What Are the Best Quizlet Decks for AP Chemistry?

Why Quizlet?

Unit 1: Atomic Structure and Properties

Key Terms:

• Electron Orbital—The most likely region where an electron is located is within subshells.
• Valence Electrons—Electrons on the outermost energy level of an atom; bonding electrons.
• Periodic Trends—Ionization Energy, Electron Affinity, and Atomic/Ionic Radius.

Unit 2: Molecular and Ionic Compound Structure and Properties

Key Terms:

• VSEPR—Valence Shell Electron Pair Repulsion; the theory that describes how electrons act in bonds. Molecules adjust their shapes so that valence electron pairs are as far apart as possible.
• Hybridization—The mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals.
• Formal Charge—The number of valence electrons in an isolated atom minus the number of electrons assigned to the atom in the Lewis structure.

Unit 3: Intermolecular Forces and Properties

Key Terms:

• Intermolecular Forces—Forces of attraction and repulsion between molecules.
• Solubility—The ability to be dissolved and dissociated into constituent ions.

• Ideal Gas Law—PV = nRT; describes the relationship between pressure, volume, moles, and temperature.
• Combined Gas Law—P1V1/T1n1 = P2V2/T2n2; describes how when certain aspects of a gas change, other quantities change as well.

Unit 4: Chemical Reactions

Key Terms:

• Acid-Base Neutralization—When an acid and a base react to form a salt (ionic compound) and water (ex. HCl + NaOH --> NaCl + H2O).
• Redox Reaction—A reaction involving electron transfers (ex. 2Ag + Cu(NO3)2 → Cu + 2AgNO3).
• Precipitation Reaction—A reaction in which an insoluble compound falls out of solution (ex. 2KI (aq) +Pb(NO3)2 (aq) --> 2KNO3 (aq) + PbI2 (s)).

Unit 5: Kinetics

Key Terms:

• Rate Law—an expression relating the rate of a reaction to the concentration of the reactants
• Rate of Reaction—change in concentration / time
• Kinetic Theory—states that chemical reactions can occur when atoms, ions, and molecules collide, with enough energy, in the correct orientation Temperature
• Activation Energy—Energy needed to get a reaction started (space between activated complex and potential energy)

Unit 6: Thermodynamics

Key Terms:

• Enthalpy: Energy in the form of heat that transfers during reactions
• Calorimetry: A coffee-cup calorimeter is a constant-pressure calorimeter. As such, the heat that is measured in such a device is equivalent to the change in enthalpy
• Bond Enthalpy: Bond enthalpy is defined as the amount of energy required to break one mole of the stated bond

Unit 7: Equilibrium

Key Terms:

• Equilibrium: The point at which the rates of the forward and backward reaction are equal
• Equilibrium Constant: A constant that describes the extent to which a reaction goes forward (K = [products]^n/[reactants]^m)
• Reaction Quotient: the relative amounts of products and reactants present during a reaction at a particular point in time
• Le Chatelier's Principle: Can be used to predict the effect of a change in conditions on some chemical equilibria

Unit 8: Acids and Bases

Key Terms:

• Arrhenius Acid and Base: Acid yields H+, Base yields OH-
• Bronsted Acid and Base: Acid donates H+, Base accepts H+
• Titration: the slow addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization
• ICE Box: A method for calculating equilibrium concentrations

Unit 9: Applications of Thermodynamics 

Key Terms:

• Entropy: A measure of disorder in a system
• Gibbs Free Energy: A thermodynamic potential that can be used to calculate the maximum of reversible work that may be performed by a thermodynamic system at a constant temperature and pressure
• Reduction Potential: Is a measure of the tendency of a chemical species to acquire electrons

Closing Thoughts

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