Download Chemistry CPA Mid-Term Exam Study Guide January 2012

Chemistry CPA Mid-Term Exam Study Guide January 2012
The mid-term consists of two parts, which are described below. You will be given a
periodic table, list of polyatomic ions and formula sheet with the exam. A copy of the
formula sheet is provided for you. You must bring a calculator, #2 pencils, and a pen
with you to the examination.
Part 1 Problem-Solving
The problem-solving section of the mid-term exam is worth 50 points of the exam grade.
When completing this section of the exam, show formulas used and dimensional
analysis. Be sure to report your answers to the correct number of significant figures with
proper units. Significant figures and units must be used when completing the problem.
Part 2 Multiple Choice (50 questions)
The multiple choice section of the mid-term exam is worth 50 points of the exam grade.
Questions are designed to test your knowledge of the topics studied in the first semester
of chemistry. Topics from this portion of the exam are covered in chapters 1-9. Also
included in the multiple choice section are questions about the labs that we have
completed during the first semester in Chemistry.
You will be given a periodic table, formula sheet and polyatomic ion chart.
CPA CHEMISTRY MIDTERM FORMULA SHEET 2012
DENSITY
D= m/V
ATOMIC STRUCTURE
mass number
atomic number
X
ionic charge
subscript
LIGHT EQUATIONS
E = hν
E = hc/λ
Plank’s constant (h) = 6.626 x 10-34 J s
c = νλ
ν = c/λ
speed of light (c) = 3.00 x 108 m/s
Ice Cp = 2.0 J/g °C
ΔHfus = 334 J/g
Q = mcΔT
Liquid water Cp = 4.184 J/g °C
Q = m ΔHfus
ΔHvap = 2261 J/g
Q = m ΔHvap
Steam Cp = 2.0 J/g °C
1|P age
For success on the exam, review the following topics:
□
□
□
□
□
□
□
□
□
□
□
□
□
□
Significant figures in measurements/calculations
Metric Conversions (including volume conversions)
Density calculations
Classification of matter (element, compound, mixture)
Structure of the atom (protons, neutrons, electrons)
Isotopes and Atomic Mass Determination
Early Development of Atomic Models (Dalton, Rutherford, Thomson, Crookes,
Millikan)
Quantum Mechanical Model of the Atom (Heisenberg, Bohr, Einstein, Planck,
deBroglie, Schrodinger)
Atomic Orbitals and Electron Configurations (Aufbau principle, Pauli exclusion
principle, Hund’s Rule)
Properties of Light; Light Formulas (c=λν and E=hv)
Formation of Ions
Dimensional Analysis (single-step conversions, multi-step conversions, complex
conversions)
Periodic Table Organization (groups, periods, representative elements, transition
metals, inner transition metals)
Periodic Table Trends (ionization energy, atomic radius, electronegativity, ionic
radius)
2|P age
□
□
□
□
Naming compounds and writing formulas
Characteristics of ionic compounds and molecular compounds
Heating Curve of Water
Graphing
Study Checklist for the Mid-Term Exam
 For extra practice, answer the review questions in your textbook. The answers to
selected problems can be found in Appendix E of your textbook. Consult
Appendix E and then try those problems!!
 Organize your notes and outlines. Review your notes. Highlight any areas that
you do not understand and ask questions after school or on a scheduled exam
review day.
 Review “Key Terms” from each Chapter Review—understanding vocabulary is
very important!!
 Use the study guides from previous assessments. They are all posted on the
website.
 Review your previous tests—retake them. All of your tests should have the
correct answers!
 Complete the Practice Problems
For success on the classification of matter section of the exam, know the following
terms:












Qualitative observation
Quantitative observation
Physical Change
Chemical Change
Element
Compound
Mixture
Pure Substance
Homogeneous Mixture
Heterogeneous Mixture
Physical Property
Chemical Property
 Given a list observations, classify the observations as qualitative or quantitative.
 Be able to distinguish between elements, compounds and mixtures.
 Be able to classify a substance as an element or a compound.
 Be able to classify a mixture as a homogenous or heterogeneous mixture.
 Be able to identify physical properties.
3|P age
 Be able to identify chemical properties.
 Be able to classify changes as physical changes or chemical changes.
For success on the scientific measurement section of the exam, be prepared to
 Identify common metric prefixes.
 Know the value of common metric prefixes.
 Use dimensional analysis to convert between units in the metric system.
 Calculate the density of a material from experimental data.
 Distinguish between a quantity, unit, and a measurement standard.
 Name SI units for length, mass, time, volume, and density.
 Perform density calculations.
 Transform a statement of equality to a conversion factor.
 Perform calculations using dimensional analysis.
 Distinguish between accuracy and precision.
 Determine the number of significant figures in a measurement.
 Use rounding rules to round a number to the correct number of significant
figures.
 Perform mathematical operations involving significant figures.
 Convert measurements into scientific notation.
For success on the atomic theory portion of the exam,
 Be able to define and apply the following:






