Chem I Review Part 2
Student: ___________________________________________________________________________
1.
What is the wavelength of radiation that has a frequency of 6.912 × 1014 s-1?
A. 1.447 × 10-15 nm
B. 4.337 × 102 nm
C. 2.304 × 106 nm
D. 2.074 × 1023 nm
E. 4.337 × 10-7 nm
2.
What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m?
A. 2.70 × 10-43 J
B. 5.43 × 10-33 J
C. 1.63 × 10-24 J
D. 4.07 × 10-10 J
E. 2.46 × 109 J
3.
Complete this sentence: Atoms emit visible and ultraviolet light
A. as electrons jump from lower energy levels to higher levels.
B. as the atoms condense from a gas to a liquid.
C. as electrons jump from higher energy levels to lower levels.
D. as they are heated and the solid melts to form a liquid.
E. as the electrons move about the atom within an orbit.
4.
Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n =
4 principal energy level. Recall that the energy levels of the H atom are given by
En = -2.18 × 10-18 J(1/n2)
A. 2.07 × 10-29 J
B. 2.19 × 105 J
C. 2.04 × 10-18 J
D. 3.27 × 10-17 J
E. 2.25 × 10-18 J
5.
In an electron microscope, electrons are accelerated to great velocities. Calculate the wavelength of an electron traveling with a
velocity of 7.0 × 103 kilometers per second. The mass of an electron is 9.1 × 10-28 g.
A. 1.0 × 10-13 m
B. 1.0 × 10-7 m
C. 1.0 m
D. 1.0 × 10-10 m
6.
A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution.
If ΔH for the reaction Cl2(g) → 2Cl(g) is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine
atoms in solution?
A. 246.3 nm
B. 465.2 nm
C. 349.3 nm
D. 698.6 nm
E. 492.6 nm
7.
Which one of the following sets of quantum numbers is not possible?
A. Row 1
B. Row 2
C. Row 3
D. Row 4
E. Row 5
8.
Which one of the following sets of quantum numbers is not possible?
A. Row 1
B. Row 2
C. Row 3
D. Row 4
E. Row 5
9.
What is the maximum number of electrons in a atom that can have the following set of quantum numbers?
3
ml = -2
ms = +1/2
A. 0
B. 1
C. 2
D. 6
E. 10
n=4
10. A possible set of quantum numbers for the last electron added to complete an atom of gallium Ga in its ground state is
A. Row 1.
B. Row 2.
C. Row 3.
D. Row 4.
E. Row 5.
11. Electrons in an orbital with l = 3 are in a
A. d orbital.
B. f orbital.
C. g orbital.
D. p orbital.
E. s orbital.
12. The number of orbitals in a d subshell is
A. 1.
B. 2.
C. 3.
D. 5.
E. 7.
13. The maximum number of electrons that can occupy an energy level described by the principal quantum number, n, is
A. n.
B. n +
1.
C. 2n.
D. 2n2.
E. n2.
14. How many orbitals are allowed in a subshell if the angular momentum quantum number for electrons in that subshell is 3?
A. 1
B. 3
C. 5
D. 7
E. 9
15. "No two electrons in an atom can have the same four quantum numbers" is a statement of
A. the Pauli exclusion principle.
B. Bohr's equation.
C. Hund's rule.
D. de Broglie's relation.
E. Dalton's atomic theory.
l=
16. The orbital diagram for a ground-state nitrogen atom is
A.
B.
C.
D.
Row 1.
Row 2.
Row 3.
Row 4.
17.
