COLLEGE CHEMISTRY

  • Purpose

    College Chemistry will be offered in place of A.P. Chemistry at Sault High.  It is intended for college-bound 11th and 12th grade students.  Students who take College Chemistry will be concurrently enrolled in General Chemistry I, CHEM 115, at Lake Superior State University (LSSU).  Students taking the course must meet LSSU's admissions requirements and the high school prerequisites given below.  The course will be taught at or above LSSU's curriculum standards to ensure that students will be well prepared for General Chemistry II at LSSU or at the Michigan college or university of their choice.  General Chemistry I, Introduction to Fundamental Principles in Chemistry, is often required for college students pursuing a science, engineering, pre-medical, pre-dental, pre-veterinary, health-related, or technology degree.  Dr. Wicks, the instructor, earned a Ph.D. in Chemistry from the University of Florida, did two years of postdoctoral research in Chemistry at the University of Chicago, and taught General Chemistry I, CHEM 115, lab and lecture, multiple times during the ten years he served as an Adjunct Instructor at Lake Superior State University.
     
     

    Prerequisites

    (1)  A grade of "B" or better in Algebra 1, Proof Geometry, and Honors Chemistry is required.
    (2)  Prior or concurrent enrollment in Algebra 2 is required.
    (3)  Prior or concurrent enrollment in Physics is recommended.
    (4)  You must also meet LSSU's admissions requirements (see your high school counselor). 
     

    Course Description

    College Chemistry (General Chemistry I) will focus on fundamental principles of chemistry with emphasis on the scientific method, basic chemical reactions, acid-base equilibria, stoichiometry, periodic trends of elements, an introduction to the energy of reactions, atomic structure, simple bonding models, molecular structure, intermolecular forces, and nuclear chemistry.  The course will include at least thirty hours of lab activities identical or equivalent to the lab activities performed by LSSU General Chemistry I students.  In order to ensure that students meet the lab standards for the course, they will spend three school days at LSSU performing labs in addition to performing labs at Sault High.  At the end of the General Chemistry I portion of the course, all students will take the American Chemical Society (ACS) First Term General Chemistry exam.  If any time remains in the school year, we will continue our study of College Chemistry to ensure that students are well prepared for success in General Chemistry II.
     
     

    "I Can" Statements

    The following review sheets are summaries of what students should know and be able to do by the end of each semester in College Chemistry.  When students study for a semester final exam, I recommend that they study their old chapter tests in addition to reviewing the information given in these files.  Before beginning to study for a final exam, students should have already made corrections to any incorrect questions on their chapter tests.  Answers to chapter tests are given and discussed in class.
     
     
     

    Additional information

    College Chemistry Syllabus  (General Information about the course)
     
    Course Agreement Sheets  (Parents and students sign these sheets to signify they have read the College Chemistry course syllabus and have had a chance to ask questions about it.  In addition, students sign these sheets agreeing to follow the lab safety rules and classroom expectations)
    The following links may be of interest to College Chemistry students:

    Tentative Schedule of Assignments:

    Course Introduction and Related Activities
    -Introduction to College Chemistry
    -Discussion of course syllabus and classroom expectations
    -Toledo Chemistry Placement Examination (designed to evaluate how well a student is prepared for college-level, introductory chemistry)
    -College Chemistry First Semester Pre-assessment
    -Concurrent Enrollment in LSSU's General Chemistry I (CHEM 115)
    -Class Meetings for the School Year

