Magic Day of Chemistry
- Page ID
- 439689
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Core Learning Goals Learning Objectives Reviewed during Magic Day of Chemistry
MAT:
- Describe the effect of intermolecular forces on a substance’s properties like the boiling point or heat of vaporization.
- Apply the Clausius-Clapeyron equation to problems involving the vapor pressures of liquids.
- Explain the essence of each of the following thermodynamic terms: enthalpy, entropy, and free energy.
- Understand what is meant by the temperature of a gas and its relationship to the average kinetic energy of a collection of gas molecules.
SOL
- Use heat capacities and the enthalpies of vaporization and fusion to calculate the heat necessary to raise the temperature of a substance a given amount.
- Construct a Born Haber cycle to calculate lattice energies of ionic compounds.
- Describe the important factors in the energetics of solution formation, both in terms of intermolecular interactions and thermodynamic variables.
- Relate the equilibrium constant to the rate constants for the forward and reverse reactions
- Define reaction quotient, Q, relate Q to the equilibrium constant, K, and explain how Q can be used to predict whether a system is at equilibrium, and if not, the direction a chemical system will move to establish equilibrium
- Given a chemical equation, write the expression for the reaction quotient and/or equilibrium constant
- Apply equilibrium concepts to calculations involving chemical reactions, concentrations, gas pressures, free energy, and other variables.
- Interpret the magnitudes of equilibrium constants regarding the extent of reaction that has occurred in the forward direction once equilibrium has been established
- Identify factors that can stress a system that is in a state of equilibrium and explain why these factors stress the equilibrium system
- Of the above factors, identify those that will alter the magnitude of the equilibrium constant, and how the constant will change as a result of the stress
- Apply Le Châtelier’s principle to predict the direction a system, originally in a state of equilibrium, will shift when stressed by adding or removing reactants, adding or removing products, or heating or cooling the system
AB1/AB2
- Write the equation for the auto-ionization of water and relate to Kw, [H+], [OH-], pH, and pOH
- Describe changes in Kw, [H+], [OH-], pH, and pOH as a solution increases in acidity or in alkalinity
- Characterize acids and bases in terms of their strength using the following properties: Ka, pKa, Kb, pKb, [H+], pH, [OH-], pOH, % ionization in water, and strength relative to water
- Perform quantitative calculations related to water solutions of acids, bases, and salts (Ka, pKa, Kb, pKb, [H+], pH, [OH-], pOH, and % ionization) including polyprotic acids, mixtures of weak acids or bases, and very dilute solutions of acids or bases
ECHEM
- Calculate the standard cell potential from a table of reduction potentials and interpret the meaning of the sign of the calculated potential.
- Calculate the cell potential when the system is not at standard state conditions.
- Relate the cell potential when the system is in a state of equilibrium and calculate the value of the equilibrium constant from the standard state cell potential or vice-versa.
- Relate the cell potential to the change in free energy.
- Explain what concentration cells are and how they are able to produce electrical energy, and calculate the cell potential for a concentration cell.