In the following reaction, identify the reactant that is oxidized and the reactant that is reduced: 2Ag + ( aq ) + Zn ( s ) → 2Ag ( s ) + Zn 2+ ( aq ) Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative. The rules for assigning oxidation number to elements are: For an element in its free state it is assigned an oxidation number of zero. Monatomic ions have oxidation number that is equal to charge of the monatomic ion. Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number. In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number. For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

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Answer 1

Question

Chapter 15.1, Problem 4PP

(a)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(b)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Ca(s) + S(s)→CaS(s)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(c)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Sn2+(aq) + 2Cr3+(aq)→Sn4+(aq) + 2Cr2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

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Answer 2

Question

Chapter 15.1, Problem 4PP

(a)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(b)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Ca(s) + S(s)→CaS(s)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(c)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Sn2+(aq) + 2Cr3+(aq)→Sn4+(aq) + 2Cr2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

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Answer 3

Question

Chapter 15.1, Problem 4PP

(a)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(b)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Ca(s) + S(s)→CaS(s)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(c)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Sn2+(aq) + 2Cr3+(aq)→Sn4+(aq) + 2Cr2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

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Answer 4

Question

Chapter 15.1, Problem 4PP

(a)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(b)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Ca(s) + S(s)→CaS(s)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(c)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Sn2+(aq) + 2Cr3+(aq)→Sn4+(aq) + 2Cr2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

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Answer 5

Chapter 15.1, Problem 4PP

(a)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(b)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Ca(s) + S(s)→CaS(s)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

(c)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Sn2+(aq) + 2Cr3+(aq)→Sn4+(aq) + 2Cr2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

Answer 6

Chapter 15.1, Problem 4PP

(a)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

Answer 7

Chapter 15.1, Problem 4PP

(a)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

Answer 8

(b)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Ca(s) + S(s)→CaS(s)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

Answer 9

(b)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Ca(s) + S(s)→CaS(s)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

Answer 10

(c)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Sn2+(aq) + 2Cr3+(aq)→Sn4+(aq) + 2Cr2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

Answer 11

(c)

Interpretation Introduction

Interpretation: In the following reaction, identify the reactant that is oxidized and the reactant that is reduced:

Sn2+(aq) + 2Cr3+(aq)→Sn4+(aq) + 2Cr2+(aq)

Concept Introduction: In an oxidation reaction the oxidation number of the element increase or becomes more positive. In a reduction reaction the oxidation number of the element decrease or becomes more negative.

The rules for assigning oxidation number to elements are:

For an element in its free state it is assigned an oxidation number of zero.

Monatomic ions have oxidation number that is equal to charge of the monatomic ion.

Alkali metals have +1 oxidation number, alkaline earth metals have +2 oxidation number and halogens are assigned -1 oxidation number.

In most compounds H is assigned a +1 oxidation number and O is assigned a -2 oxidation number.

For a neutral compound the summation of oxidation numbers of all elements in the compound is zero.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 15.1 - Identify each of the following as an oxidation or...Ch. 15.1 - Identify each of the following as an oxidation or...Ch. 15.1 - Prob. 3PP Ch. 15.1 - Prob. 4PP Ch. 15.1 - Prob. 5PP Ch. 15.1 - Prob. 6PP Ch. 15.1 - Prob. 7PP Ch. 15.1 - Prob. 8PP Ch. 15.1 - Prob. 9PP Ch. 15.1 - Prob. 10PP

Solution Summary: The author explains the rules for assigning oxidation numbers to elements.

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