Chemistry II Final Exam Review
9. Express 0.00560 in exponential notation. E) 2.7
A) 5.60 × 103
B) 5.6 × 10-3 22. How many significant figures are there in the
C) 5.60 × 10-3 number 0.04560700?
D) 5.60 A) 4
E) none of these B) 5
C) 7
10. A titration was performed to find the concentration of D) 8
hydrochloric acid with the following results: E) 9
Trial Molarity
1 1.25 ± 0.01 32. Convert 4483 mL to qts. (1 L = 1.06 qt)
2 1.24 ± 0.01 A) 4752 qts
3 1.26 ± 0.01 B) 4.229 qts
A) both accurate and precise. C) 4.229e–3 qts
B) accurate but imprecise. D) 4229 qts
C) precise but inaccurate. E) 4.752 qts
D) both inaccurate and imprecise.
E) accuracy and precision are impossible to 33. Convert 77.5 lb to g. (1 lb = 453.6 g)
determine with the available information. A) 3.52e3 g
B) 1.71e5 g
12. We generally report a measurement by recording all C) 3.52e2 g
of the certain digits plus ____ uncertain digit(s). D) 1.71e–1 g
A) no E) 3.52e4 g
B) one
C) two 39. The state of matter for an object that has a definite
D) three volume but not a definite shape is
E) four A) solid state.
B) liquid state.
13. The amount of uncertainty in a measured quantity is C) gaseous state.
determined by: D) elemental state.
A) both the skill of the observer and the limitations E) mixed state.
of the measuring instrument.
B) neither the skill of the observer nor the 49. The density of gasoline is 0.7025 g/mL at 20°C.
limitations of the measuring instrument. When gasoline is added to water:
C) the limitations of the measuring instrument A) it will float on top.
only. B) it will sink to the bottom.
D) the skill of the observer only. C) it will mix so you can't see it.
E) none of these D) the mixture will improve the running of the
motor.
15. How many significant figures are there in the E) none of these things will happen.
number 3.1400?
A) 1 55. _________ are substances with constant
B) 2 composition that can be broken down into elements by
C) 3 chemical processes.
D) 4 A) Solutions
E) 5 B) Mixtures
C) Compounds
17. Express 165,000 in exponential notation. D) Quarks
A) 1.65000 × 105 E) Heterogeneous mixtures
B) 1.65 × 105
C) 1.6500 × 10–5 56. A method of separation that employs a system with
D) 1.65 × 10–5 two phases of matter, a mobile phase and a stationary phase,
E) 165 × 103 is called
A) filtration.
21. Using the rules of significant figures, calculate the B) chromatography.
following: 4.0021-1.346 C) distillation.
A) 2.656 D) vaporization.
B) 3 E) homogenization.
C) 2.6561
D) 2.66 57. A solution is also called a
-1-
A) homogeneous mixture. D) The number of protons and neutrons is always
B) heterogeneous mixture. the same in the neutral atom.
C) pure mixture. E) All of the above statements (a-d) are true.
D) compound.
E) distilled mixture. 89. The element rhenium (Re) exists as two stable
isotopes and 18 unstable isotopes. Rhenium-185 has in its
65. The beakers shown below have different precisions nucleus
as shown. A) 75 protons, 75 neutrons.
B) 75 protons, 130 neutrons.
C) 130 protons, 75 neutrons.
D) 75 protons, 110 neutrons.
E) not enough information is given.
40
91. 20 Ca 2+ has
A) 20 protons, 20 neutrons, and 18 electrons.
B) 22 protons, 20 neutrons, and 20 electrons.
C) 20 protons, 22 neutrons, and 18 electrons.
D) 22 protons, 18 neutrons, and 18 electrons.
E) 20 protons, 20 neutrons, and 22 electrons.
93. The numbers of protons, neutrons, and electrons in
39
K+ are:
19
A) 20 p, 19 n, 19 e
B) 20 p, 19 n, 20 e
C) 19 p, 20 n, 20 e
D) 19 p, 20 n, 19 e
E) 19 p, 20 n, 18 e
96. Which among the following represent a set of
isotopes? Atomic nuclei containing:
I. 20 protons and 20 neutrons.
II. 21 protons and 19 neutrons.
Suppose you pour the water from these three beakers into one III. 22 neutrons and 18 protons.
container. What would be the volume in the container IV. 20 protons and 22 neutrons.
reported to the correct number of significant figures? V. 21 protons and 20 neutrons.
A) 78.817 mL
B) 78.82 mL A) I, II, III
C) 78.8 mL B) III, IV
D) 90 mL C) I, V
E) 79 mL D) I, IV and II, V
E) No isotopes are indicated.
79. Which of the following pairs can be used to illustrate
the law of multiple proportions? 104. Which of the following are incorrectly paired?
A) SO and SO2 A) K, alkali metal
B) CO and CaCo3 B) Ba, alkaline earth metal
C) H2O and C12H22O11 C) O, halogen
D) H2SO4 and H2S D) Ne, noble gas
E) KCl and KClO2 E) Ni, transition metal
84. Which one of the following statements about atomic 108. All of the following are characteristics of nonmetals
structure is false? except:
A) The electrons occupy a very large volume A) poor conductors of electricity
compared to the nucleus. B) often bond to each other by forming covalent
B) Almost all of the mass of the atom is bonds
concentrated in the nucleus. C) tend to form negative ions in chemical reactions
C) The protons and neutrons in the nucleus are very with metals
tightly packed.
