3.2.2 Introducing Conversions of Masses, Moles, and Number of Particles Flashcards

AP Chemistry :!: (338 decks)

• 1.1.1 An Introduction to Chemistry
• 1.1.2 The Scientific Method
• 1.2.1 States of Matter
• 1.2.2 A Word About Laboratory Safety
• 1.2.3 CIA Demonstration: Differences in Density Due to Temperature
• 1.2.4 Properties of Matter
• 1.3.1 The Measurement of Matter
• 1.3.2 Precision and Accuracy
• 1.3.3 CIA Demonstration: Precision and Accuracy with Glassware
• 1.3.4 Significant Figures
• 1.3.5 Dimensional Analysis
• 1.4.1 Scientific (Exponential) Notation
• 1.4.2 Common Mathematical Functions
• Chapter 1 Homework
• Chapter 1 review
• Chapter 1 Practice Test
• Chapter 1 Test
• 2.1.1 Early Discoveries and the Atom
• 2.1.2 Understanding Electrons
• 2.1.3 Understanding the Nucleus
• 2.2.1 Mass Spectrometry: Determining Atomic Masses
• 2.2.2 Examining Atomic Structure
• 2.2.3 CIA Demonstration: Flame Colors
• 2.3.1 Creating the Periodic Table
• 2.4.1 Describing Chemical Formulas
• 2.4.2 Naming Chemical Compounds
• 2.4.3 Organic Nomenclature
• Chapter 2 Homework
• Chapter 2 Practice Test
• Chapter 2 Test
• 3.1.1 An Introduction to Chemical Reactions and Equations
• 3.1.2 CIA Demonstration: Magnesium and Dry Ice
• 3.1.3 Balancing Chemical Equations
• 3.2.1 The Mole and Avogadro's Number
• 3.2.2 Introducing Conversions of Masses, Moles, and Number of Particles
• 3.3.1 Finding Empirical and Molecular Formulas
• 3.3.2 Stoichiometry and Chemical Equations
• 3.3.3 Finding Limiting Reagents
• 3.3.4 CIA Demonstration: Self-Inflating Hydrogen Balloons
• 3.3.5 Theoretical Yield and Percent Yield
• 3.3.6 A Problem Using the Combined Concepts of Stoichiometry
• 3.3.7 Calculating Mass Percent
• Chapter 3 Homework
• Chapter 3 Review
• Chapter 3 Practice Test
• Chapter 3 Test
• 4.1.1 Properties of Solutions
• 4.1.2 CIA Demonstration: The Electric Pickle
• 4.1.3 Concentrations of Solutions
• 4.1.4 Factors Determining Solubility
• 4.2.1 Precipitation Reactions
• 4.2.2 Acid-Base Reactions
• 4.2.3 Oxidation-Reduction Reactions
• 4.3.1 Acid-Base Titrations
• 4.3.2 Solving Titration Problems
• 4.3.3 Gravimetric Analysis
• Chapter 4 Homework
• Chapter 4 Review
• Chapter 4 Practice Test
• Chapter 4 Test
• 5.1.1 Properties of Gases
• 5.1.2 Boyle's Law
• 5.1.3 Charles's Law
• 5.1.4 The Combined Gas Law
• 5.1.5 Avogadro's Law
• 5.1.6 CIA Demonstration: The Potato Cannon
• 5.2.1 The Ideal Gas Law
• 5.2.2 Partial Pressure and Dalton's Law
• 5.2.3 Applications of the Gas Laws
• 5.2.4 The Kinetic-Molecular Theory of Gases
• 5.2.5 CIA Demonstration: The Ammonia Fountain
• 5.3.1 Molecular Speeds
• 5.3.2 Effusion and Diffusion
• 5.4.1 Comparing Real and Ideal Gases
• Chapter 5 Homework
• Chapter 5 Review
• Chapter 5 Practice Test
• Chapter 5 Test
• 6.1.1 The Nature of Energy
• 6.1.2 Energy, Calories, and Nutrition
• 6.1.3 The First Law of Thermodynamics
• 6.1.4 Work
• 6.1.5 Heat
• 6.1.6 CIA Demonstration: Cool Fire
• 6.2.1 Heats of Reaction: Enthalpy
• 6.2.2 CIA Demonstration: The Thermite Reaction
• 6.3.1 Constant Pressure Calorimetry
