Unit 1: Review of Chemistry |
PI 2 | Determine the molecular formula of a compound |
| 2.6 | Differentiate among molecular, condensed, structural, and empirical formulas. |
| 2.10 | Use chemical analysis to determine the percent composition, empirical, and molecular formulas for substances |
| 2.11a | Use mass spectrometry to determine the molecular formula of a substance |
| 2.11b | Determine the formula of a hydrated compound |
PI 3.1 | Write, balance, and simplify chemical and net ionic equations |
| 3.2 | Balance chemical equations |
| 3.4 | Determine the solubility of ionic compounds and describe dissociation of soluble compounds |
| 3.5 | Write the net ionic equation for precipitation reactions |
| 3.6 | Write balanced net ionic equations for acid/base reactions and identify acids and bases. |
PI 3.2 | Identify and classify substances as oxidizing or reducing agents |
| 3.8a | Identify the oxidation state of atoms in ions and compounds. |
| 3.8b | Classify substances as oxidizing or reducing agents. |
PI 4.1 | Use stoichiometry to calculate unknown quantities in chemical reactions |
| 4.1 | Calculate mass relations in chemical reactions using stoichiometry. |
| 4.2 | Calculate mass relations in chemical reactions when there is a limiting reactant present. |
| 4.3 | Calculate the percent yield for a chemical reaction when given experimental data. |
PI 4.2 | Use stoichiometry to calculate more complicated unknown quantities in chemical reactions, including pH |
| 4.5 | Calculate concentration of a solution and how to prepare a solution by dilution. |
| 4.6 | Calculate the pH of a solution. |
| 4.7 | Use stoichiometry to complete chemical analysis with aqueous solutions. |
PI 4.3 | Use spectrophotometry in chemical analysis to determine the concentration of a substance |
| 4.8 | Use spectrophotometry in chemical analysis to determine the concentration of a substance. |
Unit 2: Introduction to Chemical Thermodynamics |
PI 5.1 | Quantify the change in heat energy that takes place through chemical reactions |
| 5.2 | Use specific heat capacity in calculations of energy transfer as heat and of temperature changes. |
| 5.3 | Use enthalpy of fusion and enthalpy of vaporization to calculate the energy transferred as heat in changes of state. |
| 5.4 | Use the First Law of Thermodynamics to describe how energy transferred as heat and work done on or by a system contribute to changes in the internal energy of a system. |
PI 5.2 | Calculate standard molar enthalpies for chemical reactions |
| 5.5 | Calculate the change in enthalpy for a simple chemical reaction. |
| 5.6 | Describe how to measure the quantity of energy transferred as heat in a reaction by calorimetry. |
| 5.7a | Use Hess's law to find the enthalpy change, Δ4H°, for a reaction. |
| 5.7b | Draw and interpret energy level diagrams. |
| 5.7c | Use standard molar enthalpies of formation, ΔfH°, to calculate the enthalpy change for a reaction, ΔrH°. |
PI 6 | Solve quantitative wave and energy problems |
| 6.1 | Mathematically relate the wavelength and frequency of electromagnetic radiation. |
| 6.2 | Calculate the energy of a photon of electromagnetic radiation. |
Unit 3: The Periodic Table |
PI 7 | Use Periodicity and the Periodic Table to describe chemical trends |
| 7.4 | Using the Periodic Table as a guide, depict electron configurations of neutral atoms and monatomic ions. |
| 7.5 | Predict how properties of atoms - size, ionization energy, and electron attachment enthalpy - change on moving down a group or across a period of the Periodic Table. |
| 7.6 | Describe the role that ionization energy and electron attachment enthalpy play in forming ionic compounds. |
Unit 4: Chemical Bonding |
PI 8.1 | Draw Lewis Structures and calculate formal charges for polyatomic ions |
| 8.2 | Draw Lewis Dot Diagrams for atoms. |
| 8.3 | Calculate formal charges for polyatomic ions. |
PI 8.2 | Draw and interpret resonance structures |
| 8.4 | Draw resonance structure and demonstrate how and when to use this means of representing chemical bonding. |
| 8.5 | Draw resonance structures and describe exceptions to the Octet Rule. |
PI 8.3 | Predict the shape and polarity of a molecule |
| 8.6 | Predict the shape or geometry of molecules and ions of main group elements using VSEPR theory. |
| 8.7 | Define electronegativity and describe how it is used to describe the unequal sharing of electrons between atoms in a bond. |
| 8.8 | Predict the polarity of a molecule. |
| 8.9 | Define and predict trends in bond order, bond length, and bond dissociation enthalpy. |
PI 9 | Identify types of bond and bond order of ions and molecules |
| 9.2a | Identify the number of hybrid orbital, their hybridization, the electron pair geometry, and their bond angle in compounds. |
| 9.2b | Identify the hybridization of central atoms that meet and expand the octet rule. |
