U1: Perform accurate and precise basic chemistry calculations/conversions and classify matter according to chemical and physical properties.
1.1: Classify matter as elements, molecules, compounds, homogeneous, or heterogeneous mixture as well as phase; solid, liquid, and gas.
Reading: 1.1 and 1.2 Practice: 1.9, 1.10, 1.15, 1.58
1.2: Differentiate between physical and chemical properties and changes. Reading: 1.3 Practice: 1.17, 1.19
1.3: Perform calculations involving scientific notation and significant figures and make determinations on the resulting calculations precision and accuracy.
Reading: 1.4, 1.5 Practice: 1.4, 1.5, 1.35, 1.37, 1.38, 1.39, 1.41, 1.42, 1.61
1.4: Convert measurements between several common scientific units or unit prefixes using a multi-step dimensional analysis process.
Reading: 1.6 Practice: 1.25, 1.26, 1.27, 1.45, 1.47
U2: Use atomic theory and molecular structure to explain the property patterns of the periodic table.
2.1: Recall the crucial historic experiments and scientists who provided evidence supporting the existence of atoms and subatomic particles.
Reading: 2.1, 2.2 Practice: 2.1, 2.7, 2.8, 2.11, 2.13, 2.73, 2.74
2.2: Describe the number of, charge, location, and relative size of the particles that make up an element using a periodic table or complete chemical symbol.
Reading: 2.3 Practice: 2.17, 2.18, 2.20, 2.21, 2.23, 2.47, 2.48 2.3: Calculate a weighted atomic average mass for a given element.
Reading: 2.4 Practice: 2.19, 2.27, 2.28, 2.29, 2.30
2.4: Identify the groups/ regions of the P.T. with common characteristics, and predict properties of elements based on atomic #, atomic mass, isotopes, period, and family.
Reading: 2.5 Practice: 2.2, 2.35, 2.36, 2.37, 2.38, 2.49
2.5: Determine the name or formula for ionic compounds, covalent molecules, acids, and simple carbon containing organic molecules.
Reading: 2.6, 2.7, 2.8, 2.9 (Have Table 5-4 “common polyatomic ions” from
supplementary materials for summer assignment mostly memorized), “figure 6.21” sheet, “acids” sheet
Practice: 2.51, 2.53, 2.54, 2.55, 2.57, 2.59, 2.61, 2.62, 2.63, 2.65, 2.67
U3: Determine the formula/structure of product(s) of a chemical reaction, balance the reactions, and calculate precise proportions of products or reactants.
3.1: Balance chemical equations to uphold the Law of Conservation of Mass. Reading: 3.1 Practice: 3.1, 3.9, 3.11, 3.12, 3.13,
3.2: Predict the products of the four basic reaction types as well as neutralization and combustion reactions.
Reading: 3.2 (combination/decomposition and combustion), page 128 (metathesis), page 134 (neutralization), page 140 (displacement)
Practice: 3.15, 3.17, 3.19
3.3: Calculate empirical or molecular formulas and draw the structural formula for molecules given experimental percent mass composition data.
Reading: 2.6, 3.3, 3.5 Practice: 2.41, 2.39, 2.43, 2.45, 2.46, 3.5, 3.43, 3.45, 3.47, 3.49,
experiment using percent yield.
Reading: 3.4, 3.6 Practice: 3.21, 3.23, 3.25, 3.27, 3.31, 3.33, 3.34, 3.35 3.38, 3.39, 3.42, 3.57, 3.59, 3.61, 3.63, Reading: 3.7, Practice: 3.67, 3.71, 3.73, 3.75,
Reading: 3.7 Practice: 3.77, 3.79, 3.80
U4: Perform basic aqueous solution calculations and identify acids, bases, electrolytes, spectator ions, and species undergoing oxidation/reduction. 4.1: Identify a substance as non-, strong, or weak, electrolyte, acid, or base.*
Reading: 4.1, 4.3 Practice: 4.3, 4.5, 4.8, 4.14, 4.29, 4.30, 4.31, 4.32, 4.35, 4.37 4.2: Determine the balanced net-ionic equation for an aqueous reaction.
