GLEN RIDGE PUBLIC SCHOOLS

Curriculum Guide

 

 

Course Title:                             AP Chemistry

 

Subject:                                    Chemistry

 

Grade Level:                             11-12

 

Department/School:                  Science/High School

 

Duration:                                  Full Year

 

Number of Credits:                   6

 

Prerequisite:                              Grade “B” or better in Chemistry I Honors and have taken or are taking either Physics or Honors Physics, teacher recommendation

                                                and completion of the summer assignment.

 

Elective or Required:                 Elective

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Author:  Adam Smith

Date Submitted:  Summer 2004

Course Description

 

 

Advanced Placement Chemistry is a college-level class offered to juniors and seniors on an elective basis and may be taken in addition to but not instead of any one of other courses in the typical three year sequence:  Biology, Chemistry and Physics.  Students serious about science as a possible career choice should seek advice and assistance from the science department head each spring at program planning time.  The scope of the advanced placement high school program provides ample challenge, useful background, and a feeling for what is expected in attitude and responsibility from mature students preparing themselves for careers in science.  College texts, laboratory guides, reference materials and testing procedures are used throughout the advanced placement course.  With additional home study and preparation, students achieve success on the CEEB Advanced Placement Examination thereby qualifying them for advanced standing (earned credit) at colleges and universities of their choice.

 

This course is planned to meet the objectives of a general chemistry course on the college level.  The emphasis is on rigorous training in fundamental concepts required as preparation for future study in chemistry or in related fields.  Atomic structure, chemical bonding, reaction kinetics, equilibrium, oxidation-reduction, electrochemistry and acid based relationships are thoroughly treated.  All laboratory work stresses mastery of quantitative laboratory techniques.

 

The course in Advanced Placement Chemistry will involve teacher-directed presentations of content areas through class lecture, class discussion, student reports, investigations, and class group activities.  In addition, laboratory exercises will supplement and enhance topics.  Instruction will involve incorporation of current topics through readings and audiovisual presentations.  The course will be classroom, laboratory and project based instruction.

 

Assessment of student achievement each marking period will be determined by evaluations comprised of a combination of teacher-made examinations on major topics and quizzes, which will take forms to include oral, written and demonstration.  In addition, students will be graded on laboratory experiments, projects, and presentations.

 

GLEN RIDGE PUBLIC SCHOOLS

SCIENCE MISSION STATEMENT

 

 

 

The Glen Ridge Public School’s science curriculum seeks to develop scientifically literate life-long learners through a program that fosters a spirit of wonder, intellectual curiosity and collaborative problem solving that is authentic, hands-on, inquiry based and developmentally appropriate.  This is done through the study of Life, Physical, Earth and Environmental science.

 

Our students will use the scientific method to understand and respond to questions about science, technology, and societal and world problems.  Students will be challenged and encouraged to take risks and to develop critical thinking skills as they apply to real-world experiences.

 

 

New Jersey Core Curriculum Content Standards

 

Science

 

STANDARD 5.1 (SCIENTIFIC PROCESSES)  ALL STUDENTS WILL DEVELOP PROBLEM-SOLVING, DECISION-MAKING AND INQUIRY SKILLS, REFLECTED BY FORMULATING USABLE QUESTIONS AND HYPOTHESES, PLANNING EXPERIMENTS, CONDUCTING SYSTEMATIC OBSERVATIONS, INTERPRETING AND ANALYZING DATA, DRAWING CONCLUSIONS, AND COMMUNICATING RESULTS.

STANDARD 5.2 (SCIENCE AND SOCIETY)  ALL STUDENTS WILL DEVELOP AN UNDERSTANDING OF HOW PEOPLE OF VARIOUS CULTURES HAVE CONTRIBUTED TO THE ADVANCEMENT OF SCIENCE AND TECHNOLOGY, AND HOW MAJOR DISCOVERIES AND EVENTS HAVE ADVANCED SCIENCE AND TECHNOLOGY.

