Course title

Pre-requisite

Course description

Chemistry A Syllabus

Course Description
Chemistry A opens the atomic world. In particular; electrons and their uncertain but predictable behavior are examined in the submicroscopic arena. Using the atomic model; you will learn how chemical reactions can be predicted and designed to provide energy and structure for human needs. The subjects of atomic structure; periodic laws; chemical reactions; and stoichiometry are studied in detail; including the interdisciplinary subjects of fluid dynamics and solutions. To do well in Chemistry A; you should have fluency in algebra and geometry and a background in physical science.

Course Objectives
• Understand the evidences and applications of atomic theory.
• Predict and quantify the products and reactants of chemical reactions
• Understand the basis and use of the Periodic Table
• Understand the special nature of reactions within solutions
Topics to be Covered
Unit 1: The Nature of Matter
Unit Description
Chemistry is often referred to as the mother science since it has application in almost all other disciplines. To understand biology; physics; environmental science; medicine; anatomy; and physiology you must realize that all depend on chemistry. Knowledge of chemistry also assists in understanding and predicting many of the day-to-day events of life such as cooking; cleaning; and gardening. In the first unit; the focus is on understanding the nature of matter. Matter; as opposed to energy; has mass and volume. Such a definition seems so easy that it borders on trivial; yet investigation has shown that what seems easy and trivial has a profound significance in how matter reacts.
Unit Objectives
• Understand the evidences and applications of atomic theory
• Understand the place of chemistry among the sciences
• Understand the use and limitations of measurement
• Understand and apply safety procedures
Lesson 1: What is Matter?
Lesson Description
A basic description of the classifications of matter and the states of matter
Lesson Objectives
• Describe substances based on their physical and chemical properties.
Lesson 2: A Periodic Review
Lesson Description
A perusal of the Periodic Table; including groups and rows.
Lesson Objectives
• Predict properties of elements and compounds using trends of the periodic table.
Lesson 3: What’s in a Number?
Lesson Description
A discussion of significant figures; accuracy and precision; and scientific notation.
Lesson Objectives
• Choose an appropriate method for communicating the results of a specific investigation.
Lesson 4: The History of the Atom
Lesson Description
A review of the evidence that led to Dalton’s atomic theory.
Lesson Objectives
• Describe the historical development of the atom.
Lesson 5: Electron Clouds
Lesson Description
The story of atomic theory from Thomson to Rutherford; the mole concept as atomic mass in grams.
Lesson Objectives
• Describe the features and components of the atom.
• Describe the historical development of the atom.
• Explain the details of atomic structure.
• Describe the mole concept and its relationship to Avogadro’s number.
Unit 2: The Interaction of Atoms
Unit Description
Why the fuss over how an atom is built? The answer is simply that the structure of an atom—particularly the outer shell of the atom—determines how it reacts. The type of bond the atom makes determines the properties of the resulting compound. Therefore; in order to understand chemical reactions; familiarity with atomic structure is a necessity. In this unit; you will study the details of how electrons surround the nucleus as well as how elements arrange themselves into groups and families according to the structure of the electrons in their outer shell. Once you know how the electrons are arranged; you are ready to look into how the outer electrons bond with other atoms. The whole picture is incredible! You can imagine this chemical world as a place where electrons are busily searching for a stable home.
Unit Objectives
• Describe the development of the quantum mechanical model of the atom.
• Describe the configuration of electrons around the nucleus of the atom.
• Relate the electron configuration of an element to its position on the Periodic Table.
• Relate the properties of an element to its position on the Periodic Table.
Lesson 6: Quantum Theory
Lesson Description
How the photoelectric effect led to the Bohr model of the atom; contributions of Heisenberg and de Broglie.
Lesson Objectives
• Explain the details of atomic structure.
Lesson 7: Electron Shapes
Lesson Description
Electron configuration and quantum numbers lead to a mathematical model of the atom.
Lesson Objectives
• Explain the details of atomic structure.
Lesson 8: Categorizing Atoms
Lesson Description
A short tour through the Periodic Table; with explanations of groups and series.
Lesson Objectives
• Predict properties of elements and compounds using trends of the Periodic Table.
Lesson 9: Periodic Properties
Lesson Description
Introduction to periodic properties; such as atomic radii; electron affinity; ionization; and cations vs. anions.
Lesson Objectives
• Predict properties of elements and compounds using trends of the Periodic Table.
Lesson 10: Atomic Bonds
Lesson Description
Introduction to chemical bonds and the atomic theory rationale that explains and describes bonding.
Lesson Objectives
• Distinguish among the types of chemical bonds.
Unit 3: Reactions and Equations
Unit Description
Since the invention of reading and writing; human knowledge has exploded. Chemistry; as any other discipline; uses symbols to represent what can be seen and predicted in chemical reactions. Once the notation for naming and representing atoms and compounds is learned; the patterns of reactions can be more easily communicated. For example; you may know the symbol for water as H2O. What that represents is that water has two parts hydrogen for every one part oxygen. Knowing that; you can predict that; should you separate water into its elements; you will get twice as much hydrogen as you do oxygen. Not surprisingly; that is what happens. That is what makes chemistry so useful. The atomic model; combined with proper equations; makes chemical reactions predictable and useful.