Reading: 4.2 Practice: 4.7, 4.9, 4.10, 4.15, 4.19, 4.23, 4.24, 4.27, 4.39, 4.40, 4.41 4.3: Use the oxidation number for elements in a reaction to determine which
elements/molecules are being oxidized and which reduced.**
Reading: 4.4 Practice: 4.45, 4.46, 4.49, 4.50, 4.51, 4.52
4.4: Perform dilution calculations and convert between mass, moles, volume, and number of particles using Molarity.
Reading: 4.5, 4.6 Practice: 4.59, 4.60, 4.61, 4.63, 6.65, 4.67, 4.69, 4.81, 4.85, 4.71, 4.72, 4.73, 4.75
*For solubility rules you just need to know Na, K, NH4, and NO3 salts are soluble.
*Just need to know general relative reactivity’s of elements and will not have reactivity series on AP test or be expected to have it memorized.
U5: Use the laws of thermodynamics to explain and calculate basic energy exchange quantities between systems and surroundings for physical and chemical changes. 5.1: Use the first law of thermodynamics to explain and calculate system energy exchanges for physical heat change processes (calorimetry, phase change, and expanding gases.)
Reading: 5.1, 5.2, 5.3, 5.5 Practice: 5.9, 5.13, 5.17, 5.19, 5.20, 5.25, 5.27, 5.47, 5.49, 5.51, 5.53, 5.55
5.2: Use the first law of thermodynamics and reaction enthalpies ( H) to explain and Δ calculate system energy changes for chemical heat change processes.
Reading: 5.3, 5.4, 5.8 Practice: 5.31, 5.33, 5.35, 5.37, 5.38, 5.39 5.3: Apply Hess’s Law to calculate unknown enthalpies in a series of reactions.
Reading: 5.6 Practice: 5.60, 5.61, 5.63, 5.75
5.4: Calculate how the enthalpy changes ( H) for a given reaction based on the Heats of Δ formations of the reactants and products.
Reading: 5.7 Practice: 5.65, 5.67, 5.69, 5.71, 5.73
U6: Use quantum mechanical fundamental principles and discoveries to explain and diagram the electron structure of an atom.
6.1: Calculate the energy, wavelength, speed, and/or frequency of electromagnetic photons. Reading: 6.1, 6.2 Practice: 6.11, 6.15, 6.21, 6.25, 6.99
6.2: Calculate and interpret line spectra for identification of elements. Reading: 6.3, Practice: 6.33, 6.37, 6.86
6.3: Compare the electron arrangements of historic electron models and the modern quantum mechanical electron cloud models
Reading: 6.4, 6.5, 6.6 Practice: 6.41, 6.45, 6.47
element using quantum mechanical rules (Hund’s and Pauli.)
Reading: 6.6, 6.7, 6.8, 6.9 Practice: 6.55, 6.56, 6.63, 6.65, 6.66, 6.67, 6.71
U7: Describe the historic and current organization of the Periodic Table and use patterns to predict properties of elements.
7.1: Explain how the trends in the Periodic Table are influenced by effective nuclear charge. Including: shielding, atomic radii, ionization energy, and electron affinity.
Reading: 7.2, 7.3, 7.4, 7.5 Practice: 7.9, 7.11, 7.13, 7.21, 7.23, 7.26, 7.27, 7.37, 7.38, 7.41, 7.49, 7.51
7.3: Identify the groups/ regions of the P.T. with common characteristics, and can predict properties of elements.
Reading: 7.6, 7.7, 7.8 Practice: 7.55, 7.59, 7.62, 7.67, 7.71, 7.85, 7.91, 7.96
U8: Describe how and why atoms form bonds.
8.1: Compare the chemical and physical properties of ionic and covalent compounds. Reading: 8.2, 8.3, 8.8 Practice: 8.13, 8.14, 8.17, 8.19, 8.29, 8.30
8.31, 8.33, 8.43
8.2: Use Lewis Dot Diagram models and formal charges to explain the role of valence electrons in bond formation including resonance forms.
