PX0311-0709
____
1. What is the wavelength of a photon having a frequency of 4.50  10 14 Hz? (
)
A) 667 nm
B) 1.50  10 3 nm
C) 4.42  10 31 nm
D) 0.0895 nm
E) 2.98  10 10 nm
____
2. When a particular metal is illuminated with photons, one electron is observed for each absorbed
photon. What effect would decreasing the wavelength and number of photons have on the
electrons leaving the surface?
A) There would be more electrons leaving the surface.
B) They would have higher kinetic energy.
C) The electron velocity would be lower.
D) The kinetic energy of the electrons would be lower.
E) Two photons might be required to eject the electrons.
____
3. In Bohr's atomic theory, when an electron moves from one energy level to another energy level
more distant from the nucleus,
A) energy is absorbed.
B) light is emitted.
C) energy is emitted.
D) no change in energy occurs.
E) none of these
____
4. When an electron in an atom makes a transition from n = 6 to n = 4, which of the following
statements is/are correct?
I.
II.
III.
IV.
V.
A)
B)
C)
D)
E)
____
Energy is emitted.
Energy is absorbed.
The electron loses energy.
The electron gains energy.
The electron cannot make this transition.
I and III
I and IV
II and IV
II and III
III
5. Which of the following statements concerning quantum mechanics is/are true?
1.
The behavior of submicroscopic particles can sometimes be described as
waves.
,
2.
3.
A)
B)
C)
D)
E)
Quantum mechanics limits us to making statistical statements about the
location of an electron in an atom.
The uncertainty principle is important only for particles of very small mass,
such as the electron.
1 only
2 only
3 only
2 and 3
1, 2, and 3
____
6. Which of the following statements is a valid conclusion from the Heisenberg uncertainty principle?
A) The square of the wave function is proportional to the probability of finding a
particle in space.
B) Particles can exhibit wavelike behavior.
C) The orbits proposed by Bohr’s model of the atom are correct.
D) An electron in a 2p orbital is always closer to the nucleus than an electron in a 3p
orbital.
E) The act of measuring a particle's position changes its momentum, and vice versa.
____
7. Which of the following sets of quantum numbers (n, l, ml, ms) is not permissible?
A) 3 3 –3 + 1
2
B) 2 1 –1 + 1
2
C) 1 0 0 +
2
D) 3 2 –2 – 1
2
E) 4 0 0 – 1
1
2
____
8. Which of the following is a representation of a 3dxz orbital?
A)
B)
C)
D)
E)
____
9. Which of the following statements is incorrect?
A) Stern and Gerlach discovered electron spin by passing silver atoms through a
magnetic field.
B) Hund’s rule states that electrons are placed in the orbitals of a subshell in such a
way as to give a maximum number of unpaired electrons.
C) The Pauli exclusion principle states that each electron in an atom must have its
own unique set of quantum numbers.
D) Valence electrons consist of those electrons not contained within a noble-gas core
or a pseudo-noble-gas core.
E) The building-up principle states that electrons are added to atoms in order of
increasing principal quantum number.
____
10. Which of the following electron configurations represents an excited state of the indicated atom?
A) Ne: 1s2 2s2 2p6
B) N: 1s2 2s2 2p3
C) P: 1s2 2s2 2p6 3s2 3p2 4s1
D) Na: 1s2 2s2 2p6 3s2 3p2 3s1
E) He: 1s2
____
11. The ground-state valence-shell configuration of a particular atom is
which this atom belongs is a
A) noble gas.
B) inner transition element.
C) p-block main-group element.
D) transition element.
E) s-block main-group element.
____
12. Which of the following statements is incorrect?
A) A p-block main-group element belonging to period n has a completely filled
(n – 1)d subshell.
B) All noble gases have completely filled shells.
C) All s-block main-group elements have only one or two valence electrons.
D) Carbon and silicon have the same number of valence electrons.
E) All elements in the n = 4 period have a partially or completely filled n = 4 shell.
