1
Q
What is combustion analysis?
A
• Combustion analysis can be used to identify the ratios of elements in an unknown sample.
2
Q
What information can boiling point elevation provide?
A
• Boiling point elevation can provide information useful in identifying an unknown substance.
AP Chemistry 2016
flashcards
Decks in class (252)
# Cards
-
An Introduction to Chemistry (1.1.1)3
-
The Scientific Method (1.1.2)3
-
States of Matter (1.2.1)3
-
A Word About Laboratory Safety (1.2.2)1
-
CIA Demonstration: Differences in Density Due to Temperature (1.2.3)2
-
Properties of Matter (1.2.4)3
-
The Measurement of Matter (1.3.1)3
-
Precision and Accuracy (1.3.2)3
-
CIA Demonstration: Precision and Accuracy with Glassware (1.3.3)3
-
Significant Figures (1.3.4)4
-
Dimensional Analysis (1.3.5)3
-
Scientific (Exponential) Notation (1.4.1)4
-
Common Mathematical Functions (1.4.2)2
-
Early Discoveries and the Atom (2.1.1)3
-
Understanding Electrons (2.1.2)2
-
Understanding the Nucleus (2.1.3)4
-
Mass Spectrometry: Determining Atomic Masses (2.2.1)2
-
Examining Atomic Structure (2.2.2)4
-
CIA Demonstration: Flame Colors (2.2.3)1
-
Creating the Periodic Table (2.3.1)3
-
Describing Chemical Formulas (2.4.1)3
-
Naming Chemical Compounds (2.4.2)3
-
Organic Nomenclature (2.4.3)3
-
An Introduction to Chemical Reactions and Equations (3.1.1)3
-
CIA Demonstration: Magnesium and Dry Ice (3.1.2)2
-
Balancing Chemical Equations (3.1.3)2
-
The Mole and Avogadro's Number (3.2.1)2
-
Introducing Conversions of Masses, Moles, and Number of Particles (3.2.2)2
-
Finding Empirical and Molecular Formulas (3.3.1)3
-
Stoichiometry and Chemical Equations (3.3.2)2
-
Finding Limiting Reagents (3.3.3)2
-
CIA Demonstration: Self-Inflating Hydrogen Balloons (3.3.4)2
-
Theoretical Yield and Percent Yield (3.3.5)2
-
A Problem Using the Combined Concepts of Stoichiometry (3.3.6)1
-
Calculating Mass Percent (3.3.7)3
-
Properties of Solutions (4.1.1)3
-
CIA Demonstration: The Electric Pickle (4.1.2)2
-
Concentrations of Solutions (4.1.3)3
-
Factors Determining Solubility (4.1.4)2
-
Precipitation Reactions (4.2.1)2
-
Acid-Base Reactions (4.2.2)4
-
Oxidation-Reduction Reactions (4.2.3)3
-
Acid-Base Titrations (4.3.1)2
-
Solving Titration Problems (4.3.2)2
-
Gravimetric Analysis (4.3.3)1
-
Properties of Gases (5.1.1)3
-
Boyle's Law (5.1.2)1
-
Charles's Law (5.1.3)2
-
The Combined Gas Law (5.1.4)2
-
Avogadro's Law (5.1.5)1
-
CIA Demonstration: The Potato Cannon (5.1.6)1
-
The Ideal Gas Law (5.2.1)2
-
Partial Pressure and Dalton's Law (5.2.2)1
-
Applications of the Gas Laws (5.2.3)2
-
The Kinetic Molecular Theory of Gases (5.2.4)2
-
CIA Demonstration: The Ammonia Fountain (5.2.5)2
-
Molecular Speeds (5.3.1)2
-
Effusion and Diffusion (5.3.2)2
-
Comparing Real and Ideal Gases (5.4.1)2
