Loose Leaf for Chemistry: The Molecular Nature of Matter and Change
Loose Leaf for Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781260151749
Author: Silberberg Dr., Martin; Amateis Professor, Patricia
Publisher: McGraw-Hill Education
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Chapter 8, Problem 8.91P

(a)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare hypochlorous acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(a)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is dichlorine oxide and its chemical formula is Cl2O.

Explanation of Solution

The formula of hypochlorous acid is HClO.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of chlorine in HClO is as follows:

  [(oxidation number of hydrogen)+(oxidation number of chlorine )+(oxidation number of oxygen)]=0        (1)

Rearrange equation (1) for the oxidation number of chlorine as follows:

  Oxidation number of chlorine=[(oxidation number of hydrogen)(oxidation number of oxygen)]        (2)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (2).

  Oxidation number of chlorine=[1(2)]=[1+2]=+1.

The oxidation number of chlorine is +1 so the oxide formed is dichlorine oxide with the chemical formula Cl2O.

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(b)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare chlorous acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(b)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is dichlorine trioxide and its chemical formula is Cl2O3.

Explanation of Solution

The formula of chlorous acid is HClO2.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of chlorine in HClO2 is as follows:

  [(oxidation number of hydrogen)+(oxidation number of chlorine )+2(oxidation number of oxygen)]=0        (3)

Rearrange equation (3) for the oxidation number of chlorine as follows:

  Oxidation number of chlorine=[(oxidation number of hydrogen)2(oxidation number of oxygen)]        (4)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (4).

  Oxidation number of chlorine=[12(2)]=[1+4]=+3.

The oxidation number of chlorine is +3 so the oxide formed is dichlorine trioxide with the chemical formula Cl2O3.

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(c)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare chloric acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(c)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is dichlorine pentaoxide and its chemical formula is Cl2O5.

Explanation of Solution

The formula of chloric acid is HClO3.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of chlorine in HClO3 is as follows:

  [(oxidation number of hydrogen)+(oxidation number of chlorine )+3(oxidation number of oxygen)]=0        (5)

Rearrange equation (5) for the oxidation number of chlorine as follows:

  Oxidation number of chlorine=[(oxidation number of hydrogen)3(oxidation number of oxygen)]        (6)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (6).

  Oxidation number of chlorine=[13(2)]=[1+6]=+5.

The oxidation number of chlorine is +5 so the oxide formed is dichlorine pentaoxide with the chemical formula Cl2O5

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(d)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare perchloric acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(d)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is dichlorine heptaoxide and its chemical formula is Cl2O7.

Explanation of Solution

The formula of perchloric acid is HClO4.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of chlorine in HClO4 is as follows:

  [(oxidation number of hydrogen)+(oxidation number of chlorine )+4(oxidation number of oxygen)]=0        (7)

Rearrange equation (7) for the oxidation number of chlorine as follows:

  Oxidation number of chlorine=[(oxidation number of hydrogen)4(oxidation number of oxygen)]        (8)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (8).

  Oxidation number of chlorine=[14(2)]=[1+8]=+7.

The oxidation number of chlorine is +7 so the oxide formed is dichlorine heptaoxide with the chemical formula Cl2O7

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(e)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare sulphuric acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(e)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is sulfur trioxide and its chemical formula is SO3.

Explanation of Solution

The formula of sulfuric acid is H2SO4.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of sulfur in H2SO4 is as follows:

  [2(oxidation number of hydrogen)+(oxidation number of sulphur )+4(oxidation number of oxygen)]=0        (9)

Rearrange equation (9) for the oxidation number of sulfur as follows:

  Oxidation number of sulphur=[2(oxidation number of hydrogen)4(oxidation number of oxygen)]        (10)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (10).

  Oxidation number of sulphur=[2(1)4(2)]=[2+8]=+6.

The oxidation number of sulfur is +6 so the oxide formed is sulfur trioxide with the chemical formula SO3

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(f)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare sulfurous acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(f)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is sulfur dioxide and its chemical formula is SO2.

Explanation of Solution

The formula of sulfurous acid is H2SO3.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of sulfur in H2SO3 is as follows:

  [2(oxidation number of hydrogen)+(oxidation number of sulphur )+3(oxidation number of oxygen)]=0        (11)

Rearrange equation (11) for the oxidation number of sulfur as follows:

  Oxidation number of sulphur=[2(oxidation number of hydrogen)3(oxidation number of oxygen)]        (12)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (12).

  Oxidation number of sulphur=[2(1)3(2)]=[2+6]=+4.