    Chapters 1-2,24: Chemistry: The Study of Change; Atoms, Molecules, and Ions; Introductory Organic Chemistry
    -Scientific method, classification of matter, types of mixtures, elements versus compounds, atoms versus molecules, states of matter, physical and chemical properties, extensive and intensive properties; Read Sect. 1.1 to 1.6; Do p.32: 8,12,16,22
    -Measurement, unit systems, mass versus weight, volume, density, temperature scales, significant figures, dimensional analysis; Read Sect. 1.7 to 1.9; Do p.33: 34,36,38,39,40,44,61,80
    -Lab safety training
    -Mixture Separation and Percent Composition Lab
    -Dalton's atomic theory, Thompson, Millikan's oil drop experiment, Rutherford's gold foil experiment, Chadwick, atomic structure, atomic number, mass number, isotopes; Read Sect. 2.1 to 2.3.
    -Periodic table, molecules and ions, chemical formulas, naming ionic compounds; Read Sect. 2.4 to 2.7; Do p.71: 16,18,32,36,43,44,46,50
    -Naming molecular compounds, acids, bases, and hydrates; introduction to organic compounds; Read Sect. 2.7 to 2.8; Do p.73: 58,60,65,77,97
    -Inorganic Nomenclature II: Binary Compounds Dry Lab
    -Inorganic Nomenclature III: Ternary Compounds Dry Lab
    -Saturated versus unsaturated hydrocarbons, alkanes, naming alkanes, structural isomers, cycloalkanes; Skim Sect. 24.1 to 24.2
    -Distinguishing between alkanes, alkenes, and alkynes; cis-trans isomerism; benzene; Skim Sect. 24.2 to 24.3; Do p.1052: 3,16,17(skip heat of hydrogenation part),26abc,30
    -Chapters 1-2,24 Review
    -Chapters 1-2,24 Test

    Chapter 3: Mass Relationships in Chemical Reactions
    -Average atomic mass, mole concept, Avogadro's number, molar mass, molecular mass, mass spectrometers; Read Sect. 3.1 to 3.4; Do p.110: 5,6,14,16,18,20,24ab,26,30
    -Two types of percent composition problems, two types of empirical formula problems, determining molecular formulas; Read Sect. 3.5 to 3.6; Do p.111: 39,44,49,52
    -Formula of a Hydrate Lab
    -Chemical reactions, chemical equations, balancing, material balance, mass balance, stoichiometry; Read Sect. 3.7 to 3.8; Do p.112: 57,60a-k,63,68,72,75,78
    -Limiting reactant, excess reactant, actual yield, theoretical yield, percent yield; Read Sect. 3.9 to 3.10; Do p.114: 81-84,90,94,96,100,117c
    -Limiting Reactant Lab (LSSU)
    -Chapter 3 Review
    -Chapter 3 Test

    Chapter 4A and Sect. 19.1: Reactions in Aqueous Solutions, Part 1, and Balancing Redox Equations
    -Strong and weak electrolytes, nonelectrolytes, hydration, precipitation, double replacement (metathesis) reactions, solubility rules, spectator ions, writing net ionic equations; Read Sect. 4.1 to 4.2
    -Double Replacement Reactions Lab
    -Properties of acids and bases, hydronium ion, hydroxide ion, pH, litmus tests, strong versus weak acids and bases, acid ionization, base dissociation; Read Sect. 4.3
    -Arrhenius acids and bases, Bronsted acids and bases, diprotic and triprotic acids, amphoteric substances, acid-base neutralizations, gas-forming reactions; Read Sect. 4.3; Do p.160: 2,5,7-9,17,18,20,22,23,26,31-33
    -Determining oxidation numbers, oxidation-reduction reactions, half reactions, oxidizing and reducing agents, combination reactions, decomposition reactions, displacement (single replacement) reactions, activity series, disproportionations, concentration, preparing solutions, dilutions; Read Sect. 4.4 to 4.5; Do p.162: 44,46,48,50,52,54,56abc,59,62,64ab,66ab,70,72,74
    -Inorganic Nomenclature I: Oxidation Numbers Dry Lab
    -Balancing redox equations using the ion-electron method; Read Sect. 19.1; Do p.873: 1abe,2cd
    -Oxidation-Reduction Reactions Lab (LSSU)
    -Chapter 4A and Sect. 19.1 Review
    -Chapter 4A and Sect. 19.1 Test

