AP Chemistry

Atomic Theory & Structure	Gases	Reaction Types
Chemical Bonds	Condensed Phases	Stoichiometry
Nuclear Chemistry	Solutions	Equilibrium

STUDENTS SHOULD KNOW EXAMPLES OF WHAT STUDENTS SHOULD BE ABLE TO DO

I STRUCTURE OF MATTER

A. Atomic Theory and Atomic Structure (return to top)

1. The work of many scientists, such as John Dalton, J.J. Thompson, and Ernest Rutherford, provided experimental information for the development of a modern understanding of the structure of atoms. (AKSci - C.7)

• Describe the composition of an atom in terms of protons, neutrons, and electrons.

• Explain the approximate size, relative mass, and charge of an atom, proton, neutron, and electron.

• Write the chemical symbol of an element, having been given its mass number and atomic number, and perform the reverse operation.

• Describe the properties of an electron as seen in cathode rays.

• Describe the experimental evidence for the nuclear nature of the atom.

2. An element's location on the periodic table can be used to determine similarities and trends among the elements. (AKSci - A.1)

• Recognize and explain trends within groups and periods on the periodic chart in quantities/properties such as Ion charges, atomic and ionic size, ionization energy, electron affinity, reactivity, metallic character, and electronegativity.

• Identify and relate properties of elements in particular families such as alkali metals, alkaline earth metals, halogens, and noble gases.

3. The electronic structure of hydrogen atom forms the basis of electronic structure for atoms with two or more electrons. (AKSci - A.1)

• Describe the wave properties and characteristic speed of propagation of radiant energy (electromagnetic radiation)

• Explain the origin of the expression line spectra.

• List the assumptions made by Bohr in his model of the hydrogen atom.

• Explain the concept of an allowed state and how the concept is related to the quantum theory.

• Explain the concept of ionization energy.

• Describe the uncertainty principle and explain the limitation it places on our ability to define simultaneously the location and momentum of a subatomic particle, particularly an electron.

• Describe the quantum numbers, n ,l ,ml, ms used to define an orbital in an atom and list the limitations placed on the values each many have.

• Describe the shapes of the s, p, and d orbitals.

• Write the electron configurations and valence electron configuration for any element and its orbital diagram representation.

4. Certain behavior patterns of an atom and its electrons are based on the position of the atom in the periodic table. All the periodic trends can be understood in terms of three basic rules: (AKSci - A.1)

a. Electrons are attracted to the protons in the nucleus of an atom.

b. Electrons are repelled by other electrons in an atom

c. Completed shells (and to a lesser extent, subshells) are very stable.

• ExState the Pauli exclusion principle and Hund's rule, and illustrate how they are used in writing the electronic structures of the elements.

• Describe the s, p, d, and f blocks of elements.

• Given the electron configurations for any element, locate its placement in the periodic table.

B. Chemical Bonds (return to top)

1. All bonds occur because of electrostatic attractions. (AKSci - A.1, A.8a)

• Write the Lewis symbols for atoms and recognize when the octet rule applies to the arrangement of electrons in the valence shell.

• Explain the concept of an isoelectronic series.

• Describe how the radii of ions relate to corresponding atoms.

• Describe a covalent bond using Lewis symbols in terms of sharing of electron density between bonded atoms.

• Describe the singe, double and triple covalent bonds.

• Describe the various types of intermolecular attractive forces and the expected forces for a substance when given its molecular structure.

2. Electronegativity determines the bond types. (AKSci - A.1, A.8a)

• Explain the significance of electronegativity and predict the relative polarity of the bonds.

• Write resonance forms of molecules or polyatomic ions.

3. The geometric shape of a molecule can be predicted using the Valence Shell Electron Pair Repulsion Model (V.E.S.P.R ) and/or the Molecular Orbital Model (M.O.) (AKSci - A.1, A.8a)

• Write the Lewis structure for molecules and ions containing covalent bonds, using the periodic table.

• Predict the geometrical structure of a molecule or ion from its Lewis structure.