• 6.3.2 Bomb Calorimetry (Constant Volume)
• 6.4.1 Hess's Law
• 6.4.2 Enthalpies of Formation
• Chapter 6 Homework
• Chapter 6 Review
• Chapter 6 Practice Test
• Chapter 6 Test
• 7.1.1 The Wave Nature of Light
• 7.1.2 Absorption and Emission
• 7.1.3 CIA Demonstration: Luminol
• 7.1.4 The Ultraviolet Catastrophe
• 7.1.5 The Photoelectric Effect
• 7.1.6 The Bohr Model
• 7.1.7 The Heisenberg Uncertainty Principle
• 7.2.1 The Wave Nature of Matter
• 7.2.2 Radical Solutions to the Schrödinger Equation
• 7.2.3 Angular Solutions to the Schrödinger Equation
• 7.3.1 Atomic Orbital Size
• 7.3.2 Atomic Orbital Shapes and Quantum Numbers
• 7.3.3 Atomic Orbital Energy
• Chapter 7 Homework
• Chapter 7 Practice Test
• Chapter 7 Test
• 8.1.1 Understanding Electron Spin
• 8.1.2 Electron Shielding
• 8.1.3 Electron Configurations Through Neon
• 8.1.4 Electron Configurations Beyond Neon
• 8.1.5 Periodic Relationships
• 8.2.1 Periods and Atomic Size
• 8.2.2 Ionization Energy
• 8.2.3 Electron Affinity
• 8.2.4 An Introduction to Electronegativity
• 8.3.1 Hydrogen, Alkali Metals, and Alkaline Earth Metals
• 8.3.2 Transition Metals and Nonmetals
• Chapter 8 Homework
• Chapter 8 Practice Test
• Chapter 8 Test
• 9.1.1 Valence Electrons and Chemical Bonding
• 9.1.2 Ionic Bonds
• 9.1.3 CIA Demonstration: Conductivity Apparatus-Ionic versus Covalent Bonds
• 9.2.1 Lewis Dot Structures for Covalent Bonds
• 9.2.2 Predicting Lewis Dot Structures
• 9.3.1 Resonance Structures
• 9.3.2 Formal Charge
• 9.3.3 Electronegativity, Formal Charge, and Resonance
• 9.4.1 Bond Properties
• 9.4.2 Using Bond Dissociation Energies
• Chapter 9 Homework
• Chapter 9 Practice Test
• Chapter 9 Test
• 10.1.1 Valence-Shell Electron-Pair Repulsion Theory
• 10.1.2 Molecular Shapes for Steric Numbers 2-4
• 10.1.3 Molecular Shapes for Steric Numbers 5 & 6
• 10.1.4 Predicting Molecular Characteristics Using VSEPR Theory
• 10.1.5 Molecular Shapes: The AXE Method, Part 1
• 10.1.6 Molecular Shapes: The AXE Method, Part 2
• 10.2.1 Valence Bond Theory
• 10.2.2 An Introduction to Hybrid Orbitals
• 10.2.3 Pi Bonds
• 10.2.4 Molecular Orbital Theory
• 10.2.5 Applications of the Molecular Orbital Theory
• 10.2.6 Beyond Homonuclear Diatomics
• 10.2.7 CIA Demonstration: The Paramagnetism of Oxygen
• Chapter 10 Homework
• Chapter 10 Practice Test
• Chapter 10 Test
• 11.1.1 Oxidation Numbers
• 11.1.2 Balancing Redox Reactions by the Oxidation Number Method
• 11.1.3 Balancing Redox Reactions Using the Half-Reaction Method
• 11.1.4 The Activity Series of the Elements
• 11.1.5 CIA Demonstration: The Reaction Between Al and Br2
• Chapter 11 Homework
• Chapter 11 Practice Test
• Chapter 11 Test
• Practice Midterm Exam
• Midterm Exam
• 12.1.1 An Introduction to Intermolecular Forces and States of Matter
• 12.1.2 Intermolecular Forces
• 12.2.1 Properties of Liquids
• 12.2.2 CIA Demonstration: Boiling Water at Reduced Pressure
• 12.2.3 Vapor Pressure and Boiling Point
• 12.2.4 Molecular Structure and Boiling Point
• 12.2.5 Phase Diagrams
• 12.2.6 CIA Demonstration: Boiling Water in a Paper Cup
