ACS Standardized Final Exam Review for CHEM 1062

ACS Standardized Final Exam Review for CHEM 1062

The ACS Standardized Final Exam Review for CHEM 1062 prepares students for the comprehensive exam assessing chemistry knowledge. It covers essential topics such as intermolecular forces, kinetics, chemical equilibrium, and thermodynamics. This resource is designed for college students enrolled in the second semester of general chemistry, providing strategies for effective exam preparation. Key features include a list of important equations, study strategies, and a breakdown of the exam format. Students will find valuable insights into the types of questions and concepts emphasized throughout the course.

Key Points

  • Covers essential chemistry topics including kinetics, thermodynamics, and chemical equilibrium.
  • Provides strategies for tackling multiple-choice questions on the ACS standardized exam.
  • Includes a comprehensive list of important equations and constants for exam preparation.
  • Offers insights into the exam format, including timing and allowed materials.
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CHEM 1062: Reviewing for the American Chemical Society (ACS) Standardized Final Exam
The CHEM 1062 Final Exam will be a full-year standardized exam written by the ACS. The goal is to see
how well students know and understand chemistry, and to see how well the students compare to other
students across the country. There is not a huge emphasis on math problems, but more so than the
standardized exam administered at the end of CHEM 1061 this past fall. While the exam covers the entire
year, many topics covered in your first semester of chemistry have been used throughout your second
semester. Some of the topics, such as gases and atomic theory, have been used less, but should be
relatively easy to review for the final now that you have almost completed the sequence and text.
Because the exam covers what you know and understand, the best way to review and study for the exam
may be to go over previous exams in this course and end-of-the chapter questions. As with the exams in
this course, there are no direct questions on definitions or terms. However, you are expected to know
chemistry vocabulary. There will, of course, be things which we emphasized a lot which will only show
up briefly on the final exam and vice versa. However, if you understand the material, you should be able
to reason through things which you don’t remember as well.
The exam has 70 multiple choice questions, each with four choices. You will be given 110 minutes – the
exam is timed. Programmable calculators are not permitted on the exam. Please remember to bring a non
programmable calculator to use on the exam. If you don’t have one and cannot borrow one from a friend,
let me know ASAP and I’ll see what I can do.
What is provided for you?
•
A comprehensive list of abbreviations and symbols
•
The values of numerous constants used throughout the course
•
Periodic Table (just like the ones you have received in class)
•
Arrhenius Equation, Graham’s Law of Effusion, Nernst Equation, Integrated Rate Law Equations
Directions
• You may NOT make marks in the exam booklet.
• Answers will be placed onto an answer sheet using a soft #2 pencil.
• All calculations must be done on the scratch paper provided.
• Each question has only one correct answer and has four choices.
• Your score is based solely on the number of questions answered correctly. It is to your
advantage to answer every question.
Strategies
• Don’t allow yourself to get stuck on a single problem. If you don’t know how to do it, move
along and go back to it later.
• Remember, your score on the final depends on your percentile ranking – there will be several
students across the nation that were unable to perform the same problems.
• Consider writing answers onto scratch paper and transferring several onto answer sheet at one
time.
• Spend the least time studying what you know well and the most time studying what you
DON’T know well.
Things you are expected to know (items in italics are first-semester topics):
•
basic chemistry vocabulary/terminology (Look at the end of each chapter for Important Terms
given in bold)
•
intermolecular forces, lattice energy, phase transitions, relation of b.p. and m.p. to intermolecular
forces, phase diagrams, types of solids, unit cell calculations
•
types of solutions, solution concentrations (molarity, molality, %, mole fraction), solubility
curves, colligative properties, colloids, solubility curves for gases vs. curves for solids
•
kinetics, experimental determination of rate, determining the rate law using the initial rate
method, rate constants, elementary reactions, catalysis, reaction mechanisms, collision &
transition state theory, activation energy, concentration-time calculations, temperature and rate,
half-lives, graphical determinations of reaction order and rate constant, potential energy diagrams
•
chemical equilibrium, equilibrium constant, reaction quotient, LeChatlier’s Principle, predicting
reaction direction, calculating equilibrium concentrations, ICE tables
•
acid-base theories: Arrhenius and Bronsted-Lowry, acid-base strength and relation to molecular
structure, self-ionization of water, and pH , strong and weak acids and bases
•
acid & base ionization equlibria, polyprotic acids, salt solutions, common ion effect, buffers,
titration curves
•
solubility product constant, common ion effect, pH and solubility, precipitation calculations,
solubility rules, particularly for ions for which there are no exceptions to the rule
•
2
nd
& 3
rd
laws or thermodynamics, entropy and
∆
S, free energy and
∆
G, spontaneity, relation to
the equilibrium constant, work, state function, extensive property, enthalpy and
∆
H, Hess’s Law,
specific heat capacity
•
balancing redox reactions, voltaic and electrolytic cells, cell notation, emf, E
cell
, electrode
potentials, oxidation numbers (know your rules), oxidizing and reducing agents, strength of these
agents, applications of electrochemistry, electrolysis
•
fission, fusion, radioactivity, nuclear bombardment reactions, radioactive decay, half-lives, mass-
energy calculations, isotopes and nuclide symbols, mass numbers and atomic weights, subatomic
particles
•
chemical/physical change/properties, significant figures, SI units and prefixes
•
nomenclature – polyatomic ions and Greek prefixes, molecular compounds, ionic compounds,
acids, binary compounds, ion charge based on position in periodic table, diatomic elements
•
completing and balancing combustion and double replacement reactions, net ionic equations,
spectator ions, molecular equations, gas-producing reactions
•
basic stoichiometry – molar masses, molar ratios, limiting reactant, percent composition,
molarity, percentage yield, empirical and molecular formulas
•
gas laws: empirical, ideal, effusion, partial pressures, STP, kinetic-molecular theory, barometers
and manometers
•
energy, frequency, and wavelength, emission spectra, electron configurations, orbital diagrams,
quantum numbers (n, l, m
l
, m
s
)
•
periodic trends (atomic radii, ionization energies, electronegativities, ionic radii)
•
Lewis structures, resonance, formal charges, bond polarity, exceptions to octet rule, bond order
•
VSEPR model: hybridization, polarity of molecules, lone pairs, bonding pairs,
σ
and
Ï€
bonds
•
g/cm
3
may be written as g·cm
-3
and
K
mol
atmL
â‹…
â‹…
may be written as L
·
atm
·
mol
-1
·
K
-1
Know the following equations:
V
m
d =
∆
Hº =
Σ
n
∆
Hº
f
(products) -
Σ
n
∆
Hº
f
(reactants)
M
1
V
1
= M
2
V
2
∆
Gº =
Σ
n
∆
Gº
f
(products) -
Σ
n
∆
Gº
f
(reactants)
PV = nRT
∆
Sº =
Σ
n
∆
Sº(products) -
Σ
n
∆
Sº
(reactants)
q = m×s×
∆
T
∆
T
f
= K
f
c
m
and
∆
T
b
= K
b
c
m
Calculating Molarity, molality, %, mole
fraction
Formulas for equilibrium constant and reaction
quotient
2
22
1
11
T
VP
T
VP
=
[H
3
O
+
][OH
-
] =
K
w
= 1.0×10
-14
q (system) = -q (surroundings)
pH = -log[H
3
O
+
]
∆
G
o
=
∆
H
o
+ T
∆
S
o
pOH = -log[OH
-
]
∆
G
o
= -RT
ln
K
pH + pOH = 14.00
∆
G
o
= -nFE
o
cell
pH = p
K
a
+ log
[acid]
[base]
E
o
cell
=
n
0592.0
log
K
K
a
K
b
= K
w
t
1/2
=
k
693.0
Rate =
kN
t
0
ln
N
N
t
=
-kt
∆
E = (
∆
m)c
2
/ 4
End of Document
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FAQs of ACS Standardized Final Exam Review for CHEM 1062

