C
The energy required to convert a ground-state atom in the gas phase to a gaseous positive ion
(A) Activation energy
(B) Free energy
(C) Ionization energy
(D) Kinetic energy
(E) Lattice energy
E
The energy change that occurs in the conversion of an ionic solid to widely separated gaseous ions
(A) Activation energy
(B) Free energy
(C) Ionization energy
(D) Kinetic energy
(E) Lattice energy
A
Cesium chloride, CsCl (s)
(A) Lattice of positive and negative ions held together by electrostatic forces.
(B) Closely packed lattice with delocalized electrons throughout
(C) Strong single covalent bonds with weak intermolecular forces.
(D) Strong multip
B
Gold, Au(s)
(A) Lattice of positive and negative ions held together by electrostatic forces.
(B) Closely packed lattice with delocalized electrons throughout
(C) Strong single covalent bonds with weak intermolecular forces.
(D) Strong multiple covalent bo
D
Carbon dioxide, CO2(s)
(A) Lattice of positive and negative ions held together by electrostatic forces.
(B) Closely packed lattice with delocalized electrons throughout
(C) Strong single covalent bonds with weak intermolecular forces.
(D) Strong multiple
C
Methane, CH4(s)
(A) Lattice of positive and negative ions held together by electrostatic forces.
(B) Closely packed lattice with delocalized electrons throughout
(C) Strong single covalent bonds with weak intermolecular forces.
(D) Strong multiple covalen
B
When a solution of sodium chloride is vaporized in a flame, the color of the flame is
(A) blue
(B) yellow
(C) green
(D) violet
(E) White
E
A hot-air balloon rises. Which of the following is the best explanation for this observation?
(A) The pressure on the walls of the balloon increases with increasing tempearature.
(B) The difference in temperature between the air inside and outside the bal
C
The cooling curve for a pure substance as it changes from a liquid to a solid is shown right. The solid and the liquid coexist at
(A) point Q only
(B) point R only
(C) all points on the curve between Q and S
(D) all points on the curve between R and T
(E)
B
The melting point of MgO is higher than that of NaF. Explanations for this observation include which of the following?
I. Mg2+ is more positively charged than Na+
II. O2� is more negatively charged than F�
III. The O2� ion is smaller than the F� ion
(A) I
E
O
||
CH3-C-CH2-CH3
The organic compound represented above is an example of
(A) an organic acid
(B) an alcohol
(C) an ether
(D) an aldehyde
(E) a ketone
D
Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include which of the following?
I. sp
II. sp2
III. sp3
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
C
A 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. What is the minimum number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl� as AgCl(s) ? (Assume that AgCl is insoluble.)
(A)
C
The ionization energies for element X are listed in the table above. On the basis of the data, element X is most likely to be
(A) Na
(B) Mg
(C) Al
(D) Si
(E) P
D
Of the following molecules, which has the largest dipole moment?
(A) CO
(B) CO2
(C) O2
(D) HF
(E) F2
C
A sample of 61.8 g of H3BO3, a weak acid is dissolved in 1,000 g of water to make a 1.0-molal solution. Which of the following would be the best procedure to determine to molarity of the solution? (Assume no additional information is available.)
(A) Titra
D
In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius?
(A) It remains constant.
(B) It increases only.
(C) It increases, then decreases.
(D) It decreases only.
(E) It decreases, then increases.
E
Which of the following is a correct interpretation of the results of Rutherford's experiments in which gold atoms were bombarded with alpha particles?
(A) Atoms have equal numbers of positive and negative charges.
(B) Electrons in atoms are agganged in sh
A
A yellow precipitate forms when 0.5 M NaI(aq) is added to a 0.5 M solution of which of the following ions?
A) Pb2+(aq)
B) Zn2+(aq)
C) CrO42�(aq)
D) SO42�(aq)
E) OH�(aq)
C
On a mountaintop, it is observed that water boils at 90�C, not at 100�C as at sea level. This phenomenon occurs because on the mountaintop the
A) equilibrium water vapor pressure is higher due to the higher atmospheric pressure
B) equilibrium water vapor
A
Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial pressures of the gases remaining i
B
In a qualitative ananlysis for the presence of Pb2+, Fe2+, and Cu2+ ions in a aqueous solution, which of the following will allow the separation of Pb2+ from the other ions at room temperature?
