Assign oxidation numbers to all of the elements in C 2 H 3 O 2 - Concept Introduction: 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. If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

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Answer 1

Question

Chapter 15.1, Problem 10PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in C₂H₃O₂-

Concept Introduction:

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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(b)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in AlCl₃

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(c)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in NH₄+

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(d)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HBrO₄

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

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Answer 2

Question

Chapter 15.1, Problem 10PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in C₂H₃O₂-

Concept Introduction:

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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(b)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in AlCl₃

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(c)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in NH₄+

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(d)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HBrO₄

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

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Answer 3

Question

Chapter 15.1, Problem 10PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in C₂H₃O₂-

Concept Introduction:

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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(b)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in AlCl₃

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(c)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in NH₄+

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(d)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HBrO₄

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

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Answer 4

Question

Chapter 15.1, Problem 10PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in C₂H₃O₂-

Concept Introduction:

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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(b)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in AlCl₃

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(c)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in NH₄+

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(d)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HBrO₄

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

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Answer 5

Chapter 15.1, Problem 10PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in C₂H₃O₂-

Concept Introduction:

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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(b)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in AlCl₃

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(c)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in NH₄+

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

(d)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HBrO₄

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 6

Chapter 15.1, Problem 10PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in C₂H₃O₂-

Concept Introduction:

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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 7

Chapter 15.1, Problem 10PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in C₂H₃O₂-

Concept Introduction:

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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 8

(b)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in AlCl₃

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 9

(b)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in AlCl₃

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 10

(c)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in NH₄+

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 11

(c)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in NH₄+

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 12

(d)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HBrO₄

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 13

(d)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HBrO₄

Concept Introduction: 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.

If the oxidation number of an element increases then it undergoes oxidation and if the oxidation number of the element decreases then it undergoes reduction.

Answer 14

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Answer 15

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Answer 16

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Answer 17

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 all elements in C 2 H 3 O 2.

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