    Chapter 4B: Reactions in Aqueous Solutions, Part 2
    -Gravimetric analysis, acid-base titrations, indicators, endpoint versus equivalence point, titration demonstrations; Read Sect. 4.6 to 4.7; Do p.163: 77,78,83,86-88,91,95,107,110,121
    -Redox and conductimetric titrations; Read Sect. 4.8
    -Standardizing a Solution of Sodium Hydroxide Lab
    -Acid-Base Titration Lab
    -Chapter 4B Review
    -Chapter 4B Test

    Chapter 5: Gases
    -Properties of gaseous substances, gas pressure and related units, Torricelli's barometer, atmospheric pressure, ideal gas characteristics, Boyle's law, Charles' law, Gay-Lussac's law, determining absolute zero on the Kelvin scale, combined gas law; Read Sect. 5.1 to 5.3
    -Avogadro's law and its relationship to reaction stoichiometry, standard conditions of temperature and pressure (STP, 1 atm, 0ºC), standard molar volume of a gas, ideal gas law derivation, gas law constants, calculating gas densities and molar masses of gases; Read Sect. 5.4; Do p.216: 14,17,20,24,26,29,32,34,39,41,44,46,47
    -Gas stoichiometry calculations, Dalton's law of partial pressures, using mole fractions in related calculations, collecting gases over water, calculating the standard molar volume of a dry gas; Read Sect. 5.5 to 5.6; Do p.217: 51,53,54,59,63,66,68,69,71
    -Molar Mass of Oxygen Lab
    -Calcium Carbonate Analysis: Molar Volume of Carbon Dioxide Lab
    -Kinetic molecular theory of gases, review ideal gas characteristics, Maxwell-Boltzmann distribution curves for molecular speeds, root-mean-square (rms) speed, gas diffusion and effusion, Graham's law of effusion, deviations from ideal behavior (real gases differ most at high pressure and low temperature), van der Waals equation; Read Sect. 5.7 to 5.8; Do p.219: 73(1st question only),74,76,78,83-86,89
    -Chapter 5 Review
    -Chapter 5 Test

    Review for First Semester Final Exam
    First Semester Final Exam

    Chapter 6: Thermochemistry
    -Second Semester Pre-assessment
    -Energy, types of energy, radiant energy, thermal energy, chemical energy, kinetic versus potential energy, law of conservation of energy, heat versus temperature, thermochemistry, system versus surroundings, open versus closed system, isolated system, exothermic versus endothermic process; Read Sect. 6.1 to 6.2
    -Thermodynamics, state functions, first law of thermodynamics, work, heat, related sign conventions, constant volume processes, constant pressure processes, enthalpy, thermochemical equations and associated rules, comparison of enthalpy and internal energy; Read Sect. 6.3 to 6.4; Do p.262: 11,12,14-19,24,25,28
    -Heat capacity, specific heat, constant-volume calorimetry, constant-pressure calorimetry, example problems (heat of combustion, hot metal dropped in water, acid and base solutions mixed, heating curve example); Read Sect. 6.5; Do p.264: 30-32,34-38,82
    -Determining the Specific Heat of a Metal Lab
    -Calorimetry Lab (LSSU)
    -Standard enthalpy of formation, standard state, standard enthalpy of reaction, direct calculation using standard enthalpies of formation, indirect calculation using Hess's Law; Read Sect. 6.6.
    -Enthalpy of solution, lattice energy, heat of hydration, heat of dilution; Read Sect. 6.7; Do p.264: 43,48,52,54,56,59,62,64,66,70,73
    -Chapter 6 Review
    -Chapter 6 Test