. The element to
____
13. Which of the following statements is true concerning the electron configuration [Ne]3s13p1?
A) It may represent a ground-state electron configuration of a Al+ cation.
B) It may represent an excited-state electron configuration of a Mg atom.
C) It may represent an excited-state electron configuration of a Ne– anion.
D) It may represent a ground-state electron configuration of a Mg+ cation.
E) It may represent a ground-state electron configuration of a Na+ cation.
____
14. An element that has the same ground state valence-shell electron configuration as indium is
A) boron.
B) silicon.
C) krypton.
D) lithium.
E) barium.
____
15. An atom of which of the following elements is not diamagnetic in the ground state?
A) Ca
B) Rn
C) All are diamagnetic.
D) Cd
E) Pt
____
16. The ground-state electron configuration of a
A) paramagnetic with four unpaired electrons.
B) diamagnetic.
C) paramagnetic with one unpaired electron.
D) paramagnetic with five unpaired electrons.
E) paramagnetic with three unpaired electrons.
____
17. Which of the following atoms is paramagnetic in its ground state?
A) tin (Sn)
B) barium (ba)
C) cadmium (Cd)
D) ytterbium (Yb)
E) argon (Ar)
____
18. Which of the following species would be expected to have chemical properties most similar to
those of the nitrogen atom?
A) nitride ion
B) nitrite ion
C) phosphate ion
D) phosphide ion
E) phosphorus atom
____
19. In general, atomic radii
A) decrease from left to right in a period and increase down a group.
B) increase from left to right in a period and decrease down a group.
C) do not change across a period or a group.
D) decrease from left to right and decrease down a group.
. Therefore,
is
E) increase from left to right in a period and increase down a group.
____
20. An atom of which of the following elements has the largest atomic radius?
A) Cl
B) P
C) Na
D) S
E) Si
____
21. An atom of which of the following elements has the largest atomic radius?
A) Ge
B) K
C) Cl
D) Ca
E) As
____
22. Below are data on the first four ionization energies for a fictitious element X.
First ionization energy = 500 kJ/mol
Second ionization energy = 2000 kJ/mol
Third ionization energy = 3500 kJ/mol
Fourth ionization energy = 25000 kJ/mol
From the data, which of the following statements is incorrect?
A) The third ionization energy is greater than the second ionization energy because
X2+ has a bigger charge than X+.
B) X could belong to Group IIIA.
C) X could belong to Group IIIB.
D) X could belong to group VA.
E) The fourth ionization energy is much greater than the third ionization energy
because X3+ consists of a noble-gas core or a pseudo-noble-gas core.
____
23. An atom of which of the following elements has the smallest first ionization energy?
A) Sn
B) Pb
C) Ge
D) C
E) Si
____
24. The change in energy for which of the following processes corresponds to the electron affinity of
iodine?
A)
B)
C)
D)
E)
____
25. Which element forms the most acidic oxide?
A)
B)
C)
D)
E)
B
Tl
Al
In
Ga
____
26. A few atoms of the new element 113 were created in 2004 by a team of Russian and American
scientists. It has been given the temporary name "ununtrium" and the temporary symbol "Uut."
Based on ununtrium's position on the periodic table, what type of oxide(s) should it form?
A) Ununtrium should form a basic oxide with the formula Uut2O3.
B) Ununtrium should form an amphoteric oxide with the formula UutO.
C) Ununtrium should form an acidic oxide with the formula Uut2O3.
D) Ununtrium should form two acidic oxides having the formulas Uut2O and Uut2O3.
E) Ununtrium should form two basic oxides having the formulas Uut2O and Uut2O3.
____
27. The element antimony is in the same group as phosphorus. Which of the following is the formula
of antimonous acid?
A)
B)
C)
D)
E)
____
28. When the cations Na+, K+, Rb+, Cs+ are combined with chloride ion in the gas phase to form ion
pairs, which pair formation releases the greatest amount of energy?
A) KCl
B) All release the same amount of energy.
C) RbCl
D) NaCl
E) CsCl
____
29. Which of the following statements concerning lattice energy is false?
A) MgO has a larger lattice energy than NaF.