STANDARD 5.3 (MATHEMATICAL APPLICATIONS)  ALL STUDENTS WILL INTEGRATE MATHEMATICS AS A TOOL FOR PROBLEM-SOLVING IN SCIENCE, AND AS A MEANS OF EXPRESSING AND/OR MODELING SCIENTIFIC THEORIES.

STANDARD 5.4 (NATURE AND PROCESS OF TECHNOLOGY)  ALL STUDENTS WILL UNDERSTAND THE INTERRELATIONSHIPS BETWEEN SCIENCE AND TECHNOLOGY AND DEVELOP A CONCEPTUAL UNDERSTANDING OF THE NATURE AND PROCESS OF TECHNOLOGY.

STANDARD 5.5 (CHARACTERISTICS OF LIFE)  ALL STUDENTS WILL GAIN AN UNDERSTANDING OF THE STRUCTURE, CHARACTERISTICS, AND BASIC NEEDS OF ORGANISMS AND WILL INVESTIGATE THE DIVERSITY OF LIFE.

STANDARD 5.6 (CHEMISTRY)  ALL STUDENTS WILL GAIN AN UNDERSTANDING OF THE STRUCTURE AND BEHAVIOR OF MATTER.

STANDARD 5.7 (PHYSICS)  ALL STUDENTS WILL GAIN AN UNDERSTANDING OF NATURAL LAWS AS THEY APPLY TO MOTION, FORCES, AND ENERGY TRANSFORMATIONS.

STANDARD 5.8 (EARTH SCIENCE)  ALL STUDENTS WILL GAIN AN UNDERSTANDING OF THE STRUCTURE, DYNAMICS, AND GEOPHYSICAL SYSTEMS OF THE EARTH.

STANDARD 5.9 (ASTRONOMY and SPACE SCIENCE)  ALL STUDENTS WILL GAIN AN UNDERSTANDING OF THE ORIGIN, EVOLUTION, AND STRUCTURE OF THE UNIVERSE.

STANDARD 5.10 (ENVIRONMENTAL STUDIES)  ALL STUDENTS WILL DEVELOP AN UNDERSTANDING OF THE ENVIRONMENT AS A SYSTEM OF INTERDEPENDENT COMPONENTS AFFECTED BY HUMAN ACTIVITY AND NATURAL PHENOMENA.

Curriculum Description

 

 

Goal:    Each student will have the opportunity to achieve success in understanding the concepts and principles of topics in Advanced Placement Chemistry. The following learning objectives are aligned with the New Jersey Core Curriculum Content Standards for Science and Work Place Readiness as indicated after each objective.

 

Objectives:

The student will be able to:

1.      Understand the postulates of Dalton’s atomic theory.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1)

2.      Explain how the postulates of Dalton’s theory relate to the Laws of Conservation of Mass, Constant Composition, and Multiple Proportions.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1; 5.1.A2)

3.      Summarize the experimental work of Rutherford, Bohr, and de Broglie and explain how they contributed to a model of the atom.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1; 5.1.A2; 5.1.A3; 5.1.B2)

4.      Understand the postulates of the Quantum Theory.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1; 5.1.A2)

5.      Understand quantum numbers which describe an electron and interpret the physical significance of these numbers relating them to the s, p, d, and f notations.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1)

6.      Use Planck’s relationship to determine the characteristics of electromagnetic radiations (energy, frequency, or wavelength) when the appropriate data are given.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1; 5.1.A2; 5.1.A3)

7.      Understand the structure of an atom:  protons, neutrons, electrons, atomic number, mass number, isotopes.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1; 5.1.A2; 5.1.A3; 5.1.B2; 5.1.A4; 5.2.B1)

8.      Understand electron energy levels:  write electron configurations and orbital diagrams of an atom.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.A1; 5.1.A2; 5.1.A3; 5.1.B2; 5.1.A4; 5.2.B1; 5.2.B3)

9.      Understand bond polarities and electronegativities.  (5.1.B2; 5.1.A4; 5.6.A1; 5.6;A3; 5.6.A4)

10.  Write Lewis diagrams for molecules and polyatomic ions, including species where multiple bonds are present or where the central atom has an expanded octet.  (5.1.B2; 5.1.A4; 5.6.A1; 5.6;A3; 5.6.A8; 5.6.A4; 5.6.B2)

