AP Chemistry Unit 1 Selected Response Questions:
1) If matter is uniform throughout and cannot be separated into other substances by physical
processes, but can be decomposed into other substances by chemical processes, it is called a (an)
__________.
A) heterogeneous mixture
B) element
C) homogeneous mixture
D) compound
E) mixture of elements
Answer: D
2) The SI unit for mass is __________.
A) kilogram
B) gram
C) pound
D) troy ounce
E) none of the above
Answer: A
3) The temperature of 25 °C is __________ in Kelvins.
A) 103
B) 138
C) 166
D) 248
E) 298
Answer: E
4) 1 nanometer = __________ picometers
A) 1000
B) 0.1
C) 0.01
D) 1
E) 10
Answer: A
5) 1 kilogram = __________ milligrams
A) 1 10 6
B) 1,000
C) 10,000
D) 1,000,000
E) none of the above
Answer: D
6) The density of silver is 10.5 g/cm3 . A piece of silver with a mass of 61.3 g would occupy a
volume of __________ cm 3 .
A) 0.171
B) 644
C) 10.5
D) 0.00155
E) 5.84
Answer: E
7) 3.337 g/cm3 = __________ kg/m 3
A) 3.337 10 9
B) 3.337 10 5
C) 3337
D) 0.3337
E) 333.7
Answer: C
8) The number 1.00430 has __________ significant figures.
A) 2
B) 3
C) 5
D) 6
E) 4
Answer: D
9) The correct answer (reported to the proper number of significant figures) to the following is
__________.
6.3 × 3.25 = __________
A) 20.
B) 20.475
C) 20.48
D) 20.5
E) 21
Answer: A
10) The correct result of the molecular mass calculation for H 2SO4 is _____________.
4 × 15.9994 + 32.066 + 2 × 1.0079 =
A) 98.08
B) 98.079
C) 98.074
D) 98.838
E) 98.84
Answer: B
Constructed response and performance event questions:
1) Gases do not have a fixed __________ as they are able to be __________.
Answer: volume, compressed
2) Mass and volume are often referred to as __________ properties of substances.
Answer: extensive
3) 1.035 10 4 L = __________ mL
Answer: 0.1035
4) The correct answer (reported to the proper number of significant figures) to the following is
__________.
11.5 × 8.78 = __________
Answer: 101
5) What is the name given to the unit that equals (a) 10-9 gram, (b) 10-6 second, (c) 10-3 meter?
Answer: The prefix related to each of the decimal fractions: (a) nanogram, ng, (b) microsecond,
s, (c) millimeter, mm.
6) What difference exists between the measured values 4.0 g and 4.00 g?
Answer: The value 4.0 has two significant figures, while 4.00 has three. This difference implies
that the first measurement has more uncertainty
7) The width, length, and height of a small box are 15.5 cm, 27.3 cm, and 5.4 cm, respectively.
Calculate the volume of the box, using the correct number of significant figures in your answer.
Answer: 2.3 x 10-3 cm3
8) A gas at 25 °C fills a container whose volume is 1.05 103 cm3. The container plus gas have
a mass of 837.6 g. The container, when emptied of all gas, has a mass of 836.2 g. What is the
density of the gas at 25 °C?
Answer: 0.0013 gm/cm3
9) The average speed of a nitrogen molecule in air at 25 °C is 515 m/s. Convert this speed to
miles per hour.
Answer: 1.15 x 103 mi/hr
10) Earth’s oceans contain approximately 1.36
liters.
Answer: 1.36 x 1021 L
109 km3 of water. Calculate the volume in
AP Chemistry Unit 19 Selected Response Questions:
1) By what process does thorium-230 decay to radium-226?
A) gamma emission
B) alpha emission
C) beta emission
D) electron capture
E) positron emission
Answer: B
2) In balancing the nuclear reaction 238 U
92
__________.
234 E 4 He , the identity of element E is
90
2
A) Pu
B) Np
C) U
D) Pa
E) Th
Answer: E
3) What is the largest number of protons that can exist in a nucleus and still be stable?
A) 206
B) 50
C) 92
D) 83
E) 84
Answer: D
4) The largest number of stable nuclei have an __________ number of protons and an
__________ number of neutrons.
A) even, even
B) odd, odd
C) even, odd
D) odd, even
E) even, equal
Answer: A
5) Bombardment of uranium-235 with a neutron generates tellurium-135, 3 neutrons, and
__________.
A) zirconium-98.
B) krypton-101.
C) krypton-103.
D) strontium-99.
E) zirconium-99.
Answer: A
6) How many neutrons are emitted when a californium-249 nucleus (Z=98) is bombarded with a
carbon-12 nucleus to produce a 257 Rf nucleus ?