• 12.3.1 Types of Solids
• 12.3.2 CIA Demonstration: The Conductivity of Molten Salts
• 12.3.3 Crystal Structure
• 12.3.4 Calculating Atomic Mass and Radius from a Unit Cell
• 12.3.5 Crystal Packing
• Chapter 12 Homework
• Chapter 12 Practice Test
• Chapter 12 Test
• 13.1.1 Types of Solutions
• 13.1.2 Molarity and the Mole Fraction
• 13.1.3 Molality
• 13.1.4 Energy and the Solution Process
• 13.2.1 Temperature Change and Solubility
• 13.2.2 Extractions
• 13.2.3 Pressure Change and Solubility
• 13.3.1 Vapor Pressure Lowering
• 13.3.2 Boiling Point Elevation and Freezing Point Depression
• 13.3.3 Boiling Point Elevation Problem
• 13.3.4 Osmosis
• 13.3.5 Colligative Properties of Ionic Solutions
• Chapter 13 Homework
• Chapter 13 Practice Test
• Chapter 13 Test
• 14.1.1 An Introduction to Reaction Rates
• 14.1.2 Rate Laws: How the Reaction Rate Depends on Concentration
• 14.1.3 Determining the Form of a Rate Law
• 14.2.1 First-Order Reactions
• 14.2.2 Second-Order Reactions
• 14.2.3 A Kinetics Problem
• 14.3.1 The Collision Model
• 14.3.2 The Arrhenius Equation
• 14.3.3 Using the Arrhenius Equation
• 14.4.1 Defining the Molecularity of a Reaction
• 14.4.2 Determining the Rate Laws of Elementary Reactions
• 14.4.3 Calculating the Rate Laws of Multi-step Reactions
• 14.4.4 Steady State Kinetics
• 14.5.1 Catalysts and Types of Catalysts
• 14.5.2 A Word About Laboratory Safety
• 14.5.3 CIA Demonstration: Elephant Snot
• 14.5.4 CIA Demonstration: The Cobalt(II)-Catalyzed Reaction of Potassium Sodium Tartrate
• 14.5.5 CIA Demonstration: The Copper-Catalyzed Decomposition of Acetone
• Chapter 14 Homework
• Chapter 14 Practice Test
• Chapter 14 Test
• 15.1.1 The Concept of Equilibrium
• 15.1.2 The Law of Mass Action and Types of Equilibrium
• 15.1.3 Converting Between Kc and Kp
• 15.2.1 Approaching Chemical Equilibrium
• 15.2.2 Predicting the Direction of a Reaction
• 15.2.3 Strategies for Solving Equilibrium Problems
• 15.2.4 Solving Problems Far from Equilibrium
• 15.2.5 An Equilibrium Problem Using the Quadratic Equation
• 15.3.1 Le Châtelier's Principle
• 15.3.2 The Effect of Changing Amounts on Equilibrium
• 15.3.3 The Effects of Pressure and Volume on Equilibrium
• 15.3.4 The Effects of Temperature and Catalysts on Equilibrium
• 15.3.5 CIA Demonstration: NO2/N2O4
• 15.3.6 CIA Demonstration: Shifting the Equilibrium of FeSCN2+
• Chapter 15 Homework
• Chapter 15 Practice Test
• Chapter 15 Test
• 16.1.1 Arrhenius/Brønsted-Lowry Definitions of Acids and Bases
• 16.1.2 Hydronium, Hydroxide, and the pH Scale
• 16.2.1 Strong Acids and Bases
• 16.2.2 CIA Demonstration: Natural Acid-Base Indicators
• 16.2.3 Weak Acids
• 16.2.4 Weak Bases
• 16.2.5 Lewis Acids and Bases
• 16.2.6 Trends in Acid and Base Strengths
• Chapter 16 Homework
• Chapter 16 Practice Test
• Chapter 16 Test
• 17.1.1 Strong Acid-Strong Base and Weak Acid-Strong Base Reactions
• 17.1.2 Strong Acid-Weak Base and Weak Acid-Weak Base Reactions
• 17.1.3 The Common Ion Effect
• 17.2.1 An Introduction to Buffers
• 17.2.2 CIA Demonstration: Buffers in Action