The orbital diagram for a ground-state oxygen atom is
A. Row 1.
B. Row 2.
C. Row 3.
D. Row 4.
E. Row 5.
18. Which ground-state atom has an electron configuration described by the following orbital diagram?
A. phosphorus
B. nitrogen
C. arsenic
D. vanadium
E. none of these
19. How many unpaired electrons does a ground-state atom of sulfur have?
A. 0
B. 1
C. 2
D. 3
E. 4
20. Which element has the following ground-state electron configuration?
1s22s22p63s2
A. Na
B. Mg
C. Al
D. Si
E. Ne
21. Which element has the following ground-state electron configuration?
[Kr]5s24d105p3
A. Sn
B. Sb
C. Pb
D. Bi
E. Te
22. The electron configuration of a ground-state vanadium atom is
A. [Ar]4s24d3.
B. [Ar]4s24p3.
C. [Ar]4s23d3.
D. [Ar]3d5.
23. The electron configuration of a ground-state copper atom is
A. [Ar]4s24d4.
B. [Ar]4s24p63d3.
C. [Ar]4s23d9.
D. [Ar]3d9.
E. [Ar]4s13d10.
24. How many electrons are there in the 2nd principal energy level (n = 2) of a phosphorus atom?
A. 3
B. 5
C. 6
D. 8
E. 10
25. How many electrons are there in the 3rd principal energy level (n = 3) of a phosphorus atom?
A. 3
B. 5.
C. 6
D. 8
E. 10
26. A ground-state atom of manganese has ___ unpaired electrons and is _____.
A. 0, diamagnetic
B. 2, diamagnetic
C. 3, paramagnetic
D. 5, paramagnetic
E. 7, paramagnetic
27. Which of these choices is the electron configuration of an excited state of an oxygen atom?
A. 1s22s22p4
B. 1s22s22p5
C. 1s22s22p33s1
D. 1s22s22p6
E. 1s22s22p3
28. Which of these ground-state atoms is diamagnetic?
A. Ca
B. As
C. Cu
D. Fe
E. none of these
29. The nineteenth century chemists arranged elements in the periodic table according to increasing
A. atomic number.
B. number of electrons.
C. atomic mass.
D. number of neutrons.
E. nuclear binding energy.
30. The elements in Group 7A are known by what name?
A. transition metals
B. halogens
C. alkali metals
D. alkaline earth metals
E. noble gases
31. The elements in Group 2A are known by what name?
A. transition metals
B. halogens
C. alkali metals
D. alkaline earth metals
E. noble gases
32. The alkali metal elements are found in _______ of the periodic table.
A. Group 1A
B. Group 2A
C. Group 3A
D. Period 7
E. Period 1
33. Which one of these elements is a transition element?
A. Sr
B. Pb
C. As
D. Fe
E. H
34. The general electron configuration for atoms of all elements in Group 5A is
A. ns2np6.
B. ns2np5.
C. ns2np4.
D. ns2np3.
E. ns2np1.
35. The general electron configuration for noble gas atoms is
A. ns2np6.
B. ns2np5.
C. ns2np4.
D. ns2np3.
E. ns2.
36. Consider the element with the electron configuration [Kr]5s24d7. This element is
A. a representative element.
B. a transition metal.
C. a nonmetal.
D. an actinide element.
E. a noble gas.
37. Consider the element with the electron configuration [Xe]6s24f7. This element is
A. a representative element.
B. a lanthanide element.
C. a nonmetal.
D. an actinide element .
E. a noble gas.
38. How many valence electrons does a carbon atom have?
A. 1
B. 2
C. 3
D. 4
E. 6
39. How many electrons are in the 4p orbitals of selenium?
A. 0
B. 2
C. 4
D. 5
E. 6
40. How many electrons are in the 4p orbitals of vanadium?
A. 0
B. 2
C. 4
D. 5
E. 6
41. What is the charge on the monatomic ion that calcium forms in its compounds?
A. +2
B. +1
C. -1
D. -2
E. -3
42. What is the charge on the monatomic ion of nitrogen, the nitride ion?
A. +2
B. +1
C. -1
D. -2
E. -3
43. (4) [Ar]4s23d104p4
(3) [Ar]4s23d104p3
(2) 1s22s22p5
Which two electron configurations represent elements that would have similar chemical properties?
(1) 1s22s22p4
A. (1) and (2)
B. (1) and (3)
C. (1) and (4)
D. (2) and (4)
E. (2) and (3)
44. Which of these species make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+?
A. Ca2+ and Fe3+
B. O2- and F
C. F and ClD. Cl- and Ca2+
E. none of these
45. Which ion is isoelectronic with Ar?
A. Fe2+
B. FC. BrD. Ga3+
E. Ca2+
46. Which of these choices is the electron configuration for the aluminum ion?
A. 1s22s22p63s2
B. 1s22s22p63s23p2
C. 1s22s22p63s23p1
D. 1s22s22p6
E. 1s22s22p63s23p4
47. Which of these choices is the electron configuration of a sulfide ion?
A. [Ne]3s23p4
B. [Ne]
C. [Ne]3s23p1
D. [Ar]
E. [Ne]3s23p2
48. How many 3d electrons does an Fe3+ ion have?
A. 9
B. 6
C. 5
D. 4
E. 3
49. Which of these atoms has the smallest radius?
A. Al
B. P
C. As
D. Te
E. Na
50. Which of these atoms has the largest radius?
A. B
B. Ga
C. Br
D. Si
E. Cl
51. Arrange these ions in order of increasing ionic radius: K+, P3-, S2-, Cl-.
A. Row 1
B. Row 2
C. Row 3
D. Row 4
E. Row 5
52. For which of these reactions is the enthalpy change equal to the third ionization energy of vanadium?
A. V2+(g) → V3+(g) + eB. V3+(g) + e- → V2+(g)
C. V(g) → V3+(g) + 3eD. V2-(g) + e- → V3-(g)
E. V3+(g) → V4+(g) + e53. Which of these elements has the highest first ionization energy?
A. Cs
B. Ga
C. K
D. Bi
E. As
54. Which of these elements has the smallest first ionization energy?
A. Cl
B. Na
C. Be
D. K
E. As
55. Which of these elements will display an unusually large jump in ionization energy values between I3 and I4, its third and
fourth ionization energies?
A. Na
B. Mg
C. Al
D. Si
E. P
56. Which of these elements has the following pattern for its first six ionization energies? (I1 = first ionization energy, I2 = second
ionization energy, etc.)
A. Ca
B. Si
C. Al
D. Se
E. P
57. Which of these elements has the greatest electron affinity (largest positive value)?
A. Mg
B. Al
C. Si
D. P
E. S
58. Which of these elements has the greatest metallic character?
A. Br
B. F
C. Ge
D. Mn
E. Sc
59. If the radius of atom X is greater than the radius of atom Y, then it is also likely that
A. X has a larger electron affinity than Y does.
B. X has a larger effective nuclear charge than Y does.
C. X has greater metallic character than Y does.
D. X has a larger first ionization energy than Y does.
E. X is a poorer conductor of electricity than Y when in the solid state.
60. Which of these compounds is a basic oxide?
A. CO2
B. CaO
C. SO2
D. H2O
E. NO2
61. Which of these compounds is an acidic oxide?
A. P4O10
B. MgO
C. Fe2O3
D. K2O
E. Cr2O3
62. Which of these elements exhibits chemical behavior similar to that of calcium?
A. magnesium
B. sodium
C. sulfur
D. chlorine
E. iron
63. Which of these elements exhibits chemical behavior similar to that of oxygen?
A. magnesium
B. sodium
C. sulfur
D. chlorine
E. iron
F. beryllium
64. Which of these compounds is most likely to be ionic?
A. KF
B. CCl4
C. CS2
D. CO2
E. ICl
65. Which of these compounds is most likely to be ionic?
A. NCl3
B. BaCl2
C. CO
D. SO2
E. SF4
66. Which of these compounds is most likely to be covalent?
A. Rb2S
B. SrCl2
C. CS2
D. CaO
E. MgI2
67. Complete this statement: Coulomb's law states that the magnitude of the force of interaction between two charged bodies
is
A. directly proportional to the product of the charges on the bodies and directly proportional to the distance separating them.