104
A) one
B) three
C) two
D) four
E) zero
Answer: D
7) 131I has a half-life of 8.04 days. Assuming you start with a 1.53 mg sample of 131I, how
many mg will remain after 13.0 days?
A) 0.835
B) 0.268
C) 0.422
D) 0.440
E) 0.499
Answer: E
8) What order process is radioactive decay?
A) zeroth
B) first
C) second
D) third
E) fourth
Answer: B
9) On average, __________ neutrons are produced by every fission of a uranium-235 nucleus.
A) 4
B) 3.5
C) 1
D) 2.4
E) 2
Answer: D
10) The mass of a proton is 1.00728 amu and that of a neutron is 1.00867 amu. What is the mass
defect (in amu) of a 60 Co nucleus? (The mass of a cobalt-60 nucleus is 59.9338 amu.)
27
A) 27.7830
B) 0.5489
C) 0.5405
D) 0.0662
E) 0.4827
Answer: B
Constructed response and performance event questions:
1) What happens in the nucleus of an atom that undergoes positron emission?
Answer: A proton is converted to a neutron and a positron.
2) What happens to the atomic mass number and the atomic number of a radioisotope when it
undergoes alpha emission?
Answer: The mass number drops by 4 and the atomic number decreases by 2.
3) What isotope of what element is produced if krypton-81 undergoes beta decay?
Answer: rubidium-81
4) The first nuclear transmutation resulted in the conversion of nitrogen-14 to __________.
Answer: oxygen-17
5) The half-life for the beta decay of potassium-40 is 1.3 109 years . What is the rate constant for
this decay?
Answer: t1 2 0.693/ k
1.3 109 years 0.693/ k
k 5.3 10 10 year 1
6) Electrons do not exist in the nucleus, yet beta emission is ejection of electrons from the
nucleus. How does this happen?
Answer: A neutron breaks apart to produce a proton and an electron in the nucleus. The proton
remains in the nucleus and the electron is ejected.
7) List the common particles and their symbols used in descriptions of radioactive decay and
nuclear transformations.
Answer:
8) When an isotope undergoes electron capture, what happens to the captured electron?
Answer: It combines with a proton in the nucleus to form a neutron.
9) The use of radioisotopes in tracing metabolism is possible because __________.
Answer: all isotopes of an element have identical chemical properties
10) The amount of fissionable material necessary to maintain a chain reactions is called the
__________.
Answer: critical mass
AP Chemistry Unit 20 Selected Response Questions:
1) The simplest alkyne is __________.
A) ethylene
B) ethane
C) acetylene
D) propyne
E) benzene
Answer: C
2) The melting and boiling points of hydrocarbons are determined by __________.
A) ion-dipole attraction
B) dipole-dipole attraction
C) London forces
D) hydrogen bonding
E) ionic bonding
Answer: C
3) The molecular geometry of each carbon atom in an alkane is __________.
A) octahedral
B) square planar
C) trigonal planar
D) tetrahedral
E) trigonal pyramidal
Answer: D
4) The general formula of an alkane is __________.
A) C
H
2n 2n 2
B) C H
n 2n
C) C H
n 2n 2
D) C H
n 2n - 2
E) C H
n n
Answer: C
5) What is the name of the compound below?
A) 2,4-methylbutene
B) 2,5-dimethylpentane
C) 2,4-ethylbutene
D) 2,4-dimethyl-1-pentene
E) 2,4-dimethyl-4-pentene
Answer: D
6) The name of CH3 -CH=C=CH-CH-CH=CH-CH3 is __________.
A) 2, 3, 5 - octatriene
B) 2, 5, 6 - octatriene
C) 2, 3, 6 - octatriene
D) 3, 5, 6 - octatriene
E) 3, 4, 7 - octatriene
Answer: C
7) The addition of HBr to 2-butene produces __________.
A) 1-bromobutane
B) 2-bromobutane
C) 1,2-dibromobutane
D) 2,3-dibromobutane
E) no reaction
Answer: B
8) The general formula for an ether is __________.
A)
B)
C)
D)
E)
Answer: A
9) The general formula of a carboxylic acid is __________.
A)
B)
C)
D)
E)
Answer: C
10) Which structure below represents a ketone?
A)
B)
C)
D)
E)
Answer: D
Constructed response and performance event questions:
1) Why is cyclopropane more reactive than propane?
Answer: the small ring of cyclopropane forces the C-C-C bond angle to be significantly less
than 109.5 ° of __________ the tetrahedral structure of C in propane.
2) Write the formula for 2-methyl-4-propylnonane.
Answer:
3) What is the correct name for the compound, CH 3 CH 2 CH CHCH 2 CH CHCH 3 ?
Answer: 2,5-octadiene
4) What is the name of the compound below?