Reading: 8.1, 8.2, 8.3, 8.5, 8.6 Practice: 8.11, 8.45, 8.47, 8.49, 8.59, 8.61 8.3: Describe the relationship between electronegativity and bond type of a molecule or compound.
Reading: 8.4, Practice: 8.35, 8.37, 8.39, 8.40, 8.86 8.4: Relate bond energies to bond strength and use bond energies to estimate H.Δ
Reading: 8.8 Practice: 8.65, 8.67
U9: Use molecular bonding theories to explain the 3-D structures, polarities, hybridization, and resonance of molecules.
9.1: Use VSEPR theory and Lewis Dot Diagram models to explain molecular geometry. Reading: 9.1, 9.2 Practice: 9.13, 9.15, 9.17, 9.19, 9.21, 9.22, 9.25 9.2: Predict the polarity of a molecule based on molecular geometry and electronegativity.
Reading: 9.3 Practice: 9.31, 9.35, 9.36
9.3: Explain the concept of SP1, SP2, and SP3 hybridization and its relationship to molecular
geometry.
Reading: 9.5 Practice: 9.7, 9.41, 9.43, 9.47
9.4: Describe various bonds in terms of sigma, pi, and delocalized resonance bonds Reading: 9.4, 9.6 Practice: 9.49, 9,51, 9.53, 9.55, 9.57
9.5: Predict bonding in pairs of atoms based on the relationship between bonding and antibonding molecular orbitals.
Reading: 9.7, 9.8 Practice: 9.9, 9.10, 9.59, 9.65, 9.67, 9.69
U10: Describe the properties of ideal and real gases and calculate their parameters. 10.1: Use the gas laws to describe and calculate how a gas responds to changes in pressure, volume, temperature, or quantity of gas present.
Reading: 10.1, 10.2, 10.3, 10.7 Practice: 10.12, 10.13, 10.17, 10.23, 10.24, 10.25, 10.26, 10.89
10.2: Use the ideal and real gas equation to calculate the pressure, volume, temperature, or quantity of both ideal and real gases in chemical reactions.
10.41, 10.43, 10.47, 10.53, 10.54, 10.81, 10.83, 10.85 10.3: Calculate partial pressures and mole fractions for mixtures of gasses.
Reading: 10.6 Practice: 10.57, 10.59, 10.61, 10.63, 10.65, 10.66, 10.55, 10.56 10.4: Describe the relationship between the relative rates of effusion/diffusion of gases, their molar masses, and their mean free path.
Reading: 10.8 Practice: 10.69, 10.71, 10.73, 10.75, 10.76, 10.77, 10.79, 10.80
U11: Use Kinetic Molecular Theory to describe how the intermolecular and interatomic forces between molecules affect the physical properties, chemical properties, phase, and phase change parameters of substances.
11.1: Use kinetic molecular models to explain the changes in motion or structure of particles in gases, liquids, and solids.
Reading: 11.1, 11.3, 11.7 Practice: 11.9, 11.10, 11.21, 11.29, 11.30, 11.31, 11.59, 11.61, 11.63, 11.65, 11.69
11.2: Describe the various types of intermolecular and interatomic attractive forces and state the kinds of forces expected for a given substance given its chemical formula.
Reading: 11.2, 11.8 Practice: 11.13, 11.15, 11.17, 11.20, 11.21, 11.22, 11.23, 11.24, 11.25, 11.26, 11.27, 11.71, 11.72, 11.73, 11.74, 11.77 11.3: Calculate the heat absorbed or evolved when a given quantity of a chemical changes from one phase/temperature to another.
Reading: 11.4 Practice: 11.33, 11.36, 11.37, 11.38, 11.39, 11.40
11.4: Draw a phase diagram of a substance given appropriate data and/or use a phase diagram to predict phase or phase changes.
Reading: 11.5, 11.6 Practice: 11.43, 11.45, 11.48, 11.49, 11.50, 11.51, 11.52, 11.53, 11.55, 11.56
U12: Explain how reaction rates are effected using Kinetic Molecular Theory, activation energy, and rate laws. (NOTE: unit 12 but chapter 14 in book)
12.1: Determine the rate law from experimental data and use it to calculate rates, rate constants, and reactant concentrations.
