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1. To present the basic concepts of chemistry as an intellectual discipline.
2. To provide opportunities for growth in the functional understanding of facts, principles, and concepts through the integration of laboratory and class work.
3. To develop facility in analytical thinking, and critical thinking, placing emphasis on thinking which involves logical and quantitative relationships.
4. To develop scientifically literate citizens through an understanding of the methods of science and the role of science in society and everyday living.
5. To stimulate interest in chemistry, to identify promising students, and to provide adequate preparation for further scientific studies.

After completing this course the student will be able to:

1. Describe matter and the different forms of energy: potential and kinetic.
2. Differentiate between mass and weight.
3. Recognize the three major forms of matter.
4. Understand the laws of conservation of energy and mass.
5. Distinguish between chemical and physical properties.
6. Differentiate between intensive and extensive properties.
7. Recognize various forms of matter: homogeneous and heterogeneous mixtures, pure substances, compounds and elements.
8. Describe atoms and molecules.
9. Recognize the scientific method.
10. Demonstrate proficiency in the use of SI units.
11. Utilize the unit factoring method in converting units.
12. Apply appropriate units to describe the results of measurements.
13. Calculate using exponential notation.
14. Report the proper number of significant figures in a measurement and in calculations.
15. Evaluate one variable in the equation density = mass/volume given the values of the other two.
16. Interconvert temperature scales.
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17. Write the symbols of chemical elements.
18. Describe the composition of an atom.
19. Differentiate between molecular formulas, empirical formulas and formula units.
20. Define an atomic mass unit.
21. Describe the various parts of the periodic table.
22. Contrast ionic and covalent compounds.
23. Express the oxidation numbers of atoms and polyatomic ions.
24. Systematically name inorganic compounds.
25. Name several common polyatomic ions.
26. Write and balance chemical equations.
27. Classify chemical compounds and chemical reactions.
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28. Adopt the mole as the unit of amount of a substance.
29. Recognize and use molar mass and mole relationships.
30. Describe isotopes and their composition.
31. Calculate the percent compositions of elements in compounds.
32. Derive and empirical formula given the percent composition.
33. Perform chemical calculations using balanced equations.
34. Deterime the limiting reagent in a chemical reaction.
35. Compare the actual yield in a reaction with the theoretical yield in order to determine the percent yield.
36. Distinguish between the terms solute, solvent, and solution, and between the terms concentrated and dilute.
37. Report the concentration of a solution in terms of molarity.
38. Understand the concept of, and calculations for, titrations.
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39. Differentiate between exothermic and endothermic processes.
40. Use specific heat and heat capacity to determine the amount of heat needed to raise the temperature of an object.
41. Carry out calculations of calorimetry to determine changes in energy.
42. Determine the amount of heat involved in melting, vaporization, and combustion of substances.
43. Use Hess' Law to find the enthalpy change, (H, for a reaction using thermochemical equations with known (H values.
44. Use Hess' Law to find the enthalpy change, (H, for a reaction using standard molar enthalpies of formation.
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45. Understand the wave view of light and how wavelength, frequency and speed are related.
46. Correlate the wave motion of a body of water to that of light.
47. Interconvert wavelengths and frequencies of light.
48. Describe and calculate the relationship between the energy of light and its frequency.
49. Describe the particle behavior of light; photons.
50. Appreciate that ordinary laws of mechanics do not apply to very small particles like electrons.
51. Correlate an electron density diagram with the probability of finding an electron at some location in space.
52. Analyze the electron distribution in atoms.
53. Describe the electronic structure of atoms in terms of their quantum numbers.
54. Use the Aufbau Principle to determine the structure of an atom.
55. Give the electronic structures of ions and of excited states of atoms.
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56. Use the periodic table to predict: electron configurations, covalent and ionic radii, ionization energy, electron affinity.