B) The lattice energy for a solid with 2+ and 2– ions should be two times that for a
solid with 1+ and 1– ions.
C) MgO has a larger lattice energy than LiF.
D) Lattice energy is often defined as the change in energy that occurs when an ionic
solid is separated into isolated ions in the gas phase.
E) All of these are true.
____
30. Which of the following compounds would be expected to have the lowest melting point?
A) AlF3
B) RbF
C) NaF
D) MgF2
E) CaF2
____
31. Which of the following is the Lewis dot structure for the rubidium ion?
A)
B)
C)
D)
E)
____
32. All of the following species have ground-state noble-gas electron configurations except
A) Ge4+
B) K+
C) Kr
D) I–
E) P3–
____
33. All of the following species are isoelectronic except
A) S2–
B) K+
C) Na+
D) Ar
E) Cl–
____
34. All of the following species are isoelectronic except
A) O–
B) Ne
C) N3–
D) Mg2+
E) F–
____
35. For which of the following pairs of species is the difference in radius the greatest?
A) C and F
B) K+ and Br–
C) Li+ and I–
D) Na and Mg
E) O2– and F–
____
36. Which of the following is the best explanation for a covalent bond?
A)
B)
C)
D)
E)
electrons simultaneously attracted by more than one nucleus
an interaction between outer electrons
the overlapping of unoccupied orbitals of two or more atoms
the overlapping of two electron-filled orbitals having different energies
a positive ion attracting negative ions
____
37. During the formation of a chemical bond between two hydrogen atoms, which of the following
statements is always true?
A) Energy is released during the formation of the bond.
B) A polar covalent bond is formed.
C) Electrons always are between the nuclei of the atoms.
D) One of the hydrogen atoms is ionized.
E) Resonance stabilizes the bond.
____
38. An atom of which of the following elements has the highest electronegativity?
A) K
B) As
C) Ba
D) Si
E) Br
____
39. The concept of resonance describes molecular structures
A) that have several different geometric arrangements.
B) that have delocalized bonding.
C) that are formed from hybridized orbitals.
D) that have different molecular formulas.
E) that have electrons resonating.
____
40. All the following statements about resonance are true except
A) A single Lewis formula does not provide an adequate representation of the
bonding.
B) Resonance describes a more stable situation than does any one contributing
resonance formula.
C) Resonance describes the oscillation and vibration of electrons.
D) The contributing resonance formulas differ only in the arrangement of the
electrons.
E) Resonance describes the bonding as intermediate between the contributing
resonance formulas.
____
41. Which one of the following species is best described by writing three equivalent Lewis formulas?
A) SO3
B) SF4
C) SO42–
D) SO32–
E) SOF4
____
42. For each of the following species except ____, the electronic structure may be adequately
described by two resonance formulas.
A)
B)
C)
D)
E)
____
O3
SO32–
NO2–
C6H6
SO2
43. Which of the following are two appropriate resonance formulas for the acetate ion, CH3CO2–?
A)
B)
C)
D)
E)
____
44. The Lewis formula of which species does not represent an exception to the octet rule?
A) SiF5B) SCl6
C) SF4
D) BF3
E) CF3____
45. Which of the following has an incomplete octet in its Lewis structure?
A) SO2
B) F2
C) NO2
D) ICl
E) CO2
____
46. Which of the following Lewis structures best describes BF3?
A)
B)
C)
D)
E)
____
47. As the number of bonds between two carbon atoms increases, which of the following decrease(s)?
A) only the bond length
B) only the bond energy
C) only the number of electrons between the carbon atoms
D) all of these
E) none of these
____
48. Which of the following species has the shortest bond distance?
A) F2
B) Cl2
C) Br2
D) I2
E) H2
____
49. Consider the reaction
2HCl(g) ® H2(g) + Cl2(g); DH = 185 kJ
Which of the following statements is false?
A) The reaction is endothermic.
B) HCl(g) has a negative enthalpy of formation.
C) The products have more enthalpy than the reactants.