B. directly proportional to the product of the charges on the bodies, and inversely proportional to the square of the distance
separating them.
C. inversely proportional to the charges on the bodies, and directly proportional to the square of the distance separating them.
D. directly proportional to the sum of the charges on the bodies, and inversely proportional to the square of the distance
separating them.
68. The Lewis dot symbol for the S 2- ion is
A.
B.
C.
D.
E.
69. Which of these ionic solids would have the largest lattice energy?
A. NaCl
B. NaF
C. CaBr2
D. CsI
E. CaCl2
70. Which of these solids would have the highest melting point?
A. NaF
B. NaCl
C. NaBr
D. NaI
71. Which of these elements has the greatest electronegativity?
A. Na
B. As
C. Ga
D. Cs
E. Sb
72. Which of these elements is the least electronegative?
A. Sr
B. V
C. Ni
D. P
E. I
73. A polar covalent bond would form in which one of these pairs of atoms?
A.
B.
C.
D.
E.
74. What type of chemical bond holds the atoms together within a water molecule?
A. Ionic bond
B. Nonpolar covalent bond
C. Polar covalent bond
D. Coordinate covalent bond
75. A nonpolar covalent bond (i.e., pure covalent) would form in which of these pairs of atoms?
A.
B.
C.
D.
E.
76. Which of these bonds would have the greatest polarity (i.e., highest percent ionic character)?
A.
B.
C.
D.
E.
77. In which of these pairs of atoms would the bond be the least polar (i.e., lowest percent ionic character)?
A.
B.
C.
D.
E.
78. Classify the
bond in CaCl2 as ionic, polar covalent, or nonpolar covalent.
A. ionic
B. polar covalent
C. nonpolar covalent
79. The electron dot formula for O2 shows
A. a single covalent bond.
B. a double covalent bond.
C. an ionic bond.
D. a total of 8 × 2 = 16 electron dots.
E. a total of 32 electron dots.
80. The number of lone electron pairs in the N2 molecule is ___.
A. 1
B. 2
C. 3
D. 4
E. 5
81. The electron dot structure for AsCl3 shows
A. a total of 84 electron dots.
B. three single bonds and 10 lone pairs.
C. two single bonds, one double bond, and 9 lone pairs.
D. one single bond, two double bonds, and 8 lone pairs.
E. three single bonds and one lone pair.
82. The total number of bonding electrons in a molecule of formaldehyde (H2CO) is
A. 3.
B. 4.
C. 6.
D. 8.
E. 18.
83. The total number of lone pairs in NCl3 is
A. 6.
B. 8.
C. 9.
D. 10.
E. 13.
84. The Lewis structure for CS2 is:
A.
B.
C.
D.
85. Which of these Lewis structures is incorrect?
A.
B.
C.
D.
E.
