Glossary Glossary
Periodic Table A colorful periodic table
Periodic table with isotope calculator
Another colorful periodic table
A third colorful periodic table
Periodic Table with x-ray properties
Index Index Chemistry Sites
Dictionary physics and chemistry
Calculator Calculator
Calculator especially within chemistry
Algebra Review Refresh your Algebra
Graphing Make your own graphs
Dependent and independent variables
Units Different units used
SI Units SI definition
Derived or Non-SI units Derived SI units
SI Prefixes SI-prefixes
Significant Figures What are significant figures
Theoretical Yield : The maximum amount of product that can, according to chemical reactions, be obtained from a known amount of reactants. Cannot reach theoretical yield in reality, instead find percent yield.
Percent error Percent error
Dimensional Analysis : A method for solving conversion type problems Dimensional Analysis
More Dimensional Analysis with Quizzes
Accuracy : The measure of agreement between your average of measurements and the correct value What is Accuracy
Precision : The closeness of agreement among repeated measurements What is Precision
What is the difference between accuracy and precision
Scientific Notation (exponential notation) Scientific Notation
Statistics Statistics Calculator
Scientific Method Science on trial
More and more about the Scientific Method
More about the Scientific Method
Further about the Scientific Method
How and Why the Scientific Method
In depth about the Scientific Method
Famous phrases about the Scientific Method
Observations
Hypothesis Hypothesis
Law Law
Theory Theory
Matter What is matter
Mass and Weight Mass and Weight conversion
States Explanation of rigidity
| Rigidity | Expansion on heating | Compressibility | |
| Solid Solids | Rigid | Slight | Slight |
| Liquid Liquids | Flows, shapes as container | Slight | Slight |
| Gas Gases | Fills container completely | Indefinite | Easily |
Pure Substances : Separable only by chemical reactions What are pure substances
| Metals are generally: What are metals | solid (except Mercury), hard (except the alkali's), have high melting- and boiling points, opague ("nonseethrough"), lustrous, reflect light, conduct heat, high density, malleable, ductile and strong. |
| Nonmetals are generally: What are non metals | gases, liquids, low melting of solids (except Carbon as a diamond), transparent ("seethrough"), translucent (lets light through it), dull, absorb light, low density (except diamond), insulator of heat and electricity (except Carbon as graphite and Iodine). |
| Semiconductors (metalloids) What are semiconductors | They have the physical properties of metals, and the chemical properties of nonmetals. |
Mixtures : Has a variable composition, can be separated by physical or chemical means. What is a mixture
Molecule : The smallest particle of a substance that is capable of a stable, independent existence. What is a molecule
Extensive : Depends on the amount of the substance Extensive Variables
Intensive : Does not depend on the amount of the substance.Intensive Variables
Chemical : It is a characteristic that can be observed only by a reaction with another substance ex a mix that explodes. What is a chemical change
Physical : It is a characteristic that can be observed without changing the identity of the substance ex melting. What is a physical change
Colligative : It has values that depend only on the number of solute particles in a solution and not on the identity of the particles. Exercise Colligative properties
What is colligative properties
Temperature Temperature is.. and it's unitsTemperature and water What is Negative temperaure
Fahrenheit to Celsius Conversion
Fahrenheit to Celsius or vice versa with Kelvin included
Difference Temperature and Heat: Temperature is an intensive property, heat is an extensive property. Temperature is the intensity of heat. Heat is energy that is transferred between samples of matter because of the difference in temperature.
