C2 Chemistry Syllabus - Dr. Natalie Munn
The following is a listing of the topics that we will study over the course of the year. The time line is approximate, as each school year some topics may take more or less time, depending on how well your class is doing! These topics are matched to the Massachusetts Curriculum Frameworks, and they represent an excellent selection for an introductory chemistry class. This course will prepare any student for the college-level study of chemistry. Please realize that this listing is a work in progress, so changes may be made during the course of the year.
First Quarter
Chapters 1&2: Introduction to Chemistry (1.1-1.3, 2.3)
Identify five areas of study in chemistry
Distinguish between microscopic and macroscopic views
Describe Lavoisier’s contributions to chemistry
Identify the steps of the scientific method
Describe safety requirements in chemistry laboratories
Identify properties of matter as extensive or intensive
Define and give examples of physical properties and physical changes
Categorize mixtures as heterogeneous and homogeneous
Describe techniques used for separation of mixtures
Explain the difference between an element and a compound
Define and give examples of chemical changes
Apply the law of conservation of mass to chemical reactions
Chapter 3: Scientific Measurement (Skills Standards)
Convert measurements to scientific notation
Distinguish among accuracy, precision, and error of a measurement
Determine significant figures in a measurement and a calculated answer
Lists SI units of measurement and common SI prefixes
Distinguish between the mass and weight of an object
Convert between the Celsius and Kelvin temperature scales
Construct conversion factors from equivalent measurements
Apply the technique of dimensional analysis to a variety of conversion problems
Calculate density from experimental data
Interpret and represent relationships in graphic form
Independent Science Project Development (Skills Standards)
Make observations, raise questions, and formulate hypotheses
Design and conduct scientific investigations
Analyze and interpret results of scientific investigations
Communicate and apply the results of scientific investigations
Chapter 4: Atomic Structure (2.1-2.2)
Describe the ideas of Democritus, Dalton, and Rutherford concerning atoms
Identify the instruments needed to observe atoms
Identify three types of subatomic particles
Explain what makes elements and isotopes different from one another
Calculate the number of neutrons in an isotope and the atomic mass of an element
Second Quarter
Chapters 5&6: Electrons in Atoms and the Periodic Table (2.1, 2.4, 3.1-3.4)
Describe the Bohr and Quantum Mechanical Models of the atom
Describe the energies and positions of electrons according to quantum mechanics
Write electron configurations for atoms
Identify the source of atomic emission spectra
Distinguish between quantum mechanics and classical mechanics
Explain how elements are organized in a periodic table
Identify the three broad classes of elements
Describe the information found in a periodic table
Explain how ions form
Describe trends among the elements for atomic size, ionization energy, and electronegativity
Chapter 7: Ionic and Metallic Bonding (4.1-4.2, 4.6)
Determine the number of valence electrons for an element
Explain how the octet rule applies to atoms
Describe how anions and cations form
Name monatomic and polyatomic ions
Name and write formulas for ionic compounds
Describe properties of ionic compounds
Model valence electrons of metal atoms
Explain the importance of alloys
Chapter 8: Covalent Bonding (4.1-4.6)
Compare properties of molecular compounds and ionic compounds
Describe the information a molecular formula provides
Name and write formulas for molecular compounds
Describe how electrons are shared to form covalent bonds
Demonstrate how electron dot structures represent shared electrons
Describe how atoms form double, triple, and coordinate covalent bonds
Describe how the VSEPR Theory helps predict the shapes of molecules
Show how electronegativity differences result in polar and nonpolar bonds
Evaluate how molecular shape leads to polar and nonpolar molecules
Describe Van der Waals forces, hydrogen bonding, and network solid formation
Third Quarter
Chapter 10: Chemical Quantities (5.3, 5.4)
Describe methods of measuring the amount of something
Define Avogadro’s number as it relates to a mole of a substance
Describe how the mass of a mole of a substance is determined
Convert between moles and mass, particles, and gas volumes at STP
Calculate percent composition from a formula or from laboratory data
Determine empirical and molecular formulas from percent composition or laboratory data
Chapters 11&25: Chemical Reactions and Nuclear Reactions (2.5-2.7, 5.1-5.2)
Write balanced chemical equations
Describe and identify examples of the five general types of reactions
Describe the three main types of nuclear radiation
Describe the type of decay a radioactive isotope undergoes
Solve problems that involve half-life
Identify the two ways that transmutation can occur
Describe fission and fusion reactions
Identify devices used to detect radiation
Describe how radioisotopes are used in medicine
Chapter 12: Stoichiometry (5.5-5.6)
Identify the quantities conserved in all reactions
Construct mole ratios from balanced equations
Use equations to convert between mass, particles, and volumes of different substances
Identify limiting reagents
Calculate percent yield
Fourth Quarter
Chapters 13&14: States of Matter and the Behavior of Gases (6.1-6.3)
Describe the kinetic theory
Describe properties of gases, liquids, and solids
Use Boyle’s Law for calculations involving pressure and volume
Use Charles’s Law for calculations involving volume and temperature
Use Gay-Lussac’s Law for calculations involving pressure and temperature
Use the Combined Gas Law for calculations involving pressure, volume, and temperature
Use the Ideal Gas Law for calculations involving moles
Use Graham’s Law for calculations involving gas movements
Use Dalton’s Law for mixtures of gases
Chapters 15&16: Water and Solutions (4.5, 7.1-7.5)
Describe properties of water that result from its hydrogen bonding
Describe how solutions are formed
Demonstrate how the formula of a hydrate is written
Identify factors that determine the rate at which a solute dissolves
Identify factors that determine the amount of solute that will dissolve
Solve problems involving solution molarity
Solve problems involving solution molality
Identify colligative properties of solutions
Chapters 17&18: Thermochemistry, Reaction Rate, and Equilibrium (6.4-6.5, 7.6)
Explain how energy, heat, and work are related
Classify processes as exothermic or endothermic
Identify units used to measure heat transfer
Describe how calorimeters measure heat flow
Construct thermochemical equations
Describe how to express the rate of a chemical reaction
Identify factors that influence the rate of a chemical reaction
Describe a system at equilibrium and how stresses change equilibrium
Define entropy and describe its role in reactions
Chapters 19&20: Acids and Bases and Oxidation-Reduction Reactions (8.1-8.4)
Define the properties of acids and bases
Compare and contrast the Arrhenius and Bronsted-Lowry definitions of acids and bases
Calculate and evaluate pH and pOH of solutions
Describe neutralization reactions
Explain how a buffer works
State the characteristics of a Redox reaction and identify the oxidizing and reducing agents