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
mn³⁺	s²⁻
pb⁴⁺	o²⁻
pb²⁺	p³⁻
mn²⁺	n³⁻

Explanation:

Step1: Determine formula for $Mn^{3 +}$ and $S^{2 -}$

Cross - multiply the ion charges to get the subscripts. The least common multiple of 3 and 2 is 6. So for $Mn^{3+}$ and $S^{2 -}$, we need 2 $Mn$ atoms and 3 $S$ atoms. The empirical formula is $Mn_2S_3$. The name is manganese(III) sulfide.

Step2: Determine formula for $Pb^{4+}$ and $O^{2 -}$

Cross - multiply the ion charges. The least common multiple of 4 and 2 is 4. So we need 1 $Pb$ atom and 2 $O$ atoms. The empirical formula is $PbO_2$. The name is lead(IV) oxide.

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

The least common multiple of 2 and 3 is 6. We need 3 $Pb$ atoms and 2 $P$ atoms. The empirical formula is $Pb_3P_2$. The name is lead(II) phosphide.

Step4: Determine formula for $Mn^{2+}$ and $N^{3 -}$

The least common multiple of 2 and 3 is 6. We need 3 $Mn$ atoms and 2 $N$ atoms. The empirical formula is $Mn_3N_2$. The name is manganese(II) nitride.

Answer:

cation	anion	empirical formula	name of compound
$Pb^{4+}$	$O^{2 -}$	$PbO_2$	lead(IV) oxide
$Pb^{2+}$	$P^{3 -}$	$Pb_3P_2$	lead(II) phosphide
$Mn^{2+}$	$N^{3 -}$	$Mn_3N_2$	manganese(II) nitride