    Chapters 7-8: Quantum Theory and the Electronic Structure of Atoms; Periodic Relationships Among the Elements
    -Review wavelength, frequency, amplitude, electromagnetic radiation, Planck's quantum theory, photoelectric effect, photons, continuous spectra versus line spectra, emission spectrum of the hydrogen atom, Bohr's theory of the hydrogen atom, ground state, excited state, Rydberg constant and associated equations, electronic transitions, Lyman, Balmer, Paschen, and Brackett series; Read Sect. 7.1 to 7.3; Do p.312: 3,7,9,13,17,19,28,29,31,32
    -Electrons possess both wave and particle properties, de Broglie equation, Heisenberg uncertainty principle, Schrodinger equation, quantum mechanical description of the hydrogen atom, quantum numbers, allowed values, physical meaning, orbital shapes, orbital orientation, shells and subshells; Read Sect. 7.4 to 7.6; Do p.314: 40,44,53,54,56,58,63-65,70,75,100
    -Construct a table relating allowed values for quantum numbers to type and number of orbitals; include numbers of electrons allowed in shells and subshells; subshell designations, relative energies, Aufbau diagram, ground state electron configurations, Noble gas notation, Pauli exclusion principle, orbital box diagrams, Hund's rule, paramagnetism, diamagnetism; Read Sect. 7.7 to 7.9; Do p.315: 71,73,78,85,90-92,114,124
    -Development of the periodic table, Mendeleev, Meyer, Moseley, periodic law, periods, groups, alkali metals, alkaline-earth metals, halogens, noble gases, metals, nonmetals, semimetals or metalloids, transition metal elements, lanthanides, actinides, using the periodic table to determine electron configurations, valence electrons, isoelectronic, electron configurations of noble gases, cations, and anions, representing free elements in chemical equations, periodic trends in physical properties, effective nuclear charge, atomic radius, ionic radius; Read Sect. 8.1 to 8.3; Do p.356: 1,2,5,10,16,20,23,25,28,29,31,34,35,38,44,46
    -Ionization energy, electron affinity, electronegativity, general trends in chemical properties, acidic and basic oxides; Read Sect. 8.4 to 8.6; Do p.358: 51,56-58,61,72,77,81,83,91,93,120
    -Periodic Table and Periodic Law Lab (LSSU)
    -Chapter 7-8 Test Review
    -Chapter 7-8 Test

    Chapter 9: Chemical Bonding I: Basic Concepts
    -Valence electrons, Lewis dot symbols, formation of ionic bonds by electron transfer, relative stability of ionic solids, determining lattice energies directly from Coulomb's law and indirectly from a Born-Haber cycle; Read Sect. 9.1 to 9.3; Do p.400: 3,4,13-16,18,20,21,26
    -Formation of covalent bonds by electron sharing, compare and contrast the characteristics of ionic and molecular compounds, using electronegativity differences to classify bonds (nonpolar covalent, polar covalent, or ionic), rules for writing Lewis structures, octet rule, bonding and nonbonding electron pairs, structures with single, double, and triple bonds, formal charges; Read Sect. 9.4 to 9.7; Do p.401: 31,32,36,39,40,42,43,45-47
    -Lewis structures that violate the octet rule, incomplete octet, expandable octet, odd-electron molecules, Lewis structures for polyatomic ions, resonance structures and what they are intended to represent, bond energy, using bond energies in thermochemical calculations; Read Sect. 9.8 to 9.10; Do p.402: 52,54,55,60,63-66,69,71,73,79,90,104,109
    -Using bond energies in thermochemical calculations
    -Chapter 9 Review
    -Chapter 9 Test

