Introduction
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What Is Chemistry?
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Scientific Method
Measurement
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Quantitative and Qualitative
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Units of Measurement
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Unit Conversions
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Temperature Scales
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SI System of Measurement
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Significant Figures
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Scientific Notation
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Accuracy, Precision, and Percent Error
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Density
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Graphing: independent and dependent variables
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Drawing Graphs
Matter
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What is Matter?
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Everything is Made of Atoms
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Elements
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Phase Changes
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Separating Mixtures
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Physical and Chemical Changes
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Basic Atomic Structure
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Atomic Number
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Isotopes
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Atomic Mass
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Phases of Matter
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Compounds
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Mixtures
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Mass Number
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Net Charge
The Periodic Table
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The Periodic Table
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Metals and Nonmetals
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Periodic Trends in Atomic Size
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Periodic Trends in Ionic Size
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Periodic Trends in Ionization Energy
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Periodic Trends in Electronegativity
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Periodic Trends in Electron Affinity
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Valence Electrons
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Metalloids
Bonding Basics
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Bonding
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Octet Rule
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Electronegativity
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Ionic Bonding
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Properties of ionic, covalent, and metallic compounds
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Covalent Bonding
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Metallic Bonding
Ionic Bonds
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Ionic Bond Formation
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Ionic Compounds
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Polyatomic Ions
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Writing Ionic Formulas
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Naming Ionic Compounds
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Ionic vs. Molecular Bonds
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Covalent compounds
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Metallic Compounds
Covalent Bonds
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Covalent Bond Formation
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Covalent Formulas and Nomenclature
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Drawing Lewis Structures
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Resonance
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VSEPR
Intermolecular Bonding
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Intermolecular Bonds
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Polarity of Bonds
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Polarity of Molecules
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Hydrogen Bonds
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Dipole-Dipole Interactions
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Van der Waals Interactions
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Properties of Intermolecular Bonds
A Closer Look at The Atom
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Atomic Models
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Mass Conservation
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Laws of Proportions
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Cathode Ray Tube Experiment
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Millikan's Oil Drop Experiment
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Rutherford's Gold Foil Experiment
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Discovery of the Neutron
Bohr Model of the Atom
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Transverse waves
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Light and Electromagnetic Radiation
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Calculations with wavelength and frequency
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Planck's constant
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Atoms and Electromagnetic Spectra
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Excited States and Ground States
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Bohr Model of the atom
Quantum Mechanical Model of the Atom
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The Dual Nature of Light
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DeBroglie: Wave Characteristics of Matter
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Orbitals, and Probability Patterns
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Heisenberg Uncertainty Principle
Electron Configuration
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s,p,d,f Orbitals
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Noble Gas Shorthand
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Quantum Numbers
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Valence Electrons
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Electron Configuration
Molecular Orbital Theory
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Molecular Orbital Theory
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Sigma Bonds
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Molecular Geometry
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Bonding and Antibonding Orbitals
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Orbital Hybridization
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Pi Bonds
Chemical Reactions
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Review of Elements and Compounds
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Chemical and Physical Properties
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Chemical Equations
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Balancing Chemical Equations
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Chemical Reactions and Equations
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Synthesis Reactions
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Decomposition Reactions
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Single Replacement Reactions
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Double Replacement Reactions
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Redox Reactions
The Mole Concept
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The Mole
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Determining Formula
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Percent Composition
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Empirical and Molecular Formulas
Stoichiometry
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Stoichiometry
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Mole Ratios
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Equation Stoichiometry
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Limiting Reagent
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Percent Yield
Phases of Matter
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Phases of Matter
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Properties of Solids, Liquids, and Gases
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Intermolecular Forces of Attraction
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How Intermolecular Forces Affect Phases of Matter
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Changes of State
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Dynamic Equilibrium
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Vapor Pressure and Boiling
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Phase Diagrams
Gases
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Kinetic Theory of Gases
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Gas Pressure
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Measuring Gas Pressure
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Atmospheric Pressure
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Absolute Zero
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Gas Laws
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Ideal Gas Law
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Molar Volume of a Gas
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Gas Stoichiometry
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Partial Pressure
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Boyle's Law
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Charles' Law
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Avogadro's Law
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Gay Lussac's Law
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Combined Gas Law
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Preparation and Reactions of Gases
Solutions
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Solutions
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Solution Formation
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Solvation and Dissociation
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Saturated and Supersaturated Solutions
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Measuring Concentration
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Molarity
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Molality
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Percent Concentration
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Dilution Calculations
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Factors Affecting Solubility
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Solubility Graphs
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Colligative Properties
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Separating Mixtures
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Osmolarity
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Solute
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Solvent
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Solving Using PPM (Parts Per Million)
Chemical Kinetics
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Rate of Reactions
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Collision Theory
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Potential Energy Diagrams
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Rate Law
Chemical Equilibrium
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Dynamic Equilibrium
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Equilibrium Constants
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Equilibrium Stoichiometry
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Le Chatelier's principle
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Solubility Equilbria
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Ksp
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Kep
Acids and Bases
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Acids and Bases
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Properties of Acids and Bases
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Arrhenius Acids and Bases
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pH
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pH calculations
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Intermolecular Forces of Attraction
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Stoichiometry with Acid and Base Dissociation
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Conjugate Acids and Conjugate Bases
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Brønsted–Lowry Acids and Bases
