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AP Chemistry
Semester One Study Guide
Unit One: General Chemistry Review Unit Two: Organic Nomenclature
Unit Three: Reactions Unit Four: Thermochemistry Unit Five: Electronic Structure of the Atom
Unit Six: Bonding
Unit Seven: Solids, Liquids and Gases
Mr. Gray
Rockwood Summit High School 2014 - 2015
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The Real A.P. Chem Test
Vs.
The Semester 1 Final
The Real AP Chem Test The AP Chem Semester 2 Final
1. Exam time is 195 minutes 1. Exam time is 110 minutes
2. Section I is 90 minutes
60 MC questions
50% of test grade
no calculators
periodic table provided
equation sheet provided
2. Section I is 55 minutes
36 MC questions
50% of test grade
no calculators
periodic table provided
equation sheet provided
3. Section II is 105 minutes
7 FR questions
(3 multi-part, 4 single part)
50% of test grade
“Focuses on engaging students in:
experimental design, analysis of
authentic lab data and observations to
identify patterns or explain phenomena,
creating or analyzing atomic and
molecular views to explain
observations, articulating and then
translation between representations,
and following a logical / analytical
pathway to solve a problem.”
Calculators allowed
Periodic table provided
Equation sheet provided
3. Section II is 55 minutes
4 FR questions
(2 multi-part, 2 single part)
50% of test grade
Focuses on major topics such as atomic
and molecular structure, chemical
reactions, stoichiometry,
thermochemistry, bonding, gases and
solutions. Emphasis on data analysis
and relation to your lab experiences will
be incorporated wherever possible.
Calculators allowed
Periodic table provided
Equation sheet provided
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The Composition of Your Semester 1 Final Exam
Unit Questions
on Final
Topics
1. General Chemistry Review 12
1. Math
a. Scientific notation, significant figures and dimensional analysis
2. The Atom
a. Structure of the atom b. aXz notation, ions, isotopes, c. how to calculate atomic mass d. Mass spectroscopy
3. Nomenclature
a. Ionic, covalent, hydrate, and acids 4. Stoichiometry
a. Be fluent with the ENTIRE mole map (especially gases and liquids)
b. Problems: limiting reactants, percent yields, titrations, determining concentration of any species in solution, percent composition, obtaining empirical and/or molecular formulas from given data
2. Organic Nomenclature 1
5. Nomenclature
a. Hydrocarbon chains and functional groups b. isomers
3. Reactions 7
6. Reactions
a. Know all reaction types on green sheet b. Net ionic reactions and solubility rules c. Know oxidation rules, how to identify redox
reactions and how to balance redox reaction using half reaction method; know what an activity series is and how to read/use it
d. Know the 7 strong acids and 9 strong bases (because they are ions in solution)
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4. Thermochemistry 1
7. Thermochemistry
a. Know the 1st Law of Thermodynamics b. Draw and interpret enthalpy diagrams for
exo-/endo- thermic reactions
c. Calculate enthalpy by: energy diagrams, thermochemical equations (using dimensional analysis), calorimetry, Hess’
Law, Enthalpies of formation (data tables), bond enthalpies
d. Know how to calculate specific heat and heat capacity
e. Problems: calorimetry of acid/base, hot metal dropped in cool liquid
5. Electronic Structure of the Atom
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8. Electronic Structure of the Atom
a. Know something about the research of Bohr, Rutherford, Millikan and others b. Basic wave calculations, parts and sequence
of electromagnetic spectrum
c. Explanation of line spectra, Planck’s formula for quantizing energy (also Einstein’s energy of electron), Bohr model of atom
d. Calculate transition energy in Hydrogen e. Quantum numbers, orbital diagrams,
electron configurations and how they correspond to periodic table (Aufbau, Hund's, Pauli rules), PES
9. Periodic Table
a. Trends (atomic radii, ion size,
electronegativity, ionization energy, electron affinity, metallic character)
6. Bonding 5
10. Bonding
a. Ionic, covalent, metallic, lattice energy, coordinate covalent, characteristics of multiple covalent bonds, bond polarity (based on electronegativity)
b. Lewis structures, formal charges, resonance, octet rule and exceptions c. VSEPR Theory (molecular shapes), and
Valence Bond Theory (hybridization), molecular polarity, MO Theory
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11. IMF
a. Strengths of intermolecular forces and how they relate to properties (b.p, m.p., surface tension, viscosity, vapor pressure, etc) b. Rank substances in order of their melting or
boiling points
c. Enthalpy of phase changes and graphs d. Vapor pressure curves, cooling curves, solubility curves and phase diagrams 12. Gases
a. All gas laws, especially Ideal, Dalton, Graham’s and Avogadro’s
b. Use Ideal gas law to solve for molar mass and density
c. Kinetic Molecular Theory d. Ideal vs. Non ideal gas 13. Solutions
a. Factors that affect solubility of solids, liquids and gases
b. Units of concentration (molarity, molality, mole fraction, percent mass,etc.)
8. Labs – Concepts from any lab we have performed in General, Honors, or AP Chemistry could appear in any question.
a. Be familiar with proper lab and safety techniques, common errors and outcomes of all labs we did (volumetric glassware, aspirin/gravimetric analysis, emp/mol formulas,
calorimetry/heat of neutralization, chromatography, spectrophotometry/Beer's law, bonding types, etc.)
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Things You Should Have Memorized
1. Element names and symbols
2. Polyatomic ion names, formulas, and charges 3. All Reaction types
4. Solubility rules of nitrates, acetates, ammonium salts and group I metal salts 5. All VSEPR shapes and angles
6. Mole map
7. Organic functional groups (names and general formula for identification) 8. Organic hydrocarbon chain prefixes (meth, eth, prop, but, etc.)
9. Prefixes for covalent nomenclature (mono, di, tri, tetra, etc.) 10. 7 Strong acid names and formulas
11. 9 Strong base names and formulas
12. Parts of the EMS in order from low to high energy 13. Every type of IMF and their relative strengths 14. Periodic Trends
15. Colors of common flame tests and precipitates
Calculations You Should Know How To Do (from Collegeboard)
1. Percentage composition
2. Empirical and molecular formulas from experimental data
3. Molar masses from gas density, freezing point, and boiling point measurements 4. Gas laws, including the ideal gas law, Dalton’s law, and Graham’s law
5. Stoichiometric relations using the concept of the mole; titration calculations 6. Molarity of solutions
7. Thermodynamic and thermochemical calculations (enthalpy, calorimetry, specific heat)
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Descriptive / Qualitative Chemistry
You Should Know
Colors of Transition Metals (in solution)
+1 +2 +3 +4 +5 +6 +7
Sc Colorless
Ti Violet Colorless
V Violet Green Blue Yellow
Cr Blue Green Yellow/orange
Mn Pink brown Dk. Green Purple
Fe Green Yellow/brown
Co Pink Orange/yellow
Ni Green
Cu Colorless Blue
Zn colorless
Colors of Precipitates
White Blue Yellow Black Green Red/brown
AgCl Many with Cu2+ AgI Many sulfides Many with Fe2+ Many with Fe3+
BaSO4 PbI2
PbCl2
Many non- transition metal
hydroxides, carbonates and
sulfates
Flame Test Colors
ION FLAME COLOR Li+, Sr2+, Ca2+ Red
Na+ Yellow/orange
K+ Purple
Ba2+ Green
Cu2+ Blue-Green
Mg2+ White
Other Colors to Know
Fluorine gas Yellow/green Chlorine gas Green NO2 gas brown
Br2 liquid Orange/brown Iodine solid Purple
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VSEPR Shapes to Memorize
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