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AP Chemistry

AP · College BoardChemistry779 cards

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Flashcards for AP Chemistry, split into the nine units of the College Board course framework and then by topic in the framework's order. Written from the Course and Exam Description effective Fall 2024, for exams from 2027. Delete or suspend any subdeck your course leaves out once the deck is yours.

Adding it gives you your own copy, with every subdeck below. Each card then comes back just before you would forget it, and every one you get right or wrong counts towards your mastery of its topic. You can delete or suspend the parts you are not studying once it is yours.

What is inside (100 subdecks)

  • Unit 1: Atomic Structure and Properties95 cards
    • 1.1 Moles and Molar Mass17 cards
    • 1.2 Mass Spectra of Elements7 cards
    • 1.3 Elemental Composition of Pure Substances8 cards
    • 1.4 Composition of Mixtures6 cards
    • 1.5 Atomic Structure and Electron Configuration23 cards
    • 1.6 Photoelectron Spectroscopy6 cards
    • 1.7 Periodic Trends19 cards
    • 1.8 Valence Electrons and Ionic Compounds9 cards
  • Unit 2: Compound Structure and Properties74 cards
    • 2.1 Types of Chemical Bonds12 cards
    • 2.2 Intramolecular Force and Potential Energy9 cards
    • 2.3 Structure of Ionic Solids4 cards
    • 2.4 Structure of Metals and Alloys6 cards
    • 2.5 Lewis Diagrams9 cards
    • 2.6 Resonance and Formal Charge9 cards
    • 2.7 VSEPR and Hybridization25 cards
  • Unit 3: Properties of Substances and Mixtures124 cards
    • 3.1 Intermolecular and Interparticle Forces12 cards
    • 3.2 Properties of Solids22 cards
    • 3.3 Solids, Liquids, and Gases13 cards
    • 3.4 Ideal Gas Law17 cards
    • 3.5 Kinetic Molecular Theory8 cards
    • 3.6 Deviation from Ideal Gas Law6 cards
    • 3.7 Solutions and Mixtures9 cards
    • 3.8 Representations of Solutions2 cards
    • 3.9 Separation of Solutions and Mixtures7 cards
    • 3.10 Solubility4 cards
    • 3.11 Spectroscopy and the Electromagnetic Spectrum5 cards
    • 3.12 Properties of Photons11 cards
    • 3.13 Beer-Lambert Law8 cards
  • Unit 4: Chemical Reactions78 cards
    • 4.1 Introduction for Reactions6 cards
    • 4.2 Net Ionic Equations9 cards
    • 4.3 Representations of Reactions4 cards
    • 4.4 Physical and Chemical Changes7 cards
    • 4.5 Stoichiometry9 cards
    • 4.6 Introduction to Titration7 cards
    • 4.7 Types of Chemical Reactions21 cards
    • 4.8 Introduction to Acid-Base Reactions7 cards
    • 4.9 Oxidation-Reduction (Redox) Reactions8 cards
  • Unit 5: Kinetics81 cards
    • 5.1 Reaction Rates7 cards
    • 5.2 Introduction to Rate Law12 cards
    • 5.3 Concentration Changes Over Time14 cards
    • 5.4 Elementary Reactions6 cards
    • 5.5 Collision Model7 cards
    • 5.6 Reaction Energy Profile8 cards
    • 5.7 Introduction to Reaction Mechanisms7 cards
    • 5.8 Reaction Mechanism and Rate Law3 cards
    • 5.9 Pre-Equilibrium Approximation4 cards
    • 5.10 Multistep Reaction Energy Profile5 cards
    • 5.11 Catalysis8 cards
  • Unit 6: Thermochemistry69 cards
    • 6.1 Endothermic and Exothermic Processes10 cards
    • 6.2 Energy Diagrams4 cards
    • 6.3 Heat Transfer and Thermal Equilibrium5 cards
    • 6.4 Heat Capacity and Calorimetry14 cards
    • 6.5 Energy of Phase Changes9 cards
    • 6.6 Introduction to Enthalpy of Reaction8 cards
    • 6.7 Bond Enthalpies7 cards
    • 6.8 Enthalpy of Formation5 cards
    • 6.9 Hess's Law7 cards
  • Unit 7: Equilibrium73 cards
    • 7.1 Introduction to Equilibrium7 cards
    • 7.2 Direction of Reversible Reactions6 cards
    • 7.3 Reaction Quotient and Equilibrium Constant8 cards
    • 7.4 Calculating the Equilibrium Constant4 cards
    • 7.5 Magnitude of the Equilibrium Constant5 cards
    • 7.6 Properties of the Equilibrium Constant8 cards
    • 7.7 Calculating Equilibrium Concentrations7 cards
    • 7.8 Representations of Equilibrium3 cards
    • 7.9 Introduction to Le Chatelier's Principle6 cards
    • 7.10 Reaction Quotient and Le Chatelier's Principle6 cards
    • 7.11 Introduction to Solubility Equilibria8 cards
    • 7.12 Common-Ion Effect5 cards
  • Unit 8: Acids and Bases96 cards
    • 8.1 Introduction to Acids and Bases11 cards
    • 8.2 pH and pOH of Strong Acids and Bases11 cards
    • 8.3 Weak Acid and Base Equilibria15 cards
    • 8.4 Acid-Base Reactions and Buffers11 cards
    • 8.5 Acid-Base Titrations12 cards
    • 8.6 Molecular Structure of Acids and Bases8 cards
    • 8.7 pH and pKa7 cards
    • 8.8 Properties of Buffers6 cards
    • 8.9 Henderson-Hasselbalch Equation6 cards
    • 8.10 Buffer Capacity5 cards
    • 8.11 pH and Solubility4 cards
  • Unit 9: Thermodynamics and Electrochemistry89 cards
    • 9.1 Introduction to Entropy8 cards
    • 9.2 Absolute Entropy and Entropy Change5 cards
    • 9.3 Gibbs Free Energy and Thermodynamic Favorability13 cards
    • 9.4 Thermodynamic and Kinetic Control6 cards
    • 9.5 Free Energy and Equilibrium8 cards
    • 9.6 Free Energy of Dissolution3 cards
    • 9.7 Coupled Reactions6 cards
    • 9.8 Galvanic (Voltaic) and Electrolytic Cells10 cards
    • 9.9 Cell Potential and Free Energy13 cards
    • 9.10 Cell Potential Under Nonstandard Conditions9 cards
    • 9.11 Electrolysis and Faraday's Law8 cards

