1
Q
• When assumptions used to simplify math and make equilibrium problems easier to solve fail, the quadratic formula must be used.
A
• When assumptions used to simplify math and make equilibrium problems easier to solve fail, the quadratic formula must be used.
2
Q
• The quadratic formula always yields two solutions, but only one result will be physically meaningful.
A
• The quadratic formula always yields two solutions, but only one result will be physically meaningful.
AP Chemistry
flashcards
Decks in class (252)
# Cards
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An Introduction to Chemistry (1.1.1)2
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The Scientific Method (1.1.2)9
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States of Matter (1.2.1)9
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A Word About Laboratory Safety (1.2.2)2
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CIA Demonstration: Differences in Density Due to Temperature (1.2.3)4
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Properties of Matter (1.2.4)8
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The Measurement of Matter (1.3.1)10
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Precision and Accuracy (1.3.2)7
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CIA Demonstration: Precision and Accuracy with Glassware (1.3.3)6
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Significant Figures (1.3.4)8
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Dimensional Analysis (1.3.5)6
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Scientific (Exponential) Notation (1.4.1)9
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Common Mathematical Functions (1.4.2)4
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Early Discoveries and the Atom (2.1.1)9
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Understanding Electrons (2.1.2)6
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Understanding the Nucleus (2.1.3)9
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Mass Spectrometry: Determining Atomic Masses (2.2.1)7
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Examining Atomic Structure (2.2.2)9
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CIA Demonstration: Flame Colors (2.2.3)8
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Creating the Periodic Table (2.3.1)7
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Describing Chemical Formulas (2.4.1)14
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Naming Chemical Compounds (2.4.2)10
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Organic Nomenclature (2.4.3)5
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An Introduction to Chemical Reactions and Equations (3.1.1)4
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CIA Demonstration: Magnesium and Dry Ice (3.1.2)4
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Balancing Chemical Equations (3.1.3)3
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The Mole and Avogadro's Number (3.2.1)4
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Introducing Conversions of Masses, Moles, and Number of Particles (3.2.2)4
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Finding Emperical and Molecular Formulas (3.3.1)7
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Stoichiometry and Chemical Equations (3.3.2)5
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Finding Limiting Reagents (3.3.3)3
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CIA Demonstration: Self-Inflating Hydrogen Balloons (3.3.4)4
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Theoretical Yield and Percent Yield (3.3.5)5
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A Problem Using the Combined Concepts of Stoichiometry (3.3.6)2
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Calculating Mass Percent (3.3.7)4
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Properties of Solutions (4.1.1)6
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CIA Demonstration: The Electric Pickle (4.1.2)3
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Concentrations of Solutions (4.1.3)5
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Factors Determining Solubility (4.1.4)3
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Precipitation Reactions (4.2.1)3
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Acid-Base Reactions (4.2.2)7
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Oxidation-Reduction Reactions (4.2.3)4
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Acid-Base Titrations (4.3.1)5
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Solving Titration Problems (4.3.2)3
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Gravimetric Analysis (4.3.3)2
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Properties of Gases (5.1.1)4
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Boyle's Law (5.1.2)1
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Charles's Law (5.1.3)3
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The Combined Gas Law (5.1.4)3
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Avogadro's Law (5.1.5)2
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CIA Demonstration: The Potato Cannon (5.1.6)2
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The Ideal Gas Law (5.2.1)4
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Partial Pressure and Dalton's Law (5.2.2)2
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Applications of the Gas Laws (5.2.3)4
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The Kinetic-Molecular Theory of Gases (5.2.4)4
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CIA Demonstration: The Ammonia Fountain (5.2.5)4
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Molecular Speeds (5.3.1)4
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Effusion and Diffusion (5.3.2)5
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Comparing Real and Ideal Gases (5.4.1)5
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The Nature of Energy (6.1.1)3
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Energy, Calories, and Nutrition (6.1.2)4
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The First Law of Thermodynamics (6.1.3)3
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Work (6.1.4)3
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Heat (6.1.5)4
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CIA Demonstration: Cool Fire (6.1.6)3
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Heats of Reaction: Enthalpy (6.2.1)3
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CIA Demonstration: The Thermite Reaction (6.2.2)2
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Constant Pressure Calorimetry (6.3.1)3
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Bomb Calorimetry (Constant Volume) (6.3.2)3
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Hess's Law (6.4.1)3
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Enthalpies of Formation (6.4.2)5
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The Wave Nature of Light (7.1.1)6
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Absorption and Emission (7.1.2)6
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CIA Demonstration: Luminol (7.1.3)2
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The Ultraviolet Catastrophe (7.1.4)3
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The Photoelectric Effect (7.1.5)3
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The Bohr Model (7.1.6)16
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The Heisenberg Uncertainty Principle (7.1.7)13
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The Wave Nature of Matter (7.2.1)16
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Radial Solutions to the Schrodinger Equation (7.2.2)15
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Angular Solutions to the Schrodinger Equation (7.2.3)14
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Atomic Orbital Size (7.3.1)13
