Best AP Chem Quizlet Decks for Every Unit

Table of Contents

• ❓ Why Quizlet?
• ⚛️ Unit 1: Atomic Structure and Properties (7-9%)
• 🧪 Unit 2: Molecular and Ionic Compound Structure and Properties (7-9%)
• ⚗️ Unit 3: Intermolecular Forces and Properties (18-22%)
• 💥 Unit 4: Chemical Reactions (7-9%)
• 📈 Unit 5: Kinetics (7-9%)
• 🔥 Unit 6: Thermodynamics (7-9%)
• ⚖️ Unit 7: Equilibrium (7-9%)
• 🍋 Unit 8: Acids and Bases (11-15%)
• 👨‍🔬 Unit 9: Applications of Thermodynamics (7-9%)

Why Quizlet?

Unit 1: Atomic Structure and Properties 

Key Terms:

• Electron Orbital - the most probable region where an electron is located. Located 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, mols, and temperature
• Combined Gas Law - P1V1/T1n1 = P2V2/T2n2 - describes how when certain aspects of a gas change, other quantities chance

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

• 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 

• 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 

• 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

• 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 

• 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