Reading: 14.1, 14.2, 14.3, 14.4 Practice: 14.3, 14.4, 14.21, 14.23, 14.25, 14.27, 14.29, 14.31, 14.35, 14.39, 14.41, 14.42, 14.43 12.2: Calculate activation energies and explain how it relates to reaction rate, rate constants, and temperature.
Reading: 14.5 Practice: 14.6, 14.45, 14.49, 14.50, 14.51, 14.52, 14.31, 14.35, 14.39, 14.41, 14.42, 14.43 12.3: Write the mechanism steps for multi-step reactions, determine the reactants, intermediates, catalysts, and products, and determine the reaction molecularity.
Reading: 14.6 Practice: 14.7, 14.2, 14.11, 14.13, 14.15, 14.19, 14.69, 14.71, 14.77, 14.79
U13: Calculate parameters for a chemical system at equilibrium and determine how shifts in equilibrium parameters will affect the direction of a reversible reaction. 13.1: Convert between Kc and Kp equilibrium constants and use them to make predictions about equilibrium quantities of reactants and products.
13.2: Calculate equilibrium constants or concentrations of products or reactants at equilibrium given initial concentration values.
Reading: 15.5, 15.5, 15.6 Practice: 15.31, 15.32, 15.33, 15.34, 15.39, 15.41, 15.45, 15.49 13.3: Calculate the reaction quotient, Q, and by comparison with the value of Kc or Kp determine whether a reaction is at equilibrium or which direction the reaction will shift to attain equilibrium.
Reading: 15.6 Practice: 15.5, 15.35, 15.36, 15.37, 15.38
13.4: Explain how the relative equilibrium quantities of reactants and products are shifted by changes in temperature, pressure or the concentrations of substances in the equilibrium state.
Reading: 15.7 Practice: 15.1, 15.8, 15.51, 15.52, 15.53, 15.55, 15.56
U14: Identify acids and bases and calculate pH, pOH, [H+], [OH-], or % ionization for
acid-base equilibrium systems.
14.1: Identify Arrhenius, Bronsted-Lowry, and Lewis acids, bases, conjugate acids, conjugate bases, and determine their relative strengths.
Reading: 16.1, 16.2, 16.3, 16.4, 16.10, 16.11 Practice: 16.1, 16.2, 16.3, 16.8, 16.10, 16.13, 16.15, 16.16, 16.17, 16.19, 16.21, 16.25, 16.26 16.81, 16.91, 16.93, 16.95, 16.99, 16.101 14.2: Calculate pH, pOH, [H+], [OH-], or % ionization using Kw, k
a, and kb for a strong acid or
base solution.
Reading: 16.6, 16.7, 16.8 Practice: 16.5, 16.27, 16.28, 16.29, 16.30, 16.33 16.35, 16.37, 16.38, 16.41, 16.42, 16.43, 16.45, 16.47 14.3: Calculate pH, pOH, [H+], [OH-], or % ionization using Kw, k
a, and kb for a weak acid or
base solution at equilibrium.
Reading: 16.6, 16.7, 16.8 Practice: 16.51, 16.53, 16.55, 16.57, 16.58, 16.59, 16.61, 16.63, 16.65, 16.67, 16.69, 16.73, 16.75, 16.77 14.4: Calculate pH, pOH, [H+], [OH-], or % ionization using Kw, k
a, and kb for a conjugate
weak acid or base containing salt solutions at equilibrium.
Reading: 16.9 Practice: 16.83, 16.84, 16.85, 16.86, 16.87, 16.89, 16.90
U15: Calculate equilibria concentrations and equilibrium constants based on titration data, solubility, and common-ion effect equilibria systems.
15.1: Predict qualitatively and calculate quantitatively the effect of an added common ion on the pH of an aqueous solution of a weak acid or base.
Reading: 17.1 Practice: 17.9, 17.10, 17.11, 17.13, 17.14, 17.15, 17.16 15.2: Calculate the change in pH of buffer solution.
