In the following reactions, identify the reactant that is oxidized and the reactant that is reduced: Zn ( s ) + Cl 2 ( g ) → ZnCl 2 ( s ) 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 8.4, Problem 27PP

(a)

Interpretation Introduction

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

Zn(s) + Cl2(g)→ZnCl2(s)

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

Cl2(g) + 2NaBr(aq)→2NaCl(aq) + Br2(l)

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

2PbO(s)→2Pb(s) + O2(g)

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

2Fe3+(aq) + Sn2+(aq)→2Fe2+(aq) + Sn4+(aq)

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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You are a Quality Manager for a very well-known food ingredient company that produces umami powder, and you are responsible for setting specification limits. The net weight (in grams) of bags of unami powder is monitored by taking samples of six bags on an hourly basis during production. The label on every bag reports a contents of 1KG umami powder. The process mean is μ = 1012 g, and when the process is properly adjusted, it varies with σ = 11 g. QUESTION: Your organisation strives to ensure that >99.97% of bags of umami powder produced conforms to specification. What performance process index value is required to achieve this process yield? Calculate PPK using the following formula: Ppk = (USL – mean)/3 σ Ppk = (mean -LSL)/ 3 σ

You are a Quality Manager for a very well-known food ingredient company that produces umami powder, and you are responsible for setting specification limits. The net weight (in grams) of bags of unami powder is monitored by taking samples of six bags on an hourly basis during production. The label on every bag reports a contents of 1KG umami powder. The process mean is μ = 1012 g, and when the process is properly adjusted, it varies with σ = 11 g. QUESTION: Provide a valid and full justification as to whether you would advise your manager that the process is satisfactory when it is properly adjusted, or would you seek their approval to improve the process?

You are a Quality Manager for a very well-known food ingredient company that produces umami powder, and you are responsible for setting specification limits. The net weight (in grams) of bags of unami powder is monitored by taking samples of six bags on an hourly basis during production. The label on every bag reports a contents of 1KG umami powder. The process mean is μ = 1012 g, and when the process is properly adjusted, it varies with σ = 11 g. QUESTION: Using all the available information, set the upper and lower specification limits.

Answer 2

Question

Chapter 8.4, Problem 27PP

(a)

Interpretation Introduction

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

Zn(s) + Cl2(g)→ZnCl2(s)

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

Cl2(g) + 2NaBr(aq)→2NaCl(aq) + Br2(l)

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

2PbO(s)→2Pb(s) + O2(g)

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

2Fe3+(aq) + Sn2+(aq)→2Fe2+(aq) + Sn4+(aq)

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 8.4, Problem 27PP

(a)

Interpretation Introduction

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

Zn(s) + Cl2(g)→ZnCl2(s)

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

Cl2(g) + 2NaBr(aq)→2NaCl(aq) + Br2(l)

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

2PbO(s)→2Pb(s) + O2(g)

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

2Fe3+(aq) + Sn2+(aq)→2Fe2+(aq) + Sn4+(aq)

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 8.4, Problem 27PP

(a)

Interpretation Introduction

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

Zn(s) + Cl2(g)→ZnCl2(s)

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

Cl2(g) + 2NaBr(aq)→2NaCl(aq) + Br2(l)

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

2PbO(s)→2Pb(s) + O2(g)

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

2Fe3+(aq) + Sn2+(aq)→2Fe2+(aq) + Sn4+(aq)

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 8.4, Problem 27PP

(a)

Interpretation Introduction

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

Zn(s) + Cl2(g)→ZnCl2(s)

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

Cl2(g) + 2NaBr(aq)→2NaCl(aq) + Br2(l)

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

2PbO(s)→2Pb(s) + O2(g)

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

2Fe3+(aq) + Sn2+(aq)→2Fe2+(aq) + Sn4+(aq)

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 8.4, Problem 27PP

(a)

Interpretation Introduction

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

Zn(s) + Cl2(g)→ZnCl2(s)

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 8.4, Problem 27PP

(a)

Interpretation Introduction

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

Zn(s) + Cl2(g)→ZnCl2(s)

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

Cl2(g) + 2NaBr(aq)→2NaCl(aq) + Br2(l)

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

Cl2(g) + 2NaBr(aq)→2NaCl(aq) + Br2(l)

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

2PbO(s)→2Pb(s) + O2(g)

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

2PbO(s)→2Pb(s) + O2(g)

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

2Fe3+(aq) + Sn2+(aq)→2Fe2+(aq) + Sn4+(aq)

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

2Fe3+(aq) + Sn2+(aq)→2Fe2+(aq) + Sn4+(aq)

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. 8.1 - State the number of atoms of oxygen in the...Ch. 8.1 - State the number of atoms of oxygen in the...Ch. 8.1 - Prob. 3PP Ch. 8.1 - Determine whether each of the following equations...Ch. 8.1 - All of the following are balanced equations. State...Ch. 8.1 - All of the following are balanced equations. State...Ch. 8.2 - Balance each of the following chemical...Ch. 8.2 - Balance each of the following chemical...Ch. 8.2 - Prob. 9PP Ch. 8.2 - Prob. 10PP

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

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