Some of its cards

  • What do elementary reactions typically involve, in terms of bonds?
    The breaking of some bonds and the forming of new ones
  • For a weak acid dissolved in water, how does the equilibrium concentration of H3O+\mathrm{H_3O^+} compare with the acid's initial concentration?
    It is much less, because only a small percentage of the acid molecules ionize
  • How can the order of a reaction with respect to a reactant be inferred from experimental data?
    From a graph of the concentration of that reactant against time
  • Write the Henderson-Hasselbalch equation.
    pH=pKa+log⁡[A−][HA]pH = pK_a + \log \dfrac{[A^-]}{[\mathrm{HA}]}
  • What does photoelectron spectroscopy (PES) measure experimentally?
    The energies of the electrons in the shells of an atom or ion
  • Write the heat transfer equation relating heat, mass, specific heat capacity and temperature change.
    q=mcΔTq = mc\Delta T
  • What must happen when reactant particles collide, for an elementary reaction to successfully produce products?
    The collision must initiate the breaking and forming of bonds
  • For a catalyst to increase the rate of a reaction, what must it do?
    Increase the number of effective collisions, provide a reaction path with lower activation energy, or both
  • What allows a reaction energy profile to be constructed for a reaction with more than one elementary step?
    Knowledge of the energetics of each individual elementary step in the mechanism
  • By the Bronsted-Lowry definition, what is an acid?
    A proton donor

And 769 more once you add the deck.