CHEM 1042 - Principles of Chemistry II

1. Intermolecular forces
2. Solid state structure
3. Acids, bases, and their equilibria
4. Solubility equilibria
5. Chemical equilibria
6. Chemical kinetics
7. Chemical thermodynamics
8. Electrochemistry
9. Properties of solutions
10. Nuclear chemistry

1. identify the dominant intermolecular force present in a molecular compound.
2. make qualitative predictions (rankings) concerning the physical properties of various liquids based on their intermolecular forces.
3. describe the molecular interactions that differentiate solids, liquids, and gases.
4. describe and calculate the energies of phase changes and interpret phase diagrams.
5. describe the energetics of solution formation.
6. calculate and convert between the solution concentrations of percent, molarity, molality, and mole fraction.
7. describe the colligative properties of solutions and perform calculations regarding them.
8. determine the rate law of a reaction using the method of initial rates.
9. apply the integrated rate law and half-life equations for zero-order, first-order, and second-order reactions.
10. describe how temperature, activation energy, and molecular orientation influence reaction rates.
11. determine the rate law from a reaction mechanism.
12. describe how a catalyst influences the rate of a reaction.
13. write equilibrium constant expressions for chemical equations and find equilibrium
14. concentrations from initial concentrations and the equilibrium constant.
15. determine the effect of concentration change, volume change, temperature change, and addition of a catalyst on equilibrium using Le Chatelier’s Principle.
16. define and identify acids and bases using the Arrhenius, Brønsted-Lowry, and Lewis definitions.
17. analyze equilibria of acids and bases using acid/base dissociation constants.
18. calculate pH of acids, bases, and buffers solutions and construct acid/base titration curves.
19. calculate the solubility product constant from solubility data.
20. determine the solubility of a substance in water and in the presence of a common ion using the solubility product constant.
21. describe the factors the affect solubility, including a common ion, pH, and complex ion formation.
22. determine oxidation numbers and balance redox reactions in acidic or basic solutions.
23. calculate standard potentials for electrochemical cells and relate to standard free energy, potentials under nonstandard conditions, and the equilibrium constant.
24. calculate enthalpy change, entropy change, and free energy change for phase transitions and chemical reactions, using appropriate standard values from thermodynamic tables.
25. relate the change in thermodynamic quantities such as describe how enthalpy, entropy, and free energy influence the spontaneity of a reaction.
26. predict the sign of the change in entropy for reactions and phase transitions based on qualitative reasoning.
27. relate thermodynamic quantities to the value of the equilibrium constant for a reaction.
28. write balanced nuclear equations.
29. identify types of nuclear reactions, including radioactive decay, fission, and fusion.
30. analyze first-order decay of radionuclides.
31. use chemicals and basic laboratory equipment safely and with proper technique.
32. effectively communicate lab procedures, observations, and results both orally and in writing.
33. interpret and analyze qualitative observations and quantitative results from the laboratory.

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