Question

select all the element(s) from the periodic table shown that will form an ionic compound with a metal m and a nonmetal x and a formula unit of $m_3x_2$.

Explanation:

Step1: Determine the charge of metal M

In an ionic compound \(M_3X_2\), let the charge of metal \(M\) be \(+x\) and the charge of non - metal \(X\) be \( - y\). Using the rule of charge neutrality in ionic compounds (\(3x+2(-y)=0\)). For a simple ionic compound formed by a metal and a non - metal, common metal charges:
Group 1A metals have a charge of \(+1\), Group 2A metals have a charge of \(+2\), Group 3A metals (excluding \(B\)) have a charge of \(+3\).
If \(x = + 2\) (Group 2A metal, since \(3\times(+2)+2(-y)=0\) gives \(y = + 3\)).

Step2: Determine the charge of non - metal X

Non - metals in Group 5A (N, P etc.) can gain 3 electrons to form ions with a charge of \(-3\).

Answer:

\(N\) (Nitrogen) and \(P\) (Phosphorus)