A) Adding dilute Na2S(aq) solution
B) Adding dilute HCl(aq) s
B
After completing an experiment to determine gravimetrically the percentage of water in a hydrate, a student reported a value of 38 percent. The correct value for the percentage of water in the hydrate is 51 percent. Which of the following is the most like
D
The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl(aq) in order to prepare a 0.500 M HCl(aq) solution is approximately
A) 50.0 mL
B) 60.0 mL
C) 100. mL
D) 110. mL
E) 120. mL
A
Which of the following gases deviates most from ideal behavior?
A) SO2
B) Ne
C) CH4
D) N2
E) H2
D
Which of the following pairs of liquids forms the solution that is most ideal (most closely follows Raoult's law)?
A) C8H18(l) and H2O(l)
B) CH3CH2CH2OH(l) and H2O(l)
C) CH3CH2CH2OH(l) and C8H18(l)
D) C6H14(l) and C8H18(l)
E) H2SO4(l) and H2O(l)
A
What is the most electronegative element?
(A) O
(B) La
(C) Rb
(D) Mg
(E) N
E
Which element exhibits the greatest number of different oxidation states?
(A) O
(B) La
(C) Rb
(D) Mg
(E) N
D
Which of the elements above has the smallest ionic radius for its most commonly found ion?
(A) O
(B) La
(C) Rb
(D) Mg
(E) N
C
An impossible electronic configuration
(A) 1s2 2s2 2p5 3s2 3p5
(B) 1s2 2s2 2p6 3s2 3p6
(C) 1s2 2s2 2p6 2d10 3s2 3p6
(D) 1s2 2s2 2p6 3s2 3p6 3d5
(E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2
E
The ground-state configuration for the atoms of a transition element
(A) 1s2 2s2 2p5 3s2 3p5
(B) 1s2 2s2 2p6 3s2 3p6
(C) 1s2 2s2 2p6 2d10 3s2 3p6
(D) 1s2 2s2 2p6 3s2 3p6 3d5
(E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2
B
The ground-state configuration of a negative ion of a halogen
(A) 1s2 2s2 2p5 3s2 3p5
(B) 1s2 2s2 2p6 3s2 3p6
(C) 1s2 2s2 2p6 2d10 3s2 3p6
(D) 1s2 2s2 2p6 3s2 3p6 3d5
(E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2
B
The ground-state configuration of a common ion of an alkaline earth element
(A) 1s2 2s2 2p5 3s2 3p5
(B) 1s2 2s2 2p6 3s2 3p6
(C) 1s2 2s2 2p6 2d10 3s2 3p6
(D) 1s2 2s2 2p6 3s2 3p6 3d5
(E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2
E
Is used to explain why iodine molecules are held together in the solid state
(A) hydrogen bonding
(B) hybridization
(C) ionic bonding
(D) resonance
(E) van der Waals forces (London dispersion forces)
A
Is used to explain why the boiling point of HF is greater than the boiling point of HBr
(A) hydrogen bonding
(B) hybridization
(C) ionic bonding
(D) resonance
(E) van der Waals forces (London dispersion forces)
B
Is used to explain the fact that the four bonds in methane are equivalent
(A) hydrogen bonding
(B) hybridization
(C) ionic bonding
(D) resonance
(E) van der Waals forces (London dispersion forces)
D
Is used to explain the fact that the carbon-to-carbon bonds in benzene, C6H6, are identical
(A) hydrogen bonding
(B) hybridization
(C) ionic bonding
(D) resonance
(E) van der Waals forces (London dispersion forces)
C
The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is
(A) 3.10 grams
(B) 12.0 grams
(C) 29.4 grams
(D) 294 grams
(E) 300. grams
C
A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.50 mole of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?
(A) 0.13 atm
(B) 0.27 atm
(C) 0.63 atm
(D) 0.90 atm
(E) 6.3 atm
C
The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron?
(A) Cl2
(B) N2
(C) NH3
(D) CCl4
(E) H2O2
E
6 I� + 2 MnO4� + 4 H2O(l) ---> 3 I2(s) + 2 MnO2(s) + OH�
Which of the following statements regarding the reaction represented by the equation above is correct?
(A) Iodide ion is oxidized by hydroxide ion.