86. The number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is
A. 1.
B. 2.
C. 3.
D. 4.
E. none of these.
87. The number of resonance structures for the nitrate ion that satisfies the octet rule is
A. 1.
B. 2.
C. 3.
D. 4.
E. none of these.
88. Which of these statements is a useful guideline for the application of formal charges in neutral molecules?
A. A Lewis structure in which there are no formal charges is preferred.
B. Lewis structures with large formal charges (e.g., +2,+3 and/or -2,-3) are preferred.
C. The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms.
89. What is the formal charge on the oxygen atom in N2O (the atomic order is N-N-O)?
A. 0
B. +1
C. -1
D. -2
E. +2
90. In the best Lewis structure for the fulminate ion, CNO-, what is the formal charge on the central nitrogen atom?
A. +2
B. +1
C. 0
D. -1
E. -2
91. For which of these species can you draw two resonance structures?
A. CH2O
B. ClNO2
C. H2O
D. CH4
E. H2S
92. Which of these substances will display an incomplete octet in its Lewis structure?
A. CO2
B. Cl2
C. ICl
D. NO
E. SO2
93. Which of these elements is most likely to exhibit an expanded octet in its compounds?
A. O
B. S
C. Na
D. C
E. N
94. According to the VSEPR theory, the shape of the SO3 molecule is
A. pyramidal.
B. tetrahedral.
C. trigonal planar.
D. distorted tetrahedron (seesaw).
E. square planar.
95. The shape of the SF4 molecule is
A. tetrahedral.
B. trigonal pyramidal.
C. trigonal planar.
D. square planar.
E. distorted tetrahedron (seesaw).
96. Use VSEPR theory to predict the shape of the PCl3 molecule.
A. linear
B. bent
C. trigonal planar
D. trigonal pyramidal
E. tetrahedral
97. The shape of the CS2 molecule is best described as
A. linear.
B. trigonal planar.
C. tetrahedral.
D. bent.
E. trigonal pyramidal.
98. According to the VSEPR theory, the molecular shape of the carbonate ion, CO32 -, is
A. square planar.
B. tetrahedral.
C. pyramidal.
D. trigonal planar.
E. octahedral.
99. The shape of the ClF3 molecule is best described as
A. distorted tetrahedron.
B. trigonal planar.
C. tetrahedral.
D. T-shaped.
E. trigonal pyramidal.
100. According to the VSEPR theory, the molecular shape of SiCl4 is
A. linear.
B. trigonal planar.
C. bent.
D. tetrahedral.
E. trigonal pyramidal.
101. According to VSEPR theory, which one of the following molecules should have a shape that is trigonal bipyramidal?
A. SF4
B. XeF4
C. NF3
D. SF6
E. PF5
102. Which of the following substances is/are bent?
(i) H2S
(ii). CO2
(iii) ClNO
A. only (iii)
B. only (i) and (v)
C. only (i), (iii), and (v)
D. all are bent except for (iv)
E. all are bent except for (ii)
(iv) NH2-
(v) O3
103. The F-S-F bond angles in SF6 are
A. 90° and 180°.
B. 109.5°.
C. 120°.
D. 180°.
E. 90° and 120°.
104. The bond angle in Cl2O is expected to be approximately
A. 90°.
B. 109.5°.
C. 120°.
D. 145°.
E. 180°.
105. The C-N-O bond angle in nitromethane, CH3NO2, is expected to by approximately
A. 60°.
B. 90°.
C. 109.5°.
D. 120°.
E. 180°.
106. Which one of the following molecules is nonpolar?
A. NH3
B. OF2
C. CH3Cl
D. H2O
E. BeCl2
107. Complete this sentence: The PCl5 molecule has
A. nonpolar bonds, and is a nonpolar molecule.
B. nonpolar bonds, but is a polar molecule.
C. polar bonds, and is a polar molecule.
D. polar bonds, but is a nonpolar molecule.
108. Indicate the type of hybrid orbitals used by the central atom in PCl3.
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
109. Indicate the type of hybrid orbitals used by the central atom in SF6.
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
110. What is the hybridization of the As atom in the AsF5 molecule?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
111. What is the hybridization on the central atom in NO3- ?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
112. What is the hybridization of As in the AsF4- ion?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
113. The hybridization of the central nitrogen atom in the molecule N2O is
A. sp.
B. sp2.
C. sp3.
D. sp3d.
E. sp3d2.
114.
The number of pi bonds in the molecule below is
A. 1.
B. 2.
C. 3.
D. 5.
E. 9.
115.
The number of pi bonds in the molecule below is
A. 2.
B. 4.
C. 6.
D. 10.
E. 15.
Chem I Review Part 2 Key
1.
What is the wavelength of radiation that has a frequency of 6.912 × 1014 s-1?
A. 1.447 × 10-15 nm
B. 4.337 × 102 nm
C. 2.304 × 106 nm
D. 2.074 × 1023 nm
E. 4.337 × 10-7 nm
Difficulty: Easy
Raymond - 007 Quantum... #1
2.
What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m?
A. 2.70 × 10-43 J
B. 5.43 × 10-33 J
C. 1.63 × 10-24 J
D. 4.07 × 10-10 J
E. 2.46 × 109 J
Difficulty: Medium
Raymond - 007 Quantum... #5
3.
Complete this sentence: Atoms emit visible and ultraviolet light
A. as electrons jump from lower energy levels to higher levels.
B. as the atoms condense from a gas to a liquid.
C. as electrons jump from higher energy levels to lower levels.
D. as they are heated and the solid melts to form a liquid.
E. as the electrons move about the atom within an orbit.
Difficulty: Easy
Raymond - 007 Quantum... #9
4.
Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the
n = 4 principal energy level. Recall that the energy levels of the H atom are given by
En = -2.18 × 10-18 J(1/n2)
A. 2.07 × 10-29 J
B. 2.19 × 105 J
C. 2.04 × 10-18 J
D. 3.27 × 10-17 J
E. 2.25 × 10-18 J
Difficulty: Medium
Raymond - 007 Quantum... #10
5.
In an electron microscope, electrons are accelerated to great velocities. Calculate the wavelength of an electron traveling
with a velocity of 7.0 × 103 kilometers per second. The mass of an electron is 9.1 × 10-28 g.
A. 1.0 × 10-13 m
B. 1.0 × 10-7 m
C. 1.0 m
D. 1.0 × 10-10 m
Difficulty: Medium
Raymond - 007 Quantum... #16
6.
A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in
solution. If ΔH for the reaction Cl2(g) → 2Cl(g) is 242.8 kJ/mol, what is the longest wavelength of light that will produce
free chlorine atoms in solution?
A. 246.3 nm
B. 465.2 nm
C. 349.3 nm
D. 698.6 nm
E. 492.6 nm
Difficulty: Difficult
Raymond - 007 Quantum... #19
7.
Which one of the following sets of quantum numbers is not possible?
A.
B.
C.
D.
E.
Row 1
Row 2
Row 3
Row 4
Row 5
Difficulty: Medium
Raymond - 007 Quantum... #24
8.
Which one of the following sets of quantum numbers is not possible?
A.
B.
C.
D.
E.
Row 1
Row 2
Row 3
Row 4
Row 5
Difficulty: Medium
Raymond - 007 Quantum... #25
9.
What is the maximum number of electrons in a atom that can have the following set of quantum numbers?
4
l=3
ml = -2
ms = +1/2
A. 0
B. 1
C. 2
D. 6
E. 10
n=
Difficulty: Easy
Raymond - 007 Quantum... #26
10.
A possible set of quantum numbers for the last electron added to complete an atom of gallium Ga in its ground state is
A.
B.
C.
D.
E.
Row 1.
Row 2.
Row 3.
Row 4.
Row 5.
Difficulty: Medium
Raymond - 007 Quantum... #27
11.
Electrons in an orbital with l = 3 are in a
A. d orbital.
B. f orbital.
C. g orbital.
D. p orbital.
E. s orbital.
Difficulty: Easy
Raymond - 007 Quantum... #29
12.
The number of orbitals in a d subshell is
A. 1.
B. 2.
C. 3.
D. 5.
E. 7.
Difficulty: Easy
Raymond - 007 Quantum... #30
13.
The maximum number of electrons that can occupy an energy level described by the principal quantum number, n, is
A. n.
B. n +
1.
C. 2n.
D. 2n2.
E. n2.
Difficulty: Medium
Raymond - 007 Quantum... #31
14.
How many orbitals are allowed in a subshell if the angular momentum quantum number for electrons in that subshell is 3?
A.
B.
C.
D.
E.
1
3
5
7
9
Difficulty: Medium
Raymond - 007 Quantum... #32
15.