11.  Explain molecular models:  valence bond theory including hybridization, resonance, sigma and pi bonds. (5.1.B2; 5.1.A4; 5.6.A1; 5.6;A3; 5.6.A8; 5.6.A4; 5.6.B2)

12.  Use the valence shell electron pair repulsion model to explain the geometry of molecules.  Explain the bond angles, molecular geometry, polarity, and hybrid orbitals for one through six pairs of bonding electrons.  (5.1.B2; 5.1.A4; 5.6.A1; 5.6;A3; 5.6.A8; 5.6.A4; 5.6.B2)

13.  Explain the difference between structural, geometric, and optical isomerism.  (5.1.B2; 5.1.A4; 5.6.A1; 5.6;A3; 5.6.A8; 5.6.A4; 5.6.B2)

14.  Understand the essential features of molecular orbital theory.  (5.6.A1; 5.6;A3; 5.6.A8; 5.6.A4; 5.6.B2)

15.  Understand chemical bonding.  Explain how bonding in pure substances relates to the state, structure, and properties of matter.  (5.1.B2; 5.1.A4; 5.6.A1; 5.6;A3; 5.6.A8; 5.6.A4; 5.6.B2)

16.  Explain and apply the Ideal Gas Law.  (5.1.A4; 5.2.B1; 5.2.B3; 5.3.C1; 5.3.A1; 5.3.C1)

17.  Explain and apply the Laws of Boyle, Charles, Avogadro, Gay-Lussac, Dalton, and Graham.  (5.4.C1; 5.1A1; 5.1A2; 5.1;A3; 5.1B2; 5.1.A4; 5.2.B1; 5.2.B3; 5.3.C1; 5.3.A1; 5.3.C1)

18.  Use the kinetic molecular theory to explain the behavior of ideal gases.  (5.4.C1; 5.1A1; 5.1A2; 5.1;A3; 5.1B2; 5.1.A4; 5.2.B1; 5.2.B3; 5.3.C1; 5.3.A1; 5.3.C1)

19.  Interpret deviations from ideal gas behavior for real gases in terms of molecular behavior. (5.4.C1; 5.1A1; 5.1A2; 5.1;A3; 5.1B2; 5.1.A4; 5.2.B1; 5.2.B3; 5.3.C1; 5.3.A1; 5.3.C1)

20.  Understand the behavior of liquids and solids as explained by the kinetic molecular theory.  (5.4.C1; 5.1.A1; 5.1.A2; 5.1.A3; 5.1.B2; 5.1.A4)

21.  Explain changes of state, phase diagrams of one component systems, vapor pressure, boiling, and critical phenomena.  (5.4.C1; 5.1.A1; 5.1.A2; 5.1.A3; 5.1.B2; 5.1.A4)

22.  Understand crystal structures by comparing the number and arrangement of atoms in unit cells.  (5.4.C1; 5.1.A1; 5.1.A2; 5.1.A3; 5.1.B2; 5.1.A4)

23.  Understand types of solutions and factors affecting solubility.  (5.3.B1; 5.6.A6; 5.6.B1)

24.  Understand and use the concentration units molarity, molality, mole fraction, and mass percent of solute to solve solution problems.  (5.4.C1; 5.3.B1; 5.3.C1)

25.  Explain the effects of temperature and pressure on the solubility of solids, liquids, and gases in liquid solvents.  (5.4.C1; 5.3.B1; 5.3.C1)

26.  Understand and explain the effects of adding solute to solvent on vapor pressure, osmotic pressure, boiling point, and freezing point.  (5.4.C1; 5.3.B1; 5.3.C1)

27.  Apply colligative properties principles to solve problems involving vapor pressure lowering, osmotic pressure, boiling point elevation, and freezing point depression.  (5.4.C1; 5.3.B1; 5.3.C1)

28.  Explain the differences between the colligative properties of electrolytes and nonelectrolytes. (5.4.C1; 5.3.B1; 5.3.C1)

29.  Know how to write and balance chemical equations indicating ionic and molecular species present in reactions.  (5.4.C1; 5.3.B1; 5.3.C1; 5.6.A6; 5.6.B1)

