CHEMISTRY-MASTERINGCHEMISTRY W/ETEXT
CHEMISTRY-MASTERINGCHEMISTRY W/ETEXT
8th Edition
ISBN: 9780135204634
Author: Robinson
Publisher: PEARSON
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Redox Reactions
Redox reactions are considered to be the chemical reactions involving both oxidation and reduction processes. They are actually oxidation-reduction reactions. The term redox is made from two words where “red” comes from reduction and “ox” comes from oxid…
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Chapter 4, Problem 4.108SP
Interpretation Introduction

(a)

Interpretation:

The oxidation number for each of the elements present in NO2 is to be determined.

Concept introduction:

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are:

  1. The oxidation state of Group 1 elements is taken to be +1.
  2. The oxidation states of Group 2 elements are taken to be +2.
  3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
  4. Oxidation state of halogens is taken to be -1 usually.
  5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
  6. Any element when present in its elemental form has zero oxidation state.
  7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
  8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
  9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(b)

Interpretation:

The oxidation number for each of the elements present in SO3 is to be determined.

Concept introduction:

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are :

  1. The oxidation states of Group 1 elements is taken to be +1.
  2. The oxidation states of Group 2 elements is taken to be +2.
  3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
  4. Oxidation state of halogens is taken to be -1 usually.
  5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
  6. Any element when present in its elemental form has zero oxidation state.
  7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
  8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
  9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(c)

Interpretation:

The oxidation number for each of the elements present in COCl2 is to be determined.

Concept introduction:

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are :

  1. The oxidation states of Group 1 elements is taken to be +1.
  2. The oxidation states of Group 2 elements is taken to be +2.
  3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
  4. Oxidation state of halogens is taken to be -1 usually.
  5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
  6. Any element when present in its elemental form has zero oxidation state.
  7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
  8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
  9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(d)

Interpretation:

The oxidation number for each of the elements present in CH2Cl2 is to be determined.

Concept introduction:

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are :

  1. The oxidation states of Group 1 elements is taken to be +1.
  2. The oxidation states of Group 2 elements is taken to be +2.
  3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
  4. Oxidation state of halogens is taken to be -1 usually.
  5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
  6. Any element when present in its elemental form has zero oxidation state.
  7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
  8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
  9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(e)

Interpretation:

The oxidation number for each of the elements present in KClO3 is to be determined.

Concept introduction:

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are:

  1. The oxidation states of Group 1 elements is taken to be +1.
  2. The oxidation states of Group 2 elements is taken to be +2.
  3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
  4. Oxidation state of halogens is taken to be -1 usually.
  5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
  6. Any element when present in its elemental form has zero oxidation state.
  7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
  8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
  9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

Interpretation Introduction

(f)

Interpretation:

The oxidation number for each of the elements present in HNO3 is to be determined.

Concept introduction:

Oxidation number or oxidation state of an atom in a molecule is the positive or the negative charge that an atom would have possessed if the compound would have been ionic. There are many rules for assigning the oxidation state to the given atom in a molecule. Some of them are :

  1. The oxidation states of Group 1 elements is taken to be +1.
  2. The oxidation states of Group 2 elements is taken to be +2.
  3. The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
  4. Oxidation state of halogens is taken to be -1 usually.
  5. The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
  6. Any element when present in its elemental form has zero oxidation state.
  7. The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
  8. The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
  9. In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion

