Chemistry I. Chemistry Theory A. John Dalton developed the theory that mass is not created or destroyed B.William Cooke developed a cathode ray that proved particles are charged C. Robert Milliken used an oil drop experiment to measure charge to mass ratio D. Joseph John Thompson discovered electrons E. Ernest Rutherford developed a gold foil experiment that proved atoms had empty space II. Types of Radiation A. Alpha Radiation occurs when particles made of two protons and two neutrons are released (He2+ atoms) B. Beta Radiation occurs when an atom emits electrons C. Gamma Rays are when matterless particles are released III. The Quantum Theory A. Waves 1. Smaller waves move faster 2. Speed of waves is measured by frequency B. Light is electromagnetic radiation or wave-like behavior that travels through space C. Wavelength is the shortest distance between equivalent points on a continuous wave D. Frequency is the number of waves that pass at a given point per second E. Amplitude is the wave’s height from origin to crest F. the Speed of Light is 3.00 * 108 m/s 1. It is measured with the equation C = λ * ν G. Quanta are a specific amount of energy that matter can gain or lose H. A Quantum is the minimum amount of energy that can be gained or lost by an atom I. Planck’s Constant (6.626 * 10-34) can be used to determine the energy of a quantum 1. It is used in the equation EQuantum = h * ν J. Light is emitted in particles called photons K. Ground State is the lowest allowed energy level in an atom L. Atoms enter an Excited State when they gain energy M. Niels Bohr suggested that electrons orbit the nucleus in certain spheres called quantum levels (Each has a number assigned to it from 1 to 7) N. The release of energy 1. When an electron falls to the 1st quantum level UV light is released 2. When an electron falls to the 2nd quantum level visible light is released 3. When an electron falls to the 3rd quantum level Infrared light is released O. n=1 (Lyman Series) n=2 (Balmer Series) and n=3 (Paschen Series) are the levels P. Louis de Brogile hypothesized that particles have wave-like properties 1. de Brogile Equation: λ = h/mv Most of this information became know as Periodic Law VI.Q. Periodic Table Organization A. non-metals. Groups are the columns B. the Aufbau Principle states that electrons try to occupy the lowest energy orbitals C. Periods are the rows C. the D sublevel has five orbitals 4. Periodic Trends A. the P sublevel has three orbitals 3. Dmitri Mendeleev and Julius Meyer demonstrated a connection between elemental mass and the elements properties E. Octaves are the repeating pattern that occurred in every 8th element D. Erwin Schrödinger created first Quantum Mechanical Model of an Atom S. Electron Configuration is the arrangement of electrons