30.  Understand precipitation reactions and net ionic reactions.  (5.3.B1; 5.3.C1; 5.6.A6; 5.6.B1)

31.  Apply solubility product constant (Ksp) principles to the solution of solubility including common ion effect and precipitation problems. (5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.C1)

32.  Understand oxidation-reduction reactions which includes defining oxidation number, balancing redox reactions, and explaining the role of the electron in oxidation-reduction reactions.  (5.4.C1; 5.3.B1; 5.6.A6; 5.6.B1)

33.  Understand electrochemistry involving electrolytic cells using standard cell potentials to predict the direction of redox reactions and the effect of concentration changes.  (5.4.C1; 5.3.B1; 5.6.A6; 5.6.B1)

34.  Understand the concept of  physical and chemical dynamic equilibria.  (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1)

35.  Understand equilibrium constants for gas reactions (Kc, Kp) and apply the principles to solve equilibrium problems.  (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1)

36.  Use Le Chatelier’s principle to explain how to control an equilibrium system’s direction. (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1)

37.  Understand the first law of thermodynamics.  (5.2.B1; 5.2.B3; 5.3.B1; 5.3.C1; 5.7.B2)

38.   Use principles of thermochemistry to solve problems involving heat of formation, heat of reaction, change in enthalpy, Hess’s law, heat capacity, and heats of vaporization and fusion. (5.2.B1; 5.2.B3; 5.3.B1; 5.3.C1; 5.7.B2)

39.  Understand the second law of thermodynamics explaining entropy’s role as a driving force for spontaneous change.  (5.2.B1; 5.2.B3; 5.3.B1; 5.3.C1; 5.7.B2)

40.  Understand the dependence of change in free energy on enthalpy and entropy changes.  Use the Gibb-Helmholtz  equation to determine reaction spontaneity.  (5.3.B1; 5.3.C1; 5.7.B2)

41.  Use principles of thermodynamics to solve problems involving free energy of formation and free energy of reaction.  (5.2.B1; 5.2.B3; 5.3.B1; 5.3.C1; 5.7.B2)

42.  Explain the relationship of change of free energy to equilibrium constants and electrode potentials.  (5.2.B1; 5.2.B3; 5.3.B1; 5.3.C1; 5.7.B2)

43.  Explain the horizontal, vertical, and diagonal relationships in the periodic table: atomic radii, ionization energies, electronegativities, electron affinities, and oxidation numbers.  (5.2.B1; 5.2.B3; 5.6.A5; 5.6.A7)

44.  Identify various regions of the periodic table: metals, nonmetals, groups or families, transition elements, periods, and metalloids.  (5.2.B1; 5.2.B3; 5.6.A5; 5.6.A7)

45.  Understand principles of kinetics: concept of reaction rates, reaction order and rate constant, effect of temperature and concentration of reaction rates, activation energy, the role of catalysts, the relationship between rate determining step and a reaction mechanism.  (5.4.C1; 5.3.B1; 5.6.A6; 5.6.B1)

46.  Understand stoichiometry: using chemical equations explain mass and volume relationships with emphasis on the mole concept.  (5.4.C1; 5.3.B1; 5.3.C1; 5.6.A6; 5.6.B1)

47.  Apply stoichiometric principles to solve problems  involving limiting reactant, actual yield, theoretical yield, and the percentage yield for a reaction.  (5.3.B1; 5.3.C1; 5.6.A6; 5.6.B1)

48.  Explain the concepts involved in various acid-base theories: Arrhenius, Bronsted-Lowry, and Lewis.  (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1)

49.  Understand acid-base reactions which includes explaining the differences between strong and weak acids and bases.  (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1)

50.  Apply principles of acid-base reactions to solve for [H+], [OH-], pH, pOH, Ka, and Kb in problems which include titrations and buffer systems.  (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1)

51.  Knowing the pKa for an acid-base indicator, select an appropriate indicator for an acid-base titration.  (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1) 