• Explain the concept of hybridization and its relationship to geometrical structure.

• Formulate the bonding in a molecule in terms of pi (Ľ) bonds and sigma (S) bonds, from its Lewis structure.

• Explain the concept of delocalization in pi (Ľ) bonds.

C. Nuclear Chemistry (return to top)

1. A change in the structure of a nucleus may occur spontaneously, or it may be brought about artificially. (AKSci - A.1, A.8a)

• Write the nuclear symbols for protons, neutrons, electrons, alpha particles, beta particles and positrons.

• Complete and balance nuclear equations, having been given all but one of the particles involved.

• Use the half-life of a substance to predict the amount of radioisotopes present after a given period of time.

• Explain how radioisotopes can be used in dating objects and as radiotracers.

II STATES OF MATTER

A. Gases (return to top)

1. Gas pressure can be measured with devices like barometers and manometers in units including atmospheres, mm Hg, and kPa. (AKSci - A.1)

• Measure pressure and convert between common pressure units.

2. The relationship of the variable pressure, volume, temperature, and moles can be described by simple mathematical equations and relationships. The ideal gas law summarizes all these relationships. (AKSci - A.1)

• Describe and calculate how a gas responds to changes in pressure, volume, temperature, and moles.

• Use the Ideal Gas Law to calculate one of the variables from the other three.

3. The volume of a gas at any temperature and pressure can be used to determine the moles and number of particles. (AKSci - A.1)

• Calculate values of the ideal gas law constant based on the molar volume of a gas.

• Derive an equation from the Ideal Gas Law for determination of molar mass or density.

4. The partial pressure of a gas mixture is related to the mole fraction of the gases in the mixture. (AKSci - A.1)

• Use Dalton's law of partial pressures to calculate the partial pressure of a gas in a mixture.

• Calculate the mole fraction of a gas in a mixture, given its partial pressure and the total pressure of the system.

5. Gases are made of tiny particles which are far apart and in constant linear motion. The collisions are perfectly elastic. Pressure is caused by collisions of the particles with the walls. (AKSci - A.1, A.2)

• Use the Kinetic Molecular Theory to explain gas temperature and pressure at the molecular level.

• Describe how the relative rates of effusion and diffusion of two gases depend on their molar masses (Graham's Law).

6. Temperature of a gas is related to the speed and the energy of the particles. (AKSci - A.1)

• Describe the Boltzmann's distribution of molecular speeds and explain how it changes with temperature.

B. Condensed Phases (return to top)

1. The intermolecular forces in a substance determine strengths of attractions of molecules for each other, and therefore their relative freezing and boiling points. (AKSci - A.1, A.2)

• Compare and contrast the arrangement and motion of particles in the phases.

• Describe the various types of intermolecular forces and identify those present for a particular substance.

2. Phase changes are related to intermolecular forces and are expressed in a phase diagram which plots the pressure and temperature of a substance in relation to its state of matter. (AKSci - A.1, A.2)

• Explain the meaning of the terms vapor pressure, viscosity, surface tension, critical temperature and critical pressure and account for the variations in these properties in terms of intermolecular forces and temperature.

• Describe the relationship between vapor pressure, the boiling point, and melting point of a substance.

• Calculate the heat transfer as a sample is heated including phase change.

• Draw or interpret a phase diagram given appropriate data.

3. Most solids are crystalline in nature and the arrangement of their particles relates to their physical properties. (AKSci - A.1, A.2)

• Distinguish between crystalline and amorphous solids.

• Predict the type of solid (molecular, covalent network, ionic, or metallic) formed by a substance, and predict its general properties.

4. Gas behavior deviates from ideal behavior as a result of the particle volume and the intermolecular forces. (AKSci - A.2)

• Cite the general conditions of pressure and temperature under which real gases most closely approximate ideal gas behavior.

• Explain the deviations and correction from ideality using the van der Waals equation.

