CHEMISTRY CONTENT SKILLS CHART
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1 I. NATURE OF CHEMISTRY A. Safety B. Fundamental quantitative relationships 1. Metric system a. Prefixes b. Difference between base units and derived units 2. Significant figures 3. Scientific notation 4. Density 5. Temperature conversions 6. Dimensional analysis 7. Accuracy and precision C. Graphing and calculator skills 1. General graphing skills 2. Calculator graphing skills 3. Computer graphing skills D. Defining chemistry 1. Classification of matter 2. Properties and changes of matter 3. Conservation laws a. First law of thermodynamics 4. Potential energy diagram a. Exothermic reactions b. Endothermic reactions 5. Specific heat calculations The Scientific Method (Foundation Lesson) Numbers in Science (Foundation Lesson) Literal Equations (Foundation Lesson) Dimensional Analysis Making a Semimicropycnometer Graphing Skills (Foundation Lesson) Graphing Calculator (Foundation Lesson) Data Collection Devices (Foundation Lesson) Chromatography Mass, Temperature, and Heat
2 II. STRUCTURE OF MATTER A. Atomic theory and atomic structure 1. History of the atom and experiments 2. Atomic models a. Dalton b. Thomson c. Rutherford d. Bohr 3. Modern atomic structure a. Atomic number b. Atomic mass c. Isotopes d. Percent abundance e. Average atomic mass 4. Quantum mechanical model 5. Electron configuration a. Elements b. Ions c. Exceptions 6. Orbital notation 7. Quantum numbers 8. Emission and absorption spectra 9. Lewis dot structures a. Atoms b. Ions B. Periodic table 1. Relationship between electron configuration and periodic table 2. Effective nuclear charge 3. Shielding effect 4. Periodic trends a. Atomic radii b. Ionic radii c. Ionization energies d. Electron affinity e. Electronegativity 5. Oxidation states 6. Chemical families C. Nuclear chemistry 1. Types of nuclear decay a. Alpha b. Beta c. Gamma 2. Writing and balancing nuclear equations 3. Nuclear stability 4. Half-life calculations 5. Fission and fusion 6. Nuclear reactor 7. Chemical applications a. Radioisotopes b. Tracers in nuclear medicine Matter Waves Isotopic Pennies Fluorescence Demo Light and Atomic Spectra (notes) Laser Light Electron Probability Electron Configurations, Orbital Notations, and Quantum Numbers Why Do They Call It a Periodic Table? The Do s and Don ts of Teaching Periodic Trends Periodic Properties Red Hot Half-Life
3 III. CHEMICAL BONDING A. Binding forces 1. Ionic 2. Covalent bond energies 3. Metallic 4. Polarity of bonds, electronegativities B. Bonding models 1. Lewis structures for molecules, ions including exception to the octet rule 2. Valence bond theory a. Hybridization b. Sigma and pi bonds c. Resonance 3. VSEPR a. Molecular geometry b. Bond angles c. Molecular polarity Chemical Bonding and Intermolecular Forces Molecular Geometry IV. CHEMICAL NOMENCLATURE A. Ionic B. Binary molecular C. Simple organic 1. Alkanes 2. Alkene 3. Alkyne 4. Alcohols D. Acids E. Complex ions Chemical Nomenclature V. CHEMICAL EQUATIONS A. Balancing chemical equations B. Types of chemical reactions 1. Synthesis 2. Decomposition 3. Single displacement 4. Double displacement 5. Combustion C. Identifying and predicting products of chemical reactions 1. Use of solubility rules 2. Net ionic equations Types of Reactions (notes) Types of Chemical Reactions Net Ionic Equations The Eight Solution Problem
4 VI. STOICHIOMETRY A. Composition stoichiometry 1. Calculations of molar mass 2. Mole conversions a. Molar mass b. Avogadro s number c. Molar gas volume 3. Percent composition 4. Empirical formula calculations 5. Molecular formula calculations B. Reaction stoichiometry 1. Mass-mass calculations 2. Mass-volume calculations 3. Volume-volume calculations 4. Percent yield 5. Limiting reactant calculations 6. Thermochemical calculations Simple vs. True Stoichiometry Limiting Reactant