"No two electrons in an atom can have the same four quantum numbers" is a statement of
A. the Pauli exclusion principle.
B. Bohr's equation.
C. Hund's rule.
D. de Broglie's relation.
E. Dalton's atomic theory.
Difficulty: Easy
Raymond - 007 Quantum... #33
16.
The orbital diagram for a ground-state nitrogen atom is
A.
B.
C.
D.
Row 1.
Row 2.
Row 3.
Row 4.
Difficulty: Medium
Raymond - 007 Quantum... #34
17.
The orbital diagram for a ground-state oxygen atom is
A. Row 1.
B. Row 2.
C. Row 3.
D. Row 4.
E. Row 5.
Difficulty: Medium
Raymond - 007 Quantum... #35
18.
Which ground-state atom has an electron configuration described by the following orbital diagram?
A.
B.
C.
D.
E.
phosphorus
nitrogen
arsenic
vanadium
none of these
Difficulty: Medium
Raymond - 007 Quantum... #38
19.
How many unpaired electrons does a ground-state atom of sulfur have?
A. 0
B. 1
C. 2
D. 3
E. 4
Difficulty: Medium
Raymond - 007 Quantum... #39
20.
Which element has the following ground-state electron configuration?
1s22s22p63s2
A. Na
B. Mg
C. Al
D. Si
E. Ne
Difficulty: Medium
Raymond - 007 Quantum... #40
21.
Which element has the following ground-state electron configuration?
[Kr]5s24d105p3
A. Sn
B. Sb
C. Pb
D. Bi
E. Te
Difficulty: Medium
Raymond - 007 Quantum... #41
22.
The electron configuration of a ground-state vanadium atom is
A. [Ar]4s24d3.
B. [Ar]4s24p3.
C. [Ar]4s23d3.
D. [Ar]3d5.
Difficulty: Medium
Raymond - 007 Quantum... #44
23.
The electron configuration of a ground-state copper atom is
A. [Ar]4s24d4.
B. [Ar]4s24p63d3.
C. [Ar]4s23d9.
D. [Ar]3d9.
E. [Ar]4s13d10.
Difficulty: Medium
Raymond - 007 Quantum... #45
24.
How many electrons are there in the 2nd principal energy level (n = 2) of a phosphorus atom?
A. 3
B. 5
C. 6
D. 8
E. 10
Difficulty: Medium
Raymond - 007 Quantum... #48
25.
How many electrons are there in the 3rd principal energy level (n = 3) of a phosphorus atom?
A. 3
B. 5.
C. 6
D. 8
E. 10
Difficulty: Medium
Raymond - 007 Quantum... #49
26.
A ground-state atom of manganese has ___ unpaired electrons and is _____.
A. 0, diamagnetic
B. 2, diamagnetic
C. 3, paramagnetic
D. 5, paramagnetic
E. 7, paramagnetic
Difficulty: Medium
Raymond - 007 Quantum... #50
27.
Which of these choices is the electron configuration of an excited state of an oxygen atom?
A. 1s22s22p4
B. 1s22s22p5
C. 1s22s22p33s1
D. 1s22s22p6
E. 1s22s22p3
Difficulty: Medium
Raymond - 007 Quantum... #57
28.
Which of these ground-state atoms is diamagnetic?
A. Ca
B. As
C. Cu
D. Fe
E. none of these
Difficulty: Medium
Raymond - 007 Quantum... #63
29.
The nineteenth century chemists arranged elements in the periodic table according to increasing
A. atomic number.
B. number of electrons.
C. atomic mass.
D. number of neutrons.
E. nuclear binding energy.
Difficulty: Easy
Raymond - 008 Periodic... #1
30.
The elements in Group 7A are known by what name?
A. transition metals
B. halogens
C. alkali metals
D. alkaline earth metals
E. noble gases
Difficulty: Easy
Raymond - 008 Periodic... #4
31.
The elements in Group 2A are known by what name?
A. transition metals
B. halogens
C. alkali metals
D. alkaline earth metals
E. noble gases
Difficulty: Easy
Raymond - 008 Periodic... #5
32.
The alkali metal elements are found in _______ of the periodic table.
A. Group 1A
B. Group 2A
C. Group 3A
D. Period 7
E. Period 1
Difficulty: Easy
Raymond - 008 Periodic... #6
33.
Which one of these elements is a transition element?
A. Sr
B. Pb
C. As
D. Fe
E. H
Difficulty: Easy
Raymond - 008 Periodic... #7
34.
The general electron configuration for atoms of all elements in Group 5A is
A. ns2np6.
B. ns2np5.
C. ns2np4.
D. ns2np3.
E. ns2np1.
Difficulty: Medium
Raymond - 008 Periodic... #9
35.
36.
37.
The general electron configuration for noble gas atoms is
A. ns2np6.
B. ns2np5.
C. ns2np4.
D. ns2np3.
E. ns2.
Consider the element with the electron configuration [Kr]5s24d7. This element is
A. a representative element.
B. a transition metal.
C. a nonmetal.
D. an actinide element.
E. a noble gas.
Consider the element with the electron configuration [Xe]6s24f7. This element is
A. a representative element.
B. a lanthanide element.
C. a nonmetal.
D. an actinide element .
E. a noble gas.
Difficulty: Medium
Raymond - 008 Periodic... #12
Difficulty: Medium
Raymond - 008 Periodic... #15
Difficulty: Medium
Raymond - 008 Periodic... #17
38.
How many valence electrons does a carbon atom have?
A. 1
B. 2
C. 3
D. 4
E. 6
Difficulty: Medium
Raymond - 008 Periodic... #19
39.
How many electrons are in the 4p orbitals of selenium?
A. 0
B. 2
C. 4
D. 5
E. 6
Difficulty: Medium
Raymond - 008 Periodic... #21
40.
How many electrons are in the 4p orbitals of vanadium?
