CHEM-152

- Describe the basic properties of solutions and how they form - Predict whether a given mixture will yield a solution based on molecular properties of its components - Explain why some solutions either produce or absorb heat when they form.

- Define and give examples of electrolytes - Distinguish between the physical and chemical changes that accompany dissolution of ionic and covalent electrolytes - Relate electrolyte strength to solute-solvent attractive forces.

- Describe the effects of temperature and pressure on solubility. - State Henry's law and use it in calculations involving the solubility of a gas in a liquid. - Explain the degrees of solubility possible for liquid-liquid solutions.

- Express concentrations of solution components using mole fraction and molality. - Describe the effect of solute concentration on various solution properties (vapor pressure, boiling point, freezing point, and osmotic pressure) - Perform calculations using the mathematical equations that describe these various colligative effects. - Describe the process of distillation and its practical applications. - Explain the process of osmosis and describe how it is applied industrially.

- Describe the composition and properties of colloidal dispersions. - List and explain several technological applications of colloids.

- Describe the types of intermolecular forces possible between atoms or molecules in condensed phases. (dispersion forces, dipole-dipole attractions, and hydrogen bonding). - Identify the type of intermolecular forces experienced by specific molecules based on their structures. - Explain the relation between the intermolecular forces present within a substance and the temperatures associated with changes in its physical state.

- Distinguish between adhesive and cohesive forces. - Define viscosity, surface tension, and capillary rise. - Describe the roles of intermolecular attractive forces in each of these properties/phenomena.

- Define phase transitions and phase transition temperatures. - Explain the relation between phase transition temperatures and intermolecular attractive forces. - Describe the processes represented by typical heating and cooling curves, and computer heat flows and enthalpy changes accompanying these processes.

- Explain the construction and use of typical phase diagram. - Use phase diagrams to identify stable phases at given temperatures and pressures, and to describe phase transitions resulting from changes in these properties. - Describe the supercritical fluid phase of matter.

- Define and describe the bonding and properties of ionic, molecular, metallic, and covalent network crystalline solids. - Describe the main types of crystalline solids: Ionic solids, metallic solids, covalent network solids, and molecular solids. - Explain the ways in which crystal defects can occur in a solid.

- Describe the arrangement of atoms and ions in crystalline structures. - Compute ionic radii using unit cell dimensions. - Explain the use of X-ray diffraction measurements in determining crystalline structures.

- Describe the defining traits of redox chemistry. - Identify the oxidant and reductant of a redox reaction. - Balance chemical equations for redox reactions using half-reaction method.

- Describe the function of a galvanic cell and its component. - Use cell notation to symbolize the composition and construction of galvanic cells.

- Describe and relate the definitions of electrode and cell potentials. - Interpret electrode potentials in terms of relative oxidant and reductant strengths. - Calculate cell potentials and predict redox spontaneity using standard electrode potentials.

- Explain the relations between potential, free energy change, and equilibrium constants. - Perform calculations involving the relations between cell potentials, free energy changes, and equilibrium. - Use the Nernst equation to determine cell potentials under nonstandard conditions.

- Describe the electrochemistry associated with several common batteries. - Distinguish the operation of a fuel cell from that of a battery.

- Define corrosion. - List some of the methods used to prevent or slow corrosion.

- Describe the process of electrolysis. - Compare the operation of electrolytic cells with that of galvanic cells. - Perform stoichiometric calculations for electrolytic processes.

- Define chemical reaction rate. - Derive rate expressions from the balanced equation for a given chemical reaction. - Calculate reaction rates from experimental data.

- Describe the effects of chemical nature, physical state, temperature, concentration, and catalysis on reaction rates.

- Explain the form and function of rate law. - Use rate laws to calculate reaction rates. - Use rate and concentration data to identify reaction orders and derive rate laws.

- Explain the form and function of an integrated rate law. - Perform integrated rate law calculations for zero-. first-, and second-order reactions. - Define half-life and carry out related calculations. - Identify the order of a reaction from concentration/time data.

- Use the postulates of collision theory to explain the effects of physical state, temperature, and concentration on reaction rates. - Define the concepts of activation energy and transition state. - Use the Arrhenius equation in calculations related rate constants to temperature.

- Distinguish net reactions from elementary reactions (steps) - Identify the molecularity of elementary reactions. - Write a balanced chemical equation for a process given its reaction mechanism. - Derive the rate law consistent with a given reaction mechanism.

- Explain the function of a catalyst in terms of reaction mechanisms and potential energy. - List examples of catalysis in natural and industrial processes.

- Distinguish between spontaneous and nonspontaneous processes - Describe the dispersal of matter and energy that accompanies certain spontaneous processes.

- Define entropy. - Explain the relationship between entropy and the number of microstates. - Predict the sign of the entropy change for chemical and physical processes.

- State and explain the second and third laws of thermodynamics. - Calculate entropy changes for phase transitions and chemical reactions under standard conditions.

- Define Gibbs free energy, and describe its relation to spontaneity. - Calculate free energy change for a process using free energies of formation for its reactants and products. - Calculate free energy change for a process using enthalpies of formation and the entropies for its reactants and products.

- Describe the nature of the equilibrium systems. - Explain the dynamic nature of a chemical equilibrium.

- Describe the ways an equilibrium system can be stressed. - Predict the response of a stressed equilibrium using Le Châtelier’s principle.

- identify the changes in concentrations or pressure that occur for chemical species in equilibrium systems. - Calculate equilibrium concentrations or pressures and equilibrium constants, using various algebraic approaches. - Explain how temperature affects the spontaneity of some processes. - Relate standard free energy changes to equilibrium constants.