-
The Nature of Energy (6.1.1)2
-
Energy, Calories, and Nutrition (6.1.2)3
-
The First Law of Thermodynamics (6.1.3)2
-
Work (6.1.4)2
-
Heat (6.1.5)3
-
CIA Demonstration: Cool Fire (6.1.6)2
-
Heats of Reaction: Enthalpy (6.2.1)2
-
CIA Demonstration: The Thermite Reaction (6.2.2)1
-
Constant Pressure Calorimetry (6.3.1)2
-
Bomb Calorimetry (Constant Volume) (6.3.2)2
-
Hess's Law (6.4.1)1
-
Enthalpies of Formation (6.4.2)3
-
The Wave Nature of Light (7.1.1)3
-
Absorption and Emission (7.1.2)4
-
CIA Demonstration: Luminol (7.1.3)1
-
The Ultraviolet Catastrophe (7.1.4)2
-
The Photoelectric Effect (7.1.5)2
-
The Bohr Model (7.1.6)3
-
The Heisenberg Uncertainty Principle (7.1.7)2
-
The Wave Nature of Matter (7.2.1)3
-
Radial Solutions to the Schrödinger Equation (7.2.2)2
-
Angular Solutions to the Schrödinger Equation (7.2.3)2
-
Atomic Orbital Size (7.3.1)2
-
Atomic Orbital Shapes and Quantum Numbers (7.3.2)2
-
Atomic Orbital Energy (7.3.3)2
-
Understanding Electron Spin (8.1.1)2
-
Electron Shielding (8.1.2)3
-
Electron Configurations through Neon (8.1.3)3
-
Electron Configurations beyond Neon (8.1.4)3
-
Periodic Relationships (8.1.5)3
-
Periods and Atomic Size (8.2.1)4
-
Ionization Energy (8.2.2)3
-
Electron Affinity (8.2.3)2
-
An Introduction to Electronegativity (8.2.4)3
-
Hydrogen, Alkali Metals, and Alkaline Earth Metals (8.2.5)3
-
Transition Metals and Nonmetals (8.2.6)3
-
Valence Electrons and Chemical Bonding (9.1.1)3
-
Ionic Bonds (9.1.2)2
-
CIA Demonstration: Conductivity Apparatus-Ionic Versus Covalent Bonds (9.1.3)2
-
Lewis Dot Structures for Covalent Bonds (9.2.1)2
-
Predicting Lewis Dot Structures (9.2.2)4
-
Resonance Structures (9.3.1)2
-
Formal Change (9.3.2)3
-
Electronegativity, Formal Charge, and Resonance (9.3.3)4
-
Bond Properties (9.4.1)3
-
Using Bond Dissociation Energies (9.4.2)2
-
Valence-Shell Electron-Pair Repulsion Theory (10.1.1)3
-
Molecular Shapes for Steric Numbers 2-4 (10.1.2)1
-
Molecular Shapes for Steric Numbers 5 & 6 (10.1.3)2
-
Predicting Molecular Characteristics Using VSEPR Theory (10.1.4)2
-
Molecular Shapes: The AXE Method, Part 1 (10.1.5)2
-
Molecular Shapes: The AXE Method, Part 2 (10.1.6)3
-
Valence Bond Theory (10.2.1)3
-
An Introduction to Hybrid Orbitals (10.2.2)4
-
Pi Bonds (10.2.3)2
-
Molecular Orbital Theory (10.2.4)2
-
Applications of the Molecular Orbital Theory (10.2.5)2
-
Beyond Homonuclear Diatomics (10.2.6)3
-
CIA Demonstration: The Paramagnetism of Oxygen (10.2.7)2
-
Oxidation Numbers (11.1.1)2
-
Balancing Redox Reactions by the Oxidation Number Method (11.1.2)3
-
Balancing Redox Reactions Using the Half-Reaction Method (11.1.3)2
-
The Activity Series of Elements (11.1.4)3
-
CIA Demonstration: The Reaction Between Al and Br2 (11.1.5)2
-
An Introduction to Intermolecular Forces and States of Matter (12.1.1)4