The oxidation number of sulfur is +4 so the oxide formed is sulfur dioxide with the chemical formula SO2

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(g)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare nitric acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(g)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is dinitrogen pentaoxide and its chemical formula is N2O5.

Explanation of Solution

The formula of nitric acid is HNO3.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of nitrogen in HNO3 is as follows:

  [2(oxidation number of hydrogen)+(oxidation number of nitrogen )+3(oxidation number of oxygen)]=0        (13)

Rearrange equation (13) for the oxidation number of nitrogen as follows:

  Oxidation number of nitrogen=[(oxidation number of hydrogen)3(oxidation number of oxygen)]        (14)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (14).

  Oxidation number of nitrogen=[13(2)]=[1+6]=+5.

The oxidation number of nitrogen is +5 so the oxide formed is dinitrogen pentaoxide with the chemical formula N2O5

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(h)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare nitrous acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(h)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is dinitrogen trioxide and its chemical formula is N2O3.

Explanation of Solution

The formula of nitrous acid is HNO2.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of nitrogen in HNO2 is as follows:

  [(oxidation number of hydrogen)+(oxidation number of nitrogen )+2(oxidation number of oxygen)]=0        (15)

Rearrange equation (15) for the oxidation number of nitrogen as follows:

  Oxidation number of nitrogen=[(oxidation number of hydrogen)2(oxidation number of oxygen)]        (16)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (14).

  Oxidation number of nitrogen=[12(2)]=[1+4]=+3.

The oxidation number of nitrogen is +3 so the oxide formed is dinitrogen trioxide with the chemical formula N2O3

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(i)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare carbonic acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(i)

Expert Solution
Check Mark

Answer to Problem 8.91P

The name of the oxide is carbon dioxide and its chemical formula is CO2.

Explanation of Solution

The formula of carbonic acid is H2CO3.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of carbon in H2CO3 is as follows:

  [2(oxidation number of hydrogen)+(oxidation number of carbon )+3(oxidation number of oxygen)]=0        (17)

Rearrange equation (17) for the oxidation number of carbon is as follows:

  Oxidation number of carbon=[2(oxidation number of hydrogen)3(oxidation number of oxygen)]        (18)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (18).

  Oxidation number of carbon=[2(1)3(2)]=[2+6]=+4.

The oxidation number of carbon is +4 so the oxide formed is carbon dioxide with the chemical formula CO2

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

(j)

Interpretation Introduction

Interpretation:

The name and the formula of the oxide that is used to prepare phosphoric acid are to be determined.

Concept introduction:

Oxidation of a species involves the loss of electrons by that species and reduction of a species involves the gain of electrons by that species.

The oxidation number is defined as the formal charge an atom would gain if all the bonds attached to it in a compound are heterolytically cleaved. Oxidation number can be a positive or negative number but cannot be fractional.

(j)

Expert Solution
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Answer to Problem 8.91P

The name of the oxide is diphosphorus pentaoxide and its chemical formula is P2O5.

Explanation of Solution

The formula of phosphoric acid is H3PO4.

The oxidation number of hydrogen is +1 and the oxidation state of oxygen is 2.

The expression to calculate the oxidation number of phosphorous in H3PO4 is as follows:

  [3(oxidation number of hydrogen)+(oxidation number of phosphorous )+4(oxidation number of oxygen)]=0        (19)

Rearrange equation (19) for the oxidation number of phosphorous is as follows:

  Oxidation number of P=[3(oxidation number of hydrogen)4(oxidation number of oxygen)]        (20)

Substitute +1 for oxidation number of hydrogen and 2 for oxidation number of oxygen in equation (20).

  Oxidation number of phosphorous=[3(1)4(2)]=[3+8]=+5.

The oxidation number of phosphorous is +5 so the oxide formed is diphosphorus pentaoxide with the chemical formula P2O5

Conclusion

The sum of the oxidation numbers of various elements in a neutral compound is zero whereas that in an ionic compound is equal to the charge on the ion.

