compounds into their components Define chemical and physical properties and compare them by providing examples Describe and perform common separation techniques (e.g., filtration, distillation, chromatography) Days Unit/Topic Standards Activities Learning Targets (“I Can” Statements) Vocabulary Days 21-35 Atomic structure, electron configuration, and periodic law IV.B.1a-f: atomic theory, atomic structure, and quantum theory IV.B.2a-g: Periodic table and periodicity ACT Bellringers (daily) Exit slip (daily) Hands-on Labs (2 labs) Lab Reports (2) Demonstrations (2) quantitative word problems that model the AP chemistry test (about twice/week) Quiz: AP Chemistry test style open response questions (weekly) Homework: AP chemistry test style word problems (twice/week) I can do the following: Describe the importance of models for the study of atomic structure Describe the crucial contributions of scientists and the critical experiments that led to the development of the modern atomic model Describe characteristics of a wave, such as wavelength, frequency, energy, and speed Describe the role of probability in orbital theory Atom cathode ray electron nucleus proton neutron atomic number isotopes mass number atomic mass unit atomic mass radiation radiation beta radiation gamma ray electromagnetic radiation wavelength frequency amplitude quantum photoelectric effect photon
Reading and analysis of “real life” chemical research situation (weekly) Common assessment (end of unit) Describe atomic orbitals (s, p, d, f) and basic shapes Apply Hund’s rule and the Aufbau process to specify the electron configurations of the elements Describe the historical development of the modern periodic table, including work by Mendeleev and then Moseley Describe and explain the organization of elements into periods and groups in the periodic table Use the periodic table to determine the atomic number; atomic mass; mass number; and number of protons, electrons, and neutrons in isotopes of elements Calculate the weighted average atomic mass of an element from isotopic abundance, given the atomic mass of each contributor Identify regions (e.g., groups, families, series) of the periodic table and atomic emission spectrum ground state quantum number atomic orbital valence electrons electron-dot structure representative elements transition elements alkali metals alkaline earth metals halogens noble gases metalloids ion ionization energy octet rule electronegativity
describe the chemical characteristics of each Compare the periodic properties of the elements (e.g., metal/nonmetal/metalloid behavior, electrical/heat conductivity, electronegativity and electron affinity, ionization energy, atomic/covalent/ionic radius) and how they relate to position in the periodic table Use the periodic table to predict and explain the valence electron configurations of the elements, to identify members of configuration families, and to predict the common valences of the elements Days Unit/Topic Common Core Standards Activities Learning Targets (“I Can” Statements) Vocabulary Days 36-55 Ionic compounds, covalent bonding, and chemical reactions III.A.3a-m: Chemical equations and stoichiometry IV.B.3a-k: Intermolecular forces and types of bonds IV.B.4a-f: Orbital theory applied to bonding V.A.1e-h: Types of solutions, concentrations, and solubility ACT Bellringers Exit slip (daily) Hands-on Labs (2 labs) Lab Reports (2) Demonstrations (2) In-class quantitative word problems that I can do the following: Explain how conservation laws form the basis for balancing chemical reactions and know what quantities are conserved in physical, chemical, and nuclear changes Write and balance chemical equations, given Chemical bond Cation Anion ionic bond compound crystal lattice electrolyte lattice energy formula unit monatomic ion oxidation number polyatomic ion
Define and calculate the percent composition of a solution Describe the preparation and properties of solutions Solve stoichiometry calculations based on reactions involving aqueous solutions Days Unit/Topic Common Core Standards Activities Learning Targets (“I Can” Statements) Vocabulary Days 56-85 Mole and stoichiometry III.A.1e-g: empirical formula, molecular formula, and percent composition III.A.2a-c:Mole concept, mass, gram formula mass, and molecular mass III.A.3i-l: chemical equations and stoichiometry ACT Bellringers (daily) Exit slip (daily) Hands-on Labs (2 labs) Lab Reports (2) Demonstrations (2) In-class quantitative word problems that model the AP chemistry test (about twice/week) Quiz: AP Chemistry test style open response questions (weekly) Homework: AP chemistry test style word problems (twice/week) Reading and analysis of “real life” chemical research situation (weekly) I can do the following: Calculate the percent composition of a substance, given its formula or masses of each component element in a sample Determine the empirical formulas and molecular formulas of compounds, given percent composition data or mass composition data Determine percent composition experimentally and derive empirical formulas from the data (e.g., for hydrates) Explain the meaning of and Avogadro’s number Mole Avogadro’s number mass Percent composition Empirical formula Molecular formula Hydrate Stoichiometry Mole ratio Limiting reactant Excess reactant Theoretical yield Actual yield Percent yield
and Dalton and solve problems based on these laws Predict boiling point changes based on changes in atmospheric pressure Explain the basis for gaseous diffusion and effusion Describe Avogadro’s hypothesis and use it to solve stoichiometric problems Explain the difference between an and real gas, the assumptions made about an ideal gas, and what conditions favor ideal behavior for a real gas Apply the mathematical relationships that exist among the volume, temperature, pressure, and number of particles in an ideal gas Compute gas density when given molar mass, temperature, and pressure Apply the ideal gas law to determine the molar mass of a volatile compound Immiscible Concentration Molarity Molality Mole fraction Solvation Heat of solution Unsaturated solution Saturated solution Supersaturated solution Henry’s law Colligative properties Vapor pressure lowering Boiling point elevation Freezing depression Osmosis Osmotic pressure