System and surroundings System and Surroundings
Force What is force
Energy Energy is..and it's units
Kinetic : Energy of motion, KE = 1/2 mv², m=mass, v=velocity Kinetic energy
Potential : Stored energy, PE = mgh, m=mass, g=gravitational force, h=height Potential energy
Law of Conservation of Energy What is the Law of Conservation of Energy
Exothermic : The system absorbs energy. (-) Exothermic
Endothermic : The system gives up energy. (+) Endothermic
Calorimetry
Heat Heat
Specific Heat : The amount of heat required to raise the temperature of 1 gram ofa substance by 1 · C. This is an intensive property.Exercise Specific Heat
Electric Charges Electric charges
Atom : The smallest particle of an element that retains the identity of the element What is an atom
NucleusWhat is the nucleus
Atomic Number About atomic number
Mass Number, amu Amu
Isotopes Isotopes
Daltons Atomic Theory What is Daltons Atomic Theory
More about Dalton's atomic theory
The Rutherford Model
The Bohr Model
Orbital model (or quantum-mechanical model)
Particle Theory (or Wave theory) Wave Theory
Quanta or photons
Wavelength What is Wavelength
More equations about Wavelength
Relation wavelength and frequency
Frequency What is Frequency
Relation frequency and wavelength
More equations about Frequency
Wave velocity Equations about wave velocity
Planck
Spectra
Radiation
IUPAC IUPAC
Stock systemStock system
Ionic Ionic nomenclature
Molecular Molecular nomenclature
Acids Acid nomenclature
Organic Alkanes, alkenes, alkynes
| Structural | Shows the bonding relationship. ex H-O-O-H |
| Molecular Molecular formula | Tells how many of each kind of atom in the molecule that are present, only has meaning when dealing with discrete molecules, must know molar mass to find molecular formula given the empircal formula.ex H2O2 |
| Empirical Empirical formula | Tells what kinds of atoms are present, and gives the simplest whole number ratio of atoms in the compound, and are often unique.ex HO |
Limiting Reagent : The reagent or reactant that is completely consumed in a reaction.Limiting Reagent
Monatomic
Diatomic
Analysis
Ionic Compounds : This substance has positive and negative ions in such a ratio that electric neutrality is kept. When the compound is dissolved in water, the ions move freely and conduct electricity. Ionic Formulas
Stoichiometry Stoichiometry of Acid Base Titrations
Molar Mass Molar mass
Formula Weight
Molecular Weight
Mole What is a mole of a substance
Avogadro's Number Avogadro's number
STP What is STP
Percentage composition How to calculate percentage composition
Reactants : Substances that enter in reactions. They are on the left side of the equations.
Products : Substances that are formed in reactions. They are on the right side of the equation.
Classifications
| Most Reactive | Li | Replace H2(g) from H2O(l) or acid. |
| Rb | Replace H2(g) from H2O(l) or acid. | |
| K | Replace H2(g) from H2O(l) or acid. | |
| Cs | Replace H2(g) from H2O(l) or acid. | |
| Ba | Replace H2(g) from H2O(l) or acid. | |
| Sr | Replace H2(g) from H2O(l) or acid. | |
| Ca | Replace H2(g) from H2O(l) or acid. | |
| Na | Replace H2(g) from H2O(l) or acid. | |
| Mg | Replace H2(g) from acids. | |
| Al | Replace H2(g) from acids. | |
| Mn | Replace H2(g) from acids. | |
| Zr | Replace H2(g) from acids. | |
| Cr | Replace H2(g) from acids. | |
| Fe | Replace H2(g) from acids. | |
| Cd | Replace H2(g) from acids. | |
| Co | Replace H2(g) from acids. | |
| Ni | Replace H2(g) from acids. | |
| Sn | Replace H2(g) from acids. | |
| Pb | Replace H2(g) from acids. | |
| H2(g) | Reference. | |
| Cu | Will not produce H2(g) from acids. | |