• 17.2.3 Acidic Buffers
• 17.2.4 Basic Buffers
• 17.2.5 The Henderson-Hasselbalch Equation
• 17.3.1 Strong Acid-Strong Base Titration
• 17.3.2 CIA Demonstration: Barium Hydroxide-Sulfuric Acid Titration
• 17.3.3 Weak Acid-Strong Base Titration
• 17.3.4 Polyprotic Acid-Strong Base Titration
• 17.3.5 Weak Base-Strong Acid Titration
• 17.3.6 Acid-Base Indicators
• 17.4.1 The Solubility Product Constant
• 17.4.2 CIA Demonstration: Silver Chloride and Ammonia
• 17.4.3 Solubility and the Common Ion Effect
• 17.4.4 Fractional Precipitation
• Chapter 17 Homework
• Chapter 17 Practice Test
• Chapter 17 Test
• 18.1.1 Spontaneous Processes
• 18.2.1 Entropy and the Second Law of Thermodynamics
• 18.2.2 Entropy and Temperature
• 18.3.1 Gibbs Free Energy
• 18.3.2 Standard Free Energy Changes of Formation
• 18.4.1 Enthalpy and Entropy Contributions to K
• 18.4.2 The Temperature Dependence of K
• 18.4.3 Free Energy Away from Equilibrium
• Chapter 18 Homework
• Chapter 18 Practice Test
• Chapter 18 Test
• 19.1.1 Reviewing Oxidation-Reduction Reactions
• 19.2.1 Electrochemical Cells
• 19.2.2 Electromotive Force
• 19.2.3 Standard Reduction Potentials
• 19.2.4 Using Standard Reduction Potentials
• 19.2.5 The Nernst Equation
• 19.2.6 Electrochemicamical Determinants of Equilibria
• 19.3.1 Batteries
• 19.3.2 CIA Demonstration: The Fruit-Powered Clock
• 19.4.1 Corrosion and the Prevention of Corrosion
• 19.5.1 Electrolytic Cells
• 19.5.2 The Stoichiometry of Electrolysis
• Chapter 19 Homework
• Chapter 19 Practice Test
• Chapter 19 Test
• 20.1.1 The Nature of Radioactivity
• 20.1.2 The Stability of Atomic Nuclei
• 20.1.3 Binding Energy
• 20.2.1 Rates of Disintegration Reactions
• 20.2.2 Radiochemical Dating
• 20.3.1 Nuclear Fission
• 20.3.2 Nuclear Fusion
• 20.3.3 Applications of Nuclear Chemistry
• Chapter 20 Homework
• Chapter 20 Practice Test
• Chapter 20 Test
• 21.1.1 Metallurgical Processes
• 21.1.2 The Band Theory of Conductivity
• 21.1.3 Intrinsic Semiconductors
• 21.1.4 Doped Semiconductors
• 21.2.1 The Alkali Metals
• 21.2.2 The Alkaline Earth Metals
• 21.2.3 Aluminum
• 21.2.4 CIA Demonstration: The Reaction Between Al and Br2
• Chapter 21 Practice Test
• Chapter 21 Test
• 22.1.1 General Properties of Nonmetals
• 22.1.2 Hydrogen
• 22.2.1 General Properties of Carbon
• 22.2.2 Silicon
• 22.3.1 Nitrogen
• 22.3.2 Phosphorus
• 22.4.1 Oxygen
• 22.4.2 CIA Demonstration: Creating Acid Rain
• 22.4.3 Sulfur
• 22.5.1 Halogens
• 22.5.2 Aqueous Halogen Compounds
• 22.6.1 Properties of Noble Gases
• Chapters 21 and 22 Homework
• Chapter 22 Practice Test
• Chapter 22 Test
• 23.1.1 CIA Demonstration: Laboratory Safety
• 23.1.2 CIA Demonstration: Chromatography
• 23.1.3 CIA Demonstration: Distillation
• 23.1.4 CIA Demonstration: Pipetting
• 23.1.5 CIA Demonstration: Dilutions
• 23.1.6 CIA Demonstration: Titrations
• 23.1.7 CIA Demonstration: Extractions
• 23.1.8 CIA Demonstration: Filtrations
• 23.1.9 CIA Demonstration: Weighing on an Analytical Balance
• 23.1.10 CIA Demonstration: Recrystallization
• Practice Final Exam
• Final Exam