Multiple Choice by chapter
Supplemental Instruction
Iowa State University
Leader: Sara
Course: Chem 177
Instructor: Bonaccorsi
Date:
Chapter 1
1) Which of the following is a physical change?
I.
H2O (s)  H2O (l)
II.
CH4 (s) + O2 (g)  H2O (g) + CO2 (g)
III.
NaCl (s)  Na+(aq) + Cl- (aq)
IV.
C6H12O6 (s) + H2O (l)  C6H12O6 (aq) + H2O (l)
b. I only
c. II only
d. III only
e. I and III
f. I and IV
g. III and IV
h. I, III and, IV
i. All of the above
2) What is NOT a Pure substance?
a. Nickel
b. Brass
c. Nitrogen
d. C6H12O6
3) Which would have the lowest density?
a. Water
b. Alcohol with a density of .79 g/mL
c. 10.3 mL of an oil that has a mass of 13.3 g
d. Not enough information
4) Convert the following measurement to scientific notation: 101,000 grams
a. 1.01000 x 10-5 g
b. 1.0100 x 10-5 g
c. 10.1 x 104 g
d. 1.01 x 105 g
5) Solve: 345.009 g - 23.009 g =?
a. 322 g
b. 322
c. 322.00 g
d. 322.000 g
e. 3.22 * 102 g
Chapter 2
1) What is the name of HBrO
a. Hydrobromic acid
b. Hypobromous acid
c. Bromic acid
d. Perbromic acid
2) If there are 2 isotopes of carbon and three isotopes of oxygen, how many lines of
a mass spectrometry would Carbon monoxide give?
a. 2
b. 3
c. 4
d. 5
e. 6
3) What is the formula of the compound arsenic (III) oxide?
a. As2O3
b. Ar3O
c. AsO3
d. Ar2O3
e. As3O
f. ArO3
4) How many electrons are there in S2-?
a. 8
b. 14
c. 15
d. 16
e. 17
f. 18
g. 32
5) What is the element that has 38 protons, 37 electrons, and 40 neutrons?
a. Rb
b. Sr
c. Y
d. Zr
e. Nb
f.
6) Which of the following is a cation of antimony?
a. Te+
b. Sb+
c. Sn+
d. Tee. Sbf. Sn-
Chapter 3
1) What kind of formula is Acetic Acid?
a. Organic
b. Molecular
c. Empirical
d. All of the above
2) In the combustion of C3H7OH, how many moles of oxygen are needed to
combust 2 moles of C3H7OH?
a. 4.5
b. 5
c. 7
d. 9
e. 11
3) If you want to balance the final equation, what is the sum of the coefficients:
___Al2(SO3)3 + ___NaOH  ___Na2SO3 + ___Al(OH)3
a. 10
b. 11
c. 12
d. 13
e. 14
4) In the production of Potassium Oxide from solid potassium and gaseous oxygen,
how many molecules of Potassium are needed to react with 4.0 moles of
gaseous Oxygen?
None of the answers are
a. 4.0 molecules
correct. The correct
b. 8.0 molecules
answer should be
24
c. 2.4 *10 molecules
9.6 * 1024 molecules
d. 4.8 *1024 molecules
For the next three questions use the following scenario:
CuCl2 + 2 NaNO3  Cu(NO3)2 + 2NaCl
5) If 15.0 grams of copper (II) chloride (Μ= 134.5 g/mol) reacts with 20.0 grams of
sodium nitrate (Μ= 85.0 g/mol), what is the limiting reagent?
a. Sodium Chloride
b. Copper (II) chloride
c. Copper (II) nitrate
d. None of the above
6) How much sodium chloride (Μ= 58.4 g/mol) will be produced
a. 6.5 g
b. 6.9 g
c. 13.7 g
d. 13.0 g
e. 27.4 g
7) In lab 6.1 grams of sodium chloride is produced, what is the percent yield?
a. 93%
b. 88%
c. 45%
d. 47%
e. 22%
Chapter 4
1) Which of the following ionic hydroxides is a soluble base?
a. Cu(OH)2
b. Fe(OH)2
c. Fe(OH)3
d. Sr(OH)2
e. Al(OH)3
2) Which are strong electrolytes?
I.
K2CO3
III.
H2SO4
II.
HNO3
IV.
CuCO3
a. I and II
b. I and IV
c. II, III, and IV
d. III and IV
e. I, II and III
3) What is (are) the spectator ion(s) in the following reation:
2HClO3(aq) + Sr(OH)2(aq) → Sr(ClO3)2(aq) + 2H2O(l)
a. H+,OHb. H+
c. Sr2+,ClO3d. Sr2+,OHe. OH4) What is the mass of Potassium (M=39.1 g/mol) contained in 40. mL of a 3.0 M
solution of KCl?
a. 8.9 g
b. 4.7 g
c. 4.26 g
d. 9.0 g
5) Calculate the molarity after you mix 30. mL of .45 M solution with 75 mL of .90 M
solution
a. .081 M
b. .70 M
c. .74 M
d. .77 M
e. .80 M
6) Calculate the molarity of the resulting solution if 275.0 mL of water is added to
25.0 mL of a 2.40 M HCl solution.
