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If an ionic compound with the formula MX forms a primitive cubic unit cell with the
anions (Xn") at the lattice points, the cations (M2n+) will occupy
A.all of the tetrahedral holes in each unit cell.
B.half of the tetrahedral holes in each unit cell.
C.the cubic hole in the center of the each unit cell.
D.the center of each face in each unit cell.
E.all of the octahedral holes in each unit cell.
As pure molecular solids, which of the following exhibits dipole-dipole intermolecular
forces: HBr, NBr3, SBr2, and CBr4?
A.Hbr only
B.CBr4 only
C.HBr and SBr2
D.NBr3 and CBr4
E.HBr, NBr3, and SBr2
Assume that an average and a standard deviation are calculated using a large number of
measurements. A single data point has a(n) ____ chance of falling within plus and
minus two standard deviations of the calculated average.
A.50%
B.68%
C.83%
D.95%
E.100%
Which of the following elements is most likely to form a molecular structure that
disobeys the octet rule?
A.B
B.C
C.N
D.O
E.F
What is the correct formula for ammonium bromide?
A.NH4Br
B.(NH4)2Br
C.NH3Br
D.NH4Br2
E.NH2Br
Which one of the following statements is INCORRECT?
A.Polonium is the only metal that has a primitive cubic lattice.
B.The lattice structure of the alkali metals is body-centered cubic.
C.Many metals can crystallize in more than one type of crystal lattice.
D.Metals with a body-centered cubic lattice contain a net of four metal atoms per unit
cell.
E.A hexagonal close packed structure is not an example of a cubic unit cell.
Which molecule will have the following valence molecular orbital level energy
diagram?
s*2p
p*2p
s2p
p2p
s*2s
s2s
A.Li2
B.Be2
C.B2
D.C2
E.N2
Which of the following molecules may be a cycloalkene?
A.C4H8
B.C5H12
C.C5H10
D.C6H12
E.C6H10
If the reaction quotient, Q, is greater than K in a gas phase reaction, then
A.the chemical system has reached equilibrium.
B.the temperature must be increased for the reaction to proceed in the forward
direction.
C.the reaction will proceed in the forward direction until equilibrium is established.
D.the reaction will proceed in the backward direction until equilibrium is established.
E.the reaction will proceed in the direction that increases the number of gas phase
particles.
What is the correct name for MnS?
A.manganese sulfide
B.dimanganese sulfate
C.dimanganese sulfide
D.manganese(II) sulfate
E.manganese(II) sulfide
What is the net ionic equation for the reaction of aqueous hydrochloric acid and
aqueous potassium hydroxide?
A.HCl(aq) + OH"(aq) H2O( ) + Cl"(aq)
B.Cl"(aq) + K+(aq) KCl(s)
C.HCl(aq) + KOH(aq) KCl(aq) + H2O( )
D.Cl"(aq) + K+(aq) KCl(aq)
E.H+(aq) + OH"(aq) H2O( )
What mass of ethylene glycol, when mixed with 225 g H2O, will reduce the equilibrium
vapor pressure of H2O from 1.00 atm to 0.800 atm at 100 C? The molar masses of
water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal
behavior for the solution.
A.15.6 g
B.49.9 g
C.194 g
D.969 g
E.3.10 103 g
Which of the following pairs of coordination compounds are coordination isomers?
A.[Cr(H2O)6]SO4 and [Cr(NH3)6]SO4
B.[Cr(NH3)5Cl]SO4 and [Cr(NH3)5SO4]Cl
C.[Co(NH3)4(H2O)2]Cl2 and [Co(NH3)2(H2O)4]Cl2
D.[Cr(NH3)6](NO3)2 and [Fe(NH3)6](NO3)3
E.[Cr(H2O)6]Cl2 and [Fe(H2O)6]Cl2
What is the half-life of a first-order reaction if the rate constant is 6.2 10"3 s"1?
A.8.9 10"3 s
B.0.097 s
C.5.77 s
D.1.0 102 s
E.1.6 102 s
Which of the following statements is/are CORRECT?
1/ For any element, the second ionization energy is larger than the first ionization
energy.
2/ Ionization energy is a positive value for all elements.
3/ Ionization energy increases down a group of the periodic table.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2 and 3
The iron produced in a blast furnace contains significant impurities of carbon,
phosphorus, and sulfur. These impurities are removed in a basic oxygen furnace, which
converts the impurities to ________.
A.CO2, P4O10, and SO2
B.CS2 and P4S3
C.H2CO3, H3PO4, and H2SO3
D.H2CO3, H3PO4, and H2SO4
E.CH4, PH3, and H2S
What is the hybridization of the central nitrogen atom in N2O?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
The following reaction occurs spontaneously.
2 Fe(s) + 3 Cl2(aq) 2 Fe3+(aq) + 6 Cl"(aq)
Write the balanced reduction half-reaction.
A.Fe(s) Fe3+(aq) + e"
B.Fe(s) + 3 e" Fe3+(aq)
C.Fe(s) + 3/2 Cl2(aq) FeCl3(aq)
D.Cl2(aq) 2 Cl"(aq) + 2 e"
E.Cl2(aq) + 2 e" 2 Cl"(aq)
All of the following compounds are acids containing chlorine. Which compound is the
weakest acid?
A.HCl
B.HClO
C.HClO2
D.HClO3
E.HClO4
Aqueous hydrochloric acid reacts with magnesium to produce hydrogen gas according
to the balanced equation below.