C. Solutions (return to top)

1. The solution process involves energy changes and other factors which control solubilities. Colloids differ from solutions. (AKSci - A.1)

• Describe the solution process in terms of solute-solute, solute-solvent and solvent-solvent attractive forces, and enthalpy and entropy changes.

• Predict the solubilities of various substances in terms of their intermolecular forces.

• Describe the effects of temperature and pressure on solubility.

• Describe how a colloid differs from a true solution.

2. The concentration of solutions is described in different terms according to their application. (AKSci - A.2)

• Define and calculate mass percent, ppm, and ppb, mole fraction, molarity, and molality.

• Calculate any component of the above, and convert from one concentration unit to other.

3. Colligative properties of solutions result in alterations of the physical properties of the solvent. (AKSci - A.2)

• Calculate boiling-point elevation, freezing-point depression, osmotic pressure and vapor pressure.

• Determine the molar mass of a nonvolatile nonelectrolyte from its effect on the colligative properties of the solution.

• Describe the difference between electrolytes and nonelectrolytes on the magnitude of the colligative properties.

• Calculate and explain deviations from solution ideality using Raoult's Law.

III REACTIONS

A. Reaction Types (return to top)

1. Aqueous solutions of acids, bases and salts are electrolytes. (AKSci - A.1, A.8a)

• List the general properties that characterize acidic and basic solutions and identify the ions responsible for these properties.

• Define the terms Bronstead-Lowry acid and base, and conjugate acid and base.

• Explain what is meant by the autoionization of water and amphotrism.

• Determine the relationship between the strength of an acid and its conjugate base; Kb from the knowledge of Ka and vice versa.

• Predict whether a particular salt solution will be acidic, basic or neutral.

• Define an acid or base in terms of the Lewis concept.

• Predict the relative acidities of solutions of metal salts.

• Explain the mechanism by which a buffer solution resists a change in pH.

2. A heterogeneous equilibrium is a chemical reaction between ions in solution that produces an insoluble solid - a precipitate. (AKSci - A.2, A.8a)

• Define and calculate Ksp (solubility product constant).

• Determine the direction of a precipitation reaction using the ion product quotient (Q).

• Understand why and how pH will affect some precipitation reactions.

3. A reaction in which certain atoms undergo a change in oxidation states is a redox reaction. The substance increasing in oxidation state is oxidized; the substance decreasing in oxidation states is reduced. (AKSci - A.2, A.8a)

• Identify the oxidizing and reducing agents in a redox reaction.

• Balance simple oxidation-reduction reactions by the oxidation number method and by the method of half-reactions.

4. Electrochemical cells produce electricity from redox reactions. (AKSci - A.2, A.8a)

• Diagram simple voltaic and electrolytic cells, labeling the anode and the cathode, the directions of ion and electron movement and the signs of the electrode.

• Given appropriate electrode potentials calculate the emf generated by a voltaic cell.

• Use electrode potentials to predict whether a reaction will be spontaneous.

5. Electrolysis is a process in which a nonspontaneous redox reaction is made to occur by the application of a direct current of electricity to the reactants. (AKSci - A.2, A.8a)

• Interrelate time, current, and the amount of substance produced or consumed in an electrolysis reaction.

• Calculate the maximum electrical work performed by a voltaic cell and the minimum electrical work required for an electrolytic process.

B. Stoichiometry (return to top)

1. There are standard methods of naming and formula writing for elements and compounds (emphasize IUPAC system). (AKSci - A.1)

• Name or write formulas of ionic compounds, covalent compounds, and acids.

• Show a familiarity with both stock and Latin names of metals, polyatomic ions, and common names of compounds used in chemistry.

• Name or give the formula of alkanes, alkenes, alkynes, and aromatic hydrocarbons; as well as functional group derivatives of these.

2. In any chemical reaction, it is possible to calculate the amount of reactants and/or products involved in the reaction from the balanced chemical equation. Either the mass of the substances, the volume of the substances involved and/or the moles can be determined. (AKSci - A.2, A.8a)

• Calculate the mass of a particular substance produced or used in a chemical reaction.