(B) MnO4� is oxidized by iodide ion.
(C) The oxida
A
Which of the following is true at the triple point of a pure substance?
(A) The vapor pressure of the solid phase always equal the vapor pressure of the liquid phase.
(B) The temperature is always 0.01 K lower that the normal melting point.
(C) The liquid
D
__ Cr2O72� + __ e� + __ H+ ---> __ Cr3+ + __ H2O(l) When the equation for the half reaction above is balanced with the lowest whole-number coefficients, the coefficient for H2O is
(A) 2
(B) 4
(C) 6
(D) 7
(E) 14
E
How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms?
(A) 164 grams
(B) 96 grams
(C) 62 grams
(D) 50. grams
(E) 41 grams
B
The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams, 57.0 grams, 76.0 grams, and 114 grams, respectively. A possible atomic weight of Q is
(A) 12.7
(B) 19.0
(C) 27.5
(D) 38.0
(E) 57.0
D
The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is
(A) N2O
(B) NO
(C) NO2
(D) N2O3
(E) N2O5
C
How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl?
(A) 3.9 mL
(B) 35 mL
(C) 260 mL
(D) 1,000 mL
(E) 3,900 mL
B
Hydrogen gas is collected over water at 24 �C. The total pressure of the sample is 755 millimeters of mercury. At 24 �C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen gas?
(A) 22 mm Hg
(B) 733 mm Hg
A
The structural isomers C2H5OH and CH3OCH3 would be expected to have the same values for which of the following? (Assume ideal behavior.)
(A) Gaseous densities at the same temperature and pressure
(B) Vapor pressures at the same temperature
(C) Boiling poi
C
A 2.00-liter sample of nitrogen gas at 27 �C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is
(A) 68 �C
(B) 120 �C
(C) 477 �C
(D) 677 �C
(E) 950. �C
A
Which of the following conclusions can be drawn from J. J. Thomson's cathode ray experiments?
(A) Atoms contain electrons.
(B) Practically all the mass of an atom is contained in its nucleus.
(C) Atoms contain protons, neutrons, and electrons.
(D) Atoms h
B
When a hydrate of Na2CO3 is heated until all the water is removed, it loses 54.3 percent of its mass. The formula of the hydrate is
(A) Na2CO3 . 10 H2O
(B) Na2CO3 . 7 H2O
(C) Na2CO3 . 5 H2O
(D) Na2CO3 . 3 H2O
(E) Na2CO3 . H2O
D
2 K + 2 H2O ---> 2 K+ + 2 OH� + H2
When 0.400 mole of potassium reacts with excess water at standard temperature and pressure as shown in the equation above, the volume of hydrogen gas produced is
(A) 1.12 liters
(B) 2.24 liters
(C) 3.36 liters
(D) 4.48 l
D
The SbCl5 molecule has trigonal bipyramid structure. Therefore, the hybridization of Sb orbitals should be
(A) sp2
(B) sp3
(C) dsp2
(D) dsp3
(E) d2sp3
A
Which of the following does NOT behave as an electrolyte when it is dissolved in water?
(A) CH3OH
(B) K2CO3
(C) NH4Br
(D) HI
(E) Sodium acetate, CH3COONa
E
The metal calcium reacts with molecular hydrogen to form a compound. All of the following statements concerning this compound are true EXCEPT:
(A) Its formula is CaH2.
(B) It is ionic.
(C) It is solid at room temperatur(E)
(D) When added to water, it reac
D
A measured mass of an unreactive metal was dropped into a small graduated cylinder half filled with water. The following measurements were made.
Mass of metal = 19.611 grams
Volume of water before addition of metal = 12.4 milliliters
Volume of water after
C
CCl4, CO2, PCl3, PCl5, SF6 Which of the following does not describe any of the molecules above?
(A) Linear
(B) Octahedral
(C) Square planar
(D) Tetrahedral
(E) Trigonal pyramidal
B
The phase diagram above provides sufficient information for determining the
(A) entropy change on vaporization
(B) conditions necessary for sublimation
(C) deviations from ideal gas behavior of the gas phase
(D) latent heat of vaporization
(E) latent heat
D
For the substance represented in the diagram, which of the phases is most dense and which is least dense at - 15 �C.