a. 0.200 M
b. 29.0 M
c. 2.00 M
d. 0.400 M
e. 0.0400 M
7) What volume of 0.132 M KOH solution would react completely with 25.8 mL of
0.198 M HCl in the titration of KOH with HCl?
a. 86.4 mL
b. 25.7 mL
c. 38.7 mL
d. 17.2 mL
e. 3.86 mL
Chapter 5
1) If a system loses 250 kJ of heat at the same time that it is doing 500 kJ of work,
what is the chane in the internal energy of the system?
a. +250 kJ
b. -250 kJ
c. +750 kJ
d. -750 kJ
2) If 1.45 J of heat are added to a 2.00 g sample of aluminum metal and the
temperature of the metal increases by 0.798 oC what is Aluminums specific heat?
a. 0.579 J/gK
b. 0.909 J/gK
c. 1.68 J/gK
d. 3.63 J/gK
3) The heat of combustion for one mole of carbon to carbon dioxide is -410 kJ. How
many kJ of heat would be liberated from the complete combustion of 60.0 g
carbon?
a. -82 kJ
b. -2050 kJ
c. -24,600 kJ
d. -32,000 kJ
4) Water has a specific heat of 4.184 J/g deg while glass (Pyrex) has a specific heat
of 0.780 J/g deg. If 10.0 J of heat is added to 1.00 g of each of these, which will
experience the larger increase of temperature?
a. Glass
b. Water
c. They both will experience the same change is temperature
5) . Given the following data at 1 atm of pressure and 25.0 oC...
DHoformation = +64.4 kJ/mole for Cu2+
DHoformation = -152.4 kJ/mole for Zn2+
Calculate the standard heat of reaction for...
a. -217 kJ/mol
b. +217 kJ/mol
c. -88.0 kJ/mol
d. +88.0 kJ/mol
6) A 1.00-g sample of hexane, C6H14, undergoes complete combustion with
excess O2 in a bomb calorimeter. The temperature of the 1500. g of water
surrounding the bomb rises from 22.64°C to 29.30°C. The heat capacity of the
calorimeter is 4.04 kJ/°C. What is ∆E for the reaction in kJ/mol of C6H14. The
specific heat of water is 4.184 J/g•°C.
a. -9.96 × 103 kJ/mol
b. - 4.52 × 103 kJ/mol
c. -1.15 × 104 kJ/mol
d. -7.40 × 104 kJ/mol
e. -5.91 × 103 kJ/mol
Chapter 6
1) Electromagnetic radiation travels through vacuum at a speed of ________ m/s.
a. 186,000
b. 125
c. 3.00*108
d. 10,000
e. It depends on wavelength
2) Ham radio operators often broadcast on the 6-meter band. The frequency of this
electromagnetic radiation is __________ MHz.
a. 500
b. 200
c. 50
d. 20
e. 2.0
3) A mole of yellow photons of wavelength 527 nm has __________ kJ of energy.
a. 165
b. 227
c. 4.56*10-46
d. 6.05*10-3
e. 2.74*10-19
4) What color of visible light has the longest wavelength?
a. Blue
b. Violet
c. Red
d. Yellow
e. Green
5) Of the following transistions in the Bohr hydrogen atom, which transition results
in the emission of the higest-energy proton?
a. n=1  n=6
b. n=6  n=1
c. n=6  n=3
d. n=3  n=6
6) There are _____ orbitals in the third shell.
a. 25
b. 4
c. 9
d. 16
e. 1
7) The n=1 shell contains ____ p orbitals. All other shells contain _____ p orbitals.
a. 3,6
b. 0,3
c. 3,3
d. 0,6
8) The elements in what period have the same core-electron configuration as
neon’s electron configuration
a. First
b. Second
c. Third
d. Fourth
Chapter 7
1) The size of an element’s atomic radius __________ from left to right across the
periodic table.
a. Increases
b. Decreases
c. Remains constant
d. Is random
2) Arrange the following elements from lowest to highest ionization energy: Be, Mg,
Ca, Rb, Sr
a. Be, Mg, Ca, Rb, Sr
b. Rb, Sr, Ca, Be, Mg
c. Rb, Sr, Ca, Mg, Be
d. Be, Mg, Ca, Sr, Rb
3) The halogens tend to form anions because….
a. They have low first ionization energies
b. They have low electron affinities
c. They have high electron affinities
d. They don’t; they form cations
4) Electon affinity…
a. Is always positive
b. May be positive or negative
c. Is alays negative
d. Is typically higher in metals than nonmentals
5) How many valence electrons does Sulfur have?
a. 3
b. 4
c. 5
d. 6
e. 7
6) The electron affinity of chlorine is -349 kJ/mol. What is the correct equation for
the formation of chloride ion?
