magnesium phosphate