D) The HCl bond is longer than either the H2 bond or the Cl2 bond.
E) The bond order of each of the products is one.
____
50. Using bond-energy data, what is DH° for the following reaction?
CH4(g) + 2Cl2(g) ® CCl4(g) + 2H2(g)
Bond
C-H
H-H
Cl-Cl
C-Cl
A)
B)
C)
D)
E)
Bond Energy (kJ/mol)
413
432
242
328
–40 kJ
–150 kJ
40 kJ
1415 kJ
150 kJ
PX0311-0709
Answer Section
1. ANS:
OBJ:
TOP:
MSC:
2. ANS:
OBJ:
KEY:
3. ANS:
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TOP:
MSC:
4. ANS:
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TOP:
5. ANS:
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6. ANS:
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TOP:
KEY:
7. ANS:
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MSC:
8. ANS:
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TOP:
9. ANS:
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KEY:
10. ANS:
OBJ:
KEY:
11. ANS:
OBJ:
TOP:
KEY:
12. ANS:
OBJ:
TOP:
KEY:
13. ANS:
A
PTS: 1
DIF: easy
REF: 7.1
Relate the wavelength, frequency, and speed of light. (Examples 7.1 and 7.2)
atomic theory | light
KEY: electromagnetic radiation
general chemistry
B
PTS: 1
DIF: difficult
REF: 7.2
Describe the photoelectric effect.
TOP: atomic theory | light
quantum effects and photons | photoelectric effect
MSC: general chemistry
A
PTS: 1
DIF: easy
REF: 7.3
State the postulates of Bohr's theory of the hydrogen atom.
atomic theory | light
KEY: Bohr theory | Bohr's postulates
general chemistry
A
PTS: 1
DIF: easy
REF: 7.3
Relate the energy of a photon to the associated energy levels of an atom.
atomic theory | light
E
PTS: 1
DIF: easy
REF: 7.4
Define Quantum mechanics.
TOP: atomic theory | quantum mechanics
E
PTS: 1
DIF: moderate
REF: 7.4
State Heisenberg's uncertainty principle.
atomic theory | quantum mechanics
wave functions | Heisenberg's uncertainty principle
MSC: general chemistry
A
PTS: 1
DIF: easy
REF: 7.5
Apply the rules for quantum numbers. (Example 7.6)
atomic theory | quantum mechanics
KEY: quantum numbers
general chemistry
A
PTS: 1
DIF: easy
REF: 7.5
Describe the shapes of s, p, and d orbitals.
atomic theory | quantum mechanics
E
PTS: 1
DIF: easy
REF: 8.2
Define building-up principle.
TOP: atomic theory | electronic structure of atoms
electron configuration | aufbau principle
MSC: general chemistry
C
PTS: 1
DIF: moderate
REF: 8.2
Define building-up principle.
TOP: atomic theory | electronic structure of atoms
electron configuration | aufbau principle
MSC: general chemistry
C
PTS: 1
DIF: easy
REF: 8.2
Define main-group element and (d-block and f-block) transition element.
atomic theory | electronic structure of atoms
electron configuration and the periodic table
MSC: general chemistry
E
PTS: 1
DIF: moderate
REF: 8.2
Define main-group element and (d-block and f-block) transition element.
atomic theory | electronic structure of atoms
electron configuration and the periodic table
MSC: general chemistry
B
PTS: 1
DIF: difficult
REF: 8.3
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
OBJ: Determine the configuration of an atom using the building-up principle. (Example 8.2)
TOP: atomic theory | electronic structure of atoms
KEY: electron configuration and the periodic table | writing electron configurations using the
periodic table
MSC: general chemistry
ANS: A
PTS: 1
DIF: easy
REF: 8.3
OBJ: Determine the configuration of an atom using the period and group numbers. (Example
8.3)
TOP: atomic theory | electronic structure of atoms
ANS: E
PTS: 1
DIF: easy
REF: 8.4
OBJ: Define paramagnetic substance and diamagnetic substance.