-2-
D) appear in the upper left-hand corner of the 176. Adipic acid contains 49.32% C, 43.84% O, and
periodic table 6.85% H by mass. What is the empirical formula?
E) do not have a shiny (lustrous) appearance A) C3H5O2
B) C3H3O4
113. The correct name for FeO is C) C2HO3
A) iron oxide D) C2H5O4
B) iron (II) oxide E) C3HO3
C) iron (III) oxide E) 60.1 %
D) iron monoxide
E) iron (I) oxide 186. wPCl5 + xH2O yPOCl3 + zHCl
The above equation is properly balanced when
118. All of the following are in aqueous solution. Which is A) w = 1, x = 2, y = 2, z = 4
incorrectly named? B) w = 2, x = 2, y = 2, z = 2
A) HC2H3O2, acetic acid C) w = 2, x = 2, y = 2, z = 1
B) HBr, bromic acid D) w = 1, x = 1, y = 1, z = 2
C) H2SO3, sulfurous acid E) none of these
D) HNO2, nitrous acid
E) HClO3, chloric acid 189. Indium reacts with chlorine to form InCl3. In the
balanced equation for this reaction, the coefficient of the
119. Which of the following pairs is incorrect? indium trichloride is
A) NH4Br, ammonium bromide A) 1
B) K2CO3, potassium carbonate B) 2
C) BaPO4, barium phosphate C) 3
D) CuCl, copper(I) chloride D) 4
E) MnO2, manganese (IV) oxide E) 6
130. Gallium consists of two isotopes of masses 68.95 amu 201. How many grams of H2O will be formed when 32.0
and 70.95 amu with abundances of 60.16% and 39.84%, g H2 is mixed with 43.0 g of O2 and allowed to react to form
respectively. What is the average atomic mass of gallium? water?
A) 69.95 A) 48.4 g
B) 70.15 B) 286 g
C) 71.95 C) 24.2 g
D) 69.75 D) 12.1 g
E) 69.55 E) 144 g
152. Nitric acid, HNO3, contains what percent hydrogen by 206. Consider the following reaction:
mass? CH 4 ( g ) 4Cl2 ( g ) CCl4 ( g ) 4 HCl ( g )
A) 20.0 %
B) 10.0 %
C) 4.50 % What mass of CCl4 is formed by the reaction of 6.85 g of
D) 1.60 % methane with an excess of chlorine?
E) 3.45 % A) 16.4 g
B) 0.71 g
167. An oxide of iron has the formula Fe3O4. What mass C) 1.05e3 g
percent of iron does it contain? D) 65.7 g
A) 0.72 % E) none of these
B) 28 %
C) 30. % 208. When rubidium metal is exposed to air, one atom of
D) 70. % rubidium, Rb, combines with two atoms of oxygen. If 1.75
E) 72 % grams of rubidium is exposed to air, what will be the mass of
the product in grams?
175. The empirical formula of styrene is CH; its molar A) 0.328 g
mass is 104.1. What is the molecular formula of styrene? B) 0.655 g
A) C2H4 C) 1.37 g
B) C8H8 D) 2.08 g
C) C10H12 E) 2.41 g
D) C6H6
E) none of these 213. A 5.95-g sample of AgNO3 is reacted with BaCl2
according to the equation
-3-
E) HBrO
2 AgNO3 (aq) BaCl2 (aq) 2 AgCl ( s) Ba( NO3 ) 2 (aq)
246. Which of the following is not a strong base?
A) Ca(OH)2
to give 3.93 g of AgCl. What is the percent yield of AgCl?
B) KOH
A) 39.1 %
C) NH3
B) 66.1 %
D) LiOH
C) 52.2 %
E) Sr(OH)2
D) 78.3 %
E) 100. % 256. The following reactions:
Pb2+ + 2I– PbI2
231. A 30.0-g sample of HF is dissolved in water to give
2.0 102 mL of solution. The concentration of the solution 2Ce4+ + 2I– I2 + 2Ce3+
is: HOAc + NH3 NH4+ + OAc–
A) 1.50 M are examples of
B) 0.30 M A) acid-base reactions.
C) 0.15 M B) unbalanced reactions.
D) 7.5 M C) precipitation, acid-base, and redox reactions,
E) 15.0 M respectively.
D) redox, acid-base, and precipitation reactions,
233. How many grams of NaCl are contained in 350. mL respectively.
of a 0.208 M solution of sodium chloride? E) precipitation, redox, and acid-base reactions,
A) 12.2 g respectively.
B) 4.25 g
C) 8.51 g 258. The balanced molecular equation contains which one
D) 72.8 g of the following terms?
E) none of these A) AgCl(s)
B) 2AgCl(s)
235. What mass of calcium chloride, CaCl2, is needed to C) 2Ba(NO3)2
prepare 4.023 L of a 1.56 M solution? D) BaNO3
A) 286 g E) 3AgCl(s)
B) 6.28 g
C) 43.0 g 259. The balanced complete ionic equation contains
D) 111 g which of the following terms?