What topics are included in the ACS Standardized Final Exam for CHEM 1062?
The ACS Standardized Final Exam for CHEM 1062 includes a wide range of topics such as intermolecular forces, phase transitions, chemical kinetics, and equilibrium concepts. Students are expected to understand the relationship between temperature and reaction rates, as well as the principles of thermodynamics. Additionally, the exam covers acid-base theories, solubility product constants, and redox reactions, ensuring a comprehensive assessment of students' chemistry knowledge.
How is the ACS Standardized Final Exam structured?
The ACS Standardized Final Exam consists of 70 multiple-choice questions, each with four answer choices. Students are given 110 minutes to complete the exam, which is designed to assess their understanding of chemistry concepts covered throughout the course. The exam is timed, and students must use a non-programmable calculator. The scoring is based solely on the number of correct answers, encouraging students to attempt all questions.
What study strategies are recommended for the ACS Standardized Final Exam?
Effective study strategies for the ACS Standardized Final Exam include reviewing previous exams and end-of-chapter questions to reinforce understanding. Students should focus on areas where they feel less confident and practice reasoning through questions they find challenging. It is also beneficial to familiarize oneself with the exam format and types of questions that may appear, as well as to utilize scratch paper for calculations to avoid getting stuck on any single problem.
What equations should students memorize for the ACS Standardized Final Exam?
Students preparing for the ACS Standardized Final Exam should memorize key equations such as the Ideal Gas Law (PV = nRT), the Gibbs Free Energy equation (ΔGº = ΔHº - TΔSº), and the Nernst equation for electrochemistry. Understanding the Arrhenius equation and the integrated rate laws for chemical kinetics is also crucial. Familiarity with these equations will aid in solving problems related to thermodynamics, kinetics, and equilibrium during the exam.
What resources are provided during the ACS Standardized Final Exam?
During the ACS Standardized Final Exam, students are provided with a comprehensive list of abbreviations and symbols, values of numerous constants, and a periodic table. Additionally, important equations such as the Arrhenius Equation and Graham’s Law of Effusion are included. These resources are designed to assist students in answering questions effectively and efficiently, ensuring they have the necessary tools at their disposal.

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