Explain the mathematical relationship between the speed,
wavelength, and frequency of electromagnetic radiation
Calculate wavelength and frequency.
Calculate energy given wavelength or frequency.
Discuss the dual wave-particle nature of light.
Describe the Bohr model of the hydrogen atom.
Define the term quanta.
 Be able to define and apply the following:


4|P age
Atomic orbital
Aufbau principle






Electron configuration
Ground state
Excited state
Pauli Exclusion Principle
Heisenberg uncertainty principle
Hund’s rule
 Be able to draw (or analyze) orbital diagrams.
 Be able to write electron configurations for elements. Be able to write short-hand
electron configurations for elements.
 Know the basis for exceptions to the aufbau diagram.
 Be able to identify stable electron configurations.
 Be familiar with the contributions of the following scientists to the quantum
mechanical model of the atom:
 Planck, Bohr, Einstein, deBroglie, Heisenberg, Schrödinger.
 Be prepared to solve problems using the following formulas and constants:
c = 
c = 3.00 x 108 m/s
E = h
h = 6.626 x 10-34 Js
For the nomenclature section of the exam, be able to:
 Given the formulas of binary ionic compounds, write the names of the
compounds.
 Given the formulas of ternary ionic compounds, write the names of the
compounds.
 Given the names of binary ionic compounds, write the formulas of the
compounds.
 Given the names of ternary ionic compounds, write the formulas of the
compounds.
 Given the formulas of binary molecular compounds, write the names of the
compounds.
 Given the names of binary molecular compounds, write the formulas of the
compounds.
 Be able to write the names and formulas for the common acids and bases.
For success on the periodic trends portion of the exam, know the following terms:


electronegativity
ionization energy
5|P age



atomic radius
metal
transition metal





periodic law
cation
period
group
electrons
 Know the group and period trends for the following properties: ionization energy,
electronegativity, atomic radius, ionic radius.
 Be able to locate the following on the periodic table: alkali metals, alkaline earth
metals, representative elements, transition metals, inner transition elements,
halogens, noble gases.
 Be able to identify an element given its electron configuration.
 Be able to explain shielding effect and how shielding affects the trends in
ionization energy, electronegativity, atomic radius.
 Know the general trend for first and second ionization energies.
 Describe the trends in the atomic size of elements within groups and across
periods in the periodic table. Provide examples.
 Explain how ions form. Provide examples.
 Describe the trends in first ionization energy within groups and across periods in
the periodic table. Provide examples.
 Positive ions are smaller than the atoms from which they are formed, but
negative ions are larger than the atoms from which they are formed. Explain why
this is so.
 Describe the trends in electronegativity within groups and across periods in the
periodic table. Provide examples.
For success on the heating curve section of the exam, review the following:
 What is represented by a heating and cooling curve?
 Be able to interpret the following diagram and use the diagram to perform
calculations:
6|P age
Practice Problems
Chapter
Topic
1
Intro to Chemistry
Pages
34
59,60
2
Matter & Change
58-60
41, 44, 46, 47,48, 54, 55, 69, 70
3
Scientific Measurement
96-98
59, 60, 63, 68, 70a, b, 71a, 74, 80, 86
4
Atomic Structure
122-124
34,39, 41-44, 47, 50, 56, 71
5
Electrons in Atoms
149-152
23, 30, 31, 34, 39, 41-42, 55, 61, 68, 70-71
6
The Periodic Table
181-184
27-28, 30, 32, 33, 36, 38, 39, 43, 48, 51
7
Ionic and Metallic Bonding
207-210
31-36, 40-41, 45, 67, 72
7|P age
Questions
8
Covalent Bonding
247-250
40, 43-45, 54b, f, 57, 68, 69
9
Chemical Names and
Formulas
281-284
42, 44, 47, 49, 52, 53, 66, 68
55, 57
8|P age