Chapter 4, Problem 4.49QP

Give oxidation number for the underlined atoms in the following molecules and ions: (a) Cs₂O, (b) CaI₂, (c) Al₂O₃, (d) H₃AsO₃, (e) TiO₂, (f) $\underset{\_}{\text{Mo}}{\text{O}}_4^{2-}$, (g) $\underset{\_}{\text{Pt}}{\text{Cl}}_4^{2-}$, (h) $\underset{\_}{\text{Pt}}{\text{Cl}}_6^{2-}$, (i) SnF₂, (j) ClF₃, (k) $\underset{\_}{\text{Sb}}{\text{F}}_6^{-}$.

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

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

• According to the rules, the sum of oxidation numbers of all the atoms present in the compound is zero and general oxidation number for oxygen is $-2$.
• The oxygen is in $-2$ oxidation state and $\text{Cs}$ is,

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

• The oxidation number of $\text{Cs}$ in ${\text{Cs}}_{\text{2}}\text{O}$ is $+1$.

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

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

• 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 halides is -1.
• The $\text{I}$ in $-1$ oxidation state and $\text{Ca}$ is,

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

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

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

The oxidation number of $\text{Al}$ in ${\text{Al}}_{\text{2}}{\text{O}}_{\text{3}}$

• The sum of oxidation numbers of all the atoms present in the molecule is zero and the general oxidation number for oxygen is $-2$.
• The $\text{O}$ in $-2$ oxidation state and $\text{Al}$ is,

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

• The oxidation number of $\text{Al}$ in ${\text{Al}}_{\text{2}}{\text{O}}_{\text{3}}$ is $+3$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

The oxidation number of $\text{As}$ in ${\text{H}}_{\text{3}}{\text{AsO}}_{\text{3}}$

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

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

• The oxidation number of $\text{As}$ in ${\text{H}}_{\text{3}}{\text{AsO}}_{\text{3}}$ is $+3$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

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

• 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 oxygen is $-2$.
• The $\text{O}$ in $-2$ oxidation state and $\text{Ti}$ is,

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

• The oxidation number of $\text{Ti}$ in ${\text{TiO}}_{\text{2}}$ is $+4$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

The oxidation number of $\text{Mo}$ in ${\text{MoO}}_{\text{4}}{}^{\text{2-}}$

• 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 Oxygen is $-2$.
• The $\text{O}$ in $-2$ oxidation state and $\text{Mo}$ is ,

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

• The oxidation number of $\text{Mo}$ in ${\text{MoO}}_{\text{4}}{}^{\text{2-}}$ is $+6$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

The oxidation number of $\text{Pt}$ in ${\text{PtCl}}_{\text{4}}{}^{\text{2-}}$

• 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 halides is -1.
• The $\text{Cl}$ in $-1$ and oxidation state and $\text{Pt}$ is,

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

• The oxidation number of $\text{Pt}$ in ${\text{PtCl}}_{\text{4}}{}^{\text{2-}}$ is $+2$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

The oxidation number of $\text{Pt}$ in ${\text{PtCl}}_{\text{6}}{}^{\text{2-}}$

• 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 halides is -1.
• The $\text{Cl}$ in $-1$ and oxidation state and $\text{Pt}$ is,

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

• The oxidation number of $\text{Pt}$ in ${\text{PtCl}}_{\text{6}}{}^{\text{2-}}$ is $+4$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

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

• 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 halides is -1.
• The $\text{F}$ in $-1$ and oxidation state and $\text{Pt}$ is,

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

• The oxidation number of $\text{Sn}$ in ${\text{SnF}}_{\text{2}}$ is $+2$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

The oxidation number of $\text{Cl}$ in ${\text{ClF}}_{\text{3}}$

• 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 halides is -1 but in the Inter halogen compounds the Fluorine is always having $-1$ oxidation state.
• The $\text{F}$ in $-1$ and oxidation state and $\text{Cl}$ is,

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

• The oxidation number of $\text{Cl}$ in ${\text{ClF}}_{\text{3}}$ is $+3$

The oxidation number of $\text{Cl}$ in ${\text{ClF}}_{\text{3}}$

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 compound 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.
• The oxidation state of hydrogen in metal hydride is $-1$.

Explanation of Solution

The oxidation number of $\text{I}$ in ${\text{SbF}}_{\text{6}}{}^{\text{-}}$

• 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 halides is -1 and Fluorine is always having $-1$ oxidation state.
• The $\text{F}$ in $-1$ and oxidation state and $\text{Sb}$ is,

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

• The oxidation number of $\text{I}$ in ${\text{SbF}}_{\text{6}}{}^{\text{-}}$ is $+5$