-
Intermolecular Forces (12.1.2)4
-
Properties of Liquids (12.2.1)4
-
CIA Demonstration: Boiling Water at Reduced Pressure (12.2.2)2
-
Vapor Pressure and Boiling Point (12.2.3)3
-
Molecular Structure and Boiling Point (12.2.4)3
-
Phase Diagrams (12.2.5)3
-
CIA Demonstration: Boiling Water in a Paper Cup (12.2.6)2
-
Types of Solids (12.3.1)3
-
CIA Demonstration: The Conductivity of Molten Salts (12.3.2)1
-
Crystal Structure (12.3.3)3
-
Types of Solutions (13.1.1)3
-
Molarity and the Mole Fraction (13.1.2)3
-
Molality (13.1.3)2
-
Energy and the Solution Process (13.1.4)3
-
Temperature Change and Solubility (13.2.1)3
-
Extractions (13.2.2)2
-
Pressure Change and Solubility (13.2.3)2
-
Vapor Pressure Lowering (13.3.1)2
-
Boiling Point Elevation and Freezing Point Depression (13.3.2)3
-
Boiling Point Elevation Problem (13.3.3)2
-
Osmosis (13.3.4)4
-
Colligative Properties of Ionic Solutions (13.3.5)1
-
An Introduction to Reaction Rates (14.1.1)2
-
Rate Laws: How the Reaction Rate Depends on Concentration (14.1.2)2
-
Determining the Form of a Rate Law (14.1.3)3
-
First-Order Reactions (14.2.1)2
-
Second-Order Reactions (14.2.2)2
-
A Kinetics Problem (14.2.3)1
-
The Collision Model (14.3.1)3
-
The Arrhenius Equation (14.3.2)2
-
Using the Arrhenius Equation (14.3.3)3
-
Defining the Molecularity of a Reaction (14.4.1)2
-
Determining the Rate Laws of Elementary Reactions (14.4.2)3
-
Calculating the Rate Laws of Multi-step Reactions (14.4.3)4
-
Steady State Kinetics (14.4.4)4
-
Catalysts and Types of Catalysts (14.5.1)3
-
A Word About Laboratory Safety (14.5.2)1
-
CIA Demonstration: Elephant Snot (14.5.3)2
-
CIA Demonstration: The Cobalt(II)-Catalyzed Reaction of Potassium Sodium Tartrate (14.5.4)2
-
CIA Demonstration: The Copper-Catalyzed Decomposition of Acetone (14.5.5)1
-
The Concept of Equilibrium (15.1.1)3
-
The Law of Mass Action and Types of Equilibrium (15.1.2)2
-
Converting Between Kc and Kp (15.1.3)2
-
Approaching Chemical Equilibrium (15.2.1)3
-
Predicting the Direction of a Reaction (15.2.2)2
-
Strategies for Solving Equilibrium Problems (15.2.3)3
-
Solving Problems Far from Equilibrium (15.2.4)2
-
An Equilibrium Problem Using the Quadratic Equation (15.2.5)2
-
Le Châtelier's Principle (15.3.1)2
-
The Effect of Changing Amounts on Equilibrium (15.3.2)2
-
The Effects of Pressure and Volume on Equilibrium (15.3.3)3
-
The Effects of Temperature and Catalysts on Equilibrium (15.3.4)2
-
CIA Demonstration: NO2/N2O4 (15.3.5)2
-
CIA Demonstration: Shifting the Equilibrium of FeSCN2+ (15.3.6)3
-
Arrhenius/Brønsted-Lowry Definitions of Acids and Bases (16.1.1)4
-
Hydronium, Hydroxide, and the pH Scale (16.1.2)3
-
Strong Acids and Bases (16.2.1)4
-
CIA Demonstration: Neutral Acid-Base Indicators (16.2.2)2