| Hg | Will not produce H2(g) from acids. | |
| Ag | Will not produce H2(g) from acids. | |
| Pt | Will not produce H2(g) from acids. | |
| Least Reactive | Au | Will not produce H2(g) from acids. |
Some Solubility Rules
Balance Chemical equations Balance Chemical Reactions
Write ionic equations
Phase changes as melting( fusion), boiling, freezing, condensation, evaporation ( takes place at the surface, when molecule escapes from the liquid) and sublimation. Phase changes
Critical temperature and pressure
Heat of condensation and vaporization
Heat of fusion
Crystals What is a crystal
Pressure = Force÷Area What is pressure
Pressure CalculatorAnother Pressure Calculator
Vapor Pressure What is Vapor Pressure
Gases Gases
Ideal Gas Law (PV = nRT, n = mass÷molarmass) What is the Ideal Gas Law
Boyle's Law What is Boyle's Law
Avogadro's Law What is Avogadro's Law
Charles's Law Charle's Law
Guy Lussac's Law of Combining Volumes What is Guy Lussac's Law
Dalton's Law of Partial Pressure : The partial pressure of each component in a mixture of gases is the pressure it would exert if it is alone occupied the total volume at the same temperature. The partial pressure of each gas is independent of the partial pressure of the other gases.Dalton's Law of Partial Pressure
Graham's Law of Diffusion Graham's Law of Diffusion
Basic Kinetic Theory, KMT (Ideal Gas) Kinetic Molecular Theory
Real Gas About real gases
Classical Mechanics versus wave mechanics
Heisenberg's Uncertainty Principle
Orbitals Atomic Orbital Theory
Quantum Numbers
Electron Configuration Electron configuration
Cathode Ray Tube Build A Cathode Ray Tube
Quantum Theory What is Quantum Mechanics
Schroedinger Equation Schroedinger Equation
Peridic Table History of the Modern Periodic Table
Moseley
Mendelev Mendelev's periodic table
Representative Elements Representative Elements
Some common representative elements
Metals Metals
Non metals Non Metals
Periods Period
Exercise about Transition elements
More about transition elements
Groups Group
Periodicity
Electron Affinity
Allotropes Allotrope pictorially
Oxygen depletion and allotropes
Metallic Bonding : A network of ions with valence electrons free to move throughout the system. A "sea" of electrons. What is metallic bonding
Ionic Bonding : Electrostatic attraction of cation (positive ion) for anion (negative ion). What is ionic bonding
Covalent Bonding : Valence electrons are shared in pairs by two atoms. This leads to a molecular crystal. What is covalent bonding
Lewis Structure Exercise Lewis Structure
Polarizability : Ease of distortion of the electron cloud. (A larger atom is more polarizable, since there are more electrons and they are further away from the nucleus, and the electron cloud is easier to distort.)
Hybridization
Molecular Orbitals Molecular Orbital Theory
Molecular Orbitals Molecules 2
Molecular Orbitals Molecules 3
Molecular Orbitals Molecules 4
Molecular Orbitals Molecules 5
Molecular Orbitals Molecules 6
Molecular Shapes (VSEPR=Valence Shell Electron Pair Repulsion Theory)
| Number of groups of electrons around the central atom | "Electron pair geometry" | Bond Angles | Number of nonbonded electron pairs | Molecular geometry | Example |
| 2 | linear | 180° | 0 | linear | CO2 |
| 3 | triangular planar | 120° | 0 | triangular planar (trigonal) | CO3²- |
| 3 | triangular planar | 120° | 1 | bent | O3 |
| 4 | tetrahedral | 109.5° | 0 | tetrahedral | CCl4 |
| 4 | tetrahedral | 109.5° | 1 | triangular pyramidal | NH3 |
| 4 | tetrahedral | 109.5° | 2 | bent | H2O |
Polar Bonds
Intermolecular forces (Van der Waal) (As the intermolecular forces increase, density increases.)