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Atomic Orbital Shapes and Quantum Numbers (7.3.2)13
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Atomic Orbital Energy (7.3.3)15
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Understanding Electron Spin (8.1.1)13
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Electron Shielding (8.1.2)14
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Electron Configurations Through Neon (8.1.3)16
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Electron Configurations Beyond Neon (8.1.4)15
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Periodic Relationships (8.1.5)15
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Periods and Atomic Size (8.2.1)16
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Ionization Energy (8.2.2)14
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Electron Affinity (8.2.3)15
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An Introduction to Electronegativity (8.2.4)11
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Hydrogen, Alkali Metals, and Alkaline Earth Metals (8.3.1)16
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Transition Metals and Nonmetals (8.3.2)17
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Valence Electrons and Chemical Bonding (9.1.1)14
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Ionic Bonds (9.1.2)14
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CIA Demonstration: Conductivity Apparatus-Ionic versus Covalent Bonds (9.1.3)5
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Lewis Dot Structures for Covalent Bonds (9.2.1)10
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Predicting Lewis Dot Structures (9.2.2)17
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Resonance Structures (9.3.1)13
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Formal Charge (9.3.2)15
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Electronegativity, Formal Charge, and Resonance (9.3.3)14
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Bond Properties (9.4.1)17
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Using Bond Dissociation Energies (9.4.2)14
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Valence-Shell Electron-Pair Repulsion Theory (10.1.1)15
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Molecular Shapes for Steric Numbers 2-4 (10.1.2)14
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Molecular Shapes for Steric Numbers 5 & 6 (10.1.3)15
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Predicting Molecular Characteristics Using VSEPR Theory (10.1.4)14
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Molecular Shapes: The AXE Method, Part 1 (10.1.5)21
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Molecular Shapes: The AXE Method, Part 2 (10.1.6)26
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Valence Bond Theory (10.2.1)15
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An Introduction to Hybrid Orbitals (10.2.2)18
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Pi Bonds (10.2.3)14
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Molecular Orbital Theory (10.2.4)13
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Applications of the Molecular Orbital Theory (10.2.5)13
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Beyond Homonuclear Diatomics (10.2.6)16
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CIA Demonstration: The Paramagnetism of Oxygen (10.2.7)3
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Oxidation Numbers (11.1.1)14
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Balancing Redox Reactions by the Oxidation Number Method (11.1.2)14
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Balancing Redox Reactions Using the Half-Reaction Method (11.1.3)12
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The Activity Series of the Elements (11.1.4)8
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CIA Demonstration: The Reaction Between Al and Br2 (11.1.5)5
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An Introduction to Intermolecular Forces and States of Matter (12.1.1)4
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Intermolecular Forces (12.1.2)4
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Properties of Liquids (12.2.1)4
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CIA Demonstration: Boiling Water at Reduced Pressure (12.2.2)2
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Vapor Pressure and Boiling Point (12.2.3)3
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Molecular Structure and Boiling Point (12.2.4)3
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Phase Diagrams (12.2.5)3
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CIA Demonstration: Boiling Water in a Paper Cup (12.2.6)2
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Types of Solids (12.3.1)3
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CIA Demonstration: The Conductivity of Molten Salts (12.3.2)2
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Crystal Structure (12.3.3)3
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Calculating Atomic Mass and Radius from a Unit Cell (12.3.4)6
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Crystal Packing (12.3.5)13
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Types of Solutions (13.1.1)13
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Molarity and the Mole Fraction (13.1.2)12
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Molality (13.1.3)12
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Energy and the Solution Process (13.1.4)14
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Temperature Change and Solubility (13.2.1)13
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Extractions (13.2.2)12
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Pressure Change and Solubility (13.2.3)13
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Vapor Pressure Lowering (13.3.1)12
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Boiling Point Elevation and Freezing Point Depression (13.3.2)13
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Boiling Point Elevation Problem (13.3.3)2
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Osmosis (13.3.4)4
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Colligative Properties of Ionic Solutions (13.3.5)1
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An Introduction to Reaction Rates (14.1.1)2
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Rate Laws: How the Reaction Rate Depends on Concentration (14.1.2)2
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Determining the Form of a Rate Law (14.1.3)3
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First-Order Reactions (14.2.1)2
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Second-Order Reactions (14.2.2)2
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A Kinetics Problem (14.2.3)1
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The Collision Model (14.3.1)3
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The Arrhenius Equation (14.3.2)2
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Using the Arrhenius Equation (14.3.3)3
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Defining the Molecularity of a Reaction (14.4.1)2
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Determining the Rate Laws of Elementary Reactions (14.4.2)3
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Calculating the Rate Laws of Multi-step Reactions (14.4.3)4
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Steady State Kinetics (14.4.4)4
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Catalysts and Types of Catalysts (14.5.1)3
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A Word About Laboratory Safety (14.5.2)1
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CIA Demonstration: Elephant Shot (14.5.3)2
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CIA Demonstration: The Cobalt(II)-Catalyzed Reaction of Potassium Sodium Tartrate (14.5.4)2
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CIA Demonstration: The Copper-Catalyzed Decomposition of Acetone (14.5.5)1