-
Weak Acids (16.2.3)3
-
Weak Bases (16.2.4)3
-
Lewis Acids and Bases (16.2.5)3
-
Trends in Acid and Base Strengths (16.2.6)4
-
Strong Acid-Strong Base and Weak Acid-Strong Base Reactions (17.1.1)2
-
Strong Acid-Weak Base and Weak Acid-Weak Base Reactions (17.1.2)3
-
The Common Ion Effect (17.1.3)2
-
An Introduction to Buffers (17.2.1)3
-
CIA Demonstration: Buffers in Action (17.2.2)2
-
Acidic Buffers (17.2.3)3
-
Basic Buffers (17.2.4)3
-
The Henderson-Hasselbalch Equation (17.2.5)3
-
Strong Acid-Strong Base Titration (17.3.1)2
-
CIA Demonstration: Barium Hydroxide-Sulfuric Acid Titration (17.3.2)2
-
Weak Acid-Strong Base Titration (17.3.3)2
-
Polyprotic Acid-Strong Base Titration (17.3.4)2
-
Weak Base-Strong Acid Titration (17.3.5)2
-
Acid-Base Indicators (17.3.6)3
-
The Solubility Product Constant (17.4.1)4
-
CIA Demonstration: Silver Chloride and Ammonia (17.4.2)2
-
Solubility and the Common Ion Effect (17.4.3)2
-
Fractional Precipitation (17.4.4)2
-
Spontaneous Processes (18.1.1)3
-
Entropy and the Second Law of Thermodynamics (18.2.1)3
-
Entropy and Temperature (18.2.2)3
-
Gibbs Free Energy (18.3.1)3
-
Standard Free Energy Changes of Formation (18.3.2)2
-
Enthalpy and Entropy Contributions to K (18.4.1)3
-
The Temperature Dependence of K (18.4.2)2
-
Free Energy Away from Equilibrium (18.4.3)3
-
Reviewing Oxidation-Reduction Reactions (19.1.1)3
-
Electrochemical Cells (19.1.2)2
-
Electromotive Force (19.2.2)2
-
Standard Reduction Potentials (19.2.3)3
-
Using Standard Reduction Potentials (19.2.4)3
-
The Nernst Equation (19.2.5)2
-
Electrochemical Determinants of Equilibria (19.2.6)2
-
Batteries (19.3.1)3
-
CIA Demonstration: The Fruit-Powered Clock (19.3.2)2
-
Corrosion and the Prevention of Corrosion (19.4.1)3
-
Electrolytic Cells (19.5.1)3
-
The Stoichiometry of Electrolysis (19.5.2)1
-
Nature of Radioactivity (20.1.1)2
-
The Stability of Atomic Nuclei (20.1.2)3
-
Binding Energy (20.1.3)3
-
Rates of Disintegration Reactions (20.2.1)3
-
Radiochemical Dating (20.2.2)2
-
Nuclear Fission (20.3.1)3
-
Nuclear Fusion (20.3.2)3
-
Applications of Nuclear Chemistry (20.3.3)3
-
Metallurgical Processes (21.1.1)3
-
The Band Theory of Conductivity (21.1.2)2
-
Intrinsic Semiconductors (21.1.3)2
-
Doped Semiconductors (21.1.4)3
-
The Alkali Metals (21.2.1)3
-
The Alkaline Earth Metals (21.2.2)3
-
Aluminum (21.2.3)3
-
CIA Demonstration: The Reaction Between Al and Br2 (21.2.4)2
-
General Properties of Nonmetals (22.1.1)2
-
Hydrogen (22.1.2)4
-
General Properties of Carbon (22.2.1)2
-
Silicon (22.2.2)3
-
Nitrogen (22.3.1)4
-
Phosphorus (22.3.2)4
-
Oxygen (22.4.1)4
-
CIA Demonstration: Creating Acid Rain (22.4.2)3
-
Sulfur (22.4.3)3
-
Halogens (22.5.1)2
-
Aqueous Halogen Compounds (22.5.2)2
-
Properties of Noble Gases (22.6.1)2