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Lewis Acids and Bases
Reactions in Solution
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Reactions Between Ions in Solutions
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Stoichiometry of Reactions Between Ions in Solutions
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Neutralization
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Titration Calculations
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Buffer Theory
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Buffer Calculations
Thermochemistry
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Energy Change in Reactions
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Enthalpy
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Exothermic processes
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Specific Heat
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Calorimetry
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Thermochemistry of Phase Changes
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Thermochemistry with Equation Stoichiometry
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Hess' Law
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Spontaneous and Non-Spontaneous Processes
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Entropy
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Gibbs Free Energy
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Endothermic processes
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Born-Haber Cycle - Formation
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Born-Haber Cycle - Solution
Electrochemistry
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Oxidation and Reduction Reactions
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Oxidation Numbers
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Balancing Redox Equations Using the Oxidation Number Method
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Metal Activity Series
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Galvanic Cells
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Electrolysis
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Calculating Energy in Electrochemical Processes
Nuclear Chemistry
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Nuclear Chemistry
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Isotope Notation
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Isotope Stability
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Alpha Decay
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Beta Decay
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Positron Decay
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Electron Capture
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Nuclear Equations
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Nuclear Half-Life
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Nuclear Half-Life Calculations
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Nuclear Transmutation
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Fission and Fusion
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Applications of Nuclear Chemistry
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Biological Effects of Radiation
Organic Chemistry
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Introduction to Carbon Chemistry
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Naming Alkanes, Alkenes, and Alkynes
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Aromatics
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Functional Groups and Naming
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Biochemical Molecules
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Polymer Chemistry
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Isomerisms
Useful Analysis Tips
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Using Microsoft Excel for Figures and Statistical Analysis
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Using Microsoft Excel to Analyze Data Using Linear Regression
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Correct Use of a Scientific Notation on a Scientific Calculator
Uncategorized Questions
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Question #e1f0a
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Question #14194
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Question #8bcb2
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Question #60254
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Question #b6324
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Question #08b63
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Question #57859
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Question #c3d89
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In #"PbS"(s) + 4"H"_2"O"_2(aq) -> "PbSO"_4(s) + 4"H"_2"O"(l)#, what was oxidized and what was reduced?
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Question #921da
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Question #1355e
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Question #555cb
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Question #5563e
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Question #a33e0
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You have 75.0 grams of C2H2Cl4, how many L of Cl2 do you have?
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Question #8c016
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Are alkyl groups and radicals the same? For example aldehydes R-CHO.
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Question #b93ef
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Why does the double bond in alkenes make them more reactive than alkanes, which are single-bonded?
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The initial concentration of Compound A is 1.5 mol/L. It disappears in a zero-order reaction with a rate constant of #"0.2 mol·L"^"-1""s"^"-1"#. What is its concentration after 15 s?
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Question #4fed1
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0.10 mol of solid sodium hydrogen carbonate and 0.20 mol of solid sodium carbonate are dissolved in the same beaker of water, transferred to a volumetric flask and made to 250.0 mL. The Ka for HCO3 - is 4.7 x 10-11.
What is the pH of the resulting buffer?
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Question #36243
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Question #a37af
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Question #9f4ad
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Question #b6c73
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Question #a2afa
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Question #25589
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Question #c03da
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What is the molar mass of an element?
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Question #6f8e9
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Question #86d62
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Question #26fe8
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Why does the octet rule exist?
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Question #a53c0
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What are delocalized electrons?
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How is the law of definite composition related to the law of multiple proportions?
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If two oil drops can be held motionless in a Millikan oil-drop experiment, would the ratios of what two properties of the drops have to be equal?
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Question #13f80
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Why is the uncertainty principle not significant when describing the behavior of macroscopic objects, but it is very significant when describing the behavior of electrons?
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Question #a20b0
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Question #d4bcc
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Question #a6569
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Question #d4f79
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What phase of matter is peanut butter?
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Question #ccd7d
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Question #2a41e
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Question #ccf13
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Question #92ebe
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What are allotropes?
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Question #e896b
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A salt solution has a concentration of 2.4%w/v. What is the concentration if 10.0 mL of this solution is diluted to a total volume of 60.0 mL?
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Question #bf3dc
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Question #bf5b6
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Question #95aa0
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Question #7add1
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Question #85a0f
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Question #7ade8
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How can the rate law be determined?
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What is an example of a rate law practice problem?
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What is the neutralization reaction with the combination H3BO3 and BaOH?
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How does pH affect titration?
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How does enthalpy affect solubility?
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Why is heat capacity different for different materials?
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Question #e98d7
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Question #e98dc
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Question #7b4e4
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Question #9b627
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Why is the Hess' law important in physics?
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Which biomolecules are insoluble in water?
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Question #9684e
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Question #94985
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Question #07f46
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How do you solve for V2, using Avogadro's Law when moles of a gas are added(n2)?
A sample containing 7.20g O2 gas has a volume of 35.0L. Pressure and temperature remain constant. What is the new volume if 0.800mole O2 gas is added?
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Question #96ade
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Question #96d44
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How does uncertainty apply to chemists?
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Question #1cc3d
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Question #ab82c
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Question #d4b59
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What is the structure of L(+) Glucose and L(-) Glucose? What does +, -, and L tell you?
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Question #1adf2
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How do I write the formula units of ionic compounds?
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Question #5a652
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Question #3c8f0
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Question #f8480
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Question #4b705
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Question #1aff0
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Question #f8633
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Why are ideas on the nature of matter different from those held 200 years ago, and different from those held 2500 years ago?
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Question #09dee
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The temperature measured in an experiment was #"64.9"^@"C"#. The theoretical temperature is #"55.0"^@"C"#. What is the percent error?
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Question #70765
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Is the dissolution of sodium chloride in water a physical or chemical change?
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Why does an endothermic reaction occur?
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Question #347fb
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Question #fd9f0
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How do functional groups affect organic molecules?
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Question #34c15
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Question #fdf26