Reading: 17.2 Practice: 17.1, 17.3, 17.17, 17.19, 17.20, 17.21, 17.23, 17.25, 17.27, 17.28, 17.29
15.3: Calculate the pH of an unknown acid or base solution based on titration analysis data. Reading: 17.3 Practice: 17.2, 17.5, 17.31, 17.32, 17.33, 17.34, 17.35, 17.37,
17.38, 17.39, 17.40, 17.41
15.4: Calculate equilibrium concentrations and quantitatively predict solubility or Ksp of salts in solution.
U16: Calculate and use enthalpy and entropy to make predictions about the spontaneity of chemical and physical processes.
16.1: Make qualitative determinations of the entropy change for physical and chemical processes using the three Laws of Thermodynamics
Reading: 19.1, 19.2, 19.3 Practice: 19.1, 19.3, 19.7, 19.9, 19.10, 19.11, 19.13 19.17, 19.19, 19.21, 19.23, 19.29, 19.31, 19.37, 19.39 16.2: Make quantitative determinations of the entropy change for physical or chemical processes using the three Laws of Thermodynamics.
Reading: 19.4, 19.5 Practice: 19.41, 19.43, 19.45, 19.47, 19.48
16.3: Determine whether a process is spontaneous for certain standard and non-standard conditions of entropy, temperature, and enthalpy.
Reading: 19.5, 19.6 Practice: 19.2, 19.4, 19.49, 19.51, 19.52, 19.53, 19.55, 19.57, 19.59, 19.61, 19.63, 19.65
16.4: Calculate and explain the relationship between the equilibrium constant and Gibbs free energy. Reading: 19.6, 19.7 Practice: 19.5, 19.6, 19.71, 19.73, 19.75, 19.77, 19.79, 19.104
U17: Explain the function of a chemical cell and calculate its parameters for standard and non-standard conditions.
17.1: Identify elements being oxidized or reduced, balance oxidation reduction reactions, and write oxidation and reduction half-reactions.
Reading: 20.1, 20.1 Practice: 20.1, 20.5, 20.9, 20.10, 20.11, 20.12, 20.13, 20.14 20.15, 20.17, 20.19, 20.39, 20.43
17.2: Identify components and functions of an electrochemical cell.
Reading: 20.3, 20.4 Practice: 20.3, 20.4, 20.21, 20.22, 20.23, 20.24, 20.25, 20.26 17.3: Determine the spontaneous direction of electricity flow in an electrochemical cell for a given set of standard parameters.
Reading: 20.5, 20.6 Practice: 20.27, 20.29, 20.30, 20.31, 20.33, 20.35, 20.37, 20.47, 20.49, 20.51
17.4: Determine the spontaneous direction of electricity flow in an electrochemical cell for a given set of non-standard parameters.
Reading: 20.5, 20.6 Practice: 20.55, 20.57, 20.59, 20.61, 20.63, 20.65
U18: Name and explain the structure and function of micro and macro molecules in organic and biologic chemical systems.
18.1: Name simple branched and cyclical organic hydrocarbons using IUPAC nomenclature and explain some of their basic chemical properties.
Reading: 25.1, 25.2, 25.3, 25.4 Practice: 25.1, 25.4, 25.6, 25.8, 25.9, 25.11, 25.13, 25.15, 25.16, 25.17, 25.19, 25.22, 25.23, 25.24, 25.25
18.2: Name organic hydrocarbons containing more than one functional group using IUPAC nomenclature and explain some of their basic chemical properties.
Reading: 25.5, 25.6, 25.7 Practice: 25.39, 25.40, 25.41, 25.42, 25.43, 25.44, 25.47, 25.51, 25.52, 25.53, 25.84, 25.85, 25.86, 25.89
18.3: Explain the structure and function of organic molecules and primary structures in biological systems.
Reading: 25.7, 25.8, 25.9, 25.10, 25.11 Practice: 25.2, 25.3, 25.55, 25.56, 25.57, 25.59, 25.60, 25.63, 25.64, 25.65, 25.66, 25.67, 25.69, 25.70, 25.71, 25.73, 25.74 18.4: Explain the structure and function of molecular secondary, tertiary, and quaternary structures in biological systems.