52.  Explain with equations why a molecule, cation, or anion will produce an acidic, basic, or neutral solution.  (5.4.C1; 5.2.B1; 5.2.B3; 5.3.B1; 5.3.D1; 5.3.A1; 5.3.C1)

53.  Identify, name, and draw structural diagrams for organic compounds including simple hydrocarbons and compounds containing a functional group.  (5.4.C1; 5.6.A7)

54.  Understand the physical and chemical properties of simple organic compounds including identification of some types of  reactions.  (5.4.C1; 5.6.A7; 5.6.B1)

55.  Identify the monomers used and the polymers formed in simple addition and condensation polymerization reactions.  (5.4.C1; 5.6.A7; 5.6.B1)

56.  Use measuring devices for experiments which include computers and computer probes, analytical balances, Spec 20 colorimeter, pH meter, burets, pipets, volumetric flasks, and the usual assortment of less precise equipment.  (5.1.B1; 5.1.C1; 5.4.C1; 5.1.B2; 5.1.A4)

57.  Write a formal laboratory report which includes the data collected with uncertainties inherent in the measuring devices, calculations which include the percent deviation, and a complete error analysis which show an understanding of the relationship between the sophistication of the equipment used and the expected precision of the results. (5.3.B1; 5.l.Bl; 5.l.Cl; 5.4.Cl; 5.l.Al; 5.l.A2; 5.l.A3; 5.l.A4; 5.l.B2; 5.3.Dl; 5.3.Al) (WP.2:2,3,4;  WP.3:1,3,6,7,9; WP.4:2,4,10; WP.5:5,6,7,8,9)

58.  Apply computer software to analyze and present data from investigations in chemistry. (5.4.Cl; 5.l.Al; 5.l.A2; 5.l.A3; 5.l.B2; 5.l.A4) (WP.2:1,3,4,5,6,7; WP.3:4,12,15)

59.  Apply mathematical operations and technology to express results of chemistry investigations using graphs and spreadsheets.  (5.3.Bl; 5.3.Dl; 5.3.Al; 5.3.Cl)  (WP.2:7,8,9)

60.  Become aware of career opportunities in areas of chemistry and engineering.  (5.2.B1; 5.2.B3; 5.2.A1)(WP.l:2,3,7,9)

 

 

Advanced Placement Chemistry

 

 

UNIT 1 - CHEMICAL FOUNDATIONS

           

Objectives:

Each student will be able to:

1.      Identify and apply the principal operations and limitations of the scientific method.

2.      Describe and apply the SI system of units and prefixes.

3.      Identify causes of uncertainty in measurement.

4.      Use significant figures in measurement and calculations.

5.      Compare and contrast accuracy and precision.

6.      Convert between units of the metric system.

7.      Convert between Celsius, Fahrenheit, and Kelvin scales.

8.      Calculate density from data.

9.      Classify matter by phase, homogeneous or heterogeneous, element or compound.

 

Duration of Time:  Summer Assignment

 

 

UNIT 2 - ATOMS, MOLECULES, AND IONS

 

Objectives:

Each student will be able to:

1.      Describe contributions of early chemists.

2.      Illustrate the laws of conservation of mass, definite proportion, and multiple proportion.

3.      Describe Dalton’s atomic theory.

4.      Summarize experiments that characterized the structure of the atom.

5.      Describe features of subatomic particles.

6.      Use correct symbols for identifying a particular isotope of an element.

7.      Explain the bonding concept and show various ways of representing molecules.

8.      Describe and locate elemental groupings on the periodic table.

9.      Name compounds given the formula and vice versa.

 

Duration of Time:  Summer assignment

 

 

UNIT 3 - STOICHIOMETRY

 

Objectives:

Each student will be able to:

1.      Describe the basis for the atomic mass scale.

2.      Explain the significance of the mole in chemistry.

3.      Convert among moles, mass, and particles of a sample.

4.      Calculate molar mass.

5.      Calculate mass percent of an element in a compound.

6.      Calculate the empirical formula of a compound.

7.      Calculate molecular formula given the empirical formula and molar mass.

8.      Interpret the symbols of a chemical reaction.

9.      Write a balanced equation from a description of a chemical reaction.

10.  Calculate the masses of reactants and products using a chemical reaction.

11.  Define the characteristics of a limiting reactant problem.

12.  Calculate products based upon the limiting reactant concept.

 

