考卷 卷別 A
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1041_3rd Exam_1050106 (A)
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Which compound has the highest magnitude of lattice energy?
A) MgS B) CaS C) BaS D) SrS
Answer: A
2) Which pair of atoms forms the most polar bond?
A) N and F B) C and O C) N and O D) C and F
Answer: D
3) Which of the following statements is TRUE?
A) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs."
B) It is not possible for two atoms to share more than two electrons.
C) Single bonds are shorter than double bonds.
D) A covalent bond has a lower potential energy than the two separate atoms.
E) A covalent bond is formed through the transfer of electrons from one atom to another.
Answer: D
4) Which of the following statements is TRUE?
A) An ionic bond is much stronger than most covalent bonds.
B) An ionic bond is formed through the sharing of electrons.
C) Once dissolved in water, ionic compounds rarely conduct electricity.
D) Ionic compounds at room temperature typically conduct electricity.
E) None of the above are true.
Answer: A
5) Give the complete electronic configuration for S2-.
A) 1s22s22p63s24p6 B) 1s22s2p63s2p6 C) 1s22s23p64s25p6 D) 1s22s22p63s23p6 E) 1s22s22p63s23p5 Answer: D
6)Which of the following reactions is associated with the lattice energy of CaS ( H°latt)?
A) CaS(s) Ca2 (aq) + S2 (aq) B) CaS(s) Ca(s) + S(s) C) Ca2 (g) + S2 (g) CaS(s) D) Ca(s) + S(s) CaS(s)
E) Ca2 (aq) + S2 (aq) CaS(s) Answer: C
學期、次數、卷別
7) Use the data given below to construct a Born-Haber cycle to determine the heat of formation of KCl.
∆H°(kJ)
K(s) K(g) 89
K(g) K (g) + e 418
Cl2(g) 2 Cl(g) 244
Cl(g) + e Cl (g) -349
KCl(s) K (g) + Cl (g) 717
A) -437 kJ B) -1119 kJ C) +158 kJ D) -997 kJ E) +631 kJ
Answer: A
8)Choose the best Lewis structure for XeI2.
A) B) C) D) E) Answer: E
9) Place the following in order of increasing magnitude of lattice energy.
CaO MgO SrS
A) CaO < MgO < SrS B) MgO < CaO < SrS C) CaO < SrS < MgO D) SrS < MgO < CaO E) SrS < CaO < MgO Answer: E
10) Place the following in order of decreasing bond length.
H-F H-I H-Br
A) H-Br > H-F > H-I B) H-I > H-F > H-Br C) H-F > H-I > H-Br D) H-F > H-Br > H-I
E) H-I > H-Br > H-F Answer: E
11) Determine the formal charge of nitrogen in this structure.
A) -2 B) -1 C) +2 D) +1
Answer: D
12) Which of the following processes are exothermic?
A) Li(s) Li(g) B) Br(g) + e Br (g) C)Cl2(g) 2Cl(g) D) NaF(s) Na (g) + F (g)
E) None of the above are exothermic.
Answer: B
13) Use the bond energies provided to estimate H°rxn for the reaction below.
CH3OH(l) + 3
2 O2(g) CO2(g) + 2 H2O(g) H°rxn = ? Bond Bond Energy (kJ/mol)
C-H 414
C-O 360
C=O 799
O=O 498
O-H 464
A) -91 kJ B) -392 kJ C) +206 kJ D) +473 kJ E) -486 kJ
Answer: No Correct Answer Was Provided.
14) Which molecule geometry results when a central atom has five total electron groups, with three of those being bonding groups and two being lone pairs?
A) T-shaped B) seesaw
C) bent D) trigonal bipyramidal
Answer: A
15)Give the hybridization for the S in SF6.
A) sp B) sp3d C) sp2 D) sp3d2 E) sp3
Answer: D
16)Give the electron geometry (eg), molecular geometry (mg), and hybridization for XeF4.
A) eg=octahedral, mg=square planar, sp3d2 B) eg=octahedral, mg=octahedral, sp3d2 C) eg=trigonal bipyramidal, mg=seesaw, sp3d D) eg=tetrahedral, mg=tetrahedral, sp3
E) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 Answer: A
17)Place the following in order of increasing dipole moment.
I. BCl3 II. BIF2 III. BClF2
A) I < III < II B) I < II = III C) I < II < III D) II < I < III E) II < III < I Answer: A
18)How many of the following molecules are polar?