• Determine the limiting reagent and calculate the theoretical and actual yield in a chemical reaction given the appropriate data.

3. Solubility of an ionic compound depends on the nature of both the anion and cation involved. (AKSci - A.1)

• Use solubility rules to predict whether a precipitate forms when solutions of electrolytes are mixed.

• Predict the products of metathesis reactions (including both neutralization and precipitation reactions) and write balanced chemical equations for them.

• Identify the spectator ions and write the net ionic equations for solution reactions, starting with their molecular equations.

4. Oxidation and reduction reactions involve the transfer of electrons from one substance to another. (AKSci - A.2)

• Determine whether a chemical reaction involves oxidation and reduction.

• Assign oxidation numbers to atoms in molecules and ions.

• Use the activity series to predict whether a reaction will occur when a metal is added to an aqueous solution; and write the balanced molecular and net ionic equations for the reaction.

5. Solutions have variable composition. (AKSci - A.2)

• Calculate the molarity, solution volume, or number of moles of solute given any two of these quantities.

• Calculate the volume of a more concentrated solution that must be diluted to obtain a given quantity of more dilute solution.

• Calculate the volume of a solution required to react with a volume of a different solution using molarity and the stoichiometry of the reaction.

C. Equilibrium (return to top)

1. A state of chemical equilibrium exists when both forward and reverse reactions are proceeding at equal rates and concentrations of reactants and products, pressure, volume, and temperature do not change with time. (AKSci - A.2, A.8a)

• 1. A state of chemical equilibrium exists when both forward and reverse reactions are proceeding at equal rates and concentrations of reactants and products, pressure, volume, and temperature do not change with time. (AKSci - A.2, A.8a)

(return to top)

Table of Contents Guiding Principles Recommendations Science as a Process References

Life Science Biology I Biological Sciences Biology II AP Biology

Chemistry Chemistry I Conceptual Chemistry Chemistry II AP Chemistry

Earth Science Geology I Earth Sciences

Physics Physics I Conceptual Physics AP Physics B AP Physics C

ASD Secondary Science

If you have comments or questions concerning the Anchorage School District Science Frameworks,
please contact
<gillam_lori@asdk12.org> or <raymond_gail@asdk12.org>

