SOLUTION MANUAL FOR INORGANIC
CHEMISTRY 5TH EDITION 2018 BY
CATHERINE E. HOUSECROFT & ALAN G.
SHARPE 29 CHAPTERS UPDATED
, TABLE OF CONTENT
1. Basic concepts: atoms
2. Basic concepts: molecules
3. Introduction to molecular symmetry
4. Experimental techniques
5. Bonding in polyatomic molecules
6. Structures and energetics of metallic and ionic solids
7. Acids, bases and ions in aqueous solution
8. Reduction and oxidation
9. Non-aqueous media
10.Hydrogen
11.Group 1: the alkali metals
12.The group 2 metals
13.The group 13 elements
14.The group 14 elements
15.The group 15 elements
16.The group 16 elements
17.The group 17 elements
18.The group 18 elements
19.d-Block metal chemistry: general considerations
20.d-Block metal chemistry: coordination complexes
21.d-Block metal chemistry: the first row metals
22.d-Block metal chemistry: the heavier metals
23.Organometallic compounds of s- and p-block elements
24.Organometallic compounds of d-block elements
25.Catalysis and some industrial processes
26.d-Block metal complexes: reaction mechanisms
27.The f-block metals: lanthanoids and actinoids
28.Inorganic materials and nanotechnology
29.The trace metals of life
,CHAPTER 1: BASIC CONCEPTS: ATOMS
This chapter introduces atomic structure, including protons, neutrons, electrons,
isotopes, atomic mass, and electron configuration. It explains quantum theory,
atomic orbitals, periodic trends, ionization energy, and electron affinity.
Understanding atomic behavior underpins bonding, reactivity, and periodic
properties, forming the foundation for interpreting inorganic chemical structure,
stability, and material properties.
1. Which subatomic particle primarily determines an element’s identity?
A. Neutron
B. Electron
C. Proton
D. Positron
- CORRECT ANSWER - C
Rationale: The number of protons (atomic number) defines an element.
Neutrons affect isotopes, electrons affect charge and bonding, and
positrons are not components of normal atomic structure.
2. An isotope of chlorine contains 17 protons and 20 neutrons. What is its
mass number?
A. 17
B. 20
C. 37
D. 3
- CORRECT ANSWER - C
Rationale: Mass number equals protons plus neutrons (17 + 20 = 37).
Atomic number is protons only; electrons do not contribute significantly
to mass.
3. Which statement best describes atomic orbitals?
A. Fixed circular electron paths
B. Regions of high electron probability
C. Locations of paired electrons only
D. Areas containing neutrons
- CORRECT ANSWER - B
Rationale: Orbitals represent probability distributions derived from
quantum mechanics. They are not fixed paths, nor do they contain
neutrons or exclusively paired electrons.
4. What is the maximum number of electrons in a p subshell?
A. 2
B. 4
C. 6
D. 8
, - CORRECT ANSWER - C
Rationale: A p subshell contains three orbitals, each holding two
electrons, totaling six. s holds two; d holds ten.
5. Which quantum number describes orbital shape?
A. n
B. l
C. m_l
D. m_s
- CORRECT ANSWER - B
Rationale: The azimuthal quantum number (l) determines subshell shape
(s, p, d, f). n indicates energy level, m_l orientation, and m_s spin.
6. Across a period, atomic radius generally:
A. Increases
B. Decreases
C. Remains constant
D. Doubles
- CORRECT ANSWER - B
Rationale: Increasing nuclear charge pulls electrons closer, decreasing
radius. Shielding does not significantly increase across a period.
7. Which element has the highest first ionization energy in Period 2?
A. Lithium
B. Carbon
C. Oxygen
D. Neon
- CORRECT ANSWER - D
Rationale: Neon has a full valence shell, requiring the most energy to
remove an electron. Ionization energy increases across a period.
8. Electron affinity generally becomes more negative across a period
because:
A. Nuclear charge increases
B. Atomic mass increases
C. Neutrons increase
D. Orbitals decrease
- CORRECT ANSWER - A
Rationale: Increasing effective nuclear charge attracts added electrons
more strongly, releasing more energy. Mass and neutron number are not
primary factors.
9. Which electron configuration represents a ground state for oxygen?
A. 1s²2s²2p⁴
B. 1s²2s²2p⁶
C. 1s²2s²2p³
D. 1s²2p⁴
CHEMISTRY 5TH EDITION 2018 BY
CATHERINE E. HOUSECROFT & ALAN G.