a. Cl (s) + e- → Cl- (s) + 349 kJ
b. Cl (g) + e- → Cl- (g) + 349 kJ
c. Cl (s) + 349 kJ + e- → Cl- (s)
d. Cl (g) + 349 kJ + e- → Cl- (g)
7) What is true of the oxide formed when magnesium reacts with oxygen
a. Its formula is Mg2O
b. It is moleculat
c. It is basic
d. It is atmospheric
8) An element with a greater effective nuclear charge has _______ atomic radius
a. A larger
b. A smaller
c. An underfined
d. The same
Chapter 8/9
1) The C2 molecule has 6 bonding and 2 antibonding e-. What’s the bond order?
a. -2
b. -1
c. 0
d. 1
e. 2
2) Constructive combinations of atomic orbitals give:
a. Antibondind molecular orbitals
b. Hybrid orbitals
c. Other atomic orbitals
d. Bonding molecular orbitals
e. Resonant structures
3) A polar bond between two atoms is best described as
a. Equal sharing of electrons
b. Between H and O
c. Induced charge
d. Unequal sharing of electrons
e. Transferring of electrons
4) The molecule of NH4+ is best described as…
a. Linear
b. Planar
c. Three-dimensional
d. Not enough information to tell
5) Which of the following molecules do not have resonance forms?
a. SO2
b. O3
c. CH3OH
d. ClO36) Which of the following atoms may have an incomplete octet?
a. Li
b. C
c. F
d. N
7) What is the hybridization of the oxygen atom in water?
a. Sp
b. Sp2
c. Sp3
d. It is not hybridized
8) The central atom in BrF5 has ___ bonding and ___ non-bonding domains.
a. 1,5
b. 0,5
c. 5,1
d. 5,0
9) What is the shape of XeF4?
a. Octahedral
b. Tetrahedral
c. Square planer
d. Pyramidal
Chapter 10
1) Which of the following is false about gases?
a. They take the shape of their container
b. They take the volume of their container
c. They have the lowest densities
d. They have the strongest IMF
2) Which of the following has the highest density at STP?
a. Vapor water
b. Nitrogen gas
c. Carbon dioxide
d. Hydrogen gas
3) There are two boxes at the same pressure, and each contains the same number
of molecules. Box A has twice the volume as the Box B. The smaller box (Box B)
has a temperature of 300K. What is the Temperature of Box A?
a. 300 K
b. 150 K
c. 600 K
d. 225 K
e. 450 K
4) At the top of mount Everest the atmosphere is .03 molar percent Carbon
monoxide. The temperature is negative thirty degrees Celsius, and the pressure
is .35 atm. How many carbon monoxide molecules are in 1.0 L of atmosphere.
a. .018
b. 1.1 x 1022
c. 5.3 x 10-6
d. 3.2 x 1018
5) Under conditions of fixed temperature and moles of gas. Boyle’s Law states that:
I.
P1V1 = P2V2
II.
PV = constant
III.
P1/P2 = V2/V1
a. I only
b. II only
c. III only
d. I, II, and III
e. None of the above
6) Which of the following gases would have the smallest rate of effusion?
a. CH4
b. He
c. N
d. Ne
e. CO
7) A gas mixture contains 2.0 moles of helium and 8.0 moles of carbon dioxide, and
is held under conditions of standard temperature and pressure. What is the
partial pressure of carbon dioxide?
a. 2.0 atm
b. 0.20 atm
c. 8.0 atm
d. 0.80 atm
e. None of the above
Chapter 11
1) Viscosity of liquids typically increases when all of the following occur except:
a. The temperature is increased
b. Substances that can hydrogen bond are used
c. Longer molecules are used
d. Compound with greater molecular weights are used
2) The boiling point of a substance is most strongly influenced by:
a. The molecular weight of a substance
b. The specific heat of a substance
c. The melting point
d. The strength/weakness of the intermolecular forces
e. The amount of substance involved
3) Using the table below, predict the substance with the highest boiling point
4)
5)
6)
7)
8)
Substance
Molecular
Dipole
a. CH3CH2CH3
Mass
(amu)
Moment (D)
b. CH3OCH3
CH
CH
CH
44
0.1
3
2
3
c. CH3Cl
CH3OCH3
46
1.3
d. CH3CHO
CH
50
1.9
3Cl
e. CH3CN
CH3CHO
44
2.7
Which of the following molecule will
CH3CN
41
3.9
have the largest heat of vaporization?
a. I2
b. Br2
c. Cl2
d. F2
e. O2
On the phase diagram, which segment corresponds to
the conditions which solid and gas are in equilibrium?
a. AB
b. AC
c. AD
d. BC
Which of the following exhibits dipole-dipole attractions between molecules?
a. XeF4
b. AsH3
c. CO2
d. BCl3
e. Cl2
What types of IMF exist between a molecule of HF and a molecules of H2S?
a. Dipole-dipole and ion-dipole
b. Dispersion forces, dipole-dipole, and ion-dipole
c. Dispersion forces, hydrogen bonding, dipole-dipole
d. Dispersion and dipole-dipole
e. Dispersion forces, dipole-dipole, and ion-dipole
What type of IMF exsist between Cl2 and CO32-?
a. Dispersion forces
b. Dispersion forces and ion-dipole
c. Dispersion forces, ion-dipole, and induced dipole-induced dipole
d. Dispersion forces and ion-induced dipole