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Chapter 4 Solutions

CHEMISTRY-MASTERINGCHEMISTRY W/ETEXT

Ch. 4 - Prob. 4.1PCh. 4 - Prob. 4.2ACh. 4 - How many moles of solute are present in 125 mLof...Ch. 4 - Prob. 4.4ACh. 4 - Prob. 4.5PCh. 4 - APPLY 4.7 Sulfuric acid is normally purchased at a...Ch. 4 - Prob. 4.7PCh. 4 - Conceptual APPLY 4.9 Three different substances,...Ch. 4 - Write ne ionic equations for the following...Ch. 4 - Prob. 4.10A
Ch. 4 - Will a precipitation reaction occur when aqueous...Ch. 4 - APPLY 4.13 How might you use a precipitation...Ch. 4 - Conceptual PRACTICE 4.14 An aqueous solution...Ch. 4 - Conceptual APPLY 4.15 A solution containing the...Ch. 4 - Name the acids HI and HBrO2 .Ch. 4 - APPLY 4.17 Give likely chemical formulas...Ch. 4 - PRACTICE 4.18 Write a balanced ionic equation and...Ch. 4 - Milk of magnesia (active ingredient: magnesium...Ch. 4 - Prob. 4.19PCh. 4 - Prob. 4.20ACh. 4 - Prob. 4.21PCh. 4 - Assume that the buret contains H+ ions, the flask...Ch. 4 - PRACTICE 4.24 Assign an oxidation number to each...Ch. 4 - APPLY 4.25 Chlorine can have several different...Ch. 4 - Identify the oxidizing agent and reducing agent in...Ch. 4 - APPLY 4.27 Police often use a Breathalyzer test to...Ch. 4 - PRACTICE 4.28 Predict whether the following...Ch. 4 - Use the following reactions to arrange the...Ch. 4 - Prob. 4.29PCh. 4 - Prob. 4.30ACh. 4 - A viramin-fortified brand of a sports...Ch. 4 - The nutritional label on Power ade specifies that...Ch. 4 - Prob. 4.33PCh. 4 - One way to analyze a sports drink for the...Ch. 4 - To measure the concentration of chloride ions ina...Ch. 4 - The flavor of the first batch of Gatorade was...Ch. 4 - Prob. 4.37CPCh. 4 - Prob. 4.38CPCh. 4 - Assume that an aqueous solution Of a cation,...Ch. 4 - The following pictures represent aqueous solutions...Ch. 4 - Prob. 4.41CPCh. 4 - The concentration of an aqueous solution of NaOCl...Ch. 4 - Assume that the electrical conductivity of a...Ch. 4 - Based on the positions in the periodic table,...Ch. 4 - The following two redox reactions occur between...Ch. 4 - Prob. 4.46SPCh. 4 - How many grams of solute would you use to prepare...Ch. 4 - How many milliliters of a 0.45 M BaCl2 solution...Ch. 4 - How many milliliters of a 0.350 M KOH solution...Ch. 4 - The sterile saline solution used to rinse contact...Ch. 4 - Prob. 4.51SPCh. 4 - Copper reacts with dilute nitric acid according to...Ch. 4 - Prob. 4.53SPCh. 4 - How many grams of solute would you use to prepare...Ch. 4 - 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Which of the following substances are likely to be...Ch. 4 - Which of the following substances are likely to be...Ch. 4 - Predict whether a precipitation reaction will...Ch. 4 - Predict whether a precipitation reaction will...Ch. 4 - hich of the following solutions will not form a...Ch. 4 - Which of the following solutions will not form a...Ch. 4 - How would you prepare the following substances by...Ch. 4 - How would you prepare the following substances by...Ch. 4 - What are the mass and the identity of the...Ch. 4 - What are the mass and the identity of the...Ch. 4 - Assume that you have an aqueous mixture of NaNO3...Ch. 4 - Assume that you have an aqueous mixture of BaCl2...Ch. 4 - Assume that you have an aqueous solution of an...Ch. 4 - Assume that you have an aqueous solution of an...Ch. 4 - How could you use a precipitation reaction to...Ch. 4 - How could you u a precipitation reaction to...Ch. 4 - The following three solutions are mixed: 100.0 mL...Ch. 4 - A 250.0 g sample of a white solid is known to be a...Ch. 4 - Assume that you are given a solution of an unknown...Ch. 4 - Why do we use a double arrow () to show the...Ch. 4 - Write balanced ionic equations for the following...Ch. 4 - Write balanced ionic equations for the following...Ch. 4 - Write balanced net ionic equations for the...Ch. 4 - Write balanced net ionic equations for the...Ch. 4 - A flask containing 450 mL of 0.500 M HBr was...Ch. 4 - The odor of skunks is caused by chemical compounds...Ch. 4 - Prob. 4.102SPCh. 4 - Prob. 4.103SPCh. 4 - How many milliliters of 1.00 M KOH must be added...Ch. 4 - How many milliliters of 2.00 M HCl must be added...Ch. 4 - If the following solutions are mixed, is the...Ch. 4 - If the following solutions are mixed, is the...Ch. 4 - Prob. 4.108SPCh. 4 - Assign oxidation numbers to each element in the...Ch. 4 - Assign oxidation numbers to each element in the...Ch. 4 - Assign oxidation numbers to each element in the...Ch. 4 - Nitrogen can have several different oxidation...Ch. 4 - Prob. 4.113SPCh. 4 - Prob. 4.114SPCh. 4 - Where in the periodic table are the most easily...Ch. 4 - In each of the following instances, tell whether...Ch. 4 - Tell for each of the following substances whether...Ch. 4 - Which element is oxidized and which is reduced in...Ch. 4 - Which element is oxidized and which is reduced in...Ch. 4 - Use the activity series of metals (Table 4.5) to...Ch. 4 - Neither strontium (Sr) nor antimony (Sb) is shown...Ch. 4 - (a) Use the following reactions to arrange the...Ch. 4 - Prob. 4.123SPCh. 4 - Iodine, I2 , reacts with aqueous thiosulfate ion...Ch. 4 - How many milliliters of 0.250MNa2S2O3 solution is...Ch. 4 - Dichromate ion, Cr2O72 reacts with aqueous...Ch. 4 - A volume of 18.72 mL of 0.1500MK2Cr2O7 solution...Ch. 4 - What is the molar concentration of As(III) in a...Ch. 4 - Standardized solutions of KBrO3 are frequently...Ch. 4 - The metal content of iron in ores can be...Ch. 4 - Prob. 4.131SPCh. 4 - Alcohol levels in blood can he determined by a...Ch. 4 - Calcium levels in blood can be determined by...Ch. 4 - 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