Chapter 3, Problem 54QP

Interpretation Introduction

Interpretation:

The name of the compound from the given cation and anion is to be determined.

Concept Introduction:

An ionic compound consists of metal cation and a non-metal anion. The rules that are used for naming an ionic compound are as follows:

Based on the position of the element in the periodic table, identify the nature of the element as metal or non-metal.

Identify the symbol of element in the periodic table.

Then, write the first name of the element which is a cation followed by that of anion with the use of suffix.

The rules that are used for determining the chemical formulae of ionic compounds are as follow:

First, identify the symbol of an element in the periodic table.

Identify the charge on the cation and anion.

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

${\text{Ba}}^{2+}$ cation combines with ${\text{Br}}^{-}$ to form ${\text{BaBr}}_3$ ionic compound. Similarly, other ions such as $\text{S}$ ion combines with ${\text{Ba}}^{2+}$ ion to form $\text{BaS}$ , ${\text{NO}}_2^{-}$ ion combines with ${\text{Ba}}^{2+}$ ion to form $\text{Ba}{\left({\text{NO}}_2\right)}_2$ , ${\text{SO}}_4^{2-}$ ion combines with ${\text{Ba}}^{2+}$ ion to form ${\text{BaSO}}_4$ , ${\text{HCO}}_3^{-}$ ion combines with ${\text{Ba}}^{2+}$ ion to form $\text{Ba}{\left({\text{HCO}}_3\right)}_2,$ and ${\text{ClO}}_4^{-}$ ion combines with ${\text{Ba}}^{2+}$ ion to form $\text{Ba}{\left({\text{ClO}}_4\right)}_2$ .

The other cations ${\text{Fe}}^{3+}$ , ${\text{Na}}^{+}$ , ${\text{Ni}}^{2+}$ , ${\text{Cr}}^{3+}$ , and ${\text{Ag}}^{+}$ are combined with ${\text{Br}}^{-}$ , $\text{S}$ , ${\text{NO}}_2^{-}$ , ${\text{SO}}_4^{2-}$ , ${\text{HCO}}_3^{-},$ and ${\text{ClO}}_4^{-}$ anions to form the chemical formulae of ionic compounds shown below in the following table:

$\begin{array}{cccc}\text{Ions}& \begin{array}{l}{\text{Ba}}^{2+}\\ \text{Barium}\end{array}& \begin{array}{l}{\text{Fe}}^{3+}\\ \text{Iron(III)}\end{array}& \begin{array}{l}{\text{Na}}^{+}\\ \text{Sodium}\end{array}\\ \begin{array}{l}{\text{Br}}^{-}\\ \text{(Bromide)}\end{array}& \begin{array}{l}{\text{BaBr}}_2\\ \text{Barium }\\ \text{bromide}\end{array}& \begin{array}{l}{\text{FeBa}}_3\\ \text{Iron(III)}\\ \text{bromide}\end{array}& \begin{array}{l}\text{NaBr}\\ \text{Sodium }\\ \text{bromide}\end{array}\\ \begin{array}{l}{\text{S}}^{2-}\\ \text{(Sulfide)}\end{array}& \begin{array}{l}\text{BaS}\\ \text{Barium }\\ \text{sulfide}\end{array}& \begin{array}{l}{\text{Fe}}_2{\text{S}}_3\\ \text{Iron(III)}\\ \text{sulfide}\end{array}& \begin{array}{l}{\text{Na}}_{\text{2}}\text{S}\\ \text{Sodium}\\ \text{sulfide}\end{array}\\ \begin{array}{l}{\text{NO}}_2^{-}\\ \text{(Nitrite)}\end{array}& \begin{array}{l}\text{Ba}{\left({\text{NO}}_2\right)}_2\\ \text{Barium }\\ \text{nitrite}\end{array}& \begin{array}{l}\text{Fe}{\left({\text{NO}}_2\right)}_3\\ \text{Iron(III)}\\ \text{nitrite}\end{array}& \begin{array}{l}{\text{NaNO}}_3\\ \text{Sodium }\\ \text{nitrite}\end{array}\\ \begin{array}{l}{\text{SO}}_4^{2-}\\ \text{(Sulfate)}\end{array}& \begin{array}{l}{\text{BaSO}}_4\\ \text{Barium }\\ \text{sulfate}\end{array}& \begin{array}{l}{\text{Fe}}_2{\left({\text{SO}}_4\right)}_3\\ \text{Iron(III)}\\ \text{sulfate}\end{array}& \begin{array}{l}{\text{Na}}_2{\text{SO}}_4\\ \text{Sodium }\\ \text{sulfate}\end{array}\\ \begin{array}{l}{\text{HCO}}_3^{-}\\ \text{(bicarbonate)}\end{array}& \begin{array}{l}\text{Ba}{\left({\text{HCO}}_3\right)}_2\\ \text{Barium }\\ \text{bicarbonate}\end{array}& \begin{array}{l}\text{Fe}{\left({\text{HCO}}_3\right)}_3\\ \text{Iron(III)}\\ \text{bicarbonate}\end{array}& \begin{array}{l}{\text{NaHCO}}_3\\ \text{Sodium}\\ \text{bicarbonate}\end{array}\\ \begin{array}{l}{\text{ClO}}_4^{-}\\ \text{(Perchlorate)}\end{array}& \begin{array}{l}{\text{Ba(ClO}}_4{\text{)}}_{\text{2}}\\ \text{Calcium}\\ \text{perchlorate}\end{array}& \begin{array}{l}{\text{Fe(ClO}}_4{\text{)}}_3\\ \text{Iron(III)}\\ \text{perchlorate}\end{array}& \begin{array}{l}{\text{NaClO}}_4\\ \text{Sodium}\\ \text{perchlorate}\end{array}\end{array}$