BrCl3 CS2 SiF4 SO3
A) 2 B) 1 C) 3 D) 4 E) 0
Answer: B
19) Use the molecular orbital diagram shown to determine which of the following is paramagnetic.
A) Ne22 B) O22 C) F22 D) O22 E) F22
Answer: C
20) Use the molecular orbital diagram shown in Question 19 to determine which of the following is most stable.
A)F2 B) Ne22 C) F22 D) F22 E) O22
Answer: E
21)Predict the relative bond angles in BF3 and SO2 .
A) Relative bond angles cannot be predicted. B)SO2 bond angle > BF3 bond angles C)BF3 bond angles = SO2 bond angle D)BF3 bond angles > SO2 bond angle Answer: D
22)Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3.
A) eg=trigonal planar, mg=trigonal planar, sp2 B) eg=tetrahedral, mg=trigonal planar, sp2 C) eg=trigonal pyramidal, mg=tetrahedral, sp3 D) eg=tetrahedral, mg=trigonal pyramidal, sp3
E) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3 Answer: D
23) Which of the following statements is TRUE?
A) When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in energy than the separate atomic orbitals.
B) A bond order of 0 represents a stable chemical bond.
C) The total number of molecular orbitals formed doesn't always equal the number of atomic orbitals in the D) Electrons placed in antibonding orbitals stabilize the ion/molecule.set.
E) All of the above are true.
Answer: A
24)According to valence bond theory, which kind of orbitals overlap to form the P—Cl bonds in PCl5 ? A) P(sp3d) - Cl(p) B) P(sp3) - Cl(s ) C) P(sp3) - Cl(p) D) P(sp3d) - Cl(s) Answer: A
25)Determine the hybridization about O in CH3OH.
A) sp2 B) sp C) sp3d D) sp3
Answer: D
26) Consider the phase diagram shown below. A sample of the substance in the phase diagram is initially at 175 °C and 925 mmHg. What phase transition occurs when the pressure is decreased to 760 mmHg at constant
temperature?
A) liquid to gas B) solid to liquid C) solid to gas D) liquid to solid Answer: A
27) Why is water an extraordinary substance?
A) Water has an exceptionally high specific heat capacity.
B) Water is the main solvent within living organisms.
C) Water has strong hydrogen bonding.
D) Water has a low molar mass, yet it is a liquid at room temperature.
E) All of the above.
Answer: E
28) Based on the expected intermolecular forces, which halogen has the highest boiling point?
A)Br2 B)Cl2 C)I2 D)F2
Answer: C
29)What is the strongest type of intermolecular force present in NH2CH3?
A) ion-dipole
B) hydrogen bonding C) dipole-dipole D) dispersion
E) none of the above Answer: B
30)How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its Hvap is 31.6 kJ/mol?
A) 15.4 kJ B) 31.2 kJ C) 18.1 kJ D) 6.49 kJ E) 55.1 kJ
Answer: C
31) Which of the following statements is FALSE?
A) The rate of vaporization increases with increasing surface area.
B) The rate of vaporization increases with increasing temperature.
C) Molecules with hydrogen bonding are more volatile than compounds with dipole-dipole forces.
D) The rate of vaporization increases with decreasing strength of intermolecular forces.
E) None of the above are false.
Answer: C
32) Which of the following statements is TRUE?
A) Intermolecular forces are generally stronger than bonding forces.
B) Increasing the pressure on a solid usually causes it to become a liquid.
C) The potential energy of molecules decrease as they get closer to one another.
D) Energy is given off when the attraction between two molecules is broken.
E) None of the above are true.
Answer: C
33) Define triple point.
A) The temperature that is unique for a substance.
B) The temperature at which the solid and liquid co-exist.
C) The temperature, pressure, and density for a gas.
D) The temperature at which the boiling point equals the melting point.
E) The temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium.
Answer: E
34) Acetic acid has a normal boiling point of 118°C and a Hvap of 23.4 kJ/mol. What is the vapor pressure (in mmHg) of acetic acid at 25 °C? [ ln ( P1P2) = ( Hvap
R ) ( 1 T2 - 1
T1 ) , R = 8.314 J/mol , 1 atm = 760 mmHg ]
A) 80.6 mmHg B) 2.92 × 10 -39 mmHg
C) 758 mmHg D) 7.16 * 103 mmHg
Answer: A
35) How much energy must be removed from a 125 g sample of benzene (molar mass= 78.11 g/mol) at 425.0 K to liquify the sample and lower the temperature to 335.0 K? The following physical data may be useful.
