Best AP Chem Quizlet Decks for Every Unit
6 min read•july 11, 2024
Dylan Black
AP Chemistry 🧪
269 resourcesSee Units
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?
One of the most popular study sites used by AP students is Quizlet and for good reason! Quizlet combines the classic flashcard studying method with unique, fun games to learn vocabulary. However, the number of resources provided by Quizlet can make it challenging to find the best decks for each AP Chemistry Unit. For that reason, here are the most comprehensive Quizlet decks for effective studying! Vocabulary is critical for understanding different concepts, laws, and theories.
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⚛️ Unit 1: Atomic Structure and Properties
Unit 1 sets the foundation for the rest of the course, making it essential to know these 29 terms. In this unit, the material revolves around the most important things to know about how atoms are structured and the basics of chemistry, like moles and the structure of matter. This unit is one of the most vocab heavy units since it is mostly concepts and not math, but it is incredibly important to practice problems as well!
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
Unit 2 builds upon the atomic structure you learned in Unit 1 and applies it to molecules and bonding. In this unit, you’ll learn about bond types, structure, and geometry. Like unit 1, most of this unit is theory and concept related, so vocab is a big part, especially knowing the names of geometries and types of bonds.
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
Unit 3 delves into what happens between molecules. In this unit, you’ll learn about intermolecular forces, solutions, gasses, and states of matter. When dealing with gasses, a lot of the content you will learn is quantitative, so along with using this Quizlet deck, be sure to practice problems and FRQs!
- 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
Unit 4 teaches what every chemistry student wants to learn going into chemistry: reactions. This unit gets straight into how reactants turn into products in a variety of ways, such as combustion reactions, precipitation reactions, and neutralizations. You NEED to know these types of reactions and how they work to succeed in AP Chemistry.
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
Unit 5 describes the mechanics behind reactions and what makes reactions go the speed that they do. You’ll learn how to speed up reactions and what factors affect the rates of reactions. It’s important to be able to both understand these concepts and apply them mathematically, with this unit being roughly 50% math and 50% concepts.
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
Unit 6 is all about one thing: energy. You’ll learn how energy flows in reactions and how thermodynamics can be applied to chemical reactions. Unlike past units, this unit is probably 75% math, but in order to know how to apply formulas, you have to know the concepts! Therefore, knowing terms and vocab are invaluable, and this Quizlet deck will help!
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
Unit 7 goes back to unit 4 and unit 5 and describes what happens when a reaction can go backward. Through this unit, you’ll learn about reversible reactions and reactions that produce not that many products because of equilibrium. This unit is also verrry math-heavy, but equilibrium is also a hard concept to grasp with a lot of unfamiliar terms.
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
Unit 8 is a big one. This unit is typically the one that scares students, and frankly? It’s for good reason. Unit 8 is a beast. Acids, bases, equilibrium, titrations, buffers, this unit has it all. Typically, this unit is also REALLY heavily tested, so you gotta know it for the exam.
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
The final unit! Unit 9 blends units 6 and 7 to apply thermodynamics to chemical reactions even more heavily. You’ll learn some really cool topics like spontaneity, electrochemistry, and Gibbs Free Energy and equilibrium. This is a veeerry math-heavy unit, but again, concepts above all!
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
Browse Study Guides By Unit
⚛️Unit 1 – Atomic Structure & Properties
🤓Unit 2 – Molecular & Ionic Bonding
🌀Unit 3 – Intermolecular Forces & Properties
🧪Unit 4 – Chemical Reactions
👟Unit 5 – Kinetics
🔥Unit 6 – Thermodynamics
⚖️Unit 7 – Equilibrium
🍊Unit 8 – Acids & Bases
🔋Unit 9 – Applications of Thermodynamics
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