STUDENTS SHOULD KNOW	EXAMPLES OF WHAT STUDENTS SHOULD BE ABLE TO DO
I STRUCTURE OF MATTER
A. Atomic Theory and Atomic Structure (return to top)
1. The work of many scientists, such as John Dalton, J.J. Thompson, and Ernest Rutherford, provided experimental information for the development of a modern understanding of the structure of atoms. (AKSci - C.7)	• Describe the composition of an atom in terms of protons, neutrons, and electrons. • Explain the approximate size, relative mass, and charge of an atom, proton, neutron, and electron. • Write the chemical symbol of an element, having been given its mass number and atomic number, and perform the reverse operation. • Describe the properties of an electron as seen in cathode rays. • Describe the experimental evidence for the nuclear nature of the atom.
2. An element's location on the periodic table can be used to determine similarities and trends among the elements. (AKSci - A.1)	• Recognize and explain trends within groups and periods on the periodic chart in quantities/properties such as Ion charges, atomic and ionic size, ionization energy, electron affinity, reactivity, metallic character, and electronegativity. • Identify and relate properties of elements in particular families such as alkali metals, alkaline earth metals, halogens, and noble gases.
3. The electronic structure of hydrogen atom forms the basis of electronic structure for atoms with two or more electrons. (AKSci - A.1)	• Describe the wave properties and characteristic speed of propagation of radiant energy (electromagnetic radiation) • Explain the origin of the expression line spectra. • List the assumptions made by Bohr in his model of the hydrogen atom. • Explain the concept of an allowed state and how the concept is related to the quantum theory. • Explain the concept of ionization energy. • Describe the uncertainty principle and explain the limitation it places on our ability to define simultaneously the location and momentum of a subatomic particle, particularly an electron. • Describe the quantum numbers, n ,l ,ml, ms used to define an orbital in an atom and list the limitations placed on the values each many have. • Describe the shapes of the s, p, and d orbitals. • Write the electron configurations and valence electron configuration for any element and its orbital diagram representation.
4. Certain behavior patterns of an atom and its electrons are based on the position of the atom in the periodic table. All the periodic trends can be understood in terms of three basic rules: (AKSci - A.1) a. Electrons are attracted to the protons in the nucleus of an atom. b. Electrons are repelled by other electrons in an atom c. Completed shells (and to a lesser extent, subshells) are very stable.	• ExState the Pauli exclusion principle and Hund's rule, and illustrate how they are used in writing the electronic structures of the elements. • Describe the s, p, d, and f blocks of elements. • Given the electron configurations for any element, locate its placement in the periodic table.
B. Chemical Bonds (return to top)
1. All bonds occur because of electrostatic attractions. (AKSci - A.1, A.8a)	• Write the Lewis symbols for atoms and recognize when the octet rule applies to the arrangement of electrons in the valence shell. • Explain the concept of an isoelectronic series. • Describe how the radii of ions relate to corresponding atoms. • Describe a covalent bond using Lewis symbols in terms of sharing of electron density between bonded atoms. • Describe the singe, double and triple covalent bonds. • Describe the various types of intermolecular attractive forces and the expected forces for a substance when given its molecular structure.
2. Electronegativity determines the bond types. (AKSci - A.1, A.8a)	• Explain the significance of electronegativity and predict the relative polarity of the bonds. • Write resonance forms of molecules or polyatomic ions.
3. The geometric shape of a molecule can be predicted using the Valence Shell Electron Pair Repulsion Model (V.E.S.P.R ) and/or the Molecular Orbital Model (M.O.) (AKSci - A.1, A.8a)	• Write the Lewis structure for molecules and ions containing covalent bonds, using the periodic table. • Predict the geometrical structure of a molecule or ion from its Lewis structure. • Explain the concept of hybridization and its relationship to geometrical structure. • Formulate the bonding in a molecule in terms of pi (Ľ) bonds and sigma (S) bonds, from its Lewis structure. • Explain the concept of delocalization in pi (Ľ) bonds.
C. Nuclear Chemistry (return to top)
1. A change in the structure of a nucleus may occur spontaneously, or it may be brought about artificially. (AKSci - A.1, A.8a)	• Write the nuclear symbols for protons, neutrons, electrons, alpha particles, beta particles and positrons. • Complete and balance nuclear equations, having been given all but one of the particles involved. • Use the half-life of a substance to predict the amount of radioisotopes present after a given period of time. • Explain how radioisotopes can be used in dating objects and as radiotracers.
II STATES OF MATTER
A. Gases (return to top)