A. 0
B. 2
C. 4
D. 5
E. 6
Difficulty: Medium
Raymond - 008 Periodic... #22
41.
What is the charge on the monatomic ion that calcium forms in its compounds?
A. +2
B. +1
C. -1
D. -2
E. -3
Difficulty: Medium
Raymond - 008 Periodic... #24
42.
43.
What is the charge on the monatomic ion of nitrogen, the nitride ion?
A. +2
B. +1
C. -1
D. -2
E. -3
[Ar]4s23d104p4
[Ar]4s23d104p3
1s22s22p5
(4)
(3)
(2)
Which two electron configurations represent elements that would have similar chemical properties?
(1) 1s22s22p4
A.
B.
C.
D.
E.
44.
Difficulty: Medium
Raymond - 008 Periodic... #25
(1) and (2)
(1) and (3)
(1) and (4)
(2) and (4)
(2) and (3)
Which of these species make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+?
A. Ca2+ and Fe3+
B. O2- and F
C. F and ClD. Cl- and Ca2+
E. none of these
Difficulty: Medium
Raymond - 008 Periodic... #28
Difficulty: Medium
Raymond - 008 Periodic... #29
45.
Which ion is isoelectronic with Ar?
A. Fe2+
B. FC. BrD. Ga3+
E. Ca2+
Difficulty: Medium
Raymond - 008 Periodic... #31
46.
Which of these choices is the electron configuration for the aluminum ion?
A. 1s22s22p63s2
B. 1s22s22p63s23p2
C. 1s22s22p63s23p1
D. 1s22s22p6
E. 1s22s22p63s23p4
Difficulty: Medium
Raymond - 008 Periodic... #33
47.
48.
Which of these choices is the electron configuration of a sulfide ion?
A. [Ne]3s23p4
B. [Ne]
C. [Ne]3s23p1
D. [Ar]
E. [Ne]3s23p2
How many 3d electrons does an Fe3+ ion have?
A. 9
B. 6
C. 5
D. 4
E. 3
Difficulty: Medium
Raymond - 008 Periodic... #35
Difficulty: Medium
Raymond - 008 Periodic... #43
49.
Which of these atoms has the smallest radius?
A. Al
B. P
C. As
D. Te
E. Na
Difficulty: Medium
Raymond - 008 Periodic... #46
50.
51.
Which of these atoms has the largest radius?
A. B
B. Ga
C. Br
D. Si
E. Cl
Arrange these ions in order of increasing ionic radius: K+, P3-, S2-, Cl-.
A.
B.
C.
D.
E.
Difficulty: Medium
Raymond - 008 Periodic... #47
Row 1
Row 2
Row 3
Row 4
Row 5
Difficulty: Medium
Raymond - 008 Periodic... #50
52.
For which of these reactions is the enthalpy change equal to the third ionization energy of vanadium?
A. V2+(g) → V3+(g) + eB. V3+(g) + e- → V2+(g)
C. V(g) → V3+(g) + 3eD. V2-(g) + e- → V3-(g)
E. V3+(g) → V4+(g) + eDifficulty: Medium
Raymond - 008 Periodic... #52
53.
Which of these elements has the highest first ionization energy?
A. Cs
B. Ga
C. K
D. Bi
E. As
Difficulty: Medium
Raymond - 008 Periodic... #53
54.
Which of these elements has the smallest first ionization energy?
A. Cl
B. Na
C. Be
D. K
E. As
Difficulty: Medium
Raymond - 008 Periodic... #55
55.
Which of these elements will display an unusually large jump in ionization energy values between I3 and I4, its third and
fourth ionization energies?
A. Na
B. Mg
C. Al
D. Si
E. P
Difficulty: Difficult
Raymond - 008 Periodic... #57
56.
Which of these elements has the following pattern for its first six ionization energies? (I1 = first ionization energy, I2 =
second ionization energy, etc.)
A.
B.
C.
D.
E.
Ca
Si
Al
Se
P
Difficulty: Difficult
Raymond - 008 Periodic... #60
57.
Which of these elements has the greatest electron affinity (largest positive value)?
A. Mg
B. Al
C. Si
D. P
E. S
Difficulty: Medium
Raymond - 008 Periodic... #63
58.
Which of these elements has the greatest metallic character?
A. Br
B. F
C. Ge
D. Mn
E. Sc
Difficulty: Medium
Raymond - 008 Periodic... #70
59.
If the radius of atom X is greater than the radius of atom Y, then it is also likely that
A. X has a larger electron affinity than Y does.
B. X has a larger effective nuclear charge than Y does.
C. X has greater metallic character than Y does.
D. X has a larger first ionization energy than Y does.
E. X is a poorer conductor of electricity than Y when in the solid state.
Difficulty: Medium
Raymond - 008 Periodic... #73
60.
Which of these compounds is a basic oxide?
A. CO2
B. CaO
C. SO2
D. H2O
E. NO2
Difficulty: Medium
Raymond - 008 Periodic... #75
61.
Which of these compounds is an acidic oxide?
A. P4O10
B. MgO
C. Fe2O3
D. K2O
E. Cr2O3
Difficulty: Medium
Raymond - 008 Periodic... #76
62.
Which of these elements exhibits chemical behavior similar to that of calcium?
A. magnesium
B. sodium
C. sulfur
D. chlorine
E. iron
Difficulty: Medium
Raymond - 008 Periodic... #81
63.
Which of these elements exhibits chemical behavior similar to that of oxygen?
A. magnesium
B. sodium
C. sulfur
D. chlorine
E. iron
F. beryllium
Difficulty: Medium
Raymond - 008 Periodic... #83
64.
Which of these compounds is most likely to be ionic?
A. KF
B. CCl4
C. CS2
D. CO2
E. ICl
Difficulty: Easy
Raymond - 009 Chemical... #1
65.
Which of these compounds is most likely to be ionic?
