| Unit 1: Introduction to Chemistry |
| PI 1.1 | Use proper laboratory and safety procedures to investigate phenomena |
| 1.1 | Identify proper safety procedures in the laboratory |
| 1.2 | Identify and use proper tools and equipment in the laboratory |
| 1.3 | Differentiate between qualitative and quantitative data |
| 1.6 | Differentiate between accuracy and precision |
| PI 1.2 | Convert measurements among a variety of different units using dimensional analysis |
| 1.4 | Convert measurements among the metric units |
| 1.8 | Convert measurements using dimensional analysis |
| PI 1.3 | Use significant figures to communicate quantitative precision |
| 1.5 | Identify the appropriate measuring device for a specific problem and count the number of significant figures in a measurement |
| 1.7 | Convert numbers to and from scientific notation maintaining the precision of the measurement |
| 1.9 | Round numbers to the correct number of significant figures |
| 1.10 | Add and subtract numbers maintaining the precision of the measurement |
| 1.11 | Multiply and divide numbers maintaining the precision of the measurement |
| PI 1.4 | Use properties to classify and make predictions about substances |
| 1.12 | Identify and differentiate among the seven diatomic molecules |
| 1.13 | Differentiate among physical and chemical properties and changes |
| 1.14 | Distinguish among a mixture, compound, and a pure substance |
| 1.15 | Explain the states of matter in terms of particles |
| 1.16 | Classify mixtures as homogeneous or heterogeneous |
| 1.17 | Relate the atomic symbols with their correct atomic name |
| 1.18 | Calculate the density of a substance |
| Unit 2: Thermal Chemistry and the Atom |
| PI 2.1 | Use thermal energy calculations to make predictions about substances at the molecular level |
| 2.1 | Compute how heat energy added to a substance will change the substance's temperature |
| 2.2 | Apply the definition of heat to the molecular level |
| 2.3 | Identify phase changes and calculate the energy needed to change a phase |
| PI 2.2 | Differentiate among the types of energy including electromagnetic radiation |
| 2.4 | Differentiate among the different types of energy |
| 2.5 | Calculate the speed, wavelength, and frequency of electromagnetic radiation |
| 2.6 | Differentiate among different types of electromagnetic radiation |
| PI 2.3 | Use historical ideas about the atom to develop a model for atomic structure |
| 2.7 | Identify the significance of the various outcomes of Thomson's and Rutherford's experiments |
| 2.8 | Identify the charge, mass, and location of the three subatomic particles |
| 2.9 | Calculate the atomic mass of a given sample with a given percent abundance, and vice versa |
| Unit 3: The Electron |
| PI 3 | Determine the location of electrons in atoms and ions |
| 3.1 | Write the electron configuration of various atoms |
| 3.2 | Write the electron configuration of various ions |
| 3.3 | Using Aufbau's Principle and Hund's Rule, assign electrons to main energy levels and write energy level diagrams for atoms and ions |
| Unit 4: The Periodic Table |
| PI 4 | Use the Periodic Table to identify properties and periodic trends to describe and classify different elements |
| 4.1 | Use the modern periodic table to predict an element's chemical and physical properties |
| 4.2 | Define atomic radii, ionic radii, ionization energy, electron affinity, and electronegativity in terms of the Periodic Table |
| 4.3 | Define valence electrons and determine the number of valence electrons for any main group elements |
| Unit 5: Chemical Bonding |
| PI 5.1 | Define a chemical bond in terms of electrons and differentiate among different types of bonds |
| 5.1 | Define a chemical bond and calculate the electronegativity difference to determine bond type and polarity |
| 5.2 | Use the octet rule to write Lewis structures for compounds |
| 5.3 | Determine whether a given chemical is an ionic, covalent, or metallic compound |
| PI 5.2 | Differentiate among the properties of the different types of chemical bonds |
| 5.4 | Distinguish between ionic and molecular properties |
| 5.5 | Identify and describe the metallic properties of conductivity, malleability, ductility, and luster |
| 5.6 | Differentiate how electrons behave in ionic, covalent, and metallic compounds |
| PI 5.3 | Use VSEPR Theory to describe the geometric shape of molecules |
| 5.7 | Use VSEPR Theory to describe the geometric shape of molecules |
| PI 5.4 | Use intermolecular forces to describe and make predictions about a variety of substances |
| 5.8 | Differentiate among dipole-dipole forces, ion-dipole forces, hydrogen bonding, and london dispersion forces |
| 5.9 | Arrange a group of chemicals in order of increasing freezing or boiling point by considering intermolecular forces |
| Unit 6: Inorganic Nomenclature |
| PI 6.1 | Determine the name and chemical formula for ions and ionic compounds |
| 6.1 | Identify the oxidation number for an element or polyatomic ion and write the correct formula for the ion and vice versa |
| 6.2 | Use the rules for assigning oxidation numbers to determine the formula for an ionic compound from its chemical name |
| 6.3 | Name ionic compounds from given chemical formulas |
| PI 6.2 | Determine the name and chemical formula for molecular compounds |
| 6.4 | Write molecular formulas from the names and numbers of the atoms present |
| 6.5 | Name molecular compounds from given chemical formulas |
