Chemistry 12

Unit 1: Thermochemistry

Energy in chemical change: enthalpy and thermochemical vocabulary, calorimetry and experimental measurement, potential energy diagrams, Hess's Law and heats of formation, and the science-society context of energy.

• Thermochemistry vocabulary
• Molar enthalpies of combustion
• Combustion equations with energy
• Energy in changes of state
• Potential energy diagrams

• Designing a thermochemistry experiment
• Selecting instruments and processes
• Measuring reaction energy changes
• Hess's Law and reaction energy
• Applying prediction methods to data
• Displaying heats of formation

• Settings of scientific activity
• Risks and benefits of thermochemistry
• Questions thermochemistry can and cannot answer
• Courses of action on energy issues
• Co-operative thermochemistry experiments
• Identifying areas of further study
• Alternative energy solutions
• Technologies from thermochemistry
• Peer review in thermochemistry
• Research tools for information
• Integrating information sources
• Perspectives on a science decision

Unit 2: Solutions, Kinetics, and Equilibrium

How fast and how far reactions go: solubility and molar solubility, predicting precipitates, the factors and theory of reaction rate, and dynamic equilibrium applied to solubility.

• Organizing solubility data
• Molar solubility
• Variation in solubility
• Predicting precipitates
• Sources of error and uncertainty
• Solutions and equilibrium careers

• Factors affecting reaction rate
• Sampling procedures
• Collision theory
• Reaction mechanisms and catalysts
• Organizing kinetics data

• Equilibrium in solutions
• Factors affecting solubility via equilibrium
• Sampling for equilibrium expressions
• Solubility and equilibrium
• Technology revising understanding
• Technologies from scientific understanding

Unit 3: Acids and Bases

Acid-base chemistry: classification, definitions and their evolution, strength and pH, indicators, titration and stoichiometry, the water equilibrium, and the science-society context.

• Acid-base classification and nomenclature
• Acid-base definitions
• How acid-base theory evolves
• Evidence, theories, and paradigms
• Predicting acid-base products
• New questions from learning

• Strong vs weak acids and bases
• Calculating pH
• How indicators work
• Understanding from titration curves
• H+ and OH- via Le Chatelier
• Prediction and hypothesis (acid-base)

• Concentration by stoichiometry
• Collecting titration data
• Interpreting titration data
• Co-operative titration experiment
• Selecting titration instruments
• Modes of representation
• Line of best fit
• Apparatus and materials safety
• WHMIS handling and disposal
• Communicating acid-base results

• Society's influence on acid-base science
• Constructing acid-base arguments
• Acid-base careers

Unit 4: Electrochemistry

Redox and cells: defining oxidation and reduction, balancing half-reactions, galvanic and electrolytic cells, reduction potentials and spontaneity, electrolysis and electroplating, fuel cells, and evaluating electrochemical technologies.

• Questions about redox
• Scientific vs technological (redox)
• Defining oxidation and reduction
• Comparing redox to other reactions
• Balancing half-reactions

• Designing chemical cells
• Defining cell design problems
• Parts of cells
• Electrochemistry safety
• Evaluating a self-designed cell
• Designing a redox experiment
• Operational definitions

• Predicting spontaneity
• Predicting cell voltage
• Theoretical vs experimental potentials
• Reliability of redox data
• Electrochemical vs electrolytic cells
• Electrolysis and electroplating
• Hydrogen fuel cells
• Evaluating a technology design
• Analyzing natural and technological systems
• Applications of findings