Unit Objectives
• Describe the three main types of chemical bonds.
• Predict the geometries of compounds using their chemical bond types.
• Correctly name compounds based on the Stock system.
• Quantify chemical reactions based upon a balanced chemical equation.
Lesson 11: Metallic and Ionic Bonds
Lesson Description
A look at ionic solids; including lattice energy; electron sea; and resulting physical properties.
Lesson Objectives
• Predict the properties of substances based upon bond type.
Lesson 12: Chemical Geometry
Lesson Description
The VSEPR theory; dipole interactions; hybrid orbitals; hydrogen bonding; and London dispersion forces.
Lesson Objectives
• Predict the properties of substances based upon bond type.
Lesson 13: What’s in a Name?
Lesson Description
An explanation of the Stock system of nomenclature; including polyatomic ions. Oxidation numbers introduced.
Lesson Objectives
• Communicate chemical results clearly and logically.
• Determine the transfer of electrons in redox reactions.
Lesson 14: The Mole Concept
Lesson Description
Further explanations of moles and how they are used in deriving empirical formulas and percentage compositions.
Lesson Objectives
• Solve problems using the mole concept.
Lesson 15: Representing Reactions
Lesson Description
How to write and balance chemical equations; the different types of chemical reactions
Lesson Objectives
• Represent a chemical reaction by using a balanced equation.
• Predict the products of a chemical reaction by using types of reactions.
Unit 4: Quantitative Chemistry
Unit Description
There are at least two aspects of chemical reactions: changes in matter and changes in energy. Both aspects can be predicted using the mole concept. Moles are simply a certain number of molecules; a very large number of molecules. However; one mole always equals the same large number; whether it be a small molecule like water; or a larger molecule like sugar. Obviously; the larger molecule will have more mass and weigh more; but one mole of water has just as many molecules as one mole of any other material. Using a mole makes it possible to predict precisely the amount of reactants and products; and the energy produced or consumed; in a chemical reaction. The mole; in chemistry; is not a burrowing animal; but a key to understanding and predicting chemical reactions.
Unit Objectives
• Solve stoichiometric problems; including limiting reactants and percentages
• Interconvert mass and amount units
• Predict the behavior of gases using the gas laws.
• Describe the characteristics of fluids
Lesson 16: Stoichiometry
Lesson Description
A how-to of quantitative chemistry; including practice problems; the activity series
Lesson Objectives
• Predict the products of a chemical reaction using types of reaction and activity series.
• Quantify the relationships between reactants and products in chemical reactions.
Lesson 17: Conversions
Lesson Description
Further types of stoichiometric procedures; including mass to mass.
Lesson Objectives
• Quantify the relationships between reactants and products in chemical reactions.
Lesson 18: Limits and Percentages
Lesson Description
Extending stoichiometry to include limiting reactants and percent yield.
Lesson Objectives
• Quantify the relationships between reactants and products in chemical reactions.
Lesson 19: Working with Gases
Lesson Description
Kinetic molecular theory and effusion vs diffusion
Lesson Objectives
• Describe the basic assumptions of kinetic molecular theory.
• Apply kinetic molecular theory to the behavior of matter.
Lesson 20: Liquids and Solids
Lesson Description
Liquid and solid properties; including surface tension; capillary action; crystalline and amorphous types
Lesson Objectives
• Apply kinetic molecular theory to the behavior of matter.
Unit 5: Gases and Solutions
Unit Description
Matter comes in four styles: solids; liquids; gases; and plasmas. Plasmas are the most common form of matter in the universe; but are rare on Earth. Here we normally deal with the remaining three forms; and the transitions between them. The energy content of matter is relatively low in solids; higher in liquids; and relatively high in gases. Because of the kinetic molecular theory; we understand that the particular properties of gases; such as pressure and volume; are the result of the particles of the gas being in high motion. Though the energy of a gas makes the motion chaotic; the result is highly predictable. As temperature rises; for example; pressure or volume also rises. In this unit; you will come to know some of the heroes of gas: Boyle; Charles; Gay-Lussac; and Avogadro.
Unit Objectives
• Describe the structures and properties of matter
• Understand and apply the law of conservation of energy
• Understand and apply the second law of thermodynamics
• Describe the interactions of energy and matter
Lesson 21: Changing States
Lesson Description
Changes of state; including equilibrium states; water properties
Lesson Objectives
• Analyze calorimetric measurements in simple systems and the energy involved in changes of state.
• Explain how molecular motion is related to temperature and phase changes.
Lesson 22: Pressure
Lesson Description
Definition of pressure; Dalton’s law of partial pressures
Lesson Objectives
• Describe various ways that matter and energy interact; such as in gas expansion.
Lesson 23: The Gas Laws
Lesson Description
Boyle’s; Charles’; Gay-Lussac’s; and combined gas laws; Kelvin temperature
Lesson Objectives
• Apply kinetic molecular theory to the behavior of matter; such as the gas laws.
Lesson 24: Moles and Gases
Lesson Description
Relationships of amount; pressure; temperature; and volume; ideal gas law; Graham’s law of effusion