E) 696 g A) 2Ba2+(aq)
B) Cl–(aq)
238. A 51.24-g sample of Ba(OH)2 is dissolved in enough C) 2Ag+(aq)
water to make 1.581 liters of solution. How many mL of this D) NO3 – (aq)
solution must be diluted with water in order to make 1.000 E) 3NO3 – (aq)
liter of 0.1000 molar Ba(OH)2?
A) 529 mL 260. The net ionic equation contains which of the
B) 189 mL following terms?
C) 18.9 mL A) Ag+(aq)
D) 63.3 mL B) Ba2+(aq)
E) 252 mL C) NO3 – (aq)
D) 2NO3 – (aq)
243. The net ionic equation for the reaction of calcium E) none of these
bromide and sodium phosphate contains which of the
following species? 264. Which of the following salts is insoluble in water?
A) Ca2+(aq) A) Na2S
B) PO43–(aq) B) K3PO4
C) 2Ca3(PO4)2(s) C) Pb(NO3)2
D) 6NaBr(aq) D) CaCl2
E) 3Ca2+(aq) E) All of these are soluble in water.
244. Which of the following is a strong acid? 267. Which of the following ions is most likely to form
A) HF an insoluble sulfate?
B) KOH A) K+
C) HClO4 B) Li+
D) HClO C) Ca2+
D) S2–
-4-
E) Cl– C) oxidized.
D) the electron donor.
274. You mix 60. mL of 1.00 M silver nitrate with 25 mL E) two of these
of 1.73 M sodium chloride. What mass of silver chloride
should you form? 293. In the reaction N2(g) + 3H2(g) 2NH3(g), N2 is
A) 6.2 g A) oxidized.
B) 12.4 g B) reduced.
C) 8.6 g C) the electron donor.
D) 14.9 D) the reducing agent.
E) none of these E) two of these
281. You have 75.0 mL of a 2.50 M solution of 297. For the reaction of sodium bromide with chlorine
Na2CrO4(aq). You also have 125 mL of a 2.10 M solution of gas to form sodium chloride and bromine, the appropriate
AgNO3(aq). Calculate the concentration of CrO42- when the half-reactions are (ox = oxidation and re = reduction):
two solutions are added together. A) ox: Cl2 + 2e– 2Cl–; re: 2Br– Br2 +
A) 0.00 M 2e–
B) 0.281 M B) ox: 2Br– Br2 + 2e–; re: Cl2 + 2e–
C) 0.188 M 2Cl–
D) 0.263 M C) ox: Cl + e– Cl–; re: Br Br– + e–
E) 2.50 M –
D) ox: Br + 2e Br ; 2–
re: 2Cl– Cl2 +
–
2e
282. You have 75.0 mL of a 2.50 M solution of E) ox: 2Na+ + 2e– 2Na; re: 2Cl– Cl2 +
Na2CrO4(aq). You also have 125 mL of a 2.43 M solution of 2e–
AgNO3(aq). Calculate the concentration of Ag+ when the two
solutions are added together. 304. In the reaction shown below, what species is
A) 0.00 M oxidized?
B) 0.759 M
2NaI + Br2 2NaBr + I2
C) 1.52 M
A) Na+
D) 1.88 M
B) I–
E) 0.304 M
C) Br2
D) Br–
287. In which of the following does nitrogen have an
E) I2
oxidation state of +4?
A) HNO3
306. Balance the following oxidation-reduction reaction
B) NO2
using the half-reaction method:
C) N2O
Fe3+ + I– Fe2+ + I2
D) NH4Cl
In the balanced equation, the coefficient of Fe2+ is
E) NaNO2
A) 1.
B) 2.
289. The following reactions
C) 3.
ZnBr2(aq) + 2AgNO3(aq) Zn(NO3)2(aq) + 2AgBr(s)
D) 4.
KBr(aq) + AgNO3(aq) AgBr(s) + KNO3(aq) E) none of these
are examples of
A) oxidation-reduction reactions. Use the following to answer questions 308-310:
B) acid-base reactions.
C) precipitation reactions. The following reaction occurs in aqueous acid solution:
D) a and c
E) none of these NO3– + I– IO3– + NO2
308. The oxidation state of iodine in IO3– is:
291. In the reaction 2Ca(s) + O2(g) 2CaO(s), which A) 0
species is oxidized? B) +3
A) O2 C) –3
B) O2– D) +5
C) Ca E) –5
D) Ca2+ 309. In the balanced equation the coefficient of NO3– is:
E) none of these A) 2
B) 3
292. In the reaction 2Cs(s) + Cl2(g) 2CsCl(s), Cl2 is C) 4
A) the reducing agent. D) 5
B) the oxidizing agent. E) 6
-5-
B) 15.9 L
310. In the balanced equation the coefficient of water is: C) 38.4 L
A) 1 D) 99.4 L
B) 2 E) 22.4 L
C) 3
D) 4 345. Mercury vapor contains Hg atoms. What is the
E) 5 volume of 200. g of mercury vapor at 822 K and 0.386 atm?