Hvap = 33.9 kJ/mol Hfus = 9.8 kJ/mol Cliq = 1.73 J/g°C Cgas = 1.06 J/g°C Csol = 1.51 J/g°C Tmelting = 279.0 K Tboiling = 353.0 K
A) 95.4 kJ B) 74.4 kJ C) 67.7 kJ D) 54.3 kJ E) 38.9 kJ
Answer: C
36) Identify the type of solid for ice.
A) metallic atomic solid B) ionic solid
C) networking atomic solid D) nonbonding atomic solid
E) molecular solid Answer: E
37) Consider the phase diagram shown. Choose the statement below that is TRUE.
A) The solid phase of this substance is higher in density than the liquid phase.
B) The triple point of this substance occurs at a temperature of 31°C.
C)The line separating the solid and liquid phases represents the Hvap.
D) At 10 atm of pressure, there is no temperature where the liquid phase of this substance would exist.
E) None of the above are true.
Answer: A
38) Give the major force in seawater.
A) dipole-dipole B) ion-dipole C) dispersion
D) hydrogen bonding E) ion-ion
Answer: B
39)The osmotic pressure of a solution containing 22.7 mg of an unknown protein in 50.0 mL of solution is 2.88 mmHg at 25 °C. Determine the molar mass of the protein. [ = CM × R × T , R = 62.364 L·mmHg / mol·K ]
A) 3.85 g/mol B) 147 g/mol C) 2.93 × 103 g/mol D) 246 g/mol
Answer: C
40)Determine the vapor pressure of an aqueous ethylene glycol (C2H6O2) solution that is 14.8% C2H6O2 by mass.
The vapor pressure of pure water at 25 °C is 23.8 torr [ P = i × XB × P° ]
A) 1.14 torr B) 22.7 torr C) 20.3 torr D) 3.52 torr
Answer: B
41)Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water. The vapor pressure of pure water at 55°C is 118.1 torr. The van't Hoff factor for NaCl is 1.9 [ P = i × XB × P° ]
A) 112 torr B) 87.1 torr C) 115 torr D) 92.8 torr E) 108 torr
Answer: A
42)Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf
= 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water. [ T = i × Kb × Cm ]
A) 92°C B) 70°C C) -30.0°C D) 108°C E) -8.32°C
Answer: D
43) Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molality of the HCl, if the solution has a density of 1.20 g/mL.
A) 6.39 m B) 10.7 m C)17.5 m D) 9.44 m E) 39.0 m
Answer: C
44) Which of the following concentration units are temperature dependent?
A) molarity B) mole fraction C) mass percent D) molality
E) none of the above.
Answer: A
45) Which of the following statements is generally TRUE?
A) The solubility of a solid is highly dependent on pressure.
B) The solubility of a solid is highly dependent on temperature.
C) The solubility of a solid is highly dependent on both pressure and temperature.
D) The solubility of a solid is not dependent on either temperature or pressure.
E) None of the above.
Answer: B
46) Which of the following statements is TRUE?
A) The solubility of an ionic solid in water decreases with increasing temperature.
B) The solubility of a gas in water usually increases with decreasing pressure.
C) In general, the solubility of a gas in water decreases with increasing temperature.
D) In general, the solubility of a solid in water decreases with increasing temperature.
E) None of the above statements are true.
Answer: C
47) An aqueous solution is saturated in both potassium chlorate and carbon dioxide gas at room temperature. What happens when the solution is warmed to 85 °C?
A) Potassium chlorate precipitates out of solution.
B) Potassium chlorate precipitates out of solution and carbon dioxide bubbles out of solution.
C) Nothing happens; all of the potassium chloride and the carbon dioxide remain dissolved in solution.
D) Carbon dioxide bubbles out of solution.
Answer: D
48) Soap has an ionic and a polar end. It works well to remove oil by A) surrounding the oil and water with the nonpolar end.
B) surrounding the oil and water with the polar end.
C) surrounding the oil with the polar end, and the water interacts with the nonpolar end.
D) surrounding the oil with the nonpolar end, and the water interacts with the polar end.
Answer: D
49) Identify the colligative property.
A) vapor pressure lowering B) freezing point depression C) osmotic pressure
D) boiling point elevation E) all of the above Answer: E
50) The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C. What mass of sucrose (molar mass= 342.30 g/mol) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512°C/m.