Lesson Objectives
• Solve problems involving moles; mass; and volume of a gas using the mole concept.
• Apply kinetic molecular theory to the behavior of matter; such as the gas laws.
Lesson 25: Solutions
Lesson Description
Solutes; solvents; and solutions; suspensions; colloids; emulsions; rate of dissolution; Henry’s law
Lesson Objectives
• Separate mixtures of solutions based on their physical properties.
Unit 6: Solutions and Concentrations
Unit Description
Liquids can flow and blend; forming all sorts of interesting mixtures. One of the most interesting is the solution; where the particles of at least two substances mix on the atomic level. On Earth; the most common solvent is water; and a multitude of substances dissolve in water. Because the atoms in a solution are already on their own; solutions make great places for chemical reactions. Of course; the chemist always wants to know how many particles of each substance are in a solution; so concentration measures have arisen. Two are commonly used in chemistry: molarity and molality. Both measure the number of moles of a solute dissolved in a solution; and both then can be used to predict the products and amounts of products in a reaction within the solution.
Unit Objectives
• Describe the structures and properties of solutions; including colligative properties
• Distinguish between qualitative and quantitative tests
Lesson 26: Molarity and Molality
Lesson Description
Measures of concentration; computing molarity
Lesson Objectives
• Solve problems involving such quantities as moles; mass; and molarity using the mole concept.
Lesson 27: Reactions in Solution
Lesson Description
Aqueous solutions; precipitation reactions; electrolytes
Lesson Objectives
• Describe substances based upon their chemical properties.
• Predict the products of an ionic double replacement reaction.
Lesson 28: Colligative Properties
Lesson Description
Volatility; boiling and freezing point depression; osmosis
Lesson Objectives
• Describe substances based upon their physical properties.
Lesson 29: Chemical Tests
Lesson Description
Recap of the scientific method; qualitative vs. quantitative; modeling
Lesson Objectives
• Design an appropriate protocol for testing a hypothesis.
Lesson 30: Finally!
Lesson Description
Final Exam and case study discussion
Lesson Objectives
• Demonstrate mastery over the concepts of introductory chemistry
Assessment of Concepts and Skills/Evaluation of Student Progress
Pretests
Pretests assess a student’s prior knowledge of the content in a unit. These questions are taken directly from the unit exam but do not count toward a student’s grade.
Workbook Questions
Workbook questions are presented to students after most activities containing content. They assess a student’s knowledge of the content immediately after they view/learn the content. Workbook questions typically include multiple choice; true/false; and/or fill-in-the-blank questions.
Checkpoints
Checkpoints assess a student’s knowledge of the concepts taught in a lesson. Typically; multiple choice and true/false questions are presented.
Exams (including Vocabulary Exam)
Exams assess a student’s knowledge of the concepts taught in a unit. Typically; multiple choice and true/false questions are presented.
The Vocabulary Exam assesses a student’s knowledge of several key terms taught throughout the entire course. Typically; multiple choice and true/false questions are presented.
Final Exam
The Final Exam assesses a student’ knowledge of all of the content taught throughout the entire course. Typically; multiple choice and true/false questions are presented.
Discussion Boards
Discussions assess a student’s knowledge of the content taught in each lesson of a unit through answering questions and discussing the content with fellow students.
Unit 1
“Mass Spectrometer” discusses how physical and chemical properties can be intertwined and used for analysis.
Unit 2
“Electrons” discusses how electron behavior affects many physical and chemical processes.
Unit 3
“Covalent Carbon Bonding” discusses the special features of carbon bonding; focusing on the chemistry of sight.
Unit 4
“The Atmosphere” discusses the cycles of matter through the atmosphere and the protective nature of gases.
Unit 5
“Nitrogen-Fixing” discusses the nitrogen cycle and its relationship to the Haber process of ammonification and nitroglycerin synthesis and decomposition.
Unit 6
“Water” discusses the peculiar properties of water and its importance to Earth life.
Unit Labs
Unit 1: 1) Periodic Table Activity; 2) Measuring the Size of a Molecule of Oil

Unit 2: 1) Orientation of p Orbitals; 2)Periodic Table Activity 2

Unit 3: 1)Geometry of Bonds; 2)Mole Conversions

Unit 4: 1)Mole Ratios in Chemical Reaction(2period lab)

Unit 5: 1) Molar Volume of a Gas (2 period lab)

Unit 6: 1) Chromatography; 2)Freezing Point Depression

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• LCHM
• Chemistry

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Online / Virtual