Course Title:  Honors Chemistry

2 Semesters – 10 credits – 5 class periods per week 

 

Course Description:
                Students electing to take Honors Chemistry at Woodcrest Christian evaluate, study and apply chemical principles theoretically and in the laboratory setting.  From the initial stages of understanding matter and energy at the atomic level, to mathematically solving for quantitative properties and qualitatively observing the world around them, students are immersed in the world of chemical operations. 
Instruction and assignments are taken from the advanced edition of Zumdahl, Zumdahl chemistry text, published in 2007.  Semester one and two both conclude with comprehensive written and laboratory final exams.  Biblical core truths are consistently weaved throughout the course including the fact that God is the creator and sustainer of all things, God operates consistently to His character thought sometimes in an unexpected manner, God calls us to be consistent discoverers of His truth, and God calls us to be faithful stewards of His creation. 
                In addition to the college preparatory chemistry subjects, (matter and energy, phases of matter, formulas and equations, atomic structure and bonding, acids, bases and salts, and organic chemistry), Honors Chemistry covers additional topics.  The study of thermochemistry, with an in depth study of exothermic and endothermic reactions, heat capacity and specific hear, thermochemical equations, heats of fusion and solidification and Hess’ Law are examples of topics covered in Honors but not in regular Chemistry.  Chemical Equilibria , including the concept of equilibrium, equilibrium constants, Le Chatelier’s principle, buffers, calculation of pH of weak and strong acids, titration curves, solubility products, and the common ion effect are additional examples of topics covered in Honors.  Furthermore, spontaneity, entropy and free energy plus electrochemistry, with oxidation – reduction reaction and concepts, balancing half reactions, calculating cell EMF and understanding voltaic cells and cell potentials are also unique topics to Honors Chemistry curriculum.  All of these content areas are taught with an emphasis for the student to think critically, express ideas clearly and find clarity and logic within data.
                Students are required to make numerous calculations and express answers in scientific notation, significant digits and appropriate on all class and laboratory work.  In looking at the course outline, one will see that the Honors Chemistry class also takes an in depth approach to limiting reactions, solubility rules, K_sp K_eq, dipole moments, hybrid orbitals, ideal gas law, gas densities, molar mass, Graham’s law of effusion, freezing point depression and others.  The course is supplemented with instructor demonstrations and “hands on “usage of lab facilities. Students are evaluated on their performance in the laboratory, chapter quizzes, unit tests, semester exams, as well as, homework assignments, which include a variety of problems, lab reports and special projects.
 
Course Objectives:

1. Communicate that God is the creator and sustainer of all things.
2. Explain with verse reference that God calls us to be faithful stewards of His creation.   
3.  Explain the experimental basis for the discovery of the subatomic particles of an atom. 
4. Identify and know how to use the periodic table to identify atomic numbers, atomic mass, identify type and family of element.
5. Classify matter into substances and mixtures and how to separate mixtures. 