TOP: atomic theory | electronic structure of atoms
KEY: electron configuration | magnetic properties of atoms
MSC: general chemistry
ANS: A
PTS: 1
DIF: easy
REF: 8.4
OBJ: Define paramagnetic substance and diamagnetic substance.
TOP: atomic theory | electronic structure of atoms
KEY: electron configuration | magnetic properties of atoms
MSC: general chemistry
ANS: A
PTS: 1
DIF: easy
REF: 8.4
OBJ: Define paramagnetic substance and diamagnetic substance.
TOP: atomic theory | electronic structure of atoms
ANS: E
PTS: 1
DIF: easy
REF: 8.6
OBJ: State the periodic law.
TOP: atomic theory | periodicity of the elements
KEY: periodicity in main group elements | group VA elements MSC: general chemistry
ANS: A
PTS: 1
DIF: easy
REF: 8.6
OBJ: State the general periodic trends in size of atomic radii.
TOP: atomic theory | periodicity of the elements
KEY: periodic properties | atomic radius MSC: general chemistry
ANS: C
PTS: 1
DIF: easy
REF: 8.6
OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5)
TOP: atomic theory | periodicity of the elements
KEY: periodic properties | atomic radius MSC: general chemistry
ANS: B
PTS: 1
DIF: moderate
REF: 8.6
OBJ: Determine relative atomic sizes from periodic trends. (Example 8.5)
TOP: atomic theory | periodicity of the elements
KEY: periodic properties | atomic radius MSC: general chemistry
ANS: D
PTS: 1
DIF: difficult
REF: 8.6
OBJ: State the general periodic trends in ionization energy.
TOP: atomic theory | periodicity of the elements
KEY: periodic properties | ionization energy
MSC: general chemistry
ANS: B
PTS: 1
DIF: easy
REF: 8.6
OBJ: Determine relative ionization energies from periodic trends. (Example 8.6)
TOP: atomic theory | periodicity of the elements
KEY: periodic properties | ionization energy
MSC: general chemistry
ANS: B
PTS: 1
DIF: easy
REF: 8.6
OBJ: Define electron affinity.
TOP: atomic theory | periodicity of the elements
KEY: periodic properties | electron affinity
MSC: general chemistry
25. ANS: A
PTS: 1
DIF: easy
REF: 8.7
OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going through any
main group of elements.
TOP: atomic theory | periodicity of the elements
KEY: periodicity in main group elements | group IIIA elements MSC: general chemistry
26. ANS: E
PTS: 1
DIF: easy
REF: 8.7
OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going through any
main group of elements.
TOP: atomic theory | periodicity of the elements
KEY: periodicity in main group elements | group IIIA elements MSC: general chemistry
27. ANS: D
PTS: 1
DIF: moderate
REF: 8.7
OBJ: Describe the change in metallic/nonmetallic character (or reactivities) in going through any
main group of elements.
TOP: atomic theory | periodicity of the elements
KEY: periodicity in main group elements | group VA elements MSC: general chemistry
28. ANS: D
PTS: 1
DIF: difficult
REF: 9.1
OBJ: Describe the energetics of ionic bonding.
TOP: bonding | ionic bonding
KEY: properties of ionic substance
MSC: general chemistry
29. ANS: B
PTS: 1
DIF: moderate
REF: 9.1
OBJ: Define lattice energy.
TOP: bonding | ionic bonding
KEY: Born-Haber cycle
MSC: general chemistry
30. ANS: B
PTS: 1
DIF: easy
REF: 9.1
OBJ: Describe some general properties of ionic substances.
TOP: bonding | ionic bonding
KEY: properties of ionic substance
MSC: general chemistry
31. ANS: E
PTS: 1
DIF: easy
REF: 9.2
OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2)
TOP: bonding | ionic bonding
KEY: Lewis electron-dot symbol
MSC: general chemistry
32. ANS: A
PTS: 1
DIF: easy
REF: 9.2
OBJ: Write the electron configuration and Lewis symbol for a main-group ion. (Example 9.2)
TOP: bonding | ionic bonding
KEY: electron configurations of ions | ions of the main-group elements
MSC: general chemistry
33. ANS: C
PTS: 1
DIF: easy
REF: 9.3
OBJ: Define isoelectronic ions.