A) 174 L
311. When the equation Cl2 Cl– + ClO3– (basic B) 3.49e4 L
solution) is balanced using the smallest whole-number C) 232 L
coefficients, the coefficient of OH– is: D) 26.1 L
A) 1 E) 13.0 L
B) 2
C) 3 351. You have 48.7 g of O2 gas in a container with twice
D) 4 the volume as one with CO2 gas. The pressure and
E) 6 temperature of both containers are the same. Calculate the
mass of carbon dioxide gas you have in the container.
A) 67.0 g
333. A gas sample is held at constant pressure. The gas B) 0.761 g
occupies 3.62 L of volume when the temperature is 21.6 oC. C) 33.5 g
Determine the temperature at which the volume of the gas is D) 3.04 g
3.35 L. E) none of these
A) 318 K
B) 273 K 357. A 3.74-g piece of solid CO2 (dry ice) is allowed to
C) 20.0 K sublime in a balloon. The final volume of the balloon is 1.00
D) 295 K L at 300. K. What is the pressure of the gas?
E) 546 K A) 2.09 atm
B) 92 atm
334. Gaseous chlorine is held in two separate containers C) 6.58 atm
at identical temperature and pressure. The volume of D) 0.478 atm
container 1 is 1.30 L and it contains 6.70 mol of the gas. The E) none of these
volume of container 2 is 2.88 L. How many moles of the gas
are in container 2? 372. Gaseous C2H4 reacts with O2 according to the
A) 14.8 mol following equation:
B) 25.1 mol
C) 0.559 mol C2 H 4 ( g ) 3O2 ( g ) 2CO2 ( g ) 2 H 2O( g )
D) 3.02 mol
E) none of these
What volume of oxygen gas at STP is needed to react with
o 3.27 mol of C2H4? (Ignore signficant figures for this
335. A balloon has a volume of 1.97 liters at 24.0 C. The
problem.)
balloon is heated to 48.0oC. Calculate the new volume of the
A) 9.81 L
balloon.
B) 24.4 L
A) 1.97 L
C) 220 L
B) 2.13 L
D) 73.2 L
C) 1.82 L
E) Not enough information is given to solve the
D) 3.94 L
problem.
E) 0.985 L
376. If a 2.13-g sample of a gas occupies 750. mL at STP,
340. The valve between a 5-L tank containing a gas at 9
what is the molar mass of the gas at 125oC?
atm and a 10-L tank containing a gas at 6 atm is opened.
A) 3.35e-2 g/mol
Calculate the final pressure in the tanks.
B) 63.6 g/mol
A) 3 atm
C) 2.84 g/mol
B) 4 atm
D) 7.89 g/mol
C) 7 atm
E) Not enough information is given.
D) 15 atm
E) none of these
384. A mixture is prepared from 15.0 L of ammonia and
15.0 L chlorine measured at the same conditions, these
341. You fill a balloon with 2.50 moles of gas at 28 oC at a
compounds react according to the following equation:
pressure of 1.61 atm. What is the volume of the balloon?
A) 3.57 L 2NH3(g) + 3 Cl2(g) N2(g) + 6HCl(g)
-6-
When the reaction is completed, what is the volume of each 410. The van der Waals equation, nRT = [P + (n2a/V2)] (V
gas (NH3, Cl2, N2, and HCl, respectively)? Assume the final – nb), incorporates corrections to the ideal gas law in order to
volumes are measured under identical conditions. account for the properties of real gases. One of the
A) 0.00 L, 5.00 L, 7.50 L, 45.0 L corrections accounts for
B) 5.00 L, 0.00 L, 5.00 L, 30.0 L A) the possibility of chemical reaction between
C) 0.00 L, 0.00 L, 7.50 L, 45.0 L molecules.
D) 0.00 L, 0.00 L, 5.00 L, 30.0 L B) the finite volume of molecules.
E) 0.00 L, 10.0 L, 15.0 L, 90.0 L C) the quantum behavior of molecules.
D) the fact that average kinetic energy is inversely
394. What volume does 45.3 g of N2 occupy at STP? proportional to temperature.
A) 72.4 L E) the possibility of phase changes when the
B) 2.02 L temperature is decreased or the pressure is increased.
C) 36.2 L
D) 503 L 413. Order the following in increasing rate of effusion:
E) none of these F2, Cl2, NO, NO2, CH4
A) Cl2 Ca2+ > K+ > Cl– > S2– D) NaBr
B) S2– > Cl– > K+ > Ca2+ > Ga3+ E) BaS
C) Ga3+ > S2– > Ca2+ > Cl– > K+
D) Ga3+ > Ca2+ > S2– > Cl– > K+ 639. Which of the following species is best described by
E) Ga3+ > Ca2+ > S2– > K+ > Cl– drawing resonance structures?
