Chemistry
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Introduction
- What Is Chemistry?
- Scientific Method
- Quantitative and Qualitative
- Units of Measurement
- Unit Conversions
- Temperature Scales
- SI System of Measurement
- Significant Figures
- Scientific Notation
- Accuracy, Precision, and Percent Error
- Density
- Graphing: independent and dependent variables
- Drawing Graphs
- What is Matter?
- Everything is Made of Atoms
- Elements
- Phase Changes
- Separating Mixtures
- Physical and Chemical Changes
- Basic Atomic Structure
- Atomic Number
- Isotopes
- Atomic Mass
- Phases of Matter
- Compounds
- Mixtures
- Mass Number
- Net Charge
- The Periodic Table
- Metals and Nonmetals
- Periodic Trends in Atomic Size
- Periodic Trends in Ionic Size
- Periodic Trends in Ionization Energy
- Periodic Trends in Electronegativity
- Periodic Trends in Electron Affinity
- Valence Electrons
- Metalloids
- Bonding
- Octet Rule
- Electronegativity
- Ionic Bonding
- Properties of ionic, covalent, and metallic compounds
- Covalent Bonding
- Metallic Bonding
- Ionic Bond Formation
- Ionic Compounds
- Polyatomic Ions
- Writing Ionic Formulas
- Naming Ionic Compounds
- Ionic vs. Molecular Bonds
- Covalent compounds
- Metallic Compounds
- Covalent Bond Formation
- Covalent Formulas and Nomenclature
- Drawing Lewis Structures
- Resonance
- VSEPR
- Intermolecular Bonds
- Polarity of Bonds
- Polarity of Molecules
- Hydrogen Bonds
- Dipole-Dipole Interactions
- Van der Waals Interactions
- Properties of Intermolecular Bonds
- Atomic Models
- Mass Conservation
- Laws of Proportions
- Cathode Ray Tube Experiment
- Millikan's Oil Drop Experiment
- Rutherford's Gold Foil Experiment
- Discovery of the Neutron
- Transverse waves
- Light and Electromagnetic Radiation
- Calculations with wavelength and frequency
- Planck's constant
- Atoms and Electromagnetic Spectra
- Excited States and Ground States
- Bohr Model of the atom
- The Dual Nature of Light
- DeBroglie: Wave Characteristics of Matter
- Orbitals, and Probability Patterns
- Heisenberg Uncertainty Principle
- s,p,d,f Orbitals
- Noble Gas Shorthand
- Quantum Numbers
- Valence Electrons
- Electron Configuration
- Molecular Orbital Theory
- Sigma Bonds
- Molecular Geometry
- Bonding and Antibonding Orbitals
- Orbital Hybridization
- Pi Bonds
- Review of Elements and Compounds
- Chemical and Physical Properties
- Chemical Equations
- Balancing Chemical Equations
- Chemical Reactions and Equations
- Synthesis Reactions
- Decomposition Reactions
- Single Replacement Reactions
- Double Replacement Reactions
- Redox Reactions
- The Mole
- Determining Formula
- Percent Composition
- Empirical and Molecular Formulas
- Stoichiometry
- Mole Ratios
- Equation Stoichiometry
- Limiting Reagent
- Percent Yield
- Phases of Matter
- Properties of Solids, Liquids, and Gases
- Intermolecular Forces of Attraction
- How Intermolecular Forces Affect Phases of Matter
- Changes of State
- Dynamic Equilibrium
- Vapor Pressure and Boiling
- Phase Diagrams
- Kinetic Theory of Gases
- Gas Pressure
- Measuring Gas Pressure
- Atmospheric Pressure
- Absolute Zero
- Gas Laws
- Ideal Gas Law
- Molar Volume of a Gas
- Gas Stoichiometry
- Partial Pressure
- Boyle's Law
- Charles' Law
- Avogadro's Law
- Gay Lussac's Law
- Combined Gas Law
- Preparation and Reactions of Gases
- Solutions
- Solution Formation
- Solvation and Dissociation
- Saturated and Supersaturated Solutions
- Measuring Concentration
- Molarity
- Molality
- Percent Concentration
- Dilution Calculations
- Factors Affecting Solubility
- Solubility Graphs
- Colligative Properties
- Separating Mixtures
- Osmolarity
- Solute
- Solvent
- Solving Using PPM (Parts Per Million)
- Rate of Reactions
- Collision Theory
- Potential Energy Diagrams
- Rate Law
- Dynamic Equilibrium
- Equilibrium Constants
- Equilibrium Stoichiometry
- Le Chatelier's principle
- Solubility Equilbria
- Ksp
- Kep
- Acids and Bases
- Properties of Acids and Bases
- Arrhenius Acids and Bases