Duration of Time:  Summer assignment

 

 

UNIT 4 - TYPES OF CHEMICAL REACTIONS

 

Objectives:

Each student will be able to:

1.      Relate polarity of water to its effectiveness as a solvent.

2.      Define and identify electrolytes, strong electrolytes, and non-electrolytes.

3.      Apply molarity concept to problem solving involving composition of solutions.

4.      Apply solubility rules to predict whether a solid will form during aqueous reactions.

5.      Classify and write aqueous reactions as molecular, ionic, and net ionic.

6.      Complete stoichiometric calculations involving precipitation reactions.

7.      Complete stoichiometric calculations involved in acid-base titration processes.

8.      Classify oxidation-reduction reactions.

9.      Assign oxidation numbers to elements, ions, and molecules.

10.  Compare and contrast oxidizing and reducing agents.

11.  Balance redox reactions in acids and bases using the half-reaction method.

 

Duration of Time:  3 Weeks

 

 

UNIT 5 - GASES

 

Objectives:

Each student will be able to:

1.      Describe an effect of atmospheric pressure and how barometers work.

2.      Relate pressure, volume, and temperature using gas laws and calculate unknown values.

3.      State the ideal gas law and derive R for standard conditions.

4.      Calculate stoichiometric unknowns for reactions involving gases.

5.      Calculate molar mass from gas density.

6.      Relate partial pressure, total pressure, and mole fraction for gas mixtures.

7.      Define temperature and kinetic energy using the kinetic molecular theory of gases.

8.      Compare and contrast effusion and diffusion and calculate the relative velocities from gram formula masses and vice versa.

9.      Describe qualitatively how real gases deviate from ideal behavior.

 

Duration of Time:  1 Week

 

 

UNIT 6 - ELECTROCHEMISTRY

 

Objectives:

Each student will be able to:

1.      Create a galvanic cell from a redox reaction.

2.      Define the components of an electrochemical cell.

3.      Compare and contrast a galvanic and an electrolytic cell.

4.      Describe how standard reduction potentials are assigned relative to hydrogen.

5.      Calculate a cell potential based upon a redox reaction.

6.      Use line notation to describe an electrochemical cell.

7.      Calculate Gibbs free energy from the maximum cell potential.

8.      Apply the Nernst equation  to calculate cell potential from concentration differences.

9.      Calculate equilibrium constants from cell potentials by applying Nernst equation when cell potential is zero and Q=K.

10.  Explain the electrochemical nature of corrosion and describe means for preventing it.

11.  Calculate stoichiometric quantities of electrolysis reactions.

12.  Predict the order of electrolysis of the components of a mixture.

 

Approximate duration:  3 Weeks

 

 

UNIT 7 - ATOMIC STRUCTURE AND PERIODICITY

 

Objectives:

Each student will be able to:

1.      Characterize electromagnetic radiation in terms of wavelength, frequency, and speed.

2.      Compare and contrast quantized and continuous energy.

3.      Describe how light has both wave and particulate properties.

4.      Show how the line spectrum of hydrogen demonstrates the quantized nature of the electron.

5.      Calculate energy changes when the electron moves from an excited to ground state in hydrogen.

6.      Explain the significance of electron probability distributions.

7.      Explain the quantum numbers n, l, ml.

8.      Describe the orbital shapes designated by s, p, and d.

9.      Define electron spin, ms, the Pauli exclusion principle, and spin quantum number.

10.  Apply Aufbau principle, Hund’s rule, and Pauli exclusion principle to write electron configurations for elements and representative ions.