57. Predict melting points and atomic volumes of elements given data from neighboring elements.
58. Investigate the periodicity in the properties of elements and compounds using the periodic table.
59. Contrast metals, non-metals and metalloids.
60. Describe metallic and non-metallic properties.
61. Name ternary compounds.
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62. Describe ionic and covalent bonds.
63. Write the electronic structures of ions.
64. Draw Lewis dot structures of small covalent molecules and polyatomic ions with single, double and triple bonds.
65. Predict the electronegativity of an atom using the periodic table.
66. Use electronegativity as a measure of the attraction of an atom for the electrons in a bond.
67. Understand the continuum of bond descriptions starting with covalent, through polar covalent and ending with ionic bonds.
68. Determine the direction of the bond dipole in a diatomic molecule.
69. Establish the formal charge in a molecule and an polyatomic ion.
70. Predict the arrangement of atoms in a molecule or polyatomic ion from their formal charges.
71. Recognize resonance structures.
72. Calculate heats of reaction from average bond energies.
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73. Use valence shell electron pair repulsion theory to determine the shape, draw three-dimensional structures, and make models of molecules.
74. Determine the direction of a molecular dipole and hence whether it is polar or nonpolar.
75. Use valence bond theory to describe a bond.
76. Analyze the hybrid orbitals used in bonding in polyatomic molecules and ions.
77. Describe sp, sp2, and sp3 hybridization in single, double and triple bonds.
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78. Understand the basic ideas of molecular orbital theory.
79. Relate the shapes and overlap of atomic orbitals to the shapes and energies of the resulting molecular orbitals.
80. Distinguish between bonding and antibonding orbitals.
81. Apply the Aufbau Principle to find molecular orbital descriptions for homonuclear diatomic molecules and their ions.
82. Predict whether a diatomic molecule is paramagnetic or diamagnetic.
83. Find the bond order in diatomic molecules.
84. Relate bond order to bond stability.
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85. Recognize the difference in properties of gases compared to liquids and solids.
86. Read a manometer and interconvert pressure units.
87. Understand the interdependency of temperature, pressure and volume of a gas.
88. Calculate changes in pressure, volume, temperature, and amount of a gas using Boyle's Law, Charles' Law, Avogadro's Law and the Combined Gas Law.
89. Use the Ideal Gas Equation to do calculations about samples of gases.
90. Calculate gas densities and molar masses.
91. Determine the properties of mixtures of gases using Dalton's Law of Partial Pressure.
92. Calculate the relative rates of diffusion of two gases using Graham's Law.
93. Relate the observed properties of gases to the Kinetic Molecular Theory of Gases.
94. Describe the distribution of molecular velocities.
95. Explain which molecular features are responsible for nonideal behavior.
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96. Compare the kinetic-molecular theory of liquids and solids to that of gases.
97. Describe the changes of state: gas to liquid, and liquid to solid.
98. Compare intermolecular forces and intramolecular forces.
99. Differentiate between the Van Der Waals forces: hydrogen bonds, dipole-dipole and ion-dipole interactions, and London dispersion forces.
100. Understand the extraordinary physical properties of water in terms of hydrogen bonding.
101. Investigate the cause of evaporation of a pure liquid.
102. Explore the relationship between temperature and vapor pressure by tabulating and graphing the results of an experiment.
103. Describe the condition known as dynamic equilibrium.
104. Demonstrate an understanding of boiling and the equilibrium that exists during phase changes.
105. Compare cohesive forces (as in viscosity and surface tension) and adhesive forces (as in capillary action and the meniscus).
106. Describe the properties of solids.
107. Differentiate between crystalline and amorphous solids, ionic and molecular solids, metallic and covalent solids.
108. Recognize the structure of metals: closest packing and cubic.
109. Recognize the structure of simple ionic crystals.
110. Use the radius ratio rule to predict the coordination number in a crystal.
111. Recognize polymorphic structures.
112. Calculate the lattice energy of an ionic crystal using the Born-Haber cycle.