Basic Chemistry
6th Edition
ISBN: 9780134878119
Author: Timberlake, Karen C. , William
Publisher: Pearson,
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Question
Chapter 15, Problem 59APP
(a)
Interpretation Introduction
Interpretation:
To assign the oxidation number for each of the elements present in
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:
- The oxidation states of Group 1 elements are taken to be +1.
- The oxidation states of Group 2 elements are taken to be +2.
- The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
- Oxidation state of halogens is taken to be -1 usually.
- The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
- Any element when present in its elemental form has zero oxidation state.
- The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
- The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
- In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion.
(b)
Interpretation Introduction
Interpretation:
To assign the oxidation number for each of the elements present in
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 :
- The oxidation states of Group 1 elements are taken to be +1.
- The oxidation states of Group 2 elements are taken to be +2.
- The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
- Oxidation state of halogens is taken to be -1 usually.
- The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
- Any element when present in its elemental form has zero oxidation state.
- The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
- The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
- In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion
(c)
Interpretation Introduction
Interpretation:
To assign the oxidation number for each of the elements present in
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:
- The oxidation states of Group 1 elements are taken to be +1.
- The oxidation state of Group 2 elements are taken to be +2.
- The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
- Oxidation state of halogens is taken to be -1 usually.
- The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
- Any element when present in its elemental form has zero oxidation state.
- The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
- The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
- In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion
(d)
Interpretation Introduction
Interpretation:
To assign the oxidation number for each of the elements present in
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:
- The oxidation states of Group 1 elements are taken to be +1.
- The oxidation states of Group 2 elements are taken to be +2.
- The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
- Oxidation state of halogens is taken to be -1 usually.
- The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
- Any element when present in its elemental form has zero oxidation state.
- The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
- The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
- In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion
(e)
Interpretation Introduction
Interpretation:
To assign the oxidation number for each of the elements present in
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:
- The oxidation states of Group 1 elements are taken to be +1.
- The oxidation states of Group 2 elements are taken to be +2.
- The oxidation state of oxygen is always -2 in most of the compounds except peroxides.
- Oxidation state of halogens is taken to be -1 usually.
- The oxidation state of hydrogen is taken to be -1 when bonded to metals and +1 when bonded to non-metals.
- Any element when present in its elemental form has zero oxidation state.
- The oxidation state of Fluorine is taken to be -1 except when present in elemental state (F2).
- The sum of oxidation states of all the atoms present in a given molecule is equal to zero.
- In case of ions, the sum of oxidation state is equal to the total charge carried by the polyatomic ion
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Students have asked these similar questions
(5.9: Similar to For Practice 5.15) Identify the oxidizing agent in the reaction below.
Mg(s) + 2HCl(aq) --> MgCl2(aq) +
H2(g)
O Mg
O H₂
OHCI
This is not a redox reaction.
< Previous
Fill in the blanks:
(7.14) In the electrolysis of CUSO4, how
much copper is plated out on the cathode by
a current of a 0.75A in 10 minutes?
(Cu 63.546 g/mol)
Analysis/Strategy: ampere & time
coulombs ® mol e¯ (or Faraday) ® mol
Cu
(R
mass of Cu
Reduction half-reaction of copper
solution to copper metal: Cu*²(aq)
+
e¯ ® Cu(s)
copper solution, CUSO4, has the ions:
[Cu*2 SOq]
Answer: The mass of copper plated out is
g Cu. (3 sig fig)
Fill in the blanks:
(7.13) Using a current of 4.75 A, how many
minutes does it take to plate a sculpture
with 1.50 g of Cu from a CuS04 solution?