Answer: 4,6-dimethyl-1-heptyne
5) Predict the product of the catalytic hydrogenation of 6-ethyl-3-decene.
Answer: 6-ethyldecane
6) What is the name of the compound below?
Answer: 4-propyloctane
7) The formation of aspirin by reacting salicylic acid with acetic acid is a __________ reaction.
Answer: condensation
8) In the oxidation of ethanol the intermediate formed is __________.
Answer: acetaldehyde
9) The aromas of different fruit are due to the chemical compounds known as __________.
Answer: esters
10) Non-superimposable mirror-image isomers of a substance are called __________.
Answer: enantiomers
AP Chemistry Labs
All of the experiments below will require hands-on work in the laboratory. You will need
to be able to repeat experiments for the laboratory practical.
Chapter
1
2
3
4
4
5
7
10
10
10
11
13
13
14
14
15
16
16
17
17
17
17
20
25
Experiment (each experiment averages 60 – 90 minutes per week)
Basic Lab Technique experiment
Empirical Formula of an Oxide Lab
Mole Relationship in a Chemical reaction
Determination of Concentration of Vinegar by titration
Standardization of NaOH
Specific Heat, Heat of Reaction, and Hess’s Law Lab
Spectrophotometry Lab
Molecular Weight by Freezing Point Depression
Determining the Molar Volume of a Gas
Molar Mass of a Volatile liquid
Liquid Chromatography
Percentage of Water in a Hydrate
Gravimetric Analysis of a Metal Carbonate
Rates of Reaction: Iodination of Acetone
Activity Series
Spectrophotometric Determination of an Equilibrium Constant
Determination of Ka of Weak Acids
Selecting Indicators for Acid-Base Titrations
Qualitative Analysis of Cations and Anions
Oxidation – Reduction Titrations
Synthesis of a Coordination Compound containing Iron
Preparation and Properties of Buffer Solutions
Electrochemical Cells
Synthesis, Isolation, and Purification of an Ester
Pacing Guide for AP Chemistry
** Based on a 128 hour year
1ST QUARTER
Unit 1: Matter & Measurement
Unit 2: Atoms, Molecules, & Ions
4 hours
Unit 3: Stoichiometry
NOTE:
These units should be a review of topics covered in detail during the pre-AP chemistry course. Students could be provided with an
independent study project over the summer months prior to the AP course to expedite the review of this material.
Unit 4: Aqueous Reactions & Solution Stoichiometry
8 hours
Unit 5: Thermochemistry
8 hours
Unit 6: Electronic Structure of Atoms
7 hours
Unit 7: Periodic Properties of the Elements
5 hours
32 hours
2ND QUARTER
Unit 8: Chemical Bonding
6 hours
Unit 9: Molecular Geometry & VSEPR Theory
8 hours
Unit 10: Gases
6 hours
Unit 11: Intermolecular Forces, Liquids, & Solids
5 hours
Unit 12: Properties of Solutions
7 hours
32 hours
3RD QUARTER
Unit 13: Chemical Kinetics
7 hours
Unit 14: Chemical Equilibrium
10 hours
Unit 15: Acid – Base Equilibrium
8 hours
Unit 16: Titrations & Buffers
7 hours
32 hours
4TH QUARTER
Unit 17: Chemical Thermodynamics
Unit 18: Electrochemistry
8 hours
8 hours
Unit 19: Nuclear Chemistry
Unit 20: Organic & Biochemistry
Review for AP Exam
5 hours
5 hours
6 hours
32 hours
AP Chemistry Labs
All of the experiments below will require hands-on work in the laboratory. You will need
to be able to repeat experiments for the laboratory practical.
Chapter
1
2
3
4
4
5
7
10
10
10
11
13
13
14
14
15
16
16
17
17
17
17
20
25
Experiment (each experiment averages 60 – 90 minutes per week)
Basic Lab Technique experiment
Empirical Formula of an Oxide Lab
Mole Relationship in a Chemical reaction
Determination of Concentration of Vinegar by titration
Standardization of NaOH
Specific Heat, Heat of Reaction, and Hess’s Law Lab
Spectrophotometry Lab
Molecular Weight by Freezing Point Depression
Determining the Molar Volume of a Gas
Molar Mass of a Volatile liquid
Liquid Chromatography
Percentage of Water in a Hydrate
Gravimetric Analysis of a Metal Carbonate
Rates of Reaction: Iodination of Acetone
Activity Series
Spectrophotometric Determination of an Equilibrium Constant
Determination of Ka of Weak Acids
Selecting Indicators for Acid-Base Titrations
Qualitative Analysis of Cations and Anions
Oxidation – Reduction Titrations
Synthesis of a Coordination Compound containing Iron
Preparation and Properties of Buffer Solutions
Electrochemical Cells
Synthesis, Isolation, and Purification of an Ester