1. Gas pressure can be measured with devices like barometers and manometers in units including atmospheres, mm Hg, and kPa. (AKSci - A.1)	• Measure pressure and convert between common pressure units.
2. The relationship of the variable pressure, volume, temperature, and moles can be described by simple mathematical equations and relationships. The ideal gas law summarizes all these relationships. (AKSci - A.1)	• Describe and calculate how a gas responds to changes in pressure, volume, temperature, and moles. • Use the Ideal Gas Law to calculate one of the variables from the other three.
3. The volume of a gas at any temperature and pressure can be used to determine the moles and number of particles. (AKSci - A.1)	• Calculate values of the ideal gas law constant based on the molar volume of a gas. • Derive an equation from the Ideal Gas Law for determination of molar mass or density.
4. The partial pressure of a gas mixture is related to the mole fraction of the gases in the mixture. (AKSci - A.1)	• Use Dalton's law of partial pressures to calculate the partial pressure of a gas in a mixture. • Calculate the mole fraction of a gas in a mixture, given its partial pressure and the total pressure of the system.
5. Gases are made of tiny particles which are far apart and in constant linear motion. The collisions are perfectly elastic. Pressure is caused by collisions of the particles with the walls. (AKSci - A.1, A.2)	• Use the Kinetic Molecular Theory to explain gas temperature and pressure at the molecular level. • Describe how the relative rates of effusion and diffusion of two gases depend on their molar masses (Graham's Law).
6. Temperature of a gas is related to the speed and the energy of the particles. (AKSci - A.1)	• Describe the Boltzmann's distribution of molecular speeds and explain how it changes with temperature.
B. Condensed Phases (return to top)
1. The intermolecular forces in a substance determine strengths of attractions of molecules for each other, and therefore their relative freezing and boiling points. (AKSci - A.1, A.2)	• Compare and contrast the arrangement and motion of particles in the phases. • Describe the various types of intermolecular forces and identify those present for a particular substance.
2. Phase changes are related to intermolecular forces and are expressed in a phase diagram which plots the pressure and temperature of a substance in relation to its state of matter. (AKSci - A.1, A.2)	• Explain the meaning of the terms vapor pressure, viscosity, surface tension, critical temperature and critical pressure and account for the variations in these properties in terms of intermolecular forces and temperature. • Describe the relationship between vapor pressure, the boiling point, and melting point of a substance. • Calculate the heat transfer as a sample is heated including phase change. • Draw or interpret a phase diagram given appropriate data.
3. Most solids are crystalline in nature and the arrangement of their particles relates to their physical properties. (AKSci - A.1, A.2)	• Distinguish between crystalline and amorphous solids. • Predict the type of solid (molecular, covalent network, ionic, or metallic) formed by a substance, and predict its general properties.
4. Gas behavior deviates from ideal behavior as a result of the particle volume and the intermolecular forces. (AKSci - A.2)	• Cite the general conditions of pressure and temperature under which real gases most closely approximate ideal gas behavior. • Explain the deviations and correction from ideality using the van der Waals equation.
C. Solutions (return to top)
1. The solution process involves energy changes and other factors which control solubilities. Colloids differ from solutions. (AKSci - A.1)	• Describe the solution process in terms of solute-solute, solute-solvent and solvent-solvent attractive forces, and enthalpy and entropy changes. • Predict the solubilities of various substances in terms of their intermolecular forces. • Describe the effects of temperature and pressure on solubility. • Describe how a colloid differs from a true solution.
2. The concentration of solutions is described in different terms according to their application. (AKSci - A.2)	• Define and calculate mass percent, ppm, and ppb, mole fraction, molarity, and molality. • Calculate any component of the above, and convert from one concentration unit to other.
3. Colligative properties of solutions result in alterations of the physical properties of the solvent. (AKSci - A.2)	• Calculate boiling-point elevation, freezing-point depression, osmotic pressure and vapor pressure. • Determine the molar mass of a nonvolatile nonelectrolyte from its effect on the colligative properties of the solution. • Describe the difference between electrolytes and nonelectrolytes on the magnitude of the colligative properties. • Calculate and explain deviations from solution ideality using Raoult's Law.
III REACTIONS
A. Reaction Types (return to top)