A) PH3
627. Given the following information: B) NH4+
Li(s) Li(g) of sublimation of Li(s) = 166 kJ/mol C) O3
D) SO3-
HCl(g) H(g) + Cl(g) bond energy of HCl = 427 kJ/mol
E) HCN
Li(g) Li+(g) + e– ionization energy of Li(g) = 520.
kJ/mol
641. Given the following bond energies
Cl(g) + e– Cl–(g) electron affinity of Cl(g) = –349
kJ/mol C–C 347 kJ/mol
Li+(g) + Cl–(g) LiCl(s) lattice energy of LiCl(s) = –829 C=C 614 kJ/mol
kJ/mol C–O 358 kJ/mol
H2(g) 2H(g) bond energy of H2 = 432 kJ/mol C=O 799 kJ/mol
C–H 413 kJ/mol
A) 363 kJ O–H 463 kJ/mol
B) –562 kJ O–O 146 kJ/mol
C) –179 kJ
D) –73 kJ estimate H for the reaction H2O2 + CH3OH H2CO +
E) None of these 2H2O.
A) –345 kJ
629. Choose the molecule with the strongest bond. B) –199 kJ
A) F2 C) –105 kJ
B) Cl2 D) +199 kJ
C) Br2 E) +345 kJ
- 15 -
B) -1
643. As indicated by Lewis structures, which of the C) 0
following would probably not exist as a stable molecule? D) 2
A) CH3OH E) 2
B) CH2O
C) CH3O 653. How many of the following molecules—SF2, SF4,
D) C2H2 SF6, SiO2—are polar?
E) C3H4 A) 0
B) 1
645. Select the best Lewis structure for acetone, C) 2
CH3COCH3. D) 3
A) E) 4
H H
655. How many resonance structures can be drawn for the
H C C O C H molecule O3?
A) 1
H H B) 2
B) C) 3
H O H D) 4
E) 5
H C C C H
657. Choose the electron dot formula that most accurately
H H describes the bonding in CS2. (Hint: Consider formal
C) charges.)
H A) S C S
H C C O H C H B) C S S
H H C) S C S
D) S C S
D)
H
E) S C S
H H C C O C H
H H 661. Complete the Lewis structure for the molecule:
E) CH3 O
H H H
CH3 CH C C N
H C C C O This molecule has __________ single bonds and __________
H H multiple bonds.
A) 4, 2
647. Of the following, which molecule has the largest B) 6, 3
bond angle? C) 11, 5
A) O3 D) 11, 2
B) OF2 E) 13, 0
C) HCN
D) H2O 665. The force between two bodies having identical
E) More than one of the above have equally large electric charges
bond angles. A) is a force of repulsion.
B) is a force of repulsion if the charges are
649. The Cl–Kr–Cl bond angle in KrCl4 is closest to negative, and one of attraction if they are positive.
A) 90° C) increases as the bodies are moved farther apart.
B) 109° D) is independent of the distance between them.
C) 120° E) is directly proportional to the distance between
D) 150° them.
E) 360°
669. Which of the following molecules contains a double
651. –
In the cyanide ion (CN ), the nitrogen has a formal bond?
charge of A) CO2
A) -2 B) NH3
C) H2O
- 16 -
D) all 683. How many of the following molecules or ions are
E) none linear?
NH3 NH4+ HCN CO2 NO2
673. Which of the following compounds contains only
one unshared pair of valence electrons? A) 0
A) NH3 B) 1
B) H2O C) 2
C) CH4 D) 3
D) NaCl E) 4
E) BeF3
685. Which of the following molecules are nonlinear?
675. The Lewis structure for H3BO3 is NO2–, C2H2, N3–, HCN, CO2, H2O2
A) A) C2H2, HCN
H O B O H B) CO2, N3–
C) NO2–, H2O2
O D) N3–, N2–
E) all are linear
H
B) 687. Which of the following species has a trigonal
H O B O H bipyramid structure?
A) NH3
O B) IF5
H C) I3–
C) D) PCl5
E) none of these
H O B O H
O 689. Which ion is planar?
A) NH4+
H B) CO32–
D) C) SO32–
H O B O H D) ClO3–
E) all are planar
O
691. In the molecule XeF2, how many pairs of electrons
H surround Xe and what is the molecular geometry?
E) A) 4, bent
H O B O H B) 4, pyramidal
C) 5, linear
O D) 5, bent
H E) 6, linear
693. How many of the following molecules have all of
677. In the Lewis structure for SF6, the central sulfur
their atoms in the same plane?
atom shares __________ electrons.
H2C=CH2 F2O H2CO NH3 CO2 BeCl2
A) 4
B) 8
A) 3
C) 10
B) 4
D) 12
C) 5
E) none of the above, because SF6 is an ionic
D) 6
compound
E) 7
681. Which of the following molecules has a nonlinear
695. Which of the following statements are true
structure?
concerning ionic bonding?
A) XeF2
A) Ionic bonding occurs between a metal, which
B) BeCl2
has a high affinity for electrons, and a nonmetal,
C) O3
which loses electrons relatively easy.
D) CO2
B) CaCl2 forms because Ca2+ is always a more
E) N2O (central atom is N)
stable species than the calcium atom alone.
C) Compounds with ionic bonds tend to have low
melting points.
- 17 -
D) The electronegativity difference between the C) The bond order of each C—C bond in benzene
bonding atoms of ionic compounds is small since the is 1.5.
electrons are not shared but rather held together by D) Benzene is an example of a molecule that
electrostatic forces. displays ionic bonding.
E) All of the above statements are false. E) All of these statements are false.
