Chapter 3, Problem 56QP

Interpretation Introduction

Interpretation:

The given cations combine with anions to form chemical formulas that are to be analyzed.

Concept Introduction:

An ionic compound consists of a metal cation and non-metal anion. The rules that are used for determining the chemical formulae of ionic compounds are as follows:

First, identify the symbol of the elements in the periodic table.

Identify the charges on the cation and the anion.

After that, the symbol of the cation is written followed by that of the anion.

It is very important that the compound is electrically neutral or the charges of anions and cations are neutralized in the compound.

Explanation of Solution

Given Information: Table is provided in the question.

Sodium cation $\left({\text{Na}}^{+}\right)$ combines with chloride anion $\left({\text{Cl}}^{-}\right)$ to form the chemical formula of $\text{NaCl}$ in which the charges of cation and anion are neutralized to form an electrically neutral compound. Similarly, other anions such as sulfide, nitrate, sulfite, hydroxide, and chlorate are combined with sodium, chromium(II), calcium, ammonium, iron(III), and lead(II) cations to form chemical formulae of ionic compounds as shown in the following table:

$\begin{array}{|cccc|}\hline \text{Ions}& \begin{array}{l}\text{Sodium}\\ {\text{Na}}^{+}\end{array}& \begin{array}{l}\text{Chromium(II)}\\ {\text{Cr}}^{2+}\end{array}& \begin{array}{l}\text{Calcium}\\ {\text{Ca}}^{2+}\end{array}\\ \begin{array}{l}\text{Chloride}\\ \left({\text{Cl}}^{-}\right)\end{array}& \text{NaCl}& {\text{CrCl}}_2& {\text{CaCl}}_2\\ \begin{array}{l}\text{Sulfide}\\ \left({\text{S}}^{2-}\right)\end{array}& {\text{Na}}_2\text{S}& \text{CrS}& \text{CaS}\\ \begin{array}{l}\text{Nitrate}\\ \left({\text{NO}}_3^{-}\right)\end{array}& {\text{NaNO}}_3& \text{Cr}{\left({\text{NO}}_3\right)}_2& \text{Ca}{\left({\text{NO}}_3\right)}_2\\ \begin{array}{l}\text{Sulfite}\\ \left({\text{SO}}_3^{2-}\right)\end{array}& {\text{Na}}_2{\text{SO}}_3& {\text{CrSO}}_3& {\text{CaSO}}_3\\ \begin{array}{l}\text{Hydroxide}\\ \left({\text{OH}}^{-}\right)\end{array}& \text{NaOH}& \text{Cr}{\left(\text{OH}\right)}_2& \text{Ca}{\left(\text{OH}\right)}_2\\ \begin{array}{l}\text{Chlorate}\\ \left({\text{ClO}}_3^{-}\right)\end{array}& {\text{NaClO}}_3& {\text{Cr(ClO}}_3{\text{)}}_2& {\text{Ca(ClO}}_3{\text{)}}_2\\ \hline\end{array}$

$\begin{array}{|cccc|}\hline \text{Ions}& \begin{array}{l}\text{Ammonium}\\ {\text{NH}}_4^{+}\end{array}& \begin{array}{l}\text{Iron(III)}\\ {\text{Fe}}^{3+}\end{array}& \begin{array}{l}\text{Lead(II)}\\ {\text{Pb}}^{2+}\end{array}\\ \begin{array}{l}\text{Chloride}\\ \left({\text{Cl}}^{-}\right)\end{array}& {\text{NH}}_4\text{Cl}& {\text{FeCl}}_3& {\text{PbCl}}_2\\ \begin{array}{l}\text{Sulfide}\\ \left({\text{S}}^{2-}\right)\end{array}& {\left({\text{NH}}_4\right)}_2\text{S}& {\text{Fe}}_2{\text{S}}_3& \text{PbS}\\ \begin{array}{l}\text{Nitrate}\\ \left({\text{NO}}_3^{-}\right)\end{array}& {\text{NH}}_4{\text{NO}}_3& \text{Fe}{\left({\text{NO}}_3\right)}_3& \text{Pb}{\left({\text{NO}}_3\right)}_2\\ \begin{array}{l}\text{Sulfite}\\ \left({\text{SO}}_3^{2-}\right)\end{array}& {\left({\text{NH}}_4\right)}_2{\text{SO}}_3& {\text{Fe}}_2{\left({\text{SO}}_3\right)}_3& {\text{PbSO}}_3\\ \begin{array}{l}\text{Hydroxide}\\ \left({\text{OH}}^{-}\right)\end{array}& {\text{NH}}_4\text{OH}& \text{Fe}{\left(\text{OH}\right)}_3& \text{Pb}{\left(\text{OH}\right)}_2\\ \begin{array}{l}\text{Chlorate}\\ \left({\text{ClO}}_3^{-}\right)\end{array}& {\text{NH}}_4{\text{ClO}}_3& {\text{Fe(ClO}}_3{\text{)}}_3& {\text{Pb(ClO}}_3{\text{)}}_2\\ \hline\end{array}$

Conclusion

Sodium, chromium (II), calcium, ammonium, iron (III), and lead (II) cations are combined with

sulfide, nitrate, sulfite, hydroxide, and chlorate anions to form the chemical formula of ionic compounds that are shown in the table.