Bond Strength
Bond energy
Solutions What is a solution
Reactions in aqueous solutions
Composition of a solution by substance, volume or mass
Solute : What you dissolve Moles of a Solute
Solvent : What you dissolve the solute in
Types
Solubility Solubility
Saturation Saturation
Dilution
Molarity : Moles of solute÷Liter solution Molarity Exercises molarity
Molality (m) : moles solute÷kg solvent Molality What is MolarityExercises Molality
Equivalent
Normality : Equivalent solute÷Liter solution
Molefraction (X) = moles solute÷mol solute + mol solvent
Mass percent = Mass solute÷mass solute+mass solvent What is mass percent
Freezing and Boiling Point Depression
Kinetics What is Kinetics
Reaction Mechanism What is the Reaction Mechanism
Rate determining Step
Reaction rate controlled by What effects the rate of reaction
Reaction rate and the rate law
Activation energy What is Activation Energy
Further about activation energy
Activated Complex
Potential Energy Diagram
Collision Theory
Thermodynamics Entropy, enthalpy, Gibbs energy relating to a protein
Enthalpy (H) Ionization Enthalpy
Heat Heat
Heat of formation
Heat Capacity Heat Capacity
Specific heat capacity for water
Hess's Law Hess's Law
Spontaneity Spontaneity
Entropy (S) Enthropy
Entropy in thermodynamics at a higher level
Gibbs Free Energy, G Change in G
Calculations Gibbs free energy
Gibb's Free Energy and the third Law
Raolt's Law
First Law of Thermodynamics First law of thermodynamics
Second Law of Thermodynamics Second Law of Thermodynamics
More about the second law of thermodynamics
Table of Thermodynamic Properties Table of Thermodynamic Properties
Equilibrium : Rate of the forward reaction equals the rate of the reverse reaction. No net changes occur. The ratioof the concentrations of products to reactants tells us about the extent of the reaction. The extent of the reaction tells us about the driving force, the magnitude of Keq.About Equilibrium
Equilibrium and Reaction Rate 2
Equilibrium and Reaction Rate 3
Equilibrium and Reaction Rate 4
Reversible Reactions
Driving force Driving Force
Mass Action ExpressionThe Law of Mass Action
Le Chatelier's Principle : If a system is at equilibrium, and then is subjected to a stress, the system will respond in such a way as will tend to counteract the stress. The stress is partially relieved and a new equilibrium is established.Le Chatelier's Principle
Solubility Equilibrium
Common Ion Effect
Ionization Theory
Dissociation of:
Arrhenius Acids and Bases Arrhenius Acids and Bases
Ionization Constant Ionization Constant
More About Ionization Constants
Acid and Base Properties Strong and Weak Acids
Salts
Brønsted-Lowry Acids and Bases What are Bronsted-Lowry Acids and Bases
More About Brønsted-Lowry Acids and Bases
Conjugate Acid-Base Pairs What are Conjugate Acid-Base Pairs
Lewis Acids and Bases What are Lewis Acids and Bases
More about Lewis Acids and Bases
Amphotheric Substances Amphoteric Substances
Tables Table Monoprotic Acids Ionization Constants
Table Polyprotic Acids Ionization Constants
Logarithms and Antilogarithms Logarithms and Antilogarithms
Graphing with logarithms Graph on log paper
Graph Acid Base Titration Curves
Selfionization of Water Autoionization Constant
pH = -log (H3O+), pH + pOH = pKw = 14.00 PH
Buffers What are Buffers
IndicatorsIndicator
Neutralization
Titration Titration
Stoichiometry of Acid Base Titrations
Hydrolysis
Table Table of Indicators
Oxidation : Loss of electrons
Exercise in determination of oxidation of non metals
Oxidation states
Exercise in determination of oxidation states
Reduction : Gain of electrons. Reduction
Reduction States
Oxidation Number What are Oxidation Numbers
Rules for assigning oxidation numbers
Oxidizing Agents : Cause gain of electrons.
Reducing Agents : Cause loss of electrons.
Redox Redox for non metals
Balance Redox reactions (reactions where if one substance looses electrons, another substance must gain electrons) Balance Redox Reactions
Exercise in determining oxidation half reactions
Exercise in determining reduction half reactions
Chemical Formulas Exercise in chemical formula writing
Electrochemistry What is electrochemistry
Half reactions
Current
Conduction What are conductors, insulators and semi conductors
Electrolysis
| Anode Anode | Cathode Cathode |
| Oxidation | Reduction |
| Attract anions | Attract cations |
| Electrons leve cell | Electrons enter cell |
| Negative in VOLTAIC cell | Negative in ELECTROLYTIC cell |
| Voltaic (Galvanic) | Electrolytic |
| Positive potential | Negative potential |
| Spontaneous | Non spontaneous |
| May be used to do work | Requires outside energy source |
| Electrons travel spontaneously to positive electrode | Electrons are forced to go to the negative electrode |
Electroplating
Electrochemical Cell
Hydrogen Half cell
Standard Electrode Potential
The Half Cell The Half Cell
The dry cell The Dry Cell
Corrosion Corrosion
Exams and quizzes Practice exam 1 (atoms, moles, gases, equilibrium)