697. If a compound has a number of individual dipoles,
then 709. What hybridization is predicted for the nitrogen
I. it is polar overall. atom in the NO3– ion?
II. there is an electronegativity difference between the A) sp2
bonded atoms. B) sp3
III. it is ionic. C) sp3d
IV. it doesn't have resonance. D) sp3d2
E) none of these
A) II only
B) II, IV 711. Consider the following Lewis structure
C) I, II, IV H O H H
D) I, III
E) All of the above statements are correct. H C C C C H
3 2 1
699. The hybridization of the phosphorus atom in the H
cation PH2+ is: Which statement about the molecule is false?
A) sp2 A) There are 10 sigma and 2 pi bonds.
B) sp3 B) C–2 is sp2 hybridized with bond angles of 120°.
C) dsp C) Oxygen is sp3 hybridized.
D) sp D) This molecule contains 28 valence electrons.
E) none of these E) There are some H–C–H bond angles of about
109° in the molecule.
701. Which of the following statements is (are) incorrect?
I. The hybridization of boron in BF3 is sp2. 713. Consider the following Lewis structure:
II. The molecule XeF4 is nonpolar. H H H
III. The bond order of N2 is three.
H C O C C C C N H
IV. The molecule HCN has two pi bonds and two sigma 1 2 3 4
bonds. H H
A) All four statements are correct.
B) II is incorrect. O C–1 C–2 C–4
C) I and IV are incorrect.
D) II and III are incorrect. A) sp3 sp sp3 sp2
E) II, III, and IV are incorrect.
B) sp sp3 sp sp
+
703. The hybridization of the central atom in XeF5 is:
A) sp C) sp sp2 sp sp2
B) sp2
C) sp3 D) sp2 sp3 sp2 sp3
D) dsp3
E) d2sp3 E) sp sp3 sp2 sp
705. The hybridization of the central atom in I3- is: O C-1 C-2 C-4
A) sp
B) sp2
C) sp3 715. The hybridization of Cl in ClF2+ is
D) dsp3 A) sp
E) d2sp3 B) sp2
C) sp3
707. Which of these statements about benzene is true? D) dsp3
A) All carbon atoms in benzene are sp3 hybridized. E) d2sp3
B) Benzene contains only bonds between C
717. The hybridization of the central atom, Al, in AlBr3 is
atoms.
- 18 -
A) sp A) It is paramagnetic.
B) sp2 B) Its bond order is 2.
C) sp3 C) The total number of electrons is 12.
D) dsp3 D) It has two pi bonds.
E) d2sp3 E) All of these are true.
719. The hybridization of Br in BrF3 is 739. Which of the following statements is true?
A) sp A) Electrons are never found in an antibonding
B) sp2 MO.
C) sp3 B) All antibonding MOs are higher in energy than
D) dsp3 the atomic orbitals of which they are composed.
E) d2sp3 C) Antibonding MOs have electron density mainly
outside the space between the two nuclei.
721. What is the bond order of C2+? D) None of the above is true.
A) 0 E) Two of the above statements are true.
B) 1/2
C) 1 741. Which of the nitrogen-containing molecules below is
D) 1 1/2 paramagnetic in its lowest energy state?
E) 2 A) N2
B) NO
723. The hybridization of the lead atom in PbCl4 is C) NH3
A) dsp2 D) N2H4
B) sp2 E) none of these
C) d2sp3
D) sp2d 743. Which of the following molecules or ions is not
E) none of these paramagnetic in its ground state?
A) O2
725. Which of the following statements is false? B) O2+
A) C2 is paramagnetic. C) B2
B) C2 is diamagnetic. D) NO
C) The carbon-carbon bond in C22– is stronger than E) F2
the one in CH3CH3.
D) The carbon-carbon bond in C22– is shorter than 745. The configuration (2s)2(2s*)2(2py)1 (2px)1 is
the one in CH3CH3. the molecular orbital description for the ground state of
E) Two of the above. A) Li2+
B) Be2
731. Complete the Lewis structure for the following C) B2
molecule: D) B22–
CH3 O E) C2
CH3 CH C C N 747. Which of the following species has the largest
dissociation energy?
This molecule has __________ sigma and __________ pi A) O2
bonds. B) O2–
A) 4, 5 C) O22–
B) 6, 3 D) O2+
C) 11, 5 E) O22+
D) 13, 2
E) 13, 3 749. For how many of the following does the bond order
decrease if you add one electron to the neutral molecule?
733. Which of the following molecules has a bond order B2, C2, P2, F2
of 1.5? A) 0
A) O2+ B) 1
B) N2 C) 2
C) O2– D) 3
D) C2 E) 4
E) none of these
751. Which of the following diatomic molecules has a
737. Which of the following statements about the bond order of 2?
molecule BN is false? A) B2
- 19 -
B) C2 D) The ion has a total of 24 electrons.
C) P2 E) All the above statements are true.
D) F2
E) Na2 765. What is the bond order of He2+?
A) 0
753. Consider the molecular orbital energy level diagrams B) 1/2
for O2 and NO. Which of the following is true? C) 1
I. Both molecules are paramagnetic. D) 1 1/2
II. The bond strength of O2 is greater than the bond strength E) 2
of NO.