| PI 6.3 | Use the Stock System to name compounds including transition metals and name acidic compounds |
| 6.6 | Use oxidation numbers to name compounds and write formulas involving transition ions using the Stock System |
| 6.7 | Determine the name of an acid from a formula and derive the formula of an acid from its name |
| Unit 8: Chemical Equation Stoichiometry |
| PI 7.1 | Use Avogadro's Number and molar mass to calculate the number of moles of a substance |
| 7.1 | Use Avogadro's number to differentiate between number of molecules and a mole of a substance |
| 7.2 | Use the Periodic Table to calculate the molar mass of a substance |
| 7.3 | Use molar mass to differentiate among mass and a mole of a substance |
| PI 7.2 | Calculate the percent composition and use it to determine the empirical and molecular formulas |
| 7.4 | Use molar mass to calculate the percent composition of a substance |
| 7.5 | Identify a compound's empirical formula and calculate the molecular formula from the empirical formula and other data |
| Unit 8: Chemical Equation Stoichiometry |
| PI 8.1 | Write, balance, and categorize a chemical equation |
| 8.1 | Correctly write a formula equation from a word equation and vice versa |
| 8.2 | Balance chemical equations |
| 8.3 | Identify and differentiate among synthesis, decomposition, single-replacement, double-replacement, and combustion reactions |
| PI 8.2 | Use stoichiometry to calculate simple reactant and/or product quantities |
| 8.4 | Predict the products for each type of chemical reaction |
| 8.5 | Use mole ratios and dimensional analysis to solve stoichiometry problems |
| PI 8.3 | Use limiting reactants to calculate more complicated reactant and/or product quantities |
| 8.6 | Use stoichiometry to determine the limiting reactant of a reaction |
| 8.7 | Use the limiting reactant to determine the amount of product and calculate percent yield |
| PI 8.4 | Write different types of equations, including heat transfer and net ionic equations |
| 8.8 | Complete net ionic equations and identify spectator ions |
| 8.9 | Define and differentiate between exothermic and endothermic chemical reactions |
| Unit 9: The Gas Laws |
| PI 9.1 | Describe and calculate simple properties associated with gaseous substances |
| 9.1 | Use the Kinetic Molecular Theory of Matter to identify behaviors of real and ideal gases |
| 9.2 | Relate the pressure of a gas to the force exerted |
| 9.3 | Differentiate among various units of pressure |
| PI 9.2 | Solve quantitative gas properties problems using the gas laws |
| 9.4 | Use standard temperature and pressure to solve stoichiometric problems |
| 9.5 | Use the Combined Gas Law to solve for a gases volume, pressure, or temperature |
| 9.6 | Use Dalton's Law of Partial Pressures to describe different mixed-gas situations |
| 9.7 | Using the Ideal Gas Law, calculate a gases volume, pressure, temperature, or amount. |
| PI 9.3 | Define boiling and solve complicated quantitative gas property problems |
| 9.8 | Define boiling in terms of equilibrium vapor pressure |
| 9.9 | Use the ideal gas law and stoichiometry to solve application problems. |
| Unit 10: Solution Chemistry |
| PI 10.1 | Describe the dissolution process and differentiate among different dissolution constraints |
| 10.1 | Differentiate between the solute and solvent in a solution and compare electrolytes to nonelectrolytes |
| 10.2 | Describe how changing the pressure, temperature, or surface area of a solution/solute will affect the rate of dissolution |
| PI 10.2 | Determine the level of saturation in a variety of solutions |
| 10.3 | Differentiate among unsaturated, saturated, and supersaturated solutions |
| 10.4 | Calculate how many grams of a solute are needed to make a saturated solution |
| PI 10.3 | Use different measures of concentration to represent the concentration of solute in a solution |
| 10.5 | Calculate the molarity of a solution when given the amount of solute and solvent |
| 10.6 | Dilute a given solution from one concentration to a weaker concentration |
| 10.7 | Calculate other measures of solution concentration, including ppt, ppm, and ppb |
| PI 10.4 | Use molarity to make advanced stoichiometric calculations |
| 10.8 | Use molarity to make stoichiometric calculations |
| Unit 11: Chemical Equilibrium |
| PI 11 | Use chemical equilibrium to make predictions about chemical processes and situations |
| 11.1 | Calculate the equilibrium constant for a reversible chemical reaction |
| 11.2 | Calculate the reaction quotient for a given time and a given chemical reaction and compare it to the equilibrium constant |
| 11.3 | Predict how specific stresses, including temperature, pressure, and change in concentration, will affect a chemical system at equilibrium according to Le Chatelier's Principle |
| Unit 12: Acid and Base Chemistry |
| PI 12.1 | Identify compounds as acidic, basic, or neutral |
| 12.1 | Classify a compound as an Arrhenius Acid or Base |
| 12.2 | Classify a compound as a Bronsted-Lowry Acid or Base |
| 12.3 | Identify the six strong acids |
| PI 12.2 | Identify conjugate acid-base pairs and predict the product of acid-base reactions |
| 12.4 | Label conjugate acid-base pairs |
| 12.5 | Determine the products of an acid-base neutralization reaction |
| PI 12.3 | Calculate the pH of different acidic and basic solutions |
| 12.6 | Calculate the pH of strong acid and strong base solutions |
| 12.7 | Calculate the pH of weak acid and weak base solutions |
| 12.8 | Identify common indicators and the pH range they are used for |