[ T = i × Kb × Cm ] A) 130. g sucrose B) 528 g sucrose C) 223 g sucrose D) 261 g sucrose E) 762 g sucrose Answer: A
The Periodic Table of the Elements
1
H
Hydrogen 1.00794
2
He
Helium 4.003
3
Li
Lithium 6.941
4
Be
Beryllium 9.012182
5
B
Boron 10.811
6
C
Carbon 12.0107
7
N
Nitrogen 14.00674
8
O
Oxygen 15.9994
9
F
Fluorine 18.9984032
10
Ne
Neon 20.1797
11
Na
Sodium 22.989770
12
Mg
Magnesium 24.3050
13
Al
Aluminum 26.981538
14
Si
Silicon 28.0855
15
P
Phosphorus 30.973761
16
S
Sulfur 32.066
17
Cl
Chlorine 35.4527
18
Ar
Argon 39.948
19
K
Potassium 39.0983
20
Ca
Calcium 40.078
21
Sc
Scandium 44.955910
22
Ti
Titanium 47.867
23
V
Vanadium 50.9415
24
Cr
Chromium 51.9961
25
Mn
Manganese 54.938049
26
Fe
Iron 55.845
27
Co
Cobalt 58.933200
28
Ni
Nickel 58.6934
29
Cu
Copper 63.546
30
Zn
Zinc 65.39
31
Ga
Gallium 69.723
32
Ge
Germanium 72.61
33
As
Arsenic 74.92160
34
Se
Selenium 78.96
35
Br
Bromine 79.904
36
Kr
Krypton 83.80
37
Rb
Rubidium 85.4678
38
Sr
Strontium 87.62
39
Y
Yttrium 88.90585
40
Zr
Zirconium 91.224
41
Nb
Niobium 92.90638
42
Mo
Molybdenum 95.94
43
Tc
Technetium (98)
44
Ru
Ruthenium 101.07
45
Rh
Rhodium 102.90550
46
Pd
Palladium 106.42
47
Ag
Silver 107.8682
48
Cd
Cadmium 112.411
49
In
Indium 114.818
50
Sn
Tin 118.710
51
Sb
Antimony 121.760
52
Te
Tellurium 127.60
53
I
Iodine 126.90447
54
Xe
Xenon 131.29
55
Cs
Cesium 132.90545
56
Ba
Barium 137.327
57
La
Lanthanum 138.9055
72
Hf
Hafnium 178.49
73
Ta
Tantalum 180.9479
74
W
Tungsten 183.84
75
Re
Rhenium 186.207
76
Os
Osmium 190.23
77
Ir
Iridium 192.217
78
Pt
Platinum 195.078
79
Au
Gold 196.96655
80
Hg
Mercury 200.59
81
Tl
Thallium 204.3833
82
Pb
Lead 207.2
83
Bi
Bismuth 208.98038
84
Po
Polonium (209)
85
At
Astatine (210)
86
Rn
Radon (222)
87
Fr
Francium (223)
88
Ra
Radium (226)
89
Ac
Actinium (227)
104
Rf
Rutherfordium (261)
105
Db
Dubnium (262)
106
Sg
Seaborgium (263)
107
Bh
Bohrium (262)
108
Hs
Hassium (265)
109
Mt
Meitnerium (266)
110
(269)
111
(272)
112
(277)
113 114
58
Ce
Cerium 140.116
59
Pr
Praseodymium 140.90765
60
Nd
Neodymium 144.24
61
Pm
Promethium (145)
62
Sm
Samarium 150.36
63
Eu
Europium 151.964
64
Gd
Gadolinium 157.25
65
Tb
Terbium 158.92534
66
Dy
Dysprosium 162.50
67
Ho
Holmium 164.93032
68
Er
Erbium 167.26
69
Tm
Thulium 168.93421
70
Yb
Ytterbium 173.04
71
Lu
Lutetium 174.967
90
Th
Thorium 232.0381
91
Pa
Protactinium 231.03588
92
U
Uranium 238.0289
93
Np
Neptunium (237)
94
Pu
Plutonium (244)
95
Am
Americium (243)
96
Cm
Curium (247)
97
Bk
Berkelium (247)
98
Cf
Californium (251)
99
Es
Einsteinium (252)
100
Fm
Fermium (257)
101
Md
Mendelevium (258)
102
No
Nobelium (259)
103
Lr
Lawrencium (262)
1995 IUPAC masses and Approved Names from http://www.chem.qmw.ac.uk/iupac/AtWt/
masses for 107-111 from C&EN, March 13, 1995, p. 35 112 from http://www.gsi.de/z112e.html
週期表
