Chapter 4, Problem 4.43QP

(a)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

Te oxidation number of $\text{Cl}$ in$\text{ClF}$

• According to the rules, the Inter halogen compounds the Fluorine is always having $-1$ oxidation state and the sum of oxidation numbers of all the atoms present in the molecule is zero.
• The $\text{F}$ in $-1$ oxidation state and $\text{Cl}$ is in $+1$ state.

(b)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{I}$ in $\text{IF}$

• According to the rules, the Inter halogen compounds the Fluorine is always having $-1$ oxidation state and the sum of oxidation numbers of all the atoms present in the molecule is zero.
• The $\text{F}$ in $-1$ oxidation state and $\text{I}$ is,

  $\begin{array}{l}\text{7(-1)+1(X)=0}\\ \text{-7+(X)=0}\\ \text{X=+7}\end{array}$

• The oxidation number of $\text{I}$ in $\text{IF}$ is $+7$

(c)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{C}$ in ${\text{CH}}_{\text{4}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation state of hydrogen is $+1$.
• The $\text{H}$ in $+1$ oxidation state and C is,

  $\begin{array}{l}\text{4(1+)+1(X)=0}\\ \text{(4+)+(X)=0}\\ \text{X=-4}\\ \text{C=-4}\end{array}$

• The oxidation number of $\text{C}$ in ${\text{CH}}_{\text{4}}$ is $-4$.

(d)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{C}$ in ${\text{C}}_{\text{2}}{\text{H}}_{\text{2}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation state of Hydrogen is $+1$.
• The $\text{H}$ in $+1$ oxidation state and C is,

  $\begin{array}{l}\text{2(1+)+2(X)=0}\\ \text{(2+)+2(X)=0}\\ \text{2X=-2}\\ \text{C=-1}\end{array}$

• The oxidation number of $\text{C}$ in ${\text{C}}_{\text{2}}{\text{H}}_{\text{2}}$ is $-1$

(e)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{C}$ in ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation state of Hydrogen is $+1$.
• The $\text{H}$ in $+1$ oxidation state and C is,

$\begin{array}{l}\text{4(1+)+2(X)=0}\\ \text{(4+)+2(X)=0}\\ \text{2X=-4}\\ \text{C=-2}\end{array}$

• The oxidation number of $\text{C}$ in ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}$ is $-2$

(f)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

To give the oxidation number of $\text{Cr}$ in ${\text{K}}_{\text{2}}{\text{CrO}}_{\text{4}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation state of Oxygen is $-2$.
• The $\text{O}$ is in $-2$ and $\text{K}$ is in $\text{+1}$ oxidation state and $\text{Cr}$ is,

  $\begin{array}{l}\text{2(1+)+1(X)+4(-2)=0}\\ \text{(2+)+1(X)+(-8)=0}\\ \text{X=+6}\\ \text{Cr=+6}\end{array}$

• The oxidation number of $\text{Cr}$ in ${\text{K}}_{\text{2}}{\text{CrO}}_{\text{4}}$ is $+6$.

(g)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{Cr}$ in ${\text{K}}_{\text{2}}{\text{Cr}}_{\text{2}}{\text{O}}_{\text{7}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation state of Oxygen is $-2$.
• The $\text{O}$ is in $-2$ and $\text{K}$ is in $\text{+1}$ oxidation states and $\text{Cr}$ is,

  $\begin{array}{l}\text{2(1+)+2(X)+7(-2)=0}\\ \text{(2+)+2(X)+(-14)=0}\\ \text{2X=+12}\\ \text{X=+6}\\ \text{Cr=+6}\end{array}$

• The oxidation number of $\text{Cr}$ in ${\text{K}}_{\text{2}}{\text{Cr}}_{\text{2}}{\text{O}}_{\text{7}}$ is $+6$

(h)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{Mn}$ in ${\text{KMnO}}_{\text{4}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation state of Oxygen is $-2$.
• The $\text{O}$ is in $-2$ and $\text{K}$ is in $\text{+1}$ oxidation states and $\text{Mn}$ is,

  $\begin{array}{l}\text{(1+)+1(X)+4(-2)=0}\\ \text{(1+)+1(X)+(-8)=0}\\ \text{X=+7}\\ \text{Mn=+7}\end{array}$