       6.  Articulate how protons and neutrons in the nucleus are held together by nuclear forces.

1. Calculate molar masses and isotope data.
2. Describe chemical reactions by writing balanced equations.
3. Explain the quantity of one mole.
4. Determine empirical and molecular formulas.
5. Reason out basic nomenclature and formulas for ionic and molecular compounds.
6. Analyze lab data to known data to identify unknowns.
7. Safely use Bunsen burner, water bath, flame loop and identify possible sources of error.
8. Convert the mass of a molecular substance to moles, number of particles or volume of gas at STP. 
9. Articulate the steps in the scientific method and know how to make qualitative and quantitative measurements in both English and metric systems. 
10. Convert between English and metrics and how to report data in SNSDU.
11. Convert between Celsius and Kelvin. 
12. Measure in the lab and calculate density, mass and volume.
13. Calculate theoretical and percent yield based on limiting reagent data.
14. List examples in Chemistry in which God’s consistency is evident.
15. Communicate man’s responsibility to rule over and protect the Earth, especially in energy usage.
16. Explain that energy is exchanged or transformed in all chemical reactions and physical changes of matter.
17. Describe temperature and heat flow in terms of exothermic and endothermic thermal energy.
18. Articulate the heat flow as materials change phase, including phase change diagrams and calculations. 
19. Calculate thermodynamic quantities including heat flow, specific heat, molar heat, phase changes and Hess’s law.
20. Relate electron configurations to bonding patterns in atoms, including drawing Lewis dot structures. 
21. Use electronegativity and ionization energy and relate these to bond formation.
22. Calculate frequency and wavelength and energy of a photon using EMS and Planck’s constant. 
23. Apply polarity and VSEPR theory to the shapes of molecules.
24. Articulate the molecular orbital model.
25.  Articulate the kinetic molecular theory.
26. Apply the gas laws to relations between the pressure, temp, and volume of an ideal gas.
27. Know and use the values and meanings of standard temp and pressure.
28. Solve problems using the ideal gas law, density and molar mass of a gas and how to apply Dalton and Graham’s laws.
29.  Articulate the experimental basis for the development of the quantum theory of the atomic structure and the historical importance of the Bohr model. 
30. Relate the position of an element in the periodic table to its quantum electron configuration.
31. Use Hunds, Pauli and Aufbau to produce electron configs.
32. Identify the periodicity of the physical chemical properties of the elements and how it relates to atomic structure.
33. Articulate the definitions associated with solutions.
34. Describe the dissolving process at the molecular level by using the concept of random molecular motion.
35. Calculate concentrations of solutions in terms of molarity, molality, mole fraction, and % composition.
36. Calculate freezing point depression and vapor pressure of solutions.
37. Articulate factors that affect solubility.
38. Calculate molar mass of a solution using boiling point elevation.
39. Summarize osmotic pressure.
40. Illustrate a colloidal dispersion.
41.  Explain chemical equilibrium.
42. Calculate K_eqconstants and use them in discovering concentrations.
43. Use K_eq in heterogenous expressions.
44. Apply Keq to discover reaction quotients.
45. Articulate LeChatelier’s principle and predict the position of equilibrium with changes in pressure, temp or concentration.
46. List the properties of acids and bases and pH.
47. Calculate pH, pOH and concentrations of both strong and weak acids and bases using Kw.
48. Articulate and utilize the self autoionization of water in calculations.
49. Use K_a in evaluating acid strength and solving for pH and other values.
50. Calculate Ka from percent dissociation and use the 5% rule.
51.  Articulate and predict acid base properties of salts.
52. Calculate logs and antilogs of various numbers
53. Analyze a pH graph
54. Predict strength of acids and pH
55. Identify acidity based on lab data
56. Use various equipment to analyze acids including pH papers, other indicators, and burets.
57. Explain equivalents and titrations
58. Articulate the function of buffers
59. Calculate Ksp and molar solubility with and without common ions
60. Interpret and predict solutions with a common ion.
61. Predict if a ppt will form from two mixed salt solutions
62. Deduce the effect of a common ion on Ka and % dissociation of a weak acid.
63. Calculate the pH of a common ion / weak acid solution
64. Define entropy.
65. List examples of everyday processes showing increase in entropy.
66. Use entropy (2Law Thermo) to explain the need of an orderly God
67. Calculate entropy, enthalpy and Gibb’s Free energy (4 equations for Gibb’s)
68. Examine diagrams and processes to evaluate entropy changes
69. Explain LEO the lion goes GER
70. Identify redox reactions and which atom was ox / red
71. Balance redox in acidic solutions
72. Prepare galvanic cells and measure voltage
73. Generate a drawing of a typical galvanic cell labeling electrodes and flow of electrons
74. Calculate E cell from data
75. Differentiate from reduction potentials cathode and anode and calculate E cell from red potentials
76. Construct a new activity series based on lab data of metal reactivity
77. Name organic alkanes, alkenes, alkynes, and aromatic hydrocarbons including derivatives and benzene/phenyl groups
78.  Distinguish functional groups within organic molecules.

 
Textbook:                          
Chemistry, 7^th edition, Zumdahl , Zumdahl,  Houghton Mifflin 2007 ISBN 10: 0-618-71370-0
                Bible
 
Required Materials:
The materials needed to successfully complete this course are:

• Textbook Chemistry; Zumdahl/Zumdahl, 7^th edition, 2007
• three ring notebook used exclusively for chemistry (1.5-3” inches wide)
• 5 tabbed dividers
• lined notebook paper or spiral notebook for notes
• blue or black in pens
• calculator
• lab reporting book
• thin lined dry erase markers (one or more colors)
• closed toe shoes for lab
• hair ties for girls with shoulder length hair or longer

 
 
Prerequisites:

• Successful completion with a B or better of one year of laboratory science (Physics,  Biology or Honors Biology) and
• Completion or concurrent enrollment in Algebra II or Honors Algebra II and
• Mathematical entrance exam and
• Teacher Recommendations