5 VII. STATES OF MATTER A. Intermolecular forces 1. Ion-dipole 2. Dipole-dipole with H bonding 3. Induced dipole-induced dipole B. Relationship to states, structures and properties C. Gases 1. Kinetic-molecular theory 2. Avogadro s hypothesis 3. Gas laws: qualitative and quantitative relationships a. Boyle s b. Charles c. Gay-Lussac s d. Dalton s e. Graham s f. Ideal gas g. Henry s 4. Derivations from gas laws a. Combined gas law b. Gas density c. Molar mass calculations 5. Gas stoichiometry D. Liquids 1. Equilibrium vapor pressure 2. Phase changes and phase change diagrams E. Solids 1. Amorphous 2. Crystalline solids a. Ionic b. Molecular c. Metallic d. Network covalent solids F. Analyzing heating curves with calculations The Do s and Don ts of Teaching Intraparticle vs. Intermolecular Forces Dipole Dilemmas Don t Flip Your Lid May the Force Be with You Gases, Gases, Everywhere! Boyle s Law: Pressure-Volume Charles Law Pressure-Temperature Relationship in Gases Gas System Simulations Practice using Gas Laws Airbags How Sublime Heating Curves and Phase Diagrams
6 VIII. SOLUTIONS A. Properties of water B. Aqueous solutions and dissolving process C. Electrolytes and nonelectrolytes D. Solution vs. colloids vs. suspensions E. Solubility graphs F. Concentration calculations 1. Molarity 2. Molality 3. Percent by mass 4. Percent by volume 5. Mole fraction 6. Parts per million G. Colligative properties 1. Boiling point elevation 2. Freezing point depression 3. Raoult s law H. Determination of molar mass using colligative properties Solutions (notes) Preparation of Solutions How Sweet It Is! It s Not Easy Being Green (performance assessment) Conductivity of Ionic Solutions Colligative Properties IX. KINETICS A. Factors that affect rate 1. Temperature 2. Nature of reactions 3. State of subdivision 4. Concentration 5. Catalysts B. Determining rate and order of the reaction from given data C. Activation energy and the role of the catalyst D. Using mechanisms to predict order for a reaction Catalyst Demonstration Chemical Reaction Rates I Chemical Reaction Rates II The Iodine Clock Reaction Mechanisms of a Chemical Reaction
7 X. EQUILIBRIUM PLUS ACIDS AND BASES A. General equilibrium 1. Applying LeChantelier s principle 2. Calculations involving law of mass action B. Properties of acids and bases C. Theories 1. Arrhenius 2. Bronsted-Lowry 3. Lewis D. Identifying conjugate acid-base pairs E. Strengths of acids and bases F. Ionization of water 1. ph calculations of strong acids and bases 2. Relationship between ph and poh 3. Ka and Kb calculations 4. Qualitative buffer systems 5. Salt hydrolysis reactions G. Titration curves and calculations H. Ksp calculations Shifting Reactions Equilibrium Demo Le Chatelier s Principle Disturbing Equilibrium General Chemical Equilibrium Acid-Base Equilibrium How Weak Is Your Acid? Titrations Titrations Neutral or Not? What Do You Mean It s Soluble After All? XI. THERMODYNAMICS A. Calculate and interpret the value of Delta H 1. Tables of standard values 2. Hess law 3. Calorimetry 4. Bond energy B. Predict the sign of the entropy change in chemical reactions C. Calculate and interpret the value of Delta S from tables of standard values D. Calculate and interpret the value of Delta G 1. Tables of standard values 2. Gibb s equation Thermodynamics Hot and Cold How Hot Is a Candle? Hess Law XII. REDOX REACTIONS A. Assigning oxidation numbers B. Balancing redox reactions using the half-reaction method for acids and bases C. Electrochemistry 1. Voltaic cells a. Identify components b. Calculate cell potentials 2. Batteries, fuel cells, and storage batteries 3. Electrochemical cells vs. voltaic cells OIL RIG It s Electrifying Deposition
8 XIII. ORGANIC CHEMISTRY A. Draw and name: alkanes, alkenes, alkynes, alkadienes, cyclic aliphatic B. Isomers C. Draw and recognize and name 1. Structural isomers 2. Geometric isomers 3. Optical isomers D. Recognize the importance of biological molecules Long, Long Chains Biochemistry Protein Properties
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