• The oxidation number of $\text{Mn}$ in ${\text{KMnO}}_{\text{4}}$ is $+7$

(i)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{C}$ in ${\text{NaHCO}}_{\text{3}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation state of Hydrogen is $+1$.
• The earth metals always having $+1$ oxidation number only.
• The $\text{O}$ is in $-2$ and $\text{Na}$ is in $\text{+1}$ oxidation states and $\text{C}$ is,

  $\begin{array}{l}\text{(1+)+(1+)1(X)+3(-2)=0}\\ \text{(1+)+(1+)+1(X)+(-6)=0}\\ \text{X=-4}\\ \text{C=-4}\end{array}$

• The oxidation number of $\text{C}$ in ${\text{NaHCO}}_{\text{3}}$ is $+4$

(j)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{Li}$ in ${\text{Li}}_{\text{2}}$

• Acceding to the rule, the oxidation number of atom in the elemental form is zero so ${\text{Li}}_{\text{2}}$ is in elemental form so the oxidation number is zero.
• The oxidation number of $\text{Li}$ in ${\text{Li}}_{\text{2}}$ is $0$

(k)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

To give the oxidation number of $\text{I}$ in ${\text{NaIO}}_{\text{3}}$is $+5$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and in the oxohalide compounds oxidation number of halide is in positive.
• The earth metals always having $+1$ oxidation number only.
• The $\text{O}$ is in $-2$ and $\text{Na}$ is in $\text{+1}$ oxidation states and $\text{I}$ is,

  $\begin{array}{l}\text{1(1+)+X+3(-2)=0}\\ \text{(1+)+X+(-6)=0}\\ \text{X=+5}\\ \text{I=+5}\end{array}$

• The oxidation number of $\text{I}$ in ${\text{NaIO}}_{\text{3}}$ is $+5$

(l)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{O}$ in ${\text{KO}}_{\text{2}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the earth metals always having $+1$ oxidation number only.
• The $\text{K}$ is in $\text{+1}$ oxidation state and $\text{O}$ is,

  $\begin{array}{l}\text{1(1+)+2X=0}\\ \text{(1+)+2X=0}\\ \text{2X=-1}\\ \text{X=-}\raisebox{1ex}{$\text{1}$}\!\left/ \!\raisebox{-1ex}{$\text{2}$}\right.\end{array}$

• The oxidation number of $\text{O}$ in ${\text{KO}}_{\text{2}}$ is $-\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.$

(m)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{P}$ in ${\text{PF}}_{\text{6}}{}^{\text{-}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is -1 and the general oxidation state of Fluorine is $-1$.

  $\begin{array}{l}\text{6(-1)+X=-1}\\ \text{X=(6+)-1}\\ \text{X=+5}\\ \text{P=+5}\end{array}$

• The oxidation number of $\text{P}$ in ${\text{PF}}_{\text{6}}{}^{\text{-}}$ is $+5$.

(n)

Interpretation Introduction

Interpretation:

The oxidation numbers of underlined atoms in given species are should be given.

Concept introduction:

Rules for assigning the Oxidation number

• The oxidation number of atom in the elemental form is zero.
• The sum of oxidation numbers of all the atoms present in the molecule is zero.
• The general oxidation number for oxygen is $-2$ and hydrogen is $+1$.
• The combination of any atoms in group 7 the oxidation number is varied.
• The Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• In the oxohalide compounds oxidation number of halide is in positive.
• The general oxidation state of halides is -1.
• The earth metals always having $+1$ oxidation number only.

Explanation of Solution

The oxidation number of $\text{Au}$ in ${\text{KAuCl}}_{\text{4}}$

• According to the rules, the sum of oxidation numbers of all the atoms present in the molecule is zero and the earth metals always having $+1$ oxidation number only.
• Halides are having -1 general oxidation number.
• The $\text{Cl}$ in $-1$ and $\text{K}$ is in $\text{+1}$ oxidation states and $\text{Au}$ is,

  $\begin{array}{l}\text{1(1+)+1X+4(-1)=0}\\ \text{(1+)+1X+(-4)}\\ \text{X=}\text{3+}\\ \text{Au=3+}\end{array}$

• The oxidation number of $\text{Au}$ in ${\text{KAuCl}}_{\text{4}}$ is $+3$