| 9.2c | Differentiate between pi and sigma bonds and identify each of a molecule. |
| 9.3 | Identify the bond order of ions. |
Unit 5: The Gas Laws |
PI 11.1 | Use the gas laws to solve a variety of quantitative gaseous substance problems |
| 11.1 | Define pressure and convert among different units of pressure. |
| 11.2 | Apply the gas laws to various situations. |
| 11.3 | Apply the ideal gas law to various situations and calculate the molar mass of a compound from a knowledge of the pressure of a known quantity of gas in a given volume at a known temperature. |
| 11.4 | Apply the gas laws to a study of the stoichiometry of reactions. |
PI 11.2 | Use the Kinetic Molecular Theory to describe more complication gaseous compound situations |
| 11.5 | Apply Dalton's law of partial pressures to various situations. |
| 11.6 | Apply the kinetic-molecular theory of gas behavior at the molecular level. |
| 11.7 | Understand the phenomena of diffusion and effusion and how to use Graham's Law. |
| 11.8 | Identify and describe situations where gases do and/or do not behave as ideal gases. |
Unit 6: Intermolecular Forces and Solids |
PI 12.1 | Identify intermolecular forces present in different molecules |
| 12.5a | Identify intermolecular forces that would be expected between certain inorganic molecules. |
| 12.5b | Identify situations of likely hydrogen bonding among organic molecules. |
| 12.5c | Identify intermolecular forces that would be expected between certain organic molecules. |
| 12.5d | Identify likely consequences of varying levels of intermolecular forces among molecules. |
PI 12.2 | Use intermolecular forces to determine a molecule's likely properties |
| 12.6a | Describe the equilibrium vapor pressure of a liquid, and explain the relationship between the vapor pressure and the boiling point of a liquid. |
| 12.6b | Describe the phenomena of the critical temperature and critical pressure of a substance. |
| 12.6c | Describe how intermolecular interactions affect the cohesive forces between identical liquid molecules, the energy necessary to break through the surface of a liquid, capillary action, and the resistance to flow, or viscosity, of liquids. |
| 12.6d | Explain the processes of evaporation and condensation, and use the enthalpy of vaporization in calculations. |
PI 13 | Describe the properties of metals and ionic solids |
| 13.2 | Describe the relation of unit cell structure and formula for ionic compounds. |
| 13.3 | Relate the band theory of bonding in metals and the electrical conductivity in metals. |
| 13.4 | Describe lattice energy and how it is calculated. |
| 13.5 | Describe the general properties of other types of solids. |
Unit 7: Solution Chemistry |
PI 14 | Describe, both qualitatively and quantitatively, the properties of solutions |
| 14.2a | Differentiate among saturation, unsaturated, and supersaturated solutions; miscible vs. immiscible; describe the process of dissolving a solute in a solvent, including the energy changes that may occur |
| 14.2b | Relate intermolecular forces to solubility |
| 14.3a | Describe the effect of pressure and temperature on the solubility of a solute. |
| 14.3b | Use Henry's law to calculate the solubility of a gas in a solvent, and apply Le Chatelier's principle to the change in solubility of gases with temperature changes. |
Unit 8: Chemical Kinetics |
PI 15.1 | Determine a rate equation from experimental data |
| 15.1 | Explain the concept of reaction rate and derive the average and instantaneous rates of a reaction from concentration vs. time data. |
| 15.3a | Write rate laws and complete rate law calculations. |
| 15.3b | Derive a rate equation from experimental data. |
PI 15.2 | Complete integrated rate law calculations and use graphical methods to determine reaction order | #colspan |
| 15.4a | Complete integrated rate law calculations on first order reactions |
| 15.4b | Complete integrated rate law calculations on zeroth and second order reactions |
| 15.4c | Apply graphical methods for determining reaction order and the rate constant from experimental data |
PI 15.3 | Use reaction coordinate diagrams to help understand the effect of different variables on reaction rate |
| 15.5a | Describe the collision theory of reaction rates and use collision theory to describe the effect of reactant concentration on reaction rate |
| 15.5b | Describe the effect of molecular orientation, temperature, and activation energy to the rate of a reaction |
| 15.5c | Understand and interpret reaction coordinate diagrams |
PI 15.4 | Determine the rate-determining step in a mechanism and identify reaction intermediates |
| 15.6a | Describe the elementary steps of a mechanism, and give their molecularity |
| 15.6b | Define the rate-determining step in a mechanism, and identify any reaction intermediates |
Unit 9: Advanced Equilibrium Chemistry |
