Chapter 15.1, Problem 17PP

(a)

Interpretation Introduction

Interpretation: For the following reaction, identify the substances that is oxidized, the substance that is reduced, the oxidizing agent, and the reducing agent.

  $\text{2Li}\left(\text{s}\right){\text{ + Cl}}_{\text{2}}\left(\text{g}\right)\to \text{2LiCl}\left(\text{s}\right)$

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: For the following reaction, identify the substances that is oxidized, the substance that is reduced, the oxidizing agent, and the reducing agent.

  ${\text{Cl}}_{\text{2}}\left(\text{g}\right)\text{ + 2NaBr}\left(\text{aq}\right)\to \text{2NaCl}\left(\text{aq}\right){\text{ + Br}}_{\text{2}}\left(\text{l}\right)$

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: For the following reaction, identify the substances that is oxidized, the substance that is reduced, the oxidizing agent, and the reducing agent.

  $\text{2Pb}\left(\text{s}\right){\text{ + O}}_{\text{2}}\left(\text{g}\right)\to \text{2PbO}\left(\text{s}\right)$

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.

(d)

Interpretation Introduction

Interpretation: For the following reaction, identify the substances that is oxidized, the substance that is reduced, the oxidizing agent, and the reducing agent.

  $\text{Al}\left(\text{s}\right){\text{ + 3Ag}}^{\text{+}}\left(\text{aq}\right)\to {\text{Al}}^{\text{3+}}\left(\text{aq}\right)\text{ + 3Ag}\left(\text{s}\right)$

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.