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The Concept of Equilibrium (15.1.1)3
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The Law of Mass Action and Types of Equilibrium (15.1.2)2
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Predicting the Direction of a Reaction (15.2.2)2
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Strategies for Solving Equilibrium Problems (15.2.3)3
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Le Châtelier's Principle (15.3.1)2
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The Effect of Changing Amounts on Equilibrium (15.3.2)2
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Solving Problems Far from Equilibrium (15.2.4)2
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An Equilibrium Problem Using the Quadratic Equation (15.2.5)2
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The Effects of Pressure and Volume on Equilibrium (15.3.3)3
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The Effects of Temperature and Catalysts on Equilibrium (15.3.4)2
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CIA Demonstration: NO2/N2O4 (15.3.5)2
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CIA Demonstration: Shifting the Equilibrium of FeSCN2+ (15.3.6)3
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Arrhenius/Brønsted-Lowry Definitions of Acids and Bases (16.1.1)3
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Hydronium, Hydroxide, and the pH Scale (16.1.2)3
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Strong Acids and Bases (16.2.1)4
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CIA Demonstration: Natural Acid-Base Indicators (16.2.2)2
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Weak Acids (16.2.3)3
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Weak Bases (16.2.4)3
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Lewis Acids and Bases (16.2.5)3
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Trends in Acid and Base Strengths (16.2.6)4
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Strong Acid-Strong Base and Weak Acid-Strong Base Reactions (17.1.1)2
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Strong Acid-Weak Base and Weak Acid-Weak Base Reactions (17.1.2)3
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The Common Ion Effect (17.1.3)2
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An Introduction to Buffers (17.2.1)3
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CIA Demonstration: Buffers in Action (17.2.2)2
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Acidic Buffers (17.2.3)3
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Basic Buffers (17.2.4)3
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The Henderson-Hasselbalch Equation (17.2.5)4
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Strong Acid-Strong Base Titration (17.3.1)2
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CIA Demonstration: Barium Hydroxide-Sulfuric Acid Titration (17.3.2)2
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Weak Acid-Strong Base Titration (17.3.3)2
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Polyprotic Acid-Strong Base Titration (17.3.4)2
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Weak Base-Strong Acid Titration (17.3.5)2
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Acid-Base Indicators (17.3.6)3
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The Solubility Product Constant (17.4.1)4
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CIA Demonstration: Silver Chloride and Ammonia (17.4.2)2
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Solubility and the Common Ion Effect (17.4.3)2
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Fractional Precipitation (17.4.4)2
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Spontaneous Processes (18.1.1)3
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Entropy and the Second Law of Thermodynamics (18.2.1)3
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Entropy and Temperature (18.2.2)3
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Gibbs Free Energy (18.3.1)3
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Standard Free Energy Changes of Formation (18.3.2)2
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Enthalpy and Entropy Contributions to K (18.4.1)3
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The Temperature Dependence of K (18.4.2)2
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Free Energy Away from Equilibrium (18.4.3)3
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Reviewing Oxidation-Reduction Reactions (19.1.1)3
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Electrochemical Cells (19.2.1)2
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Electromotive Force (19.2.2)2
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Standard Reduction Potentials (19.2.3)3
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Using Standard Reduction Potentials (19.2.4)3
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The Nernst Equation (19.2.5)2
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Electrochemical Determinants of Equilibria (19.2.6)2
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Batteries (19.3.1)3
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CIA Demonstration: The Fruit-Powered Clock (19.3.2)2
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Corrosion and the Prevention of Corrosion (19.4.1)3
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Electrolytic Cells (19.5.1)3
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The Stoichiometry of Electrolysis (19.5.2)1
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The Nature of Radioactivity (20.1.1)2
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The Stability of Atomic Nuclei (20.1.2)3
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Binding Energy (20.1.3)3
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Rates of Disintegration Reactions (20.2.1)3
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Radiochemical Dating (20.2.2)2
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Nuclear Fission (20.3.1)3
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Nuclear Fusion (20.3.2)3
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Applications of Nuclear Chemistry (20.3.3)3
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Metallurgical Processes (21.1.1)3
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The Band Theory of Conductivity (21.1.2)2
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Intrinsic Semiconductors (21.1.3)2
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Doped Semiconductors (21.1.4)3
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The Alkali Metals (21.2.1)3
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The Alkaline Earth Metals (21.2.2)3
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Aluminum (21.2.3)3
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CIA Demonstration: The Reaction Between Al and Br2 (21.2.4)2
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General Properties of Nonmetals (22.1.1)2
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Hydrogen (22.1.2)4
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General Properties of Carbon (22.2.1)2
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Silicon (22.2.2)3
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Nitrogen (22.3.1)4
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Phosphorus (22.3.2)4
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Oxygen (22.4.1)4
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CIA Demonstration: Creating Acid Rain (22.4.2)3
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Sulfur (22.4.3)3
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Halogens (22.5.1)2
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Aqueous Halogen Compounds (22.5.2)2
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Properties of Noble Gases (22.6.1)2
