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Topic

Description

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3

Periodic Table

Crossword puzzle and periodic table activity.

4

Atomic model

Historical overview of the atom from Democritus to Bohr.

5

Alkali Metals Lab

Combining alkali metals with water – what could be more fun than explosions?

6

Periodic Trends

Examining how ionization energy and electron affinity change with an element's position on the periodic table.

8

Ionic Bonding

Lewis dot diagrams and chemical bonding between metals and nonmetals.

9

Covalent Bonding

Chemical bonding between two nonmetals (a continuation of yesterday's worksheet).

10

Physical Properties Lab

Comparing the physical properties of two solids. (This is a good time to teach students how to light and use Bunsen burners.)

11

Electronegativity

Using electronegativity to predict bond strength and solubility. The second half of today's class is spent learning element names and symbols.

12

Naming

Rules for naming ionic and covalent compounds.

13

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Continuing yesterday's work. Rules for naming acids, bases, and hydrates.

14

Naming Review

It is difficult to name all types of compounds. Today's assignment is a good way for students to gauge their understanding of this topic.

15

Types of chemical reactions

Reaction types include synthesis, decomposition, single displacement, and double displacement. Part 1 is set up as a lab but is better as a demonstration. Students should do part 2 themselves - it's fun.

16

The Activity Series

Predicting chemical reactions using the activity series. (Note: brief lab activity.)

17

Review

Review of unit 1: matter and chemical bonding.

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Topic

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20

Proportions

Proportions and percentage composition – lab and calculations.

21

Significant Digits

Significant digits and isotopic abundance.

22

The Mole

Introducing the mole concept. Today's lesson is brief, which leaves time to return and discuss the tests from Unit 1.

23

Molar Mass

Molar mass and simplest formula calculations (see yesterday's lesson for files).

 

24

Molecular Formula

Empirical (i.e. simplest) and molecular formula calculations.

25

Hydrates Lab

Applying the molecular calculations from yesterday to determine the number of moles in a hydrate.

26

Balancing Equations

Balancing chemical equations and balancing nuclear equations.

27

Calcium Lab

The reaction of calcium with water.

28

Factor Label Method

Introducing the factor label method, which will be used for all subsequent lessons in this unit.

29

Stoichiometry

Introducing stoichiometry - used to calculate the relative quantities of two chemicals in a reaction.

30

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Continuing the calculations from yesterday.

 

31

Limiting Reagents

Limiting reagents adds another layer of complexity to stoichiometry.

32

Limiting Reagents Lab

Using the concepts from yesterday's lesson to predict the limiting reagent in a reaction.

33

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Completing yesterday's lab and the calculations from the first "Limiting Reagents" class.

 

34

Percentage Yield

Comparing theoretical and actual yields to determine percentage yield. Builds on stoichiometry and limiting reagents.

35

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Continuing the percentage yield calculations from yesterday.

 

36

Review

Review of unit 2: quantities in chemical reactions.

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Topic

Description

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38

Solubility

Introduction to solubility, including a discussion of intermolecular forces.

39

Concentration

Concentration = quantity of solute ÷ quantity of solution. This lesson focuses on concentration calculations (V/V, W/W, W/V, ppm, ppb, mol/L).

41

Molar Solutions

Making molar solutions from solids – procedure and calculations. (Note: brief lab activity.)

42

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Making molar solutions from liquids – similar to molar solutions from solids except pipettes are used to measure moles (via volume). (Note: brief lab activity.)

43

Net Ionic Equations

Writing net ionic equations by breaking salts into ions: e.g. MgCl₂(aq) really means Mg²⁺(aq) + 2Cl^–(aq).

44

Solubility Rules

Today's lab involves a series of double displacement reactions that yield precipitates. Results are summarized as a series of solubility rules.

45

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Finishing the questions from yesterday's lesson.

 

47

Solubility Curves

Students investigate the solubility of a chemical at different temperatures. Class data is plotted to create a "solubility curve".

48

Water Treatment

Water treatment crossword puzzle.

49

Solutions Stoichiometry

Extending the stoichiometry calculations from Unit 2 to include solutions.

50

Conductivity Lab

Students investigate why some solutions conduct electricity but others do not.

51

Acids & Bases

Looking at acid/base properties, pH, the Arrhenius definition of acids and bases, and the Bronsted-Lowry concept. (Note: brief lab activity.)

52

Neutralization

Writing and balancing neutralization reactions.

53

Titration

Titration: the quantitative analysis of neutralization reactions. Note: teachers should spend time before the lab showing students how to set up and use equipment.

54

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Finishing yesterday's work. Students compete in a competition to see who is "best with a burette".

55

Review

Review of unit 3: solutions and solubility.

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Topic

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58

KMT

Introduction to gases, starting with a discussion of the Kinetic Molecular Theory. Students complete questions 1-10.

59

Pressure

Finishing yesterday's lesson, including demonstrations. The last demonstration is more dramatic with a balloon rabbit. This lesson is short to give time to return tests from Unit 3.

 

60

Boyle's Law

Students investigate the mathematical relationship between pressure and volume (i.e. Boyle's Law).

62

Charles's Law

Finishing the Boyles' Law questions from last class. The second half of today's lesson is spent on Charles's Law.

63

Combined Gas Law

Combining Boyle's Law and Charles's Law to get the "combined gas law".

64

Weighing Gases Lab

How do you weigh a gas? In today's lab, students find out.

65

Partial Pressures

Dalton's law of partial pressures: the total pressure of a mixture of gases is equal to the sum of the pressure of individual gases.

66

Molar Volume Lab

In today's lab, students determining the "molar volume" of hydrogen gas.

67

Ideal Gas Law

The ideal gas law (PV=nRT), like the other gas laws, is used to calculate one unknown variable when all other variables are known. (Note: brief lab activity.)

68

Gas Stoichiometry

Extending the stoichiometry calculations from Unit 2 to include gases.

69

Review

Review of unit 4: gases & atmospheric chemistry.

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Topic

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71

Foods Lab

Introduction to organic chemistry.

72

Hydrocarbon Models

Students build models and draw diagrams of hydrocarbons: alkanes, alkenes, alkynes, and aromatics.

73

Combustion

Students investigate the products of complete and incomplete combustion.

74

Hydrocarbon Naming

Organic nomenclature follows a different set of rules than inorganic nomenclature. Students learn these rules and try several examples.

75

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This period is spent entirely on practice problems. Students apply the rules they learned yesterday.

76

Chemsketch

Students learn to use ChemSketch - a program for drawing organic molecules. A computer lab with ChemSketch installed is needed.

77

Isomers & Polymers

Students build models of isomers (compounds with the same chemical formula but different structures) and polymers (long chains of carbon-containing monomers).

78

Alkanes and alkenes  Lab

Comparing the chemical properties of alkanes and alkenes to illustrate the reactivity of a double bond. This is a lab, but it may be better as a demonstration.

79

Thermochemistry

Concepts related to thermochemistry are introduced, including calorimetry, heat capacity, molar heat of reaction, etc.

80

Candle Lab

Students determine the molar heat of combustion for paraffin wax, applying the concepts learned in yesterday's lesson.

81

Bond Energies

Using bond energies to predict the energy change when atoms rearrange themselves in chemical reactions.

82

Review

Review of unit 5: hydrocarbons and energy.

 

 

 

 

85

Exam Review

Review of the course, mainly focusing on calculations.

86

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Continuation of yesterday's lesson.

 

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