Chapter 10, Problem 10.120AP

(a)

Interpretation Introduction

To determine: The identification of halogen species that have higher oxidation number from the given pair.

Interpretation: The identification of halogen species that have higher oxidation number from the given pair is to be stated.

Concept introduction: The oxidation number determines the exact charge on element of given substance.

Answer to Problem 10.120AP

Chlorine in $\text{HOCl}$ has higher oxidation number.

Explanation of Solution

The given pair is hypochlorous acid and ${\text{Cl}}^{-}$. The molecular formula hypochlorous acid is $\text{HOCl}$.

The oxidation number of ${\text{Cl}}^{-}$ is $-1$.

Calculate the oxidation number of $\text{Cl}$ in $\text{HOCl}$.

The oxidation number of $\text{Cl}$ in $\text{HOCl}$ is assumed to be $x$. The oxidation number of $\text{H}$ is $+1$. The oxidation number of $\text{O}$ is $-2$. The oxidation number of $\text{Cl}$ in $\text{HOCl}$ is calculated as,

$\begin{array}{c}1\times \left(+1\right)+1\times \left(-2\right)+1\times x=0\\ 1-2+x=0\\ -1+x=0\\ x=+1\end{array}$

Thus, chlorine in $\text{HOCl}$ has higher oxidation number.

(b)

Interpretation Introduction

To determine: The identification of halogen species that have higher oxidation number from the given pair.

Interpretation: The identification of halogen species that have higher oxidation number from the given pair is to be stated.

Concept introduction: The oxidation number determines the exact charge on element of given substance.

Answer to Problem 10.120AP

Chlorine in ${\text{HClO}}_3$ has the higher oxidation number.

Explanation of Solution

The given pair is chlorous acid and ${\text{HClO}}_3$. The molecular formula chlorous acid is ${\text{HClO}}_2$.

Calculate the oxidation number of $\text{Cl}$ in ${\text{HClO}}_2$.

The oxidation number of $\text{Cl}$ in ${\text{HClO}}_2$ is assumed to be $x$. The oxidation number of $\text{H}$ is $+1$. The oxidation number of $\text{O}$ is $-2$. The oxidation number of $\text{Cl}$ in ${\text{HClO}}_2$ is calculated as,

$\begin{array}{c}1\times \left(+1\right)+1\times x+2\times \left(-2\right)=0\\ 1+x-4=0\\ x-3=0\\ x=+3\end{array}$

Calculate the oxidation number of $\text{Cl}$ in ${\text{HClO}}_3$.

The oxidation number of $\text{Cl}$ in ${\text{HClO}}_3$ is assumed to be $x$. The oxidation number of $\text{H}$ is $+1$. The oxidation number of $\text{O}$ is $-2$. The oxidation number of $\text{Cl}$ in ${\text{HClO}}_3$ is calculated as,

$\begin{array}{c}1\times \left(+1\right)+1\times x+3\times \left(-2\right)=0\\ 1+x-6=0\\ x-5=0\\ x=+5\end{array}$

Thus, the chlorine in ${\text{HClO}}_3$ has the higher oxidation number.

(c)

Interpretation Introduction

To determine: The identification of halogen species that have higher oxidation number from the given pair.

Interpretation: The identification of halogen species that have higher oxidation number from the given pair is to be stated.

Concept introduction: The oxidation number determines the exact charge on element of given substance.

Answer to Problem 10.120AP

Chlorine in ${\text{HClO}}_3$ has the higher oxidation number.

Explanation of Solution

The given pair is chloric acid and ${\text{BrO}}_2{}^{-}$. The molecular formula chloric acid is ${\text{HClO}}_3$.

Calculate the oxidation number of $\text{Cl}$ in ${\text{HClO}}_3$.

The oxidation number of $\text{Cl}$ in ${\text{HClO}}_3$ is assumed to be $x$. The oxidation number of $\text{H}$ is $+1$. The oxidation number of $\text{O}$ is $-2$. The oxidation number of $\text{Cl}$ in ${\text{HClO}}_3$ is calculated as,

$\begin{array}{c}1\times \left(+1\right)+1\times x+3\times \left(-2\right)=0\\ 1+x-6=0\\ x-5=0\\ x=+5\end{array}$

Calculate the oxidation number of $\text{Br}$ in ${\text{BrO}}_2{}^{-}$.

The oxidation number of $\text{Br}$ in ${\text{BrO}}_2{}^{-}$ is assumed to be $x$. The oxidation number of $\text{O}$ is $-2$. The oxidation number of $\text{Br}$ in ${\text{BrO}}_2{}^{-}$ is calculated as,

$\begin{array}{c}1\times x+2\times \left(-2\right)=-1\\ x-4=-1\\ x-4=-1\\ x=+3\end{array}$

Thus, chlorine in ${\text{HClO}}_3$ has the higher oxidation number.

(d)

Interpretation Introduction

To determine: The identification of halogen species that have higher oxidation number from the given pair.

Interpretation: The identification of halogen species that have higher oxidation number from the given pair is to be stated.

Concept introduction: The oxidation number determines the exact charge on element of given substance.

Answer to Problem 10.120AP

Chlorine in ${\text{HClO}}_4$ has the higher oxidation number.

Explanation of Solution

The given pair is perchloric acid and ${\text{IO}}^{-}$. The molecular formula perchloric acid is ${\text{HClO}}_4$.

Calculate the oxidation number of $\text{Cl}$ in ${\text{HClO}}_4$.

The oxidation number of $\text{Cl}$ in ${\text{HClO}}_4$ is assumed to be $x$. The oxidation number of $\text{H}$ is $+1$. The oxidation number of $\text{O}$ is $-2$. The oxidation number of $\text{Cl}$ in ${\text{HClO}}_4$ is calculated as,

$\begin{array}{c}1\times \left(+1\right)+1\times x+4\times \left(-2\right)=0\\ 1+x-8=0\\ x-7=0\\ x=+7\end{array}$

Calculate the oxidation number of $\text{I}$ in ${\text{IO}}^{-}$.

The oxidation number of $\text{I}$ in ${\text{IO}}^{-}$ is assumed to be $x$. The oxidation number of $\text{O}$ is $-2$. The oxidation number of $\text{I}$ in ${\text{IO}}^{-}$ is calculated as,

$\begin{array}{c}1\times x+1\times \left(-2\right)=-1\\ x-2=-1\\ x-2=-1\\ x=+1\end{array}$

Thus, chlorine in ${\text{HClO}}_4$ has the higher oxidation number.

Conclusion

1. a. Chlorine in $\text{HOCl}$ has higher oxidation number.
2. b. Chlorine in ${\text{HClO}}_3$ has the higher oxidation number.
3. c. Chlorine in ${\text{HClO}}_3$ has the higher oxidation number.
4. d. Chlorine in ${\text{HClO}}_4$ has the higher oxidation number.