Chapter 4, Problem 4.109EP

(a)

Interpretation Introduction

Interpretation:

The following table of chemical formulas for polyatomic ion containing ionic compounds is to be filled.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{Al}}^{\text{3+}}& & & & \end{array}$

Concept Introduction:

Chemical formulas and names for ionic compounds containing polyatomic ions:

Ionic compounds containing positive and negative charges present must add to zero.

If more than one polyatomic ion is present in a compound, the chemical formula can be written as a polyatomic ion is enclosed in parentheses and a subscript, placed outside of the parentheses.  Example- ${\text{Fe(OH)}}_{\text{3}}$.

Sometimes same element is present at two different locations.  For example, ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$- in this chemical formula “N” is present in two different locations as ${\text{NH}}_{\text{4}}^{\text{+}}{\text{ and NO}}_{\text{3}}^{\text{-}}$ ions.

Answer to Problem 4.109EP

The complete table as shown below.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{Al}}^{\text{3+}}& {\text{Al(CN)}}_{\text{3}}& {\text{Al(NO}}_{\text{3}}{\text{)}}_{\text{3}}& {\text{Al(HCO}}_{\text{3}}{\text{)}}_{\text{3}}& {\text{Al}}_{\text{2}}{{\text{(SO}}_{\text{4}}\text{)}}_{\text{3}}\end{array}$

Explanation of Solution

The given two ions are ${\text{Al}}^{\text{3+}}$ and ${\text{CN}}^{\text{-}}$.

Three cyanide ions (1- charge) are required to balance the charge on one aluminium ion (3+ charge).  Hence, the chemical formula of the compound is ${\text{Al(CN)}}_{\text{3}}$.

The given two ions are ${\text{Al}}^{\text{3+}}$ and ${\text{NO}}_{\text{3}}^{\text{-}}$.

Three nitrate ions (1- charge) are required to balance the charge on one aluminium ion (3+ charge).   Hence, the chemical formula of the compound is ${\text{Al(NO}}_{\text{3}}{\text{)}}_{\text{3}}$

.

The given two ions are ${\text{Al}}^{\text{3+}}$ and ${\text{HCO}}_{\text{3}}^{\text{-}}$.

Three ${\text{HCO}}_{\text{3}}^{\text{-}}$ ions (1- charge) are required to balance the charge on one aluminium ion (3+ charge).  Hence, the chemical formula of the compound is ${\text{Al(HCO}}_{\text{3}}{\text{)}}_{\text{3}}$

The given two ions are ${\text{Al}}^{\text{3+}}$ and ${\text{SO}}_{\text{4}}^{\text{2-}}$.

Three sulfate ions (2- charge) are required to balance the charge on two aluminium ions (3+ charge).  Hence, the chemical formula of the compound is ${\text{Al}}_{\text{2}}{{\text{(SO}}_{\text{4}}\text{)}}_{\text{3}}$

(b)

Interpretation Introduction

Interpretation:

The following table of chemical formulas for polyatomic ion containing ionic compounds is to be filled.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{Ag}}^{+}& & & & \end{array}$

Concept Introduction:

Chemical formulas and names for ionic compounds containing polyatomic ions:

Ionic compounds containing positive and negative charges present must add to zero.

If more than one polyatomic ion is present in a compound, the chemical formula can be written as a polyatomic ion is enclosed in parentheses and a subscript, placed outside of the parentheses.  Example- ${\text{Fe(OH)}}_{\text{3}}$.

Sometimes same element is present at two different locations.  For example, ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$- in this chemical formula “N” is present in two different locations as ${\text{NH}}_{\text{4}}^{\text{+}}{\text{ and NO}}_{\text{3}}^{\text{-}}$ ions.

Answer to Problem 4.109EP

The complete table as shown below.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{Ag}}^{\text{+}}& \text{AgCN}& {\text{AgNO}}_{\text{3}}& {\text{AgHCO}}_{\text{3}}& {\text{Ag}}_{\text{2}}{\text{SO}}_{\text{4}}\end{array}$

Explanation of Solution

The given two ions are ${\text{Ag}}^{\text{+}}$ and ${\text{CN}}^{\text{-}}$.

One cyanide ion (1- charge) is required to balance the charge on one silver ion (1+ charge).  Hence, the chemical formula of the compound is $\text{AgCN}$.

The given two ions are ${\text{Ag}}^{\text{+}}$ and ${\text{NO}}_{\text{3}}^{\text{-}}$.

One nitrate ion (1- charge) is required to balance the charge on one silver ion (1+ charge).  Hence, the chemical formula of the compound is ${\text{AgNO}}_{\text{3}}$.

The given two ions are ${\text{Ag}}^{\text{+}}$ and ${\text{HCO}}_{\text{3}}^{\text{-}}$.

One bicarbonate ion (1- charge) is required to balance the charge on one silver ion (1+ charge).  Hence, the chemical formula of the compound is ${\text{AgHCO}}_{\text{3}}$.

The given two ions are ${\text{Ag}}^{\text{+}}$ and ${\text{SO}}_{\text{4}}^{\text{2-}}$.

One sulphate ion (2- charge) is required to balance the charge on two silver ions (1+ charge).  Hence, the chemical formula of the compound is ${\text{Ag}}_{\text{2}}{\text{SO}}_{\text{4}}$.