11.  Indicate types of information that can be obtained from the periodic table.

12.  Show general trends in ionization energy, electron affinity, atomic radius, ionic radii, and shielding.

 

Duration of Time:  1 Week

 

 

UNIT 8 - BONDING AND ORBITALS

 

Objectives:

Each student will be able to:

1.      Explain why an ionic or covalent bond forms.

2.      Use electronegativity different to describe the nature of a bond.

3.      Relate bond polarity and molecular dipole moment.

4.      Predict the formula of an ionic compound.

5.      Relate the electronegativity different to the percent ionic character of a bond.

6.      Describe the covalent bonding model.

7.      Use bond energies to calculate heats of reaction.

8.      Compare and contrast lone pair and bonding pair electrons.

9.      Write Lewis structures for basic and some exceptions to the octet rule.

10.  Write Lewis structures for substances displaying resonance.

11.  Predict molecular geometry of substances with and without lone pairs on the central atom.

12.  Describe how special hybridized orbitals are formed in covalent bonding.

13.  Describe paramagnetism and diamagnetism and give and example of a substance which illustrates paramagnetism.

 

Duration of Time:  2 Weeks

 

 

UNIT 9 - LIQUIDS AND SOLIDS

 

Objectives:

Each student will be able to:

1.      Compare and contrast intermolecular forces, such as London dispersion, dipole-dipole, and hydrogen bonding.

2.      Describe the effect of intermolecular forces on surface tension, capillary action, viscosity, vapor pressure, boiling point, melting point.

3.      Compare and contrast crystalline and amorphous solids.

4.      Define lattice energy and compare lattice energies of different ionic substances (not in Zumdahl text).

5.      Describe closest packing of metal atoms.

6.      Use the electron sea model for metal bonding to explain properties of metals.

7.      Classify alloys by how they are created and the resulting alloy properties.

8.      Describe the bonding in molecular solids.

9.      Describe the structures of ionic solids and the resulting physical properties.

10.  Calculate vapor pressure using the Clausius-Clapyron equation.

11.  Describe the heating curve for water and state how the curve may change for other species.

 

Duration of Time:  2 Weeks

 

 

UNIT 10 - THERMODYNAMICS IN CHEMISTRY

 

Objectives:

Each student will be able to:

1.      Illustrate energy flow between a system and its surroundings.

2.      State the first law of thermodynamics.

3.      Define enthalpy and calculate the change in enthalpy in a chemical reaction using a calorimeter.

4.      Apply Hess’ law to calculate H° for a reaction.

5.      Use standard enthalpies of formation to calculate H° for a reaction.

6.      Define a spontaneous process.

7.      Predict entropy change in a process.

8.      State the second law of thermodynamics.

9.      Relate entropy changes in a system and surroundings.

10.  Define free energy and relate it to spontaneity.

11.  Explain why free energy equals zero at equilibrium.

12.  Predict the sign of entropy for a given process.

13.  Calculate the change in standard entropy values for a reaction.

14.  Calculate standard free energy change in a chemical reaction and use the results to predict spontaneity.

15.  Define equilibrium in terms of free energy.

16.  Relate equilibrium constant K to changes in standard free energy.

 

Duration of Time:  2 Weeks

 

 

UNIT 11 - KINETICS

 

Objectives:

Each student will be able to:

1.      Compare and contrast integrated and differential rate laws.

2.      Define reaction rate and how rates can be measured from experimental data.

3.      Describe methods for determining the rate law of a reaction.

4.      Summarize kinetics of zero, first, and second order reactions.

5.      Relate reaction mechanism and corresponding rate law.

6.      Describe the collision model for reaction progress.

7.      Relate temperature changes to reaction rates.

8.      Explain how a catalyst speeds up a reaction.

9.      Compare and contrast heterogeneous and homogeneous catalysis.

 

Approximate duration: 2 Weeks

 

 

UNIT 12 - SOLUTIONS

 

Objectives:

Each student will be able to:

1.      Describe solution composition as molarity, molality, mass percent, and mole fraction.

2.      Show how molecular structure, pressure, and temperature affect solubility.

3.      Show how a solution’s vapor pressure is affected by the concentration of solute and the interaction of solute and solvent.