PI 16.1 | Calculate an equilibrium constant by writing a mass-action expression and using experimental data |
| 16.2a | Write equilibrium constant expressions for chemical reactions. |
| 16.2b | Use the reaction quotient to determine how a reaction will proceed towards equilibrium. |
| 16.3 | Calculate an equilibrium constant using concentrations or partial pressures. |
| 16.4 | Calculate equilibrium concentrations using an equilibrium constant. |
PI 16.2 | Use Le Chatelier's Principle to predict changes in concentration after a system at equilibrium is stressed |
| 16.5 | Describe how an equilibrium constant changes as different stoichiometry coefficients are used in a balanced equation, if an equation is reversed, or if several equations are added to give a new net equation. |
| 16.6 | Predict, using Le Chatelier's principle, the effect of a distubance on a chemical equilibrium - a change in termperature, a change in concentrations, or a change in volume or pressure for a reaction involving gases. |
Unit 10: Advanced Acid/Base Chemistry |
PI 17.1 | Write basic acid/base reactions and calculate the pH of strong acid and base solutions |
| 17.2 | Write net ionic equations for acid/base reactions and identify conjugate pairs in reactions. |
| 17.3a | Calculate the hydroxide and/or hydronium ion concentrations in various solutions. |
| 17.3b | Calculate the pH of strong acid and strong base solutions. |
PI 17.2 | Use Ka and Kb values to determine the pH of weak acid and base solutions |
| 17.4a | Write balanced chemical equations and equilibrium constant expressions for Ka and Kb. |
| 17.4b | Compare acid and base strength of Ka and Kb values, respectively. |
| 17.5 | Approximate the pH value of various solutions created from salt solutes. |
PI 17.3 | Calculate different quantitative variables, including pH, pOH, Ka, and Kb for acid and base mixtures |
| 17.6 | Write balanced, net ionic equations for the reaction between acids and bases and determine whether the equilibrium lies predominantly to the left or the right. |
| 17.7 | Calculate the pH of the resulting solution when combining acids and bases. |
| 17.8a | Calculate a Ka or Kb value from a measured pH or pOH. |
| 17.8b | Calculate equilibrium concentrations and pH from a given Ka. |
PI 18.1 | Determine the pH of various solutions including buffered solutions |
| 18.2a | Describe the functioning of buffer solutions and use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution of given composition. |
| 18.2b | Describe how to prepare a buffer of given pH and predict pH change when an acid or base is added to the buffer. |
| 18.3a | Predict the pH of an acid-base reaction at its equivalence point. |
| 18.3b | Describe the differences between the titration curves for a strong acid-strong base titration and titrations in which one of the substances is weak. |
PI 18.2 | Use Ksp values to determine the solubility of an ionic salt |
| 18.4 | Write the equilibrium constant expression - relating concentrations of ions in solutions to Ksp - for any insoluble salt and calculate Ksp values from experimental data |
| 18.5 | Calculate the ion concentrations that are required to begin precipitation of an insoluble salt. |
Unit 11: Advanced Chemical Thermodynamics |
PI 19 | Calculate various quantitative thermodynamic variables associated with chemical reactions |
| 19.4 | Identify common processes that are entropy-favored and calculate entropy changes from tables of standard entropy values. |
| 19.5 | Use standard entropy and enthalpy changes to predict whether a reaction will be spontaneous under standard conditions and recognize how temperature influences whether a reaction is spontaneous. |
| 19.6 | Describe and use the relationship of ΔrG, ΔrG°, Q, K, reaction spontaneity, and product- or reactant-favorability, as well as free energy change under standard condition and equilibrium constants, to calculate various values. |
| 19.7 | Calculate the change in free energy at standard conditions for a reaction from the enthalpy and entropy changes under standard conditions or from the standard free energy of formation of reactants and products (ΔfG°). |
Unit 12: Electrochemistry |
PI 20 | Determine the cell voltage in a voltaic cell |
| 20.1 | Balance net ionic equations, identify the species oxidized and the species reduced, and show the balanced half-reactions. |
| 20.2 | In a voltaic cell, identify the half-reactions occurring at the anode and the cathode, the polarity of the electrodes, the direction of electron flow in the external circuit, and the direction of ion flow in the salt bridge. |
| 20.4 | Calculate the cell voltage in a voltaic cell. |
| 20.6 | Use the relationships between cell voltage and free energy and between cell voltage and an equilibrium constant for the cell reaction. |
| 20.8 | Relate the amount of a substance oxidized or reduced to the amount of current and the time the current flows. |