Most Dense Least Dense
(A) Solid Gas
(B) Solid Liquid
(C) Liquid Solid
(D) Liquid Gas
(E) The diagram gives no information about densities
E
Which of the following compounds is ionic and contains both sigma and pi covalent bonds?
(A) Fe(OH)3
(B) HClO
(C) H2S
(D) NO2
(E) NaCN
C
As the temperature is raised from 20 � C to 40 � C, the average kinetic energy of neon atoms changes by a factor of
(A) 1/2
(B) [square root of](313/293)
(C) 313/293
(D) 2
(E) 4
E
A solution is known to contain an inorganic salt of one of the following elements. The solution is colorless. The solution contains a salt of
(A) Cu
(B) Mn
(C) Fe
(D) Ni
(E) Zn
A
A white solid is observed to be insoluble in water, insoluble in excess ammonia solution, and soluble in dilute HCl. Which of the following compounds could the solid be?
(A) CaCO3
(B) BaSO4
(C) Pb(NO3)2
(D) AgCl
(E) Zn(OH)2
A
How many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20-molar Fe(NO3)3 to increase the concentration of the NO3� ion to 1.0-molar? (Assume that the volume of the solution remains constant.)
(A) 0.060 mole
(B) 0.12 mole
(C) 0.24 mole
(
A
Adding water to some chemicals can be dangerous because large amounts of heat are liberated. Which of the following does NOT liberate heat when water is added to it?
(A) KNO3
(B) NaOH
(C) CaO
(D) H2SO4
(E) Na
C
Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic
(A) Heisenberg uncertainty principle
(B) Pauli exclusion principle
(C) Hund's rule (principle of maximum multiplicity)
(D) Shielding effect
(E) Wave nature of matter
E
Explains the experimental phenomenon of electron diffraction
(A) Heisenberg uncertainty principle
(B) Pauli exclusion principle
(C) Hund's rule (principle of maximum multiplicity)
(D) Shielding effect
(E) Wave nature of matter
B
Indicates that an atomic orbital can hold no more than two electrons
(A) Heisenberg uncertainty principle
(B) Pauli exclusion principle
(C) Hund's rule (principle of maximum multiplicity)
(D) Shielding effect
(E) Wave nature of matter
A
Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron
(A) Heisenberg uncertainty principle
(B) Pauli exclusion principle
(C) Hund's rule (principle of maximum multiplicity)
(D) Shielding effect
C
Has the largest bond-dissociation energy
(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2
D
Has a bond order of 2
(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2
C
Contains 1 sigma (s) and 2 pi (p) bonds
(A) Li2
(B) B2
(C) N2
(D) O2
(E) F2
C
Utilized as a coating to protect Fe from corrosion
(A) Pb
(B) Ca
(C) Zn
(D) As
(E) Na
D
Is added to silicon to enhance its properties as a semiconductor
(A) Pb
(B) Ca
(C) Zn
(D) As
(E) Na
A
Utilized as a shield from sources of radiation
(A) Pb
(B) Ca
(C) Zn
(D) As
(E) Na
C
Which of the following is lower for a 1.0-molar aqueous solution of any solute than it is for pure water?
(A) pH
(B) Vapor pressure
(C) Freezing point
(D) Electrical conductivity
(E) Absorption of visible light
E
In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron pairs are directed toward the corners of
(A) a tetrahedron
(B) a square-based pyramid
(C) a trigonal bipyramid
(D) a square
(E) an octahedron
B
In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00 ?
(A) CrO3
(B) CrO2
(C) CrO
(D) Cr2O
(E) Cr2O3
C
A sample of 0.0100 mole of oxygen gas is confined at 37� C and 0.216 atmosphere. What would be the pressure of this sample at 15� C and the same volume?
(A) 0.0876 atm
(B) 0.175 atm
(C) 0.201 atm
(D) 0.233 atm
(E) 0.533 atm
D
H2(g) + (1/2) O2(g) ---> H2O(l) DH� = - 286 kJ
2 Na(s) + (1/2) O2(g) ---> Na2O(s) DH� = - 414 kJ
Na(s) + (1/2) O2(g) + (1/2) H2(g) ---> NaOH(s) DH� = - 425 kJ
Based on the information above, what is the standard enthalpy change for the following reaction?
C
Which of the following actions would be likely to change the boiling point of a sample of a pure liquid in an open container?