4.      Calculate colligative properties of solutions.

5.      Describe osmosis and calculate molar mass from osmotic pressure.

6.      Describe a colloid and explain its stability.

 

Duration of Time:  2 Weeks

 

 

UNIT 13 - CHEMICAL EQUILIBRIUM

 

Objectives:

Each student will be able to:

1.      Explain how a dynamic equilibrium is established.

2.      Write the law of mass action for a reversible reaction and define the equilibrium constant.

3.      Define Kp and Kc.

4.      Write equilibrium expressions for heterogeneous phase reaction.

5.      Define the reaction quotient and use its value to predict shifting to an equilibrium position.

6.      Calculate equilibrium concentrations or pressures given Kp or Kc.

7.      Write and apply a generalized procedure for calculating equilibrium concentrations.

8.      Solve quadratic equations using the quadratic formula and successive substitution.

9.      Apply Le Chatelier’s Principle to predict the direction of shift of a system at equilibrium.

 

Duration of Time:  2 Weeks

 

 

UNIT 14 - ACIDS AND BASES

 

Objectives:

Each student will be able to:

1.      Compare and contrast Arrhenius, Bronsted-Lowry, and Lewis models of acids and bases.  (Lewis is in text section 14.11)

2.      Define Ka as an equilibrium constant.

3.      Relate acid strength to the dissociation equilibrium.

4.      Define amphoterism and apply the concept to water.

5.      Describe the pH scale and convert between [H+], [OH-], pH, and pOH.

6.      Calculate [H+], [OH-], pH, and pOH for strong and weak acids.

7.      Calculate percent dissociation (or ionization) for a weak acid.

8.      Calculate [H+], [OH-], pH, and pOH for strong and weak bases.

9.      Describe the dissociation equilibrium of polyprotic acids.

10.  Calculate [H+], [OH-], pH, and pOH for polyprotic acids.

11.  Determine and explain the resulting pH from common salt solutions.

12.  Relate molecular structure to acid-base properties.

13.  Predict the products from reactions of oxides with water and determine if resulting solution is acidic or basic.

14.  Describe a general problem approach for acid-base calculations.

 

Duration of Time:  3 Weeks

 

 

UNIT 15 - APPLICATIONS IN AQUEOUS EQUILIBRIUM

 

Objectives:

Each student will be able to:

1.      Describe the effect of a common ion on acid dissociation equilibria and solve problems.

2.      Describe the species present in a buffer solution and calculate pH.

3.      Apply the Henderson-Hasselbalch equation to buffer problems.

4.      Compare the buffering capacity of different solutions.

5.      Calculate the pH at any point of an acid-base titration using strong and weak acids and bases.

6.      Explain how acid-base indicators work.

7.      Calculate the solubility product of a salt given its solubility and vice versa.

8.      Predict relative solubilities from Ksp values.

9.      Determine salt solubility in various pH solutions.

10.  Predict precipitate when solutions are mixed and use of selective precipitation rules.

11.  Calculate equilibrium concentrations of complex ions.

12.  Relate complex ion formation to a salt’s solubility.

 

Duration of Time:  2 Weeks

 

 

UNIT 16 - NUCLEAR CHEMISTRY

 

Objectives:

Each student will be able to:

1.      Relate the stability of the nucleus to the relative number of protons and neutrons in the nucleus.

2.      Classify the types of radioactive decay and illustrate the decay particle using standard symbols.

3.      Calculate the half-life of a radioactive nuclide.

4.      Describe how one element may be changed into another using particle bombardment.

5.      Calculate the age of an organic sample using carbon dating.

6.      Describe the mass/energy interchange described by E=mc 2.

7.      Compare and contrast nuclear fission and nuclear fusion.

8.      Describe results from radiation exposure on humans.

 

Duration of Time:  1 Week

UNIT 17 - BASIC ORGANIC STRUCTURES

 

Objectives:

Each student will be able to:

1.      Describe the nomenclature system of organic chemistry.

2.      Apply naming rules for alkanes, including structural isomerism.

3.      Write basic reactions involving alkanes.

4.      Apply naming rules for alkenes and alkynes.

5.      Write basic reactions involving alkenes and alkynes.

6.      Identify basic functional groups and give an example of each.

 

Duration of Time:  2 Weeks

 

 

Advanced Placement Course Description (The College Board)

Recommended Laboratory Experiments

 

1.      Determination of the Formula of a Compound

2.      Determination of the