solute in a given solvent and its rate of solution Describe qualitatively the effect of adding solute on freezing point, boiling point, and vapor pressure of a solvent Define molality and fraction Calculate changes in the boiling and freezing point when nonvolatile, nonelectrolyte solutes are added to solvents Days Unit/Topic Standards Activities Learning Targets (“I Can” Statements) Vocabulary Days 106-135 Energy, reaction rates, and chemical equilibrium V.B.3a-e: Chemical processes and heat; calorimetry V.B.4a-d: Enthalpy and Entropy V.B.1a-i: Chemical equilibrium and factors affecting reaction rates: Le Chatelier’s principle V.B.2a-f: Mechanisms, rate-determining step, activation energy, and catalysts ACT Bellringers (daily) Exit slip Hands-on Labs (2 labs) Lab Reports (2) Demonstrations (2) In-class quantitative word problems that model the AP chemistry test (about twice/week) Quiz: AP Chemistry test style open response questions (weekly) I can do the following: Explain the law of conservation of energy in chemical reactions Describe the concept of heat, and explain the difference between heat energy and temperature Explain physical and chemical changes as endothermic or exothermic energy changes Solve heat capacity and heat transfer problems involving specific heat, Energy Law of conservation of energy Chemical potential energy Heat Calorie Joule Specific heat Calorimeter Thermochemistry System Surroundings Enthalpy Hess’s law Standard enthalpy of formation Spontaneous process
Homework: AP chemistry test style word problems (twice/week) Reading and analysis of “real life” chemical research situation (weekly) Common assessment (end of unit) heat of fusion, and heat of vaporization Calculate the heat of reaction for a given chemical reaction when given calorimetric data Define enthalpy and explain how changes in enthalpy determine whether a reaction is endothermic or exothermic Compute ΔHrxn from ΔHfº values and explain why the ΔHfº values for elements are zero Explain and apply, mathematically, the relationship between ΔHrxnº (forward) and ΔHrxnº (reverse) Define entropy and explain the role of entropy in chemical and physical changes, and explain the changes that favor increases in entropy Explain the collision theory of reactions Analyze factors (e.g., temperature, nature of reactants) affecting reaction in relation to the kinetic theory Entropy Second law of thermodynamics Free energy Reaction rate Collision theory Activated complex Activation energy Catalyst Inhibitor Heterogeneous catalyst Homogeneous catalyst Rate law Specific rate constant Reaction order Method of initial rates Instantaneous rate Complex reaction Reaction mechanism Intermediate Rate-determining step Reversible reaction Chemical equilibrium Law of chemical equilibrium Equilibrium constant Homogeneous equilibrium Heterogeneous equilibrium Le Chatelier’s principle Solubility product constant Common ion Common ion effect
Relate the rate of a chemical reaction to the appearance of products and the disappearance of reactants Describe the meaning of reaction mechanism and rate-determining step Relate collision theory to the factors that affect the rate of reaction Describe the meaning of activation energy and activated complex Interpret and label a plot of energy versus reaction coordinate Explain the effects of catalysts on reaction rates (e.g., mechanism, activation energy/activated complex) Days Unit/Topic Common Core Standards Activities Learning Targets (“I Can” Statements) Vocabulary Days 136-165 Acids, Bases, Redox reactions V.C.1a-f: Acid/base theories V.C.2a-f: Acid/base constants and pH; titration; buffers V.Da-c: reactions and electrochemistry ACT Bellringers (daily) Exit slip (daily) Hands-on Labs (2 labs) Lab Reports (2) Demonstrations (2) I can do the following: Describe the nature and interactions of acids and bases Describe the hydronium ion and the concept of amphoterism Acidic solution Basic solution Arrhenius model Bronsted-Lowry model Conjugate acid Conjugate base Conjugate acid-base pair Amphoteric
In-class quantitative word problems that model the AP chemistry test (about twice/week) Quiz: AP Chemistry test open response questions (weekly) Homework: AP chemistry test style word problems (twice/week) Reading and analysis of “real life” chemical research situation (weekly) Common assessment (end of unit) Describe Arrhenius and acids and bases; identify conjugate acids and bases in reactions Relate solvent interaction to the formation of acidic and basic solutions Define the water constant, Kw, and the pH scale Describe characteristics of strong and weak and bases, and identify common examples of both Write and balance a simple equation for a neutralization reaction Calculate hydrogen ion concentration, hydroxide ion concentration, pH, and pOH for acidic or solutions Explain how the acid-base indicators work Define percent ionization, Ka, and Kb and explain how they relate to acid/base strength Conduct a titration experiment in order to determine the model Strong acid Weak acid Acid ionization constant Strong base Weak base Base ionization constant Ion product constant for water pH pOH neutralization reaction salt titration titrant equivalence acid-base indicators end point salt hydrolysis buffer buffer capacity redox reaction oxidation reduction oxidizing agent reducing agent Oxidation-number method Species Half-reaction
In-class quantitative word problems that model the AP chemistry test (about twice/week) Quiz: AP Chemistry test style open response questions (weekly) Homework: AP chemistry test style word problems (twice/week) Reading and analysis of “real life” chemical research situation (weekly) Common assessment (end of unit) Describe alpha, beta, and gamma decay, half-life, and fission and fusion Write appropriate equations for nuclear decay reactions, using particle balance; describe how the nucleus changes during these reactions and compare the resulting radiation with regard to penetrating ability Primary battery Secondary battery Fuel cell Corrosion Galvanization Electrolysis Electrolytic cell Radioisotope X rays Penetrating power Transmutation Nucleons Strong nuclear force Band of stability Positron emission Positron Electron capture Radioactive decay series Half-life Radiochemical dating Induced transmutation Transuranium elements Mass defect Nuclear fission Critical mass Breeder reactors Nuclear fusion Thermonuclear reactions Ionizing radiation Radiotracer