III. NO is an example of a homonuclear diatomic molecule. 767. Consider the benzene molecule. Which of the
IV. The ionization energy of NO is smaller than the ionization following statements about the molecule is false?
A) All six C C bonds are known to be
energy of NO+.
equivalent.
B) Each carbon atom is sp2 hybridized.
A) I only
C) The localized electron model must invoke
B) I and II
C) I and IV resonance to account for the six equal C C bonds.
D) II and III D) It has delocalized pi bonding in the molecule.
E) I, II, and IV E) The pi bonds of carbon involve sp2 orbitals.
755. Order the following from shortest to longest bond: 769. If a molecule demonstrates paramagnetism, then
C2, B2, H2, N2 I. the substance can have both paired and unpaired electrons.
A) H2, N2, C2, B2 II. the bond order is not a whole number.
B) N2, C2, B2, H2 III. it can be determined by drawing a Lewis structure.
C) C2, N2, H2, B2 IV. it must be an ion.
D) C2, B2, H2, N2
E) none of these A) I, II
B) I, II, IV
757. For how many of the following does bond order C) II, III
decrease if you take away one electron from the neutral D) I only
molecule? E) all of the above are correct
B2, C2, P2, F2
A) 0 773. Which of the following statements are incorrect?
B) 1 A) For the molecule NO, the molecular orbital
C) 2 model is preferred over the localized electron model
D) 3 because NO contains an unpaired electron.
E) 4 B) Electrons in antibonding orbitals will cause a
molecule to be paramagnetic.
759. In the molecular orbital description of CO, C) According to the molecular orbital model,
A) the highest energy electrons occupy when bonding occurs between hydrogen and
antibonding orbitals. bromine to make HBr, the 1s orbital of the hydrogen
B) six molecular orbitals contain electrons. atom no longer exists.
C) there are two unpaired electrons. D) Antibonding electrons are higher in energy than
D) the bond order is 3. the atomic orbitals from which they came from.
E) All of the above are false. E) At least two of the above are incorrect.
761. The bond order in the NO molecule is 775. Name the following:
A) 1. CH3
B) 1.5.
C) 2.
D) 2.5. CH3CH2CCH3
E) 3.
763. Which of the following statements (a–d) about the CH2CH3
CO32– ion is false?
A) The orbitals on the carbon atom are sp2 A) n-heptane
hybridized. B) 2-methyl-2-ethylbutane
B) The ion is expected to be diamagnetic. C) 3,3-dimethylpentane
C) One C–O bond is shorter than the other. D) 2,2-diethylpropane
- 20 -
777. Name the following: E) I, II, III, IV
H
783. Which of the following names is a correct one?
HCH A) 3-methyl-4-isopropylpentane
B) 2-ethyl-4-tertiary-butylpentane
H HCH H H H C) 2,2,3,5-tetramethylheptane
D) t-butylethane
H C C C C C H E) trans-1,2-dimethylethane
785. How many isomers of C3H8 are there?
H H H HCH H
A) 1
B) 2
HCH C) 3
H D) 5
E) 6
A) 2,4-diethylpentane
B) 3,5-dimethylheptane
787. How many isomers are there of "dichloroethene"?
C) secondary ethylpentane
A) 2
D) 2,3-dimethyl-2,3-diethylpropane
B) 3
E) none of these
C) 4
D) 5
779. Name the following:
E) 6
CH3
789. Which is a possible product of the chlorination of
CH3CH2CHCH2CH3 butane in the presence of light?
A) n-hexane A) C4H9Cl
B) isohexane B) C4H8Cl
C) 1,2,3-trimethylpropane C) C4H10Cl2
D) methyl-diethylmethane D) C4H6Cl2
E) 3-methylpentane E) C4H9Cl2
780. Name the following: 791. Which of the following pairs is incorrect?
CH3(CH2)7 CH3 A) ethane – C2H4
A) heptane B) pentane – C5H12
B) hexane C) hexane – C6H14
C) octane D) heptane – C7H16
D) nonane E) octane – C8H18
E) decane
793. Propane undergoes dehydrogenation. The product of
781. The compound below is the carbon skeleton (minus this is
any hydrogen atoms) of A) 1-propene
B) 2-propene
C C C) cis-1-propene
D) trans-1-propene
C C C C C C C E) cis-2-propene
C C C 795. How many of the following molecules exist?
I. methene
I. C12H26
II. cycloethane
II. a substituted octane
III. cyclopropyne
III. a compound with 3 tertiary carbons
IV. neobutane
IV. a compound with 3 secondary carbons
V. a compound with 2 isopropyl groups A) 0
B) 1
A) I, II, III C) 2
B) II, III, IV D) 3
C) III, IV, V E) 4
D) II, IV, V
- 21 -
797. Name the following: D) 5
E) 6
807. For which of the following compound(s) are cis and
trans isomers possible?
A) 2-chloro-3-chloro-cis-2-butene A) 2,3-dimethyl-2-butene
B) 2,3-dichloro-cis-2-butene B) 3-methyl-2-pentene
C) 2,3-dichloro-trans-2-butene C) 4,4-dimethylcyclohexanol
D) 1-chloro-1-methyl-2-chloro-propene D) ortho-chlorotoluene
E) 2,3-dichloro-1-methyl-propene E) All can exhibit cis/trans isomers.
