Assign oxidation numbers to all of the elements in HSO 4 - 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 11PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HSO₄-

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 H₃PO₃

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 Cr₂O₇²-

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 Na₂CO₃

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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(EXM 2, PRBLM 3) Here is this problem, can you explain it to me and show how its done. Thank you I need to see the work for like prbl solving.

Answer 2

Question

Chapter 15.1, Problem 11PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HSO₄-

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 H₃PO₃

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 Cr₂O₇²-

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 Na₂CO₃

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 11PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HSO₄-

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 H₃PO₃

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 Cr₂O₇²-

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 Na₂CO₃

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.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 15.1, Problem 11PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HSO₄-

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 H₃PO₃

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 Cr₂O₇²-

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 Na₂CO₃

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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See solution

Answer 5

Chapter 15.1, Problem 11PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HSO₄-

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 H₃PO₃

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 Cr₂O₇²-

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 Na₂CO₃

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 11PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HSO₄-

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 11PP

(a)

Interpretation Introduction

Interpretation: Assign oxidation numbers to all of the elements in HSO₄-

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 H₃PO₃

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 H₃PO₃

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 Cr₂O₇²-

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 Cr₂O₇²-

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 Na₂CO₃

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 Na₂CO₃

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 elements in HSO 4.

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