Question

we know that ionic compounds have an overall neutral charge. we can also use the periodic table to predict the types of ions different elements will form. which of the following are not neutral ionic compounds? mg₂cl kbr nal pcl₂ srcl

Explanation:

Step1: Determine the charge of ions

• Magnesium (\(Mg\)) forms \(Mg^{2 +}\) ion, chlorine (\(Cl\)) forms \(Cl^{-}\) ion. For \(Mg_2Cl\), total positive charge \(=2\times(+ 2)=+4\), total negative charge \(=-1\). Net charge \(=+4+( - 1)=+3

eq0\).

• Potassium (\(K\)) forms \(K^{+}\) ion, bromine (\(Br\)) forms \(Br^{-}\) ion. For \(KBr\), total positive charge \(=+1\), total negative charge \(=-1\). Net charge \(=+1+( - 1)=0\).
• Sodium (\(Na\)) forms \(Na^{+}\) ion, iodine (\(I\)) forms \(I^{-}\) ion. For \(NaI\), total positive charge \(=+1\), total negative charge \(=-1\). Net charge \(=+1+( - 1)=0\).
• Phosphorus (\(P\)) and chlorine (\(Cl\)) form covalent compound \(PCl_2\) (not ionic as \(P\) does not form simple cation in this case, ionic compounds are formed by transfer of electrons from metal to non - metal. \(P\) is not a metal here in the context of simple ionic compound formation).
• Strontium (\(Sr\)) forms \(Sr^{2+}\) ion, chlorine (\(Cl\)) forms \(Cl^{-}\) ion. For \(SrCl\), total positive charge \(=+2\), total negative charge \(=-1\). Net charge \(=+2+( - 1)=+1

eq0\).

Answer:

\(\text{Mg}_2\text{Cl}\), \(\text{PCl}_2\), \(\text{SrCl}\)