809. How many different possible tetramethylbenzenes
799. CH3C CCH2CH2Cl is named:
exist?
A) 1-chloro-3-pentyne
A) 2
B) 5-chloro-2-pentene
B) 3
C) 1-acetylenyl-3-chloropropane
C) 4
D) 5-chloro-2-pentyne
D) 5
E) 1-chloro-3-pentene
E) 6
801. Which of the following compounds can exhibit
811. Mothballs contain what aromatic hydrocarbon?
geometrical isomerism?
A) naphthalene
A)
B) benzene
C) anthracene
D) phenanthrene
E) toluene
B)
813. Which of the following has an optical isomer?
A)
C)
B)
D)
C)
E)
D)
803. How many structural and geometrical isomers are
there of chloropropene?
A) 2
B) 3
C) 4
D) 5
E) none of these
E) more than 5
815. Name the following:
805. How many geometric isomers can be drawn for the
following compound: CH3CH=CHCH2CH=C(CH3)2
A) 2
B) 3
C) 4
- 22 -
H 827. The boiling point of methanol is much higher than
that of ethane. This is primarily due to
H O H C H A) the difference in molar masses of methanol and
ethane.
H C C O C H B) the hydrogen bonding in methanol.
C) the significant molecular size difference
H H C H between methanol and ethane.
D) the carbon oxygen double bond in the
H methanol.
A) n-propyl acetate E) none of these.
B) isopropyl formate
C) isopropyl acetate 829. Referring to the structures below, which statement is
D) ethyl propanoate true?
E) none of these O
817. Name the following:
I.
H C O CH2 CH2OH
H H H H O
H C C O C C H
II.
HOCH2CH2 C OH
H H H H O
A) acetone
B) butyraldehyde III
HOCH2CH2 O C H
C) diethylketone
D) diethyl ether A) I and II have different molecular formulas.
E) none of these B) I and III are structural isomers of each other.
C) II and III are stereoisomers of each other.
819. Oxidation of 2-methyl-l-butanol could yield D) II and III are different conformations of the
A) 2-methyl-l-butanone same compound.
B) 2-methyl-l-butanol E) I and III are the same compound.
C) 2-methylbutanoic acid
D) both b and c 831. Identify the type of organic compound shown:
E) both a and c H3C C CH2CH3
821. Which of the following is known as rubbing O
alcohol?
A) methanol A) aldehyde
B) ethanol B) ester
C) propanol C) amine
D) isopropanol D) alcohol
E) none of these E) none of these
823. Oxidation of a primary alcohol results in a(n) 833. Identify the type of organic compound shown:
__________ and oxidation of a secondary alcohol results in (CH3)3N
a(n) _________. A) aldehyde
A) carboxylic acid, amine B) ester
B) aldehyde, ketone C) amine
C) ester, ether D) ketone
D) ketone, aldehyde E) none of these
E) amine, carboxylic acid
835. Classify the following molecule:
825. Which of the following has only one single C-O CH3 H
bond?
A) ketone H3C C C CH2 CH3
B) alcohol
C) ether O H
D) ester
E) aldehyde H
A) primary alcohol
B) secondary alcohol
- 23 -
C) tertiary alcohol H
D) ether
E) phenol CH3CH2 C OH
837. Which molecule is an ester? CH3
A) B)
H
CH3CH2 C CHO
B) CH3CH2OCH3 CH3
C)
O
C) CH3 CH C CH3
D) CH3CH2NH2
E) none of these CH3
D)
839. Which molecule is an ether? H
A)
CH3 CH2 C NH2
CH3
E)
B) CH3CH2OCH3
CH3
CH3 C CH2 CHO
C)
D) CH3CH2NH2 CH3
E) none of these
847. Which of the following molecules exhibits chirality?
841. Identify the secondary amine. A) CH4
A) CH3NH2 B) CH3OH
B) (CH3)2NH C) CH3CH2OH
H H H D)
H H H
H C C C H
H C C C H
C)
H NH2 H
D) NH3 H OH H
E) (CH3)3N E) none of these
843. Classify the following molecule: 849. Which of the following becomes more soluble in
water upon addition of NaOH?
O A) an amine
B) a carboxylic acid
H3C C CH2CH3 C) an amine
A) acid D) an aromatic hydrocarbon
B) aldehyde E) an alkane
C) amine
D) ketone 851. When C4H8 is treated with water and H2SO4 a
E) carbonyl tertiary alcohol is produced. Which of the following
structures could represent C4H8 in this reaction?
845. Which structure represents an optically active A) CH3CH = CHCH3
aldehyde? B) CH3CH2CH = CH2
A) C)
- 24 -
CH3 C CH2 A) orange juice
B) aspirin
CH3 C) acetone
D) CH3CH2CH2CH3 D) bananas
E) none of these E) vinegar
853. Which of the following will yield a carboxylic acid 863. A carboxylic acid will react with an alcohol to form
upon oxidation? a(n) __________ and a water molecule.
A) a secondary alcohol A) ester
B) an aldehyde B) amine
C) a cycloalkane C) polymer
D) a ketone D) ketone
E) tertiary alcohol E) aldehyde
861. What is the common name for acetylsalicylic acid?
- 25 -