A. NCl3
B. BaCl2
C. CO
D. SO2
E. SF4
Difficulty: Easy
Raymond - 009 Chemical... #3
66.
Which of these compounds is most likely to be covalent?
A. Rb2S
B. SrCl2
C. CS2
D. CaO
E. MgI2
Difficulty: Easy
Raymond - 009 Chemical... #5
67.
68.
Complete this statement: Coulomb's law states that the magnitude of the force of interaction between two charged bodies
is
A. directly proportional to the product of the charges on the bodies and directly proportional to the distance separating
them.
B. directly proportional to the product of the charges on the bodies, and inversely proportional to the square of the distance
separating them.
C. inversely proportional to the charges on the bodies, and directly proportional to the square of the distance separating
them.
D. directly proportional to the sum of the charges on the bodies, and inversely proportional to the square of the distance
separating them.
The Lewis dot symbol for the S 2- ion is
A.
Difficulty: Medium
Raymond - 009 Chemical... #8
B.
C.
D.
E.
Difficulty: Medium
Raymond - 009 Chemical... #10
69.
Which of these ionic solids would have the largest lattice energy?
A. NaCl
B. NaF
C. CaBr2
D. CsI
E. CaCl2
Difficulty: Medium
Raymond - 009 Chemical... #13
70.
Which of these solids would have the highest melting point?
A. NaF
B. NaCl
C. NaBr
D. NaI
Difficulty: Medium
Raymond - 009 Chemical... #15
71.
Which of these elements has the greatest electronegativity?
A. Na
B. As
C. Ga
D. Cs
E. Sb
Difficulty: Medium
Raymond - 009 Chemical... #22
72.
Which of these elements is the least electronegative?
A. Sr
B. V
C. Ni
D. P
E. I
Difficulty: Medium
Raymond - 009 Chemical... #25
73.
A polar covalent bond would form in which one of these pairs of atoms?
A.
B.
C.
D.
E.
Difficulty: Medium
Raymond - 009 Chemical... #27
74.
What type of chemical bond holds the atoms together within a water molecule?
A. Ionic bond
B. Nonpolar covalent bond
C. Polar covalent bond
D. Coordinate covalent bond
Difficulty: Medium
Raymond - 009 Chemical... #28
75.
A nonpolar covalent bond (i.e., pure covalent) would form in which of these pairs of atoms?
A.
B.
C.
D.
E.
Difficulty: Medium
Raymond - 009 Chemical... #29
76.
Which of these bonds would have the greatest polarity (i.e., highest percent ionic character)?
A.
B.
C.
D.
E.
Difficulty: Medium
Raymond - 009 Chemical... #30
77.
In which of these pairs of atoms would the bond be the least polar (i.e., lowest percent ionic character)?
A.
B.
C.
D.
E.
Difficulty: Medium
Raymond - 009 Chemical... #35
78.
Classify the
bond in CaCl2 as ionic, polar covalent, or nonpolar covalent.
A. ionic
B. polar covalent
C. nonpolar covalent
Difficulty: Medium
Raymond - 009 Chemical... #38
79.
The electron dot formula for O2 shows
A. a single covalent bond.
B. a double covalent bond.
C. an ionic bond.
D. a total of 8 × 2 = 16 electron dots.
E. a total of 32 electron dots.
Difficulty: Medium
Raymond - 009 Chemical... #39
80.
The number of lone electron pairs in the N2 molecule is ___.
A. 1
B. 2
C. 3
D. 4
E. 5
Difficulty: Medium
Raymond - 009 Chemical... #40
81.
The electron dot structure for AsCl3 shows
A. a total of 84 electron dots.
B. three single bonds and 10 lone pairs.
C. two single bonds, one double bond, and 9 lone pairs.
D. one single bond, two double bonds, and 8 lone pairs.
E. three single bonds and one lone pair.
Difficulty: Medium
Raymond - 009 Chemical... #41
82.
The total number of bonding electrons in a molecule of formaldehyde (H2CO) is
A. 3.
B. 4.
C. 6.
D. 8.
E. 18.
Difficulty: Medium
Raymond - 009 Chemical... #42
83.
The total number of lone pairs in NCl3 is
A. 6.
B. 8.
C. 9.
D. 10.
E. 13.
Difficulty: Medium
Raymond - 009 Chemical... #43
84.
The Lewis structure for CS2 is:
A.
B.
C.
D.
Difficulty: Medium
Raymond - 009 Chemical... #44
85.
Which of these Lewis structures is incorrect?
A.
B.
C.
D.
E.
Difficulty: Medium
Raymond - 009 Chemical... #46
86.
The number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is
A. 1.
B. 2.
C. 3.
D. 4.
E. none of these.
Difficulty: Difficult
Raymond - 009 Chemical... #48
87.
The number of resonance structures for the nitrate ion that satisfies the octet rule is
A. 1.
B. 2.
C. 3.
D. 4.
E. none of these.
Difficulty: Difficult
Raymond - 009 Chemical... #49
88.
Which of these statements is a useful guideline for the application of formal charges in neutral molecules?
A. A Lewis structure in which there are no formal charges is preferred.
B. Lewis structures with large formal charges (e.g., +2,+3 and/or -2,-3) are preferred.
C. The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms.
Difficulty: Easy
Raymond - 009 Chemical... #53
89.
90.
What is the formal charge on the oxygen atom in N2O (the atomic order is N-N-O)?
A. 0
B. +1
C. -1
D. -2
E. +2
In the best Lewis structure for the fulminate ion,
A. +2
B. +1
C. 0
D. -1
E. -2
CNO-,
Difficulty: Difficult
Raymond - 009 Chemical... #54
what is the formal charge on the central nitrogen atom?
Difficulty: Difficult
Raymond - 009 Chemical... #61
91.
For which of these species can you draw two resonance structures?
