Chapter 3, Problem 55QP

Complete the following table by writing formulas for the compounds formed when the cations listed across the top combine with the anions listed along the side.

Interpretation Introduction

Interpretation:

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

Concept Introduction:

An ionic compound consists of metal cation and a non-metal anion. The rules that are used for determining the chemical formula 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.

Potassium cation $\left({\text{K}}^{+}\right)$ combines with iodide anion $\left({\text{I}}^{-}\right)$ to form the chemical formula of $\text{KI}$ in which the charges of cation and anion are neutralized to form electrically neutral compound. Similarly, other anions such as oxide, sulfate, nitrite, acetate, and hypochlorite are combined with potassium, iron(III), strontium, aluminium, cobalt(II), and lead(IV) cations to form chemical formula of an ionic compound as shown in the following table:

$\begin{array}{cccc}\text{Ions}& \begin{array}{l}\text{Potassium}\\ {\text{K}}^{+}\end{array}& \begin{array}{l}\text{Iron(III)}\\ {\text{Fe}}^{3+}\end{array}& \begin{array}{l}\text{Strontium}\\ {\text{Sr}}^{2+}\end{array}\\ \begin{array}{l}\text{Iodide}\\ \left({\text{I}}^{-}\right)\end{array}& \text{KI}& {\text{FeI}}_3& {\text{SrI}}_2\\ \begin{array}{l}\text{Oxide}\\ \left({\text{O}}^{2-}\right)\end{array}& {\text{K}}_2\text{O}& {\text{Fe}}_2{\text{O}}_3& \text{SrO}\\ \begin{array}{l}\text{Sulfate}\\ \left({\text{SO}}_4^{2-}\right)\end{array}& {\text{K}}_2{\text{SO}}_4& {\text{Fe}}_2{\left({\text{SO}}_4\right)}_3& {\text{SrSO}}_4\\ \begin{array}{l}\text{Nitrite}\\ \left({\text{NO}}_2^{-}\right)\end{array}& {\text{KNO}}_2& \text{Fe}{\left({\text{NO}}_2\right)}_3& \text{Sr}{\left({\text{NO}}_2\right)}_2\\ \begin{array}{l}\text{Acetate}\\ \left({\text{CH}}_3{\text{CO}}_2^{-}\right)\end{array}& {\text{KCH}}_3{\text{CO}}_2& \text{Fe}{\left({\text{CH}}_3{\text{CO}}_2\right)}_3& \text{Sr}{\left({\text{CH}}_3{\text{CO}}_2\right)}_3\\ \begin{array}{l}\text{Hypochlorite}\\ \left({\text{ClO}}^{-}\right)\end{array}& \text{KClO}& {\text{Fe(ClO)}}_3& \text{Sr}{\left(\text{ClO}\right)}_2\end{array}$

$\begin{array}{cccc}\text{Ions}& \begin{array}{l}\text{Aluminium}\\ {\text{Al}}^{3+}\end{array}& \begin{array}{l}\text{Cobalt(II)}\\ {\text{Co}}^{2+}\end{array}& \begin{array}{l}\text{Lead}\\ {\text{Pb}}^{4+}\end{array}\\ \begin{array}{l}\text{Iodide}\\ \left({\text{I}}^{-}\right)\end{array}& {\text{AlI}}_3& {\text{CoI}}_2& {\text{PbI}}_4\\ \begin{array}{l}\text{Oxide}\\ \left({\text{O}}^{2-}\right)\end{array}& {\text{Al}}_2{\text{O}}_3& \text{CoO}& {\text{PbO}}_2\\ \begin{array}{l}\text{Sulfate}\\ \left({\text{SO}}_4^{2-}\right)\end{array}& {\text{Al}}_2{\left({\text{SO}}_4\right)}_3& {\text{CoSO}}_4& \text{Pb}{\left({\text{SO}}_4\right)}_2\\ \begin{array}{l}\text{Nitrite}\\ \left({\text{NO}}_2^{-}\right)\end{array}& \text{Al}{\left({\text{NO}}_2\right)}_3& \text{Co}{\left({\text{NO}}_2\right)}_2& \text{Pb}{\left({\text{NO}}_2\right)}_4\\ \begin{array}{l}\text{Acetate}\\ \left({\text{CH}}_3{\text{CO}}_2^{-}\right)\end{array}& \text{Al}{\left({\text{CH}}_3{\text{CO}}_2\right)}_3& \text{Co}{\left({\text{CH}}_3{\text{CO}}_2\right)}_2& \text{Pb}{\left({\text{CH}}_3{\text{CO}}_2\right)}_4\\ \begin{array}{l}\text{Hypochlorite}\\ \left({\text{ClO}}^{-}\right)\end{array}& \text{Al}{\left(\text{ClO}\right)}_3& {\text{Co(ClO)}}_2& \text{Pb}{\left(\text{ClO}\right)}_4\end{array}$

Conclusion

The potassium, iron(III), strontium, aluminum, cobalt(II), and lead(IV) cations are combined with iodide, oxide, sulfate, nitrite, acetate, and hypochlorite anions to form chemical formulae of ionic compounds that are shown in the above table.