TOP: bonding | ionic bonding
MSC: general chemistry
34. ANS: A
PTS: 1
DIF: easy
REF: 9.3
OBJ: Define isoelectronic ions.
TOP: bonding | ionic bonding
MSC: general chemistry
35. ANS: C
PTS: 1
DIF: moderate
REF: 9.3
OBJ: Use periodic trends to obtain relative ionic radii. (Example 9.4)
TOP: bonding | ionic bonding
KEY: ionic radii
MSC: general chemistry
36. ANS: A
PTS: 1
DIF: moderate
REF: 9.4
OBJ: Describe the formation of a covalent bond between two atoms.
TOP: bonding | covalent bonding
MSC: general chemistry
37. ANS: A
PTS: 1
DIF: moderate
REF: 9.4
OBJ: Describe the formation of a covalent bond between two atoms.
TOP: bonding | covalent bonding
MSC: general chemistry
38. ANS:
OBJ:
TOP:
MSC:
39. ANS:
OBJ:
KEY:
40. ANS:
OBJ:
KEY:
41. ANS:
OBJ:
TOP:
MSC:
42. ANS:
OBJ:
TOP:
MSC:
43. ANS:
OBJ:
TOP:
MSC:
44. ANS:
OBJ:
TOP:
45. ANS:
OBJ:
TOP:
46. ANS:
OBJ:
TOP:
MSC:
47. ANS:
OBJ:
TOP:
48. ANS:
OBJ:
TOP:
49. ANS:
OBJ:
KEY:
50. ANS:
OBJ:
TOP:
E
PTS: 1
DIF: easy
REF: 9.5
State the general periodic trends in the electronegativity.
bonding | covalent bonding
KEY: electronegativity
general chemistry
B
PTS: 1
DIF: easy
REF: 9.7
Define resonance description.
TOP: bonding | covalent bonding
resonance
MSC: general chemistry
C
PTS: 1
DIF: easy
REF: 9.7
Define resonance description.
TOP: bonding | covalent bonding
resonance
MSC: general chemistry
A
PTS: 1
DIF: difficult
REF: 9.7
Write resonance formulas. (Example 9.9)
bonding | covalent bonding
KEY: resonance | delocalization
general chemistry
B
PTS: 1
DIF: easy
REF: 9.7
Write resonance formulas. (Example 9.9)
bonding | covalent bonding
KEY: resonance | delocalization
general chemistry
A
PTS: 1
DIF: easy
REF: 9.7
Write resonance formulas. (Example 9.9)
bonding | covalent bonding
KEY: resonance | delocalization
general chemistry
E
PTS: 1
DIF: easy
REF: 9.8
Write Lewis formulas (exceptions to the octet rule). (Example 9.10)
bonding | covalent bonding
C
PTS: 1
DIF: moderate
REF: 9.8
Write Lewis formulas (exceptions to the octet rule). (Example 9.10)
bonding | covalent bonding
C
PTS: 1
DIF: easy
REF: 9.8
Note exceptions to the octet rule in Groups IIA and Group IIIA elements.
bonding | covalent bonding
KEY: exceptions to the octet rule
general chemistry
A
PTS: 1
DIF: easy
REF: 9.10
Explain how bond order and bond length are related. (Example 9.12)
bonding | covalent bonding
KEY: bond length MSC: general chemistry
E
PTS: 1
DIF: moderate
REF: 9.10
Explain how bond order and bond length are related. (Example 9.12)
bonding | covalent bonding
KEY: bond length MSC: general chemistry
D
PTS: 1
DIF: easy
REF: 9.11
Define bond energy.
TOP: bonding | covalent bonding
bond energy MSC: general chemistry
A
PTS: 1
DIF: easy
REF: 9.11
Estimate delta H from bond energies. (Example 9.13)
bonding | covalent bonding
KEY: bond energy MSC: general chemistry