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chemistry 12

Chemistry 12

Periodic Table PT – no names polyatomic ions

Welcome,

On this page you will find resources for high school chemistry: worksheets, labs, handouts, and PowerPoint lessons. These resources are the product of many years of teaching, and I am happy to share them with you. I also want to share an important message.

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Introductory Notes:

The resources under "Links" below can be identified by their icons:

			PowerPoint lessons for teachers to use in class
			Handouts of PowerPoint lessons – no need for students to copy notes
			Study notes in Q&A format to highlight important concepts
			Other notes (not a PowerPoint handout or study note)
			Labs (students work with chemicals and equipment)
			Assignments and worksheets that require student participation

Most lessons represent approximately 70–80 minutes of class time. Some lessons are missing because there are no resources to post. This is true for study periods, student presentations, library periods, tests, field trips, videos, etc.

Some lessons in Chemistry 12 overlap material from Chemistry 11 because the two courses are from different curricula.

All text references refer to Fundamentals of Chemistry, 3rd Edition, by Brady & Holum. If you do not have access to this book, in many cases, page references from other textbooks can be substituted.

Unit 1: Atomic Structure

#	Topic	Description	Links
5	Atomic Structure	An overview of the model of the atom, stopping at Bohr and introducing EM radiation.
6	Bohr's Model, Photons	Discussing Bohr's successes and failures, ending with the conclusion that electrons are waves.
7	Quantum Mechanics	Discussing the characteristics of electrons and the first two quantum numbers.
8	...	Continuing with yesterday's lesson.
9	Orbitals	Using orbital diagrams and shorthand electron configurations to keep track of electrons.
10	Periodic Table	Using shorthand electron configurations to understand the structure of the modern periodic table
11	Orbital Characteristics	Discussing the shape of orbitals, their orientation, and the physical location of electrons in atoms.
12	Atomic Size	Linking atomic number, atomic size, electron affinity, and ionization energy.

Unit 2: Molecular Architecture

#	Topic	Description	Links
14	Bonding	How and why atoms combine to form molecules.
15	Hybrid Orbitals	Explaining bonding with orbital diagrams and Lewis diagrams.
16	Lewis Structures	Following a series of rules to draw Lewis structures.
17	VSEPR	Students build models of molecules according to the Valence Shell Electron Pair Repulsion theory.
18	Lone Pairs	Students build models to show how lone pairs affect VSEPR shapes. See yesterday's lesson for handout.
19	Electronegativity	Using electronegativity and VSEPR shapes to explain the polarity of molecules. See yesterday's lesson for study notes.
20	Intermolecular Forces	Discussing types of intermolecular bonds: ionic, dipole-dipole, hydrogen bonding, and London forces.
21	Crystals	Explaining the properties of solids with reference to intermolecular forces.
22	Predicting Properties	Students predict the relative melting point of solids and conduct an experiment to test their predictions.

Unit 3: Organic Chemistry

#	Topic	Description	Links
25	Foods Lab	Organic chemistry and the unique properties of carbon.
26	Functional Groups	Categorizing organic compounds into groups. Students build molecular models.
27	Hydrocarbon Naming	Discussing and practicing the rules for naming hydrocarbons.
28	...	Continuation of yesterday's lesson.
29	Alkanes and Alkenes Lab	Contrasting the chemical properties of alkanes and alkenes to illustrate the reactivity of a double bond.
31	Isomers	Students build models of isomers (compounds with the same chemical formula but different structures).
32	Naming Groups	Naming organic compounds with different functional groups.
33	Organic Synthesis	Introducting organic reactions and how these are used to synthesize compounds. See tomorrow's lesson for study notes.
34	Esters	Students make esters from alcohols and organic acids.
35	Review	Review of unit 3: organic chemistry.

Unit 4: Energy and Rates in Chemical Reactions

#	Topic	Description	Links
37	Heat of Combustion	Students determine the molar heat of combustion for paraffin wax.
38	Thermochemistry	Introducing concepts related to thermochemistry: calorimetry, heat capacity, molar heat of reaction, etc.
39	Thermochemical Equations	Adding heat terms to balanced chemical equations.
41	Hess's Law Lab	Students determine whether the heat released in a chemical reaction changes when the reaction is carried out in steps.
42	Hess's Law	Drawing enthalpy diagrams and combining equations according to Hess's law.
43	Heats of Formation	Using heats of formation instead of Hess's law to calculate energy changes.
44	Rates Demonstrations	Demonstrating factors that affect reaction rate. See tomorrow's lesson for files.
45	Rates of Reaction	Students graph reactant concentration versus time to determine reaction rates.
46	The Collision Theory	The Maxwell-Botzman distribution, the kinetic energy of particles, and the collision theory are used to explain reaction rates.
47	Transition State	Discussing activation energy and the affect of catalysts. (Note: brief lab activity.)
48	Nuclear Energy	Introducing concepts related to nuclear energy: radiation, fission, fusion, half-life, nuclear equations, the strong force, etc.
49	Review	Review of unit 4: energy and rates in chemical reactions.

Unit 5: Equilibrium - Introduction

#	Topic	Description	Links
51	Straw Lab	Students investigate equilibrium by transferring volumes of water with drinking straws.
52	...	Finishing the graphing and questions from yesterday's lab.
53	Reaction reversibility	Discussing how reactions travel in both directions: reactants to products and products to reactants.
54	Equilibrium Law	Calculating equilibrium constants and using these to determine concentrations in other reactions.
55	Le Chatelier's Principle	Explaining Le Chatelier's principle and what happens when an equilibrium is disturbed.
56	Le Chatelier Lab	Students apply the concepts learned in yesterday's lesson to explain changes they observe in a chemical equilibrium.
57	Equilibrium Calculations	Using RICE charts to help with equilibrium law calculations.
58	...	Continuing yesterday's lesson.
59	Net Ionic Equations	Writing net ionic equations by breaking salts into ions: e.g. MgCl₂(aq) really means Mg²⁺(aq) + 2Cl^–(aq).

Unit 6: Equilibrium - Applications

#	Topic	Description	Links
61	Ksp	Explaining how Ksp (solubility product) is different from Kc and starting calculations related to Ksp.
62	Common Ion	Students investigate the effect of a common ion on an existing equilibrium and calculate Ksp when a common ion is present.
63	...	Continuing yesterday's lesson.
65	Acids and Bases	Looking at different definitions of acids and bases: Arrhenius, Lewis, Bronsted.
66	Kw, pH	Explaining the ion-product constant of water and starting calculations related to pH.
67	Titration	Students perform an acid-base titration and graph the results to reveal a sharp change near the equivalence point.
68	Ka, Kb	Working with the last two equilibrium constants: Ka and Kb. (Brief lab activity.)
69	...	Continuing yesterday's lesson.
70	pH of Salts, Buffers	Predicting the pH of salt solutions and using buffers to resist changes in pH. (Brief lab activity.)

Unit 7: Redox and Electrochemistry

#	Topic	Description	Links
74	Redox	Introducing concepts related to redox: oxidation, reduction, oxidizing agent, oxidation numbers, etc.
75	Balancing	Balancing chemical equations using oxidation numbers.
76	Cell Types	Discussing the difference between electrolytic and galvanic cells. (Brief lab activity.)
77	Galvanic Cells	Students construct galvanic cells with different solutions and metals.
78	Cell Potential	Calculating cell potentials using standard reduction potentials.
79	...	Continuing yesterday's lesson.

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