Objectives

1. Identify the areas that encompass chemistry.
2. Differentiate between physical and chemical changes.
3. Differentiate between mixtures and compounds.
4. Explain the implications of the Law of Definite Composition and the Law of Multiple Proportions.
5. Identify Dalton's atomic theory, and give rationale that supports or disapproves each point in his theory.
6. Explain what spectral lines are and how Bohr used this information to develop his model of the atom.
7. Explain the contributions made by the mass spectrometer to the development of the atomic theory.
8. Explain the differences the model of the atom proposed by between Bohr's and Schrödinger.
9. Determine the electronic configuration of an element.
10. Draw Lewis dot diagrams.
11. Explain the contributions made by Mendeleef and Meyer.
12. Explain the arrangement of elements on the periodic table in terms of valence electrons, energy levels, and orbitals.
13. Identify and explain periodic trends for ionization energy, electronegativity and atomic radius.
14. Explain how ionization energy and electronegativity are used in predicting the metallic or nonmetallic character of an element.
15. Use electronegativity differences to predict bond types.
16. Use Lewis dot diagrams to show how an ionic bond is formed.
17. Explain how charges develop as a result of an ionic bond.
18. Explain how and why the size of an atom varies as it loses and gains an electron.
19. Use Lewis dot diagrams to show how a covalent bond forms.
20. Explain how charges develop as a result of a covalent bond.
21. Identify if a bond/molecule is polar or nonpolar.
22. Explain what factor(s) determines the physical properties of a substance.
23. Explain how bond strength varies in a periodic fashion.
24. Compare and contrast the properties of ionic and covalent bonded substances.
25. Explain what a coordinate covalent bond is, and identify when it occurs within a substance.
26. Explain how metallic bonds form.
27. Explain what a hybrid is and the cause for its development.
28. Identify sp, sp2, sp3. dsp2 and d2sp3 hybrids within molecules.
29. Explain differences between single, double, and triple bonds, and the properties associated with these differences.
30. Identify the limitations of the octet rule.
31. Explain what factors determine bond angles within a molecule.
32. Use VSEPR to identify molecular geometries.
33. Calculate molecular weights and formula weights.
34. Calculate the percentage composition of a compound.
35. Determine the empirical and molecular formula of a compound.
36. Explain what a mole is and how the concept is used in stoichiometric applications.
37. Use Gay-Lussac's Law and Avogadro's law in mass-mass, mass-volume, and volume-volume stoichiometric problems.
39. Identify the limiting reagent in a reaction.
40. Calculate theoretical yield in a chemical reaction.
43. Explain the postulates of the kinetic molecular theory.
44. Explain the theory behind and usage of Charles' Law, Boyle's Law, Gay-Lussac's Law, the Combined Gas Law, the Ideal Gas Law and Graham's Law of Diffusion.
45. Identify differences between ideal and real gases.
46. Identify the conditions needed to create an ideal gas.
47. Compare and contrast hydrogen bonds, dipole-dipole attractions, and induced dipoles, and their effect on the properties of molecules.
48. Use kinetic molecular theory to explain condensation, evaporation, boiling point, freezing point, and melting point.
49. Identify and explain the solubility amongst polar and non polar solvents.
50. Compare and contrast volatility, melting point, electrical conductivity, and hardness of ionic, molecular, covalent and metallic crystals.
51. Draw heating and cooling curves, and explain where potential energy and kinetic energy changes take place on these curves.
52. Calculate enthalpy changes associated with heating and cooling curves.
53. Define supercooling and the conditions under which it occurs.
54. Draw and interpret the significance of a phase diagram.
55. Explain trends in boiling points for the hydrogen halides.
56. Explain differences between exothermic and endothermic reactions.
57. Use Hess' Law to determine enthalpy changes in phase changes and chemical reactions.
58. Identify kinetic and potential energy changes on cooling and heating curves.
59. Explain the process of dissolution on a molecular/ionic level.
60. Explain the theory behind distillation.
61. Explain the concept of colligative properties.
62. Calculate freezing point depressions and boiling point elevations.
63. Explain what electrolytes and non-electrolytes are.
64. Discuss the relationship between electrolytes/non-electrolytes and colligative properties.
65. Explain the process of electrolysis.
67. Explain conduction that takes place in a fused salt and in a dissolved salt.
68. Define acids and bases according to Arrhenius and Brønsted-Lowry.
69. Identify the factors that determine the strength of an acid and base.
70. Explain variations in the acid strengths of the hydrogen halides.
71. Explain what acidic and basic anhydrides are.
72. Explain the relationship between Kw , [H +] and [OH -] of a solution.
73. Explain how the pH scale is constructed.
74. Calculate the pH and pOH of a solution.
75. Illustrate several ways the pH of a solution can be determined.
76. Explain the relationship between the molarity and normality of a solution.
77. Explain what a neutralization reaction is, and the products they form.
78. Identify mono, di, and triprotic/hydroxy acids and bases.
79. Name common acids, bases and their salts.
80. Explain a titration procedure and the role indicators play in the titration process.
81. Identify factors that influence the rate of a reaction.
82. Identify the rate law, rate constant, and reaction order for a reaction.
83. Explain collision theory.
84. Draw and interpret energy of activation diagrams.
85. Explain the role of a catalyst, and how it alters a reaction pathway.
86. Identify what a reversible and nonreversible reaction is.
87. Explain the concept of equilibrium.
88. Explain and illustrate LeChatlier's Principle.
89. Use the Law of Mass Action to determine an equilibrium constant.
90. Use a Keq to determine equilibrium concentrations for reactants and products.
91. Identify the equilibrium expression for acids/bases undergoing dissociation.
92. Explain what oxidation-reduction reactions are.
93. Identify oxidizing and reducing agents.
94. Explain what the activity series of metals represents.
95. Use the activity series of metals to predict single displacement reactions.
96. Classify the type of reaction that occurs.
97. Define the major components of an electrochemical cell.
98. Explain how an electrochemical cell works.
99. Use half-cell reactions to predict spontaneous/nonspontaneous reactions
100. Explain how a battery works.
101. Explain what causes a metal to corrode.
102. Explain the process of electrolysis.