SHARPE 29 CHAPTERS UPDATED
, TABLE OF CONTENT
1. Basic concepts: atoms
2. Basic concepts: molecules
3. Introduction to molecular symmetry
4. Experimental techniques
5. Bonding in polyatomic molecules
6. Structures and energetics of metallic and ionic solids
7. Acids, bases and ions in aqueous solution
8. Reduction and oxidation
9. Non-aqueous media
10.Hydrogen
11.Group 1: the alkali metals
12.The group 2 metals
13.The group 13 elements
14.The group 14 elements
15.The group 15 elements
16.The group 16 elements
17.The group 17 elements
18.The group 18 elements
19.d-Block metal chemistry: general considerations
20.d-Block metal chemistry: coordination complexes
21.d-Block metal chemistry: the first row metals
22.d-Block metal chemistry: the heavier metals
23.Organometallic compounds of s- and p-block elements
24.Organometallic compounds of d-block elements
25.Catalysis and some industrial processes
26.d-Block metal complexes: reaction mechanisms
27.The f-block metals: lanthanoids and actinoids
28.Inorganic materials and nanotechnology
29.The trace metals of life
,CHAPTER 1: BASIC CONCEPTS: ATOMS
This chapter introduces atomic structure, including protons, neutrons, electrons,
isotopes, atomic mass, and electron configuration. It explains quantum theory,
atomic orbitals, periodic trends, ionization energy, and electron affinity.
Understanding atomic behavior underpins bonding, reactivity, and periodic
properties, forming the foundation for interpreting inorganic chemical structure,
stability, and material properties.
1. Which subatomic particle primarily determines an element’s identity?
A. Neutron
B. Electron
C. Proton
D. Positron
- CORRECT ANSWER - C
Rationale: The number of protons (atomic number) defines an element.
Neutrons affect isotopes, electrons affect charge and bonding, and
positrons are not components of normal atomic structure.
2. An isotope of chlorine contains 17 protons and 20 neutrons. What is its
mass number?
A. 17
B. 20
C. 37
D. 3
- CORRECT ANSWER - C
Rationale: Mass number equals protons plus neutrons (17 + 20 = 37).
Atomic number is protons only; electrons do not contribute significantly
to mass.
3. Which statement best describes atomic orbitals?
A. Fixed circular electron paths
B. Regions of high electron probability
C. Locations of paired electrons only
D. Areas containing neutrons
- CORRECT ANSWER - B
Rationale: Orbitals represent probability distributions derived from
quantum mechanics. They are not fixed paths, nor do they contain
neutrons or exclusively paired electrons.
4. What is the maximum number of electrons in a p subshell?
A. 2
B. 4
C. 6
D. 8
, - CORRECT ANSWER - C
Rationale: A p subshell contains three orbitals, each holding two
electrons, totaling six. s holds two; d holds ten.
5. Which quantum number describes orbital shape?
A. n
B. l
C. m_l
D. m_s
- CORRECT ANSWER - B
Rationale: The azimuthal quantum number (l) determines subshell shape
(s, p, d, f). n indicates energy level, m_l orientation, and m_s spin.
6. Across a period, atomic radius generally:
A. Increases
B. Decreases
C. Remains constant
D. Doubles
- CORRECT ANSWER - B
Rationale: Increasing nuclear charge pulls electrons closer, decreasing
radius. Shielding does not significantly increase across a period.
7. Which element has the highest first ionization energy in Period 2?
A. Lithium
B. Carbon
C. Oxygen
D. Neon
- CORRECT ANSWER - D
Rationale: Neon has a full valence shell, requiring the most energy to
remove an electron. Ionization energy increases across a period.
8. Electron affinity generally becomes more negative across a period
because:
A. Nuclear charge increases
B. Atomic mass increases
C. Neutrons increase
D. Orbitals decrease
- CORRECT ANSWER - A
Rationale: Increasing effective nuclear charge attracts added electrons
more strongly, releasing more energy. Mass and neutron number are not
primary factors.
9. Which electron configuration represents a ground state for oxygen?
A. 1s²2s²2p⁴
B. 1s²2s²2p⁶
C. 1s²2s²2p³
D. 1s²2p⁴