A. CH2O
B. ClNO2
C. H2O
D. CH4
E. H2S
Difficulty: Medium
Raymond - 009 Chemical... #64
92.
Which of these substances will display an incomplete octet in its Lewis structure?
A. CO2
B. Cl2
C. ICl
D. NO
E. SO2
Difficulty: Medium
Raymond - 009 Chemical... #68
93.
Which of these elements is most likely to exhibit an expanded octet in its compounds?
A. O
B. S
C. Na
D. C
E. N
Difficulty: Easy
Raymond - 009 Chemical... #69
94.
According to the VSEPR theory, the shape of the SO3 molecule is
A. pyramidal.
B. tetrahedral.
C. trigonal planar.
D. distorted tetrahedron (seesaw).
E. square planar.
Difficulty: Medium
Raymond - 010 Chemical... #1
95.
The shape of the SF4 molecule is
A. tetrahedral.
B. trigonal pyramidal.
C. trigonal planar.
D. square planar.
E. distorted tetrahedron (seesaw).
Difficulty: Medium
Raymond - 010 Chemical... #2
96.
Use VSEPR theory to predict the shape of the PCl3 molecule.
A. linear
B. bent
C. trigonal planar
D. trigonal pyramidal
E. tetrahedral
Difficulty: Medium
Raymond - 010 Chemical... #3
97.
98.
The shape of the CS2 molecule is best described as
A. linear.
B. trigonal planar.
C. tetrahedral.
D. bent.
E. trigonal pyramidal.
According to the VSEPR theory, the molecular shape of the carbonate ion, CO32 -, is
A. square planar.
B. tetrahedral.
C. pyramidal.
D. trigonal planar.
E. octahedral.
Difficulty: Medium
Raymond - 010 Chemical... #5
Difficulty: Medium
Raymond - 010 Chemical... #7
99.
The shape of the ClF3 molecule is best described as
A. distorted tetrahedron.
B. trigonal planar.
C. tetrahedral.
D. T-shaped.
E. trigonal pyramidal.
Difficulty: Medium
Raymond - 010 Chemical... #6
100.
According to the VSEPR theory, the molecular shape of SiCl4 is
A. linear.
B. trigonal planar.
C. bent.
D. tetrahedral.
E. trigonal pyramidal.
Difficulty: Medium
Raymond - 010 Chemical... #9
101.
According to VSEPR theory, which one of the following molecules should have a shape that is trigonal bipyramidal?
A. SF4
B. XeF4
C. NF3
D. SF6
E. PF5
Difficulty: Medium
Raymond - 010 Chemical... #13
102.
Which of the following substances is/are bent?
A.
B.
C.
D.
E.
(i) H2S
(ii). CO2
(iii) ClNO
only (iii)
only (i) and (v)
only (i), (iii), and (v)
all are bent except for (iv)
all are bent except for (ii)
(iv) NH2-
(v) O3
Difficulty: Medium
Raymond - 010 Chemical... #21
103.
The F-S-F bond angles in SF6 are
A. 90° and 180°.
B. 109.5°.
C. 120°.
D. 180°.
E. 90° and 120°.
Difficulty: Medium
Raymond - 010 Chemical... #24
104.
The bond angle in Cl2O is expected to be approximately
A. 90°.
B. 109.5°.
C. 120°.
D. 145°.
E. 180°.
Difficulty: Medium
Raymond - 010 Chemical... #23
105.
The C-N-O bond angle in nitromethane, CH3NO2, is expected to by approximately
A. 60°.
B. 90°.
C. 109.5°.
D. 120°.
E. 180°.
Difficulty: Medium
Raymond - 010 Chemical... #27
106.
Which one of the following molecules is nonpolar?
A. NH3
B. OF2
C. CH3Cl
D. H2O
E. BeCl2
Difficulty: Medium
Raymond - 010 Chemical... #28
107.
Complete this sentence: The PCl5 molecule has
A. nonpolar bonds, and is a nonpolar molecule.
B. nonpolar bonds, but is a polar molecule.
C. polar bonds, and is a polar molecule.
D. polar bonds, but is a nonpolar molecule.
Difficulty: Medium
Raymond - 010 Chemical... #29
108.
Indicate the type of hybrid orbitals used by the central atom in PCl3.
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
Difficulty: Medium
Raymond - 010 Chemical... #36
109.
Indicate the type of hybrid orbitals used by the central atom in SF6.
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
Difficulty: Medium
Raymond - 010 Chemical... #38
110.
What is the hybridization of the As atom in the AsF5 molecule?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
Difficulty: Medium
Raymond - 010 Chemical... #39
111.
112.
What is the hybridization on the central atom in NO3- ?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
What is the hybridization of As in the AsF4- ion?
A. sp
B. sp2
C. sp3
D. sp3d
E. sp3d2
Difficulty: Medium
Raymond - 010 Chemical... #40
Difficulty: Medium
Raymond - 010 Chemical... #42
113.
The hybridization of the central nitrogen atom in the molecule N2O is
A. sp.
B. sp2.
C. sp3.
D. sp3d.
E. sp3d2.
Difficulty: Medium
Raymond - 010 Chemical... #44
114.
The number of pi bonds in the molecule below is
A. 1.
B. 2.
C. 3.
D. 5.
E. 9.
Difficulty: Medium
Raymond - 010 Chemical... #49
115.
The number of pi bonds in the molecule below is
A. 2.
B. 4.
C. 6.
D. 10.
E. 15.
Difficulty: Medium
Raymond - 010 Chemical... #50
Chem I Review Part 2 Summary
Category
Difficulty: Difficult
Difficulty: Easy
Difficulty: Medium
Raymond - 007 Quantum...
Raymond - 008 Periodic...
Raymond - 009 Chemical...
Raymond - 010 Chemical...
# of Questions
7
16
92
28
35
30
22