Experiments

(1) Observations vs. Interpretations
(2) Measurement & Uncertainty
(3) The Density of an Unknown Liquid
(4) Mixtures vs. Compounds
(5) Spectral Lines of Hydrogen
(6) Identifying & Understanding Periodic Trends
(7) Paper Chromatography
(8) Molecular Shapes & Polarity
(9) The Empirical Formula of a Compound
(10) Stoichiometric Relationships & Limiting Reactants
(11) Copper-Silver Nitrate Reaction
(12) The Percent Composition of a Mixture
(13) A Reaction Between Magnesium & Hydrochloric Acid
(14) The Gelation of Polyvinyl Alcohol with Borax
(15) IMF & their Effect on the Properties of a Substance
(16) Heat of Fusion
(17) Hess' Law of Heats of Summation
(18) Metathesis Reactions & Using the Solubility Rules
(19) Cooling Patterns for a Substance and a Solution
(20) The Relationship Between Conductivity & F.P./B.P.
(21) Freezing Point Depression & Making Ice Cream
(22) Water of Crystallization & the Formula of a Hydrate
(23) Rate Determining Law of the Crystal Violet Reaction
(24) Altering the Rate of a Reaction
(25) Chemical Equilibrium
(26) Ksp and the Common Ion Effect
(27) Properties of Acids & Bases
(28) Standardizing a Base
(29) The Percentage of Acetic Acid in Vinegar
(30) Acid Dissociation Constant, Ka
(31) Titration Curves of Strong and Weak Acids & Bases
(32) Electrolysis of Aqueous Potassium Iodide
(33) Electroplating
(34) Chemical Activity of Metals
(35) Determining Cell Voltages
(36) Corrosion: An Electrochemical Problem
(37) Partial Thermal Degradation of Mixed Saacharides with Protein Inclusions