(Cu 63.546 g/mol)
Analysis/Strategy: mass of Cu ® mol Cu
® mol e" (or Faraday) ® coulombs ®
time in minutes (given current
in
amperes)
Reduction half-reaction of copper
solution to copper metal: Cu*2(aq) ·
+
e¯ ® Cu(s)
copper solution, CUSO4, has the ions:
[Cu*2_SOq]
Answer: The time needed to plate out a
sculpture is
minutes. (3
sig fig)
Chapter 15 Solutions
Basic Chemistry
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. 3PPCh. 15.1 - Prob. 4PPCh. 15.1 - Prob. 5PPCh. 15.1 - Prob. 6PPCh. 15.1 - Prob. 7PPCh. 15.1 - Prob. 8PPCh. 15.1 - Prob. 9PPCh. 15.1 - Prob. 10PP
Ch. 15.1 - Prob. 11PPCh. 15.1 - Prob. 12PPCh. 15.1 - What is the oxidation number of the specified...Ch. 15.1 - What is the oxidation number of the specified...Ch. 15.1 - Prob. 15PPCh. 15.1 - Prob. 16PPCh. 15.1 - Prob. 17PPCh. 15.1 - Prob. 18PPCh. 15.1 - Prob. 19PPCh. 15.1 - Prob. 20PPCh. 15.2 - Balance each of the following half-reactions in...Ch. 15.2 - Prob. 22PPCh. 15.2 - Prob. 23PPCh. 15.2 - Use the half-reaction method to balance each of...Ch. 15.2 - Use the half-reaction method to balance each of...Ch. 15.2 - Use the half-reaction method to balance each of...Ch. 15.3 - Use the activity series in Table 15.3 to predict...Ch. 15.3 - Use the activity series in Table 15.3 to predict...Ch. 15.3 - Prob. 29PPCh. 15.3 - Prob. 30PPCh. 15.3 - Prob. 31PPCh. 15.3 - Prob. 32PPCh. 15.3 - The following half-reaction takes place in a...Ch. 15.3 - The following half-reaction takes place in a...Ch. 15.3 - The following half-reaction takes place in a...Ch. 15.3 - Prob. 36PPCh. 15.4 - What we call "tin cans" are really iron cans...Ch. 15.4 - Prob. 38PPCh. 15.4 - Prob. 39PPCh. 15.4 - Prob. 40PPCh. 15.4 - Prob. 41PPCh. 15.4 - Prob. 42PPCh. 15 - Prob. 43UTCCh. 15 - Prob. 44UTCCh. 15 - Prob. 45UTCCh. 15 - Prob. 46UTCCh. 15 - The chapter sections to review are shown in...Ch. 15 - The chapter sections to review are shown in...Ch. 15 - The chapter sections to review are shown in...Ch. 15 - Prob. 50UTCCh. 15 - Prob. 51UTCCh. 15 - Prob. 52UTCCh. 15 - The chapter sections to review are shown in...Ch. 15 - The chapter sections to review are shown in...Ch. 15 - Which of the following are oxidation-reduction...Ch. 15 - Which of the following are oxidation-reduction...Ch. 15 - In the mitochondria of human cells, energy is...Ch. 15 - Prob. 58APPCh. 15 - Prob. 59APPCh. 15 - Prob. 60APPCh. 15 - Prob. 61APPCh. 15 - Prob. 62APPCh. 15 - Prob. 63APPCh. 15 - Write the balanced half-reactions and a balanced...Ch. 15 - Prob. 65APPCh. 15 - Use the activity series in Table 15.3 to predict...Ch. 15 - Prob. 67APPCh. 15 - Prob. 68APPCh. 15 - Prob. 69APPCh. 15 - Prob. 70APPCh. 15 - Prob. 71APPCh. 15 - In an acidic dry-cell battery, the following...Ch. 15 - Steel bolts made for sailboats are coated with...Ch. 15 - Copper cooking pans are stainless steel pans...Ch. 15 - Prob. 75CPCh. 15 - Prob. 76CPCh. 15 - Prob. 77CPCh. 15 - The following problems are related to the topics...Ch. 15 - The following problems are related to the topics...Ch. 15 - The following problems are related to the topics...Ch. 15 - Prob. 81CPCh. 15 - Prob. 82CPCh. 15 - Prob. 83CPCh. 15 - Prob. 84CPCh. 15 - Prob. 85CPCh. 15 - Prob. 86CPCh. 15 - Prob. 87CPCh. 15 - Prob. 88CP
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