1. Aqueous solutions of acids, bases and salts are electrolytes. (AKSci - A.1, A.8a)	• List the general properties that characterize acidic and basic solutions and identify the ions responsible for these properties. • Define the terms Bronstead-Lowry acid and base, and conjugate acid and base. • Explain what is meant by the autoionization of water and amphotrism. • Determine the relationship between the strength of an acid and its conjugate base; Kb from the knowledge of Ka and vice versa. • Predict whether a particular salt solution will be acidic, basic or neutral. • Define an acid or base in terms of the Lewis concept. • Predict the relative acidities of solutions of metal salts. • Explain the mechanism by which a buffer solution resists a change in pH.
2. A heterogeneous equilibrium is a chemical reaction between ions in solution that produces an insoluble solid - a precipitate. (AKSci - A.2, A.8a)	• Define and calculate Ksp (solubility product constant). • Determine the direction of a precipitation reaction using the ion product quotient (Q). • Understand why and how pH will affect some precipitation reactions.
3. A reaction in which certain atoms undergo a change in oxidation states is a redox reaction. The substance increasing in oxidation state is oxidized; the substance decreasing in oxidation states is reduced. (AKSci - A.2, A.8a)	• Identify the oxidizing and reducing agents in a redox reaction. • Balance simple oxidation-reduction reactions by the oxidation number method and by the method of half-reactions.
4. Electrochemical cells produce electricity from redox reactions. (AKSci - A.2, A.8a)	• Diagram simple voltaic and electrolytic cells, labeling the anode and the cathode, the directions of ion and electron movement and the signs of the electrode. • Given appropriate electrode potentials calculate the emf generated by a voltaic cell. • Use electrode potentials to predict whether a reaction will be spontaneous.
5. Electrolysis is a process in which a nonspontaneous redox reaction is made to occur by the application of a direct current of electricity to the reactants. (AKSci - A.2, A.8a)	• Interrelate time, current, and the amount of substance produced or consumed in an electrolysis reaction. • Calculate the maximum electrical work performed by a voltaic cell and the minimum electrical work required for an electrolytic process.
B. Stoichiometry (return to top)
1. There are standard methods of naming and formula writing for elements and compounds (emphasize IUPAC system). (AKSci - A.1)	• Name or write formulas of ionic compounds, covalent compounds, and acids. • Show a familiarity with both stock and Latin names of metals, polyatomic ions, and common names of compounds used in chemistry. • Name or give the formula of alkanes, alkenes, alkynes, and aromatic hydrocarbons; as well as functional group derivatives of these.
2. In any chemical reaction, it is possible to calculate the amount of reactants and/or products involved in the reaction from the balanced chemical equation. Either the mass of the substances, the volume of the substances involved and/or the moles can be determined. (AKSci - A.2, A.8a)	• Calculate the mass of a particular substance produced or used in a chemical reaction. • Determine the limiting reagent and calculate the theoretical and actual yield in a chemical reaction given the appropriate data.
3. Solubility of an ionic compound depends on the nature of both the anion and cation involved. (AKSci - A.1)	• Use solubility rules to predict whether a precipitate forms when solutions of electrolytes are mixed. • Predict the products of metathesis reactions (including both neutralization and precipitation reactions) and write balanced chemical equations for them. • Identify the spectator ions and write the net ionic equations for solution reactions, starting with their molecular equations.
4. Oxidation and reduction reactions involve the transfer of electrons from one substance to another. (AKSci - A.2)	• Determine whether a chemical reaction involves oxidation and reduction. • Assign oxidation numbers to atoms in molecules and ions. • Use the activity series to predict whether a reaction will occur when a metal is added to an aqueous solution; and write the balanced molecular and net ionic equations for the reaction.
5. Solutions have variable composition. (AKSci - A.2)	• Calculate the molarity, solution volume, or number of moles of solute given any two of these quantities. • Calculate the volume of a more concentrated solution that must be diluted to obtain a given quantity of more dilute solution. • Calculate the volume of a solution required to react with a volume of a different solution using molarity and the stoichiometry of the reaction.
C. Equilibrium (return to top)
1. A state of chemical equilibrium exists when both forward and reverse reactions are proceeding at equal rates and concentrations of reactants and products, pressure, volume, and temperature do not change with time. (AKSci - A.2, A.8a)	• 1. A state of chemical equilibrium exists when both forward and reverse reactions are proceeding at equal rates and concentrations of reactants and products, pressure, volume, and temperature do not change with time. (AKSci - A.2, A.8a)

Life Science	Biology I	Biological Sciences	Biology II	AP Biology
Chemistry	Chemistry I	Conceptual Chemistry	Chemistry II	AP Chemistry
Earth Science	Geology I	Earth Sciences
Physics	Physics I	Conceptual Physics	AP Physics B	AP Physics C