    Chapter 10: Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
    -Valence-shell electron-pair repulsion (VSEPR) model, electron-pair geometry, molecular geometry, associated bond angle(s), axial and equatorial positions, using bond polarity and molecular geometry to determine molecular polarity, bond moment, dipole moment; Read Sect. 10.1 to 10.2; Do p.453: 5,7,9,10,12-14,16,18,19-21
    -Valence bond (V.B.) theory, potential energy curve for two H atoms, atomic orbital hybridization, hybridization in molecules containing double and triple bonds, atomic orbital overlap resulting in sigma and pi bonds; Read Sect. 10.3 to 10.5; Do p.454: 27,29,30,33,35,36,38,41
    -Molecular Geometry Lab
    -Molecular orbital (M.O.) theory, bonding and antibonding sigma and pi molecular orbitals, associated energy level diagrams, writing electron configurations, paramagnetism, diamagnetism, rules governing stability of M.O. configurations, bond order calculations, homonuclear diatomic molecules for second-period elements; Read Sect. 10.6 to 10.8; Do p.455: 45,46,48,54,55,58,60,62,64,69,71,82,83
    -Delocalized molecular orbitals in benzene and selected polyatomic ions
    -Chapter 10 Review
    -Chapter 10 Test

    Chapter 11: Intermolecular Forces, Liquids, and Solids
    -Kinetic molecular theory of liquids and solids, related properties, intermolecular forces of attraction (hydrogen bonding, dipole-dipole forces, and London dispersion forces), discuss how intermolecular forces influence boiling point, melting point, surface tension, viscosity, and specific heat; Read Sect. 11.1 to 11.3; Do p.504: 2,5,7,10,12,13,15,22,27,31
    -Crystal structure, unit cell, coordination number, compare and contrast crystal packing in a simple cubic cell (simple cubic, body-centered cubic, and face-centered cubic cells), compare and contrast intermolecular forces of attraction and physical properties for ionic, covalent, molecular, and metallic crystals; Read Sect. 11.4 to 11.7; Do p.505: 37,38,51-53,55
    -Phase changes, equilibrium vapor pressure, vapor pressure-temperature graphs, molar heat of vaporization, Clausius-Clapeyron equation, phase diagrams, determining the melting and boiling points, triple point, critical point, molar heat of fusion, molar heat of sublimation, heating curves; Read Sect. 11.8 to 11.9; Do p.507: 77,78,80,81,84,86,88,90,94,96,107
    -Chapter 11 Review
    -Chapter 11 Test

    Chapter 23: Nuclear Chemistry
    -Distinguishing between alpha, beta, and gamma radiation; writing and balancing equations for nuclear reactions; nuclear stability and nuclear binding energy; Read Sect. 23.1 to 23.2
    -Natural radioactivity, U-238 decay series, half life, nuclear fission and fusion; Read Sect. 23.3 to 23.6
    -Health hazards associated with radioactivity, radon gas, concerns regarding nuclear power plants, and radioactive waste disposal; Read Sect. 23.7 to 23.8
    -Understanding Half-Life Lab

    Review Chapters 1-10, Sect. 11.1-11.3, Sect. 19.1, Sect. 23.1-23.2, and Sect. 24.1-24.2 for the American Chemical Society (ACS) First Term General Chemistry Exam
    American Chemical Society (ACS) First Term General Chemistry Exam (Required for all College Chemistry students)

    If any time remains in the school year, we will continue our study of College Chemistry to ensure that students are well prepared for success in General Chemistry II. One or more of the following units will be selected for study:

    Chapter 12: Physical Properties of Solutions
    -Solute, solvent, solution, solubility, types of solutions; unsaturated, saturated, and supersaturated solutions; miscible and immiscible liquids; solubility rule and its meaning, how soap works; solutions, suspensions, colloids, and the Tyndall effect; molecular view of the solution process; Read Sect. 12.1, 12.2, and 12.8
    -Concentration units, percent by mass, mole fraction, molarity, molality, converting one concentration unit into another; Read Sect. 12.3; Do p.546: 11,16-18,19a,22
    -Temperature and solubility trends for solids and gases, effect of pressure on the solubility of gases, Henry's law, colligative properties of nonelectrolyte solutions, nonvolatile solute, vapor-pressure lowering, Raoult's law; Read Sect. 12.4 to 12.6; Do p.547: 27-29,37,38,49,52
    -Boiling point elevation, freezing point depression, osmosis review, osmotic pressure, colligative properties of electrolyte solutions, van't Hoff factor; Read Sect. 12.6 to 12.7; Do p.548: 55,56,58,59,63,64,68,71,73
    -Using Freezing Point Depression to Find Molar Mass Lab
    -Chapter 12 Review
    -Chapter 12 Test