2 HCl(aq) + Mg(s) MgCl2(aq) + H2(g)
If 250.0 mL of 3.00 M HCl is combined with 9.92 g Mg, what volume of hydrogen gas
can be produced? Assume the temperature and pressure of the gas are 25 C and 0.988
atm, respectively. (R = 0.08206 Latm/molK)
A.4.60 L
B.5.05 L
C.9.28 L
D.10.1 L
E.18.6 L
The pH of aqueous 0.10 M pyridine (C5H5N) ion is 9.09. What is the Kb of this base?
A.8.0 10"10
B.1.5 10"9
C.9.0 10"6
D.1.6 10"5
E.1.2 10"5
Write a balanced chemical equation which corresponds to the following equilibrium
constant expression.
A.HNO2(aq) + H2O( ) NO2
"(aq) + H3O+(aq)
B.NO2
"(aq) + H3O+(aq) HNO2(aq) + H2O( )
C.NO2
"(aq) + H3O+(aq) HNO2(aq)
D.H+(aq) + OH"(aq) H2O( )
E.HNO2(aq) NO2
"(aq) + H3O+(aq)
A flask contains the following chemical system at equilibrium.
CuCO3(s) Cu2+(aq) + 2 CO3
2"(aq)
Addition of which of the following substances will increase the solubility of CuCO3(s)
in water?
1/ aqueous hydrochloric acid
2/ aqueous sodium carbonate
3/ solid copper(II) carbonate
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
Which of the following processes is/are exothermic?
1/ the reaction of butane with oxygen
2/ the melting of gold
3/ cooling copper from 225 C to 65 C
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
One resonance structure for OCN" ion is drawn below. What is the formal charge on
each atom?
A.O atom = 0, C atom = 0, and N atom = 0
B.O atom = 0, C atom = 0, and N atom = "1
C.O atom = "1, C atom = 0, and N atom = 0
D.O atom = "1, C atom = "1, and N atom = +1
E.O atom = +1, C atom = 0, and N atom = "2
The procedure by which electrons are assigned to (or built up into) orbitals is known as
the ____ principle.
A.Aufbau
B.Bohr
C.Planck
D.Hund
E.Pauli
A(n) ____ is a colloidal dispersion of a liquid in a solid.
A.gel
B.emulsion
C.aerosol
D.foam
E.sol
What is the correct name for SrCl2?
A.strontium dichloride
B.strontium dichlorine
C.strontium(II) dichloride
D.strontium chloride
E.iodine strontide
Which of the following statements is/are CORRECT for an oxygen atom?
1/ The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s
electron.
2/ The effective nuclear charges felt by 2s and 2p electrons are identical.
3/ The effective nuclear charge felt by a 2p electron is less than that felt by a 2s
electron.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
What is the molecular formula for heptane?
A.C6H12
B.C6H14
C.C7H14
D.C7H16
E.C9H20
Which functional group does not contain a double bond to an oxygen atom?
A.ester
B.aldehyde
C.ether
D.amide
E.ketone
Which of the following compounds might be used to oxidize an aldehyde to a
carboxylic acid?
A.H2
B.Na
C.LiAlH4
D.KMnO4
E.NaBH4
Which of the following are possible Lewis structures for C2H6O?
A.1
B.2
C.3
D.2 and 3
E.1, 2, and 3
Which of the following phase transitions is/are endothermic?
1/ liquid water freezing to a solid at its normal freezing point of 0.0 C.
2/ the sublimation of solid carbon dioxide into the gas phase.
3/ gaseous sulfur dioxide condensing into a liquid at its boiling point of "10.0 C.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Pure oxygen can exist as O2 or O3. Elements that exist in more than one distinct form
are called ________.
When a glass tube with a small diameter is placed in water, the water rises in the tube.
This is known as ________ action.
Which ion, K+ or Ca2+, is expected to have the more negative enthalpy of hydration?
Why?
The heat required to convert a solid at its melting point to a liquid is called the heat of
________.
A pressure of 1.00 atm has a metric equivalent of 1.01 105 ________.
In 1913, the Haber-Bosch process was patented. The product of the Haber-Bosch
process is ________.
In reactions, metals generally lose electrons to become ________, and nonmetals gain
electrons to become anions.
Above a substance's ________ temperature, it is not possible to compress the substance
into the liquid phase. If enough pressure is applied the substance will become a
supercritical fluid.
The pressure exerted by gas molecules inside a container is due to gas molecules
colliding with the walls of the container. Why does one mole of oxygen molecules exert
the same pressure inside a flask as one mole of hydrogen molecules, although the mass
of an oxygen molecule is sixteen times greater than the mass of a hydrogen molecule?
The use of electrical energy to produce chemical change is known as ________. An
example of this process is the reduction of NaCl( ) to produce Na(s).
The ________ equation relates the equilibrium vapor pressure of a volatile liquid to the
molar enthalpy of vaporization at a given temperature.
The f-block elements are also referred to as the ________ and actinides.
In benzene, C6H6, the six carbon atoms are arranged in a ring. Two equivalent Lewis
structures can be drawn for benzene. In both structures, the carbon atoms have a
trigonal planar geometry. These two equivalent structures are referred to as ________
structures.
Which is the stronger Brnsted-Lowry acid, Fe(H2O)6
2+ or Fe(H2O)6
3+?Explain.
Sodium chloride crystallizes in a(n) ________ cubic unit cell with chloride ions
occupying the lattice points. The sodium ions occupy interstitial regions, with each
cation in contact with six chloride ions.
A salt with a 1:1 ratio of anions to cations may pack in a face-centered cubic unit cell
with the anions at the lattice points and the cations occupying one-half of the ________
holes. Zinc sulfide is an example of this structure.
All isotopes of atomic number greater than ________ are unstable and radioactive.
Electron ________ is defined as the energy change for a process in which a gas phase
atom acquires an electron.
