Honors 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. Additionally, we will cover the content included on the Chemistry SAT Subject Test. 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 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
Apply the technique of dimensional analysis to a variety of conversion problems
Calculate density from experimental data
Chapters 4, 5, & 6: Atomic Structure and the Periodic Table (2.1-2.2, 2.4, 3.1-3.4)
Describe the development of the models of the atom
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
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
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
Second Quarter
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
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
Third Quarter
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
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
Calculate the new boiling and freezing points of solutions
Fourth Quarter
Chapter 17: Thermochemistry (6.4)
Explain how energy, heat, and work are related
Classify processes as endothermic or exothermic
Identify the units used to measure heat transfer
Distinguish between heat capacity and specific heat
Describe how calorimeters are used to measure heat flow
Solve for enthalpy changes in chemical reactions by using heats of reactions
Classify the enthalpy change that occurs when a substance changes phase or dissolves
Solve for enthalpy changes by using Hess’s Law or standard heats of formation
Chapter 18: Reaction Rates and Equilibrium (6.5, 7.6)
Describe how to express the rate of a chemical reaction
Identify factors that influence the rate of reaction
Describe chemical equilibrium and identify how stresses can change equilibrium
Calculate and evaluate Keq
Describe solubility equilibrium and calculate Ksp
Identify characteristics of spontaneous reactions
Describe the role of entropy in chemical reactions
Define Gibbs free energy and use it to evaluate reactions
Use energy graphs to monitor reaction progress
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
Describe how hydrogen and hydroxide ion concentration are related in aqueous solutions
Classify a solution as neutral, acidic, or basic
Calculate and evaluate pH and pOH of solutions
Calculate and evaluate Ka and Kb
Describe the purpose of an acid-base indicator
Describe neutralization reactions
Explain how titration works to calculate the concentration of an acid or base
Explain how a buffer works
State the characteristics of a Redox reaction and identify the oxidizing and reducing agents
Determine the oxidation number of an atom
Define oxidation and reduction in terms of a change in oxidation number