I. Placing it in a smaller container
II. Increasing the number of moles of the liquid in the container
III. Moving the container
C
Which of the following sets of quantum numbers (n, l, ml, ms) best describes the valence electron of highest energy in a ground-state gallium atom (atomic number 31) ?
(A) 4, 0, 0, 1/2
(B) 4, 0, 1, 1/2
(C) 4, 1, 1, 1/2
(D) 4, 1, 2, 1/2
(E) 4, 2, 0, 1/2
D
CH3CH2OH boils at 78 �C and CH3OCH3 boils at - 24 �C, although both compounds have the same composition. This difference in boiling points may be attributed to a difference in
(A) molecular mass
(B) density
(C) specific heat
(D) hydrogen bonding
(E) heat
C
A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0 �C and 1.00 atmosphere. A possible formula for the hydrocarbon is
(A) CH2
(B) C2H4
(C) C3H6
(D) C4H8
(E) C5H10
E
X = CH3-CH2-CH2-CH2-CH3
Y = CH3-CH2-CH2-CH2-OH
Z = HO-CH2-CH2-CH2-OH
Based on concepts of polarity and hydrogen bonding, which of the following sequences correctly lists the compounds above in the order of their increasing solubility in water?
(A) Z < Y <
D
A sample of 3.30 grams of an ideal gas at 150.0 �C and 1.25 atmospheres pressure has a volume of 2.00 liters. What is the molar mass of the gas? The gas constant, R, is 0.0821 L atm mol�1 K�1).
(A) 0.0218 gram/mole
(B) 16.2 grams/mole
(C) 37.0 grams/mole
C
The system shown above is at equilibrium at 28 �C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is
(A) 28 mm Hg
(B) 56 mm Hg
(C) 133 mm Hg
(D) 161 mm Hg
(E) 189 mm Hg
D
Mass of an empty container = 3.0 grams
Mass of the container plus the solid sample = 25.0 grams
Volume of the solid sample = 11.0 cubic centimeters
The data above were gathered in order to determinethe density of an unknown solid. The density of the sampl
CH3-CH2-CH2-CH3 and CH (with 3 CH3 attached w/ a single bond)
Examples of isomers
C
A sample of an ideal gas is cooled from 50.0 �C to 25.0 �C in a sealed container of constant volume. Which of the following values for the gas will decrease?
I. The average molecular mass of the gas
II. The average distance between the molecules
III. The
E
Which of the following solids dissolves in water to form a colorless solution?
(A) CrCl3
(B) FeCl3
(C) CoCl2
(D) CuCl2
(E) ZnCl2
D
Which of the following has the lowest conductivity?
(A) 0.1 M CuS04
(B) 0.1 M KOH
(C) 0.1 M BaCl2
(D) 0.1 M HF
(E) 0.1 M HNO3
E
Which of the following acids can be oxidized to form a stronger acid?
(A) H3PO4
(B) HNO3
(C) H2CO3
(D) H3BO3
(E) H2SO3
E
If 87 grams of K2 SO4 (molar mass 174 grams) is dissolved in enough water to make 250 milliliters of solution, what are the concentrations of the potassium and the sulfate ions?
[K+] [SO42�]
(A) 0.020 M 0.020 M
(B) 1.0 M 2.0 M
(C) 2.0 M 1.0 M
(D) 2.0 M 2.
A
Molecules that have planar configurations include which of the following?
I. BCl3
II. CHCl3
III. NCl3
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
B
I2(g) + 3 Cl2(g) ---> 2 ICl3(g)
According to the data in the table below, what is the value of DH� for the reaction represented above?
Bond Average Bond Energy (KJ/mole)
I---I 149
Cl---Cl 239
I---Cl 208
(A) - 860 kJ
(B) - 382 kJ
(C) + 180 kJ
(D) + 450 kJ
A
The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom?
(A) H2S
(B) NH3
(C) CH4
(D) HCN
(E) CO2
D
At 25 �C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 mole per minute. Under the same conditions, which of the following gases effuses at approximately one-half that rate?
(A) O2 (molar mass 32 grams)
(B) He2 (molar mass 4.0 grams)
A
Which of the following molecules has a dipole moment of zero?
(A) C6H6 (benzene)
(B) NO
(C) SO2
(D) NH3
(E) H2S