(c)

Interpretation Introduction

Interpretation:

The following table of chemical formulas for polyatomic ion containing ionic compounds is to be filled.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{Ca}}^{\text{2+}}& & & & \end{array}$

Concept Introduction:

Chemical formulas and names for ionic compounds containing polyatomic ions:

Ionic compounds containing positive and negative charges present must add to zero.

If more than one polyatomic ion is present in a compound, the chemical formula can be written as a polyatomic ion is enclosed in parentheses and a subscript, placed outside of the parentheses.  Example- ${\text{Fe(OH)}}_{\text{3}}$.

Sometimes same element is present at two different locations.  For example, ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$- in this chemical formula “N” is present in two different locations as ${\text{NH}}_{\text{4}}^{\text{+}}{\text{ and NO}}_{\text{3}}^{\text{-}}$ ions.

Answer to Problem 4.109EP

The complete table as shown below.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{Ca}}^{\text{2+}}& {\text{Ca(CN)}}_{\text{2}}& {\text{Ca(NO}}_{\text{3}}{\text{)}}_{\text{2}}& {\text{Ca(HCO}}_{\text{3}}{\text{)}}_{\text{2}}& {\text{CaSO}}_{\text{4}}\end{array}$

Explanation of Solution

The given two ions are ${\text{Ca}}^{\text{2+}}$ and ${\text{CN}}^{\text{-}}$.

Two cyanide ions (1- charge) are required to balance the charge on one calcium ion (2+ charge).  Hence, the chemical formula of the compound is ${\text{Ca(CN)}}_{\text{2}}$.

The given two ions are ${\text{Ca}}^{\text{2+}}$ and ${\text{NO}}_{\text{3}}^{\text{-}}$.

Two nitrate ions (1- charge) are required to balance the charge on one calcium ion (2+ charge).  Hence, the chemical formula of the compound is ${\text{Ca(NO}}_{\text{3}}{\text{)}}_{\text{2}}$.

The given two ions are ${\text{Ca}}^{\text{2+}}$ and ${\text{HCO}}_{\text{3}}^{\text{-}}$.

Two carbonate ions (1- charge) are required to balance the charge on one calcium ion (2+ charge).  Hence, the chemical formula of the compound is ${\text{Ca(HCO}}_{\text{3}}{\text{)}}_{\text{2}}$.

The given two ions are ${\text{Ca}}^{\text{2+}}$ and ${\text{SO}}_{\text{4}}^{\text{2-}}$.

One sulphate ion (2- charge) are required to balance the charge on one calcium ion (2+ charge).

Hence, the chemical formula of the compound is ${\text{CaSO}}_{\text{4}}$.

(d)

Interpretation Introduction

Interpretation:

The following table of chemical formulas for polyatomic ion containing ionic compounds is to be filled.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{NH}}_{\text{4}}^{\text{+}}& & & & \end{array}$

Concept Introduction:

Chemical formulas and names for ionic compounds containing polyatomic ions:

Ionic compounds containing positive and negative charges present must add to zero.

If more than one polyatomic ion is present in a compound, the chemical formula can be written as a polyatomic ion is enclosed in parentheses and a subscript, placed outside of the parentheses.  Example- ${\text{Fe(OH)}}_{\text{3}}$.

Sometimes same element is present at two different locations.  For example, ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$- in this chemical formula “N” is present in two different locations as ${\text{NH}}_{\text{4}}^{\text{+}}{\text{ and NO}}_{\text{3}}^{\text{-}}$ ions.

Answer to Problem 4.109EP

The complete table as shown below.

  $\begin{array}{ccccc}& {\text{CN}}^{\text{-}}& {\text{NO}}_{\text{3}}^{\text{-}}& {\text{HCO}}_{\text{3}}^{\text{-}}& {\text{SO}}_{\text{4}}^{\text{2-}}\\ {\text{NH}}_{\text{4}}^{\text{+}}& {\text{NH}}_{\text{4}}\text{CN}& {\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}& {\text{NH}}_{\text{4}}{\text{HCO}}_{\text{3}}& {{\text{(NH}}_{\text{4}}\text{)}}_{\text{2}}{\text{SO}}_{\text{4}}\end{array}$

Explanation of Solution

The given two ions are ${\text{NH}}_{\text{4}}^{\text{+}}$ and ${\text{CN}}^{\text{-}}$.

One cyanide ion (1- charge) is required to balance the charge on one ammonium ion (1+ charge).  Hence, the chemical formula of the compound is ${\text{NH}}_{\text{4}}\text{CN}$.

The given two ions are ${\text{NH}}_{\text{4}}^{\text{+}}$ and ${\text{NO}}_{\text{3}}^{\text{-}}$.

One nitrate ion (1- charge) is required to balance the charge on one ammonium ion (1+ charge).  Hence, the chemical formula of the compound is ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$.

The given two ions are ${\text{NH}}_{\text{4}}^{\text{+}}$ and ${\text{HCO}}_{\text{3}}^{\text{-}}$.

One bicarbonate ion (1- charge) is required to balance the charge on one ammonium ion (1+ charge).  Hence, the chemical formula of the compound is ${\text{NH}}_{\text{4}}{\text{HCO}}_{\text{3}}$.

The given two ions are ${\text{NH}}_{\text{4}}^{\text{+}}$ and ${\text{SO}}_{\text{4}}^{\text{2-}}$.

One sulfate ion (2- charge) is required to balance the charge on two ammonium ions (1+ charge).  Hence, the chemical formula of the compound is ${{\text{(NH}}_{\text{4}}\text{)}}_{\text{2}}{\text{SO}}_{\text{4}}$.