- pH
- pH calculations
- Intermolecular Forces of Attraction
- Stoichiometry with Acid and Base Dissociation
- Conjugate Acids and Conjugate Bases
- Brønsted–Lowry Acids and Bases
- Lewis Acids and Bases
- Reactions Between Ions in Solutions
- Stoichiometry of Reactions Between Ions in Solutions
- Neutralization
- Titration Calculations
- Buffer Theory
- Buffer Calculations
- Energy Change in Reactions
- Enthalpy
- Exothermic processes
- Specific Heat
- Calorimetry
- Thermochemistry of Phase Changes
- Thermochemistry with Equation Stoichiometry
- Hess' Law
- Spontaneous and Non-Spontaneous Processes
- Entropy
- Gibbs Free Energy
- Endothermic processes
- Born-Haber Cycle - Formation
- Born-Haber Cycle - Solution
- Oxidation and Reduction Reactions
- Oxidation Numbers
- Balancing Redox Equations Using the Oxidation Number Method
- Metal Activity Series
- Galvanic Cells
- Electrolysis
- Calculating Energy in Electrochemical Processes
- Nuclear Chemistry
- Isotope Notation
- Isotope Stability
- Alpha Decay
- Beta Decay
- Positron Decay
- Electron Capture
- Nuclear Equations
- Nuclear Half-Life
- Nuclear Half-Life Calculations
- Nuclear Transmutation
- Fission and Fusion
- Applications of Nuclear Chemistry
- Biological Effects of Radiation
- Introduction to Carbon Chemistry
- Naming Alkanes, Alkenes, and Alkynes
- Aromatics
- Functional Groups and Naming
- Biochemical Molecules
- Polymer Chemistry
- Isomerisms
- Using Microsoft Excel for Figures and Statistical Analysis
- Using Microsoft Excel to Analyze Data Using Linear Regression
- Correct Use of a Scientific Notation on a Scientific Calculator
- How do we use stable isotopes in science?
- What is radioactive dating?
- Does the following reaction show an increase or decrease in entropy? H2O(l) ---> H2O(s)
- How do gas laws apply to scuba diving?
- How do gas laws affect hot air balloons?
- What are some common mistakes students make when naming Alkanes?
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- Does hydrogen bonding have a directional character?
- How is hydrogen bonding among water molecules related to the structure of the water molecule?
- How many valence electrons would an element with the atomic number 113 have?
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- What is an example of an electron orbital practice problem?
- Why is it impossible to predict exactly where an electron is at a given moment?
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- How can the low vapor pressure of water be explained?
- What transverse wave can travel in a vacuum?
- How do transverse waves transfer energy?
- Is the dissociation of water endothermic?
- Why do the properties of elements change in regular pattern across a period?
- What are synthesis reactions?
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- How are atomic size and electronegativity related?
- When a full glass of water covered by a thin piece of cardboard is inverted, the cardboard remains in place. Why does this happen?
- What happens to the partial pressure of oxygen in the air if the air temperature is increased?
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- How do I prepare 1 L of 2 mol/L phenylmagnesium bromide?
- ΔHoreaction=∑ΔHof(products)−∑ΔHof(Reactants) --> What exactly is happening in this equation?
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- Why is thermochemistry important?
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- How can I find the molecular formula from molar mass?
- How can I calculate wavelength given frequency?
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- What physical properties does oil have?
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- How does a covalent bond form?
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- What do the subscripts mean in a chemical formula?
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- What is a supersaturated solution?
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