$\begin{array}{cccc}\text{Ions}& \begin{array}{l}{\text{Ni}}^{2+}\\ \text{Nickel}(\text{II})\end{array}& \begin{array}{l}{\text{Cr}}^{3+}\\ \text{Chromium(III)}\end{array}& \begin{array}{l}{\text{Ag}}^{+}\\ \text{Silver}\end{array}\\ \begin{array}{l}{\text{Br}}^{-}\\ \text{(Bromide)}\end{array}& \begin{array}{l}{\text{NiBr}}_2\\ \text{Nickel(II) }\\ \text{bromide}\end{array}& \begin{array}{l}{\text{CrBr}}_3\\ \text{Chromium(III)}\\ \text{bromide}\end{array}& \begin{array}{l}\text{AgBr}\\ \text{Silver }\\ \text{bromide}\end{array}\\ \begin{array}{l}{\text{S}}^{2-}\\ \text{(Sulfide)}\end{array}& \begin{array}{l}\text{NiS}\\ \text{Nickel(II) }\\ \text{sulfide}\end{array}& \begin{array}{l}{\text{Cr}}_2{\text{S}}_3\\ \text{Chromium(III)}\\ \text{sulfide}\end{array}& \begin{array}{l}{\text{Ag}}_{\text{2}}\text{S}\\ \text{Silver}\\ \text{sulfide}\end{array}\\ \begin{array}{l}{\text{NO}}_2^{-}\\ \text{(Nitrite)}\end{array}& \begin{array}{l}\text{Ni}{\left({\text{NO}}_2\right)}_2\\ \text{Nickel(II)}\\ \text{nitrite}\end{array}& \begin{array}{l}\text{Cr}{\left({\text{NO}}_2\right)}_3\\ \text{Chromium(III)}\\ \text{nitrite}\end{array}& \begin{array}{l}{\text{AgNO}}_2\\ \text{Silver }\\ \text{nitrite}\end{array}\\ \begin{array}{l}{\text{SO}}_4^{2-}\\ \text{(Sulfate)}\end{array}& \begin{array}{l}{\text{NiSO}}_4\\ \text{Nickel(II) }\\ \text{sulfate}\end{array}& \begin{array}{l}{\text{Cr}}_2{\left({\text{SO}}_4\right)}_3\\ \text{Chromium(III)}\\ \text{sulfate}\end{array}& \begin{array}{l}{\text{Ag}}_2{\text{SO}}_4\\ \text{Silver }\\ \text{sulfate}\end{array}\\ \begin{array}{l}{\text{HCO}}_3^{-}\\ \text{(bicarbonate)}\end{array}& \begin{array}{l}\text{Ni}{\left({\text{HCO}}_3\right)}_2\\ \text{Nickel(II) }\\ \text{bicarbonate}\end{array}& \begin{array}{l}\text{Cr}{\left({\text{HCO}}_3\right)}_3\\ \text{Chromium(III)}\\ \text{bicarbonate}\end{array}& \begin{array}{l}{\text{AgHCO}}_3\\ \text{Silver}\\ \text{bicarbonate}\end{array}\\ \begin{array}{l}{\text{ClO}}_4^{-}\\ \text{(Perchlorate)}\end{array}& \begin{array}{l}{\text{Ni(ClO}}_4{\text{)}}_{\text{2}}\\ \text{Nickel(II)}\\ \text{perchlorate}\end{array}& \begin{array}{l}{\text{Cr(ClO}}_4{\text{)}}_3\\ \text{Chromium(III)}\\ \text{perchlorate}\end{array}& \begin{array}{l}{\text{NaClO}}_4\\ \text{Silver}\\ \text{perchlorate}\end{array}\end{array}$

Conclusion

${\text{Ba}}^{2+}$ , ${\text{Fe}}^{3+}$ , ${\text{Na}}^{+}$ , ${\text{Ni}}^{2+}$ , ${\text{Cr}}^{3+}$ , ${\text{Ag}}^{+}$ cations are combined with ${\text{Br}}^{-}$ , $\text{S}$ , ${\text{NO}}_2^{-}$ , ${\text{SO}}_4^{2-}$ , ${\text{HCO}}_3^{-}$ and ${\text{ClO}}_4^{-}$ anions to form chemical formula of ionic compounds shown in the above table.