    Chapter 13: Chemical Kinetics
    -Chemical kinetics, reaction rate, associated graph, average rate, rate constant, writing rate expressions; Read Sect. 13.1
    -Determining reactant orders, determining overall orders, writing rate laws; Read Sect. 13.2; Do p.603: 6-8,12,15,16,18
    -Summary of the kinetics of first-order, second-order, and zero-order reactions including rate laws, concentration-time equations, half-life equations, associated graphs, and rate constants determined from the slopes of the graphs; Read Sect. 13.3
    -Collision theory of chemical kinetics, temperature dependence of rate constants, reaction progress diagrams, activation energy, standard molar heat of reaction, exothermic and endothermic reactions, activated complex, transition state, Arrhenius equation, associated graph, activation energy determined from the slope of the graph; Read Sect. 13.4; Do p.604: 25-27,30,31,35,38-40
    -Rate Determination and Activation Energy Lab
    -Reaction mechanisms, elementary steps, relationship between the rate law and the rate determining step, molecularity, experimental support for reaction mechanisms, catalysts, characteristics, related reaction progress diagrams, enzyme catalysis; Read Sect. 13.5 to 13.6; Do p.605: 45,47,51,54,55,62,66,70,74,90,94,111
    -Chapter 13 Review
    -Chapter 13 Test

    Chapter 14: Chemical Equilibrium
    -Physical equilibrium, chemical equilibrium, equilibrium constant, law of mass action, homogeneous equilibria involving concentrations and pressures, relationship between Kp and Kc; Read Sect. 14.1 to 14.2; Do p.648: 5,7,9,11,14,15,17,19-21,24,26,31,32
    -Heterogeneous equilibria, multiple equilibria, summary of guidelines for writing equilibrium constant expressions, discuss equilibria homework; Read Sect. 14.2
    -Relationship between chemical kinetics and chemical equilibrium, reaction quotient, predicting the direction of an equilibrium reaction, calculating equilibrium concentrations; Read Sect. 14.3 to 14.4; Do p.650: 33,36,40,42,44,46,48
    -Determination of an Equilibrium Constant lab
    -Le Chatelier's principle, factors that affect equilibrium (concentration, pressure, volume, temperature), only a change in temperature changes the value of the equilibrium constant, catalusts have no effect on equilibrium concentrations of reactants and products; Read Sect. 14.5; Do p651: 51-53,55,56,59
    -Chapter 14 Review
    -Chapter 14 Test

    Chapter 15: Acids and Bases
    -Bronsted acids and bases, conjugate acid-base pairs, autoionization of water, Kw expression, pH, pOH, and related calculations, compare and contrast strong acids, weak acids, strong bases, and weak bases; Read Sect. 15.1 to 15.3; Do p.702: 4-6,15,17-19,23,24
    -Relative strengths of conjugate acid-base pairs, equilibrium expression for weak acids, acid ionization constant, percent ionization; Read Sect. 15.4 to 15.5
    -Equilibrium expression for weak bases, base ionization constants, relationship between ionization constants of acids and their conjugate bases; Read Sect. 15.6 to 15.7; Do p.703: 27,29,33,35,37,39,43,45,47,53,55
    -Diprotic and polyprotic acids, molecular structure and acid strength; Read Sect. 15.8 to 15.9
    -Acid-base properties of salts, acid-base properties of oxides and hydroxides, Lewis acids and bases; Read Sect. 15.10 to 15.12; Do p.704: 63,64,67-69,74-76,79,83,91
    -Chapter 15 Review
    -Chapter 15 Test

    Have a nice summer!
     
     
Last Modified on September 3, 2023