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Chapter 8 Solutions

Loose Leaf for Chemistry: The Molecular Nature of Matter and Change

Ch. 8.4 - Prob. 8.6AFPCh. 8.4 - Prob. 8.6BFPCh. 8.4 - Prob. 8.7AFPCh. 8.4 - Prob. 8.7BFPCh. 8.4 - Prob. 8.8AFPCh. 8.4 - Prob. 8.8BFPCh. 8 - Prob. 8.1PCh. 8 - Prob. 8.2PCh. 8 - Prob. 8.3PCh. 8 - To test Döbereiner’s idea (Problem 8.3),...Ch. 8 - Summarize the rules for the allowable values of...Ch. 8 - Prob. 8.6PCh. 8 - State the exclusion principle. What does it imply...Ch. 8 - What is the key distinction between sublevel...Ch. 8 - Prob. 8.9PCh. 8 - Prob. 8.10PCh. 8 - Prob. 8.11PCh. 8 - How many electrons in an atom can have each of the...Ch. 8 - Prob. 8.13PCh. 8 - How many electrons in an atom can have each of the...Ch. 8 - Prob. 8.15PCh. 8 - State Hund’s rule in your own words, and show its...Ch. 8 - Prob. 8.17PCh. 8 - For main-group elements, are outer electron...Ch. 8 - Prob. 8.19PCh. 8 - Prob. 8.20PCh. 8 - Prob. 8.21PCh. 8 - Prob. 8.22PCh. 8 - Write the full ground-state electron configuration...Ch. 8 - Prob. 8.24PCh. 8 - Prob. 8.25PCh. 8 - Prob. 8.26PCh. 8 - Prob. 8.27PCh. 8 - Draw a partial (valence-level) orbital diagram,...Ch. 8 - Prob. 8.29PCh. 8 - Draw a partial (valence-level) orbital diagram,...Ch. 8 - Draw the partial (valence-level) orbital diagram,...Ch. 8 - Prob. 8.32PCh. 8 - Prob. 8.33PCh. 8 - Prob. 8.34PCh. 8 - Prob. 8.35PCh. 8 - Prob. 8.36PCh. 8 - How many inner, outer, and valence electrons are...Ch. 8 - How many inner, outer, and valence electrons are...Ch. 8 - Prob. 8.39PCh. 8 - Prob. 8.40PCh. 8 - Prob. 8.41PCh. 8 - Prob. 8.42PCh. 8 - Prob. 8.43PCh. 8 - Prob. 8.44PCh. 8 - If the exact outer limit of an isolated atom...Ch. 8 - Given the following partial (valence-level)...Ch. 8 - In what region of the periodic table will you find...Ch. 8 - Why do successive IEs of a given element always...Ch. 8 - Prob. 8.49PCh. 8 - Prob. 8.50PCh. 8 - Prob. 8.51PCh. 8 - Prob. 8.52PCh. 8 - Prob. 8.53PCh. 8 - Prob. 8.54PCh. 8 - Prob. 8.55PCh. 8 - Prob. 8.56PCh. 8 - Prob. 8.57PCh. 8 - Prob. 8.58PCh. 8 - Prob. 8.59PCh. 8 - Prob. 8.60PCh. 8 - Prob. 8.61PCh. 8 - Prob. 8.62PCh. 8 - Prob. 8.63PCh. 8 - Prob. 8.64PCh. 8 - Prob. 8.65PCh. 8 - What is a pseudo-noble gas configuration? Give an...Ch. 8 - How are measurements of paramagnetism used to...Ch. 8 - Prob. 8.68PCh. 8 - Prob. 8.69PCh. 8 - Prob. 8.70PCh. 8 - Prob. 8.71PCh. 8 - Prob. 8.72PCh. 8 - Prob. 8.73PCh. 8 - Prob. 8.74PCh. 8 - Prob. 8.75PCh. 8 - Prob. 8.76PCh. 8 - Prob. 8.77PCh. 8 - Prob. 8.78PCh. 8 - Prob. 8.79PCh. 8 - Prob. 8.80PCh. 8 - Which of these atoms are paramagnetic in their...Ch. 8 - Prob. 8.82PCh. 8 - Prob. 8.83PCh. 8 - Write the condensed ground-state electron...Ch. 8 - Prob. 8.85PCh. 8 - Prob. 8.86PCh. 8 - Rank the ions in each set in order of increasing...Ch. 8 - Prob. 8.88PCh. 8 - Prob. 8.89PCh. 8 - Prob. 8.90PCh. 8 - Prob. 8.91PCh. 8 - A fundamental relationship of electrostatics...Ch. 8 - Prob. 8.93PCh. 8 - Prob. 8.94PCh. 8 - Prob. 8.95PCh. 8 - Prob. 8.96PCh. 8 - Prob. 8.97PCh. 8 - Prob. 8.98PCh. 8 - Use Figure 8.16, to find: (a) the longest...Ch. 8 - Prob. 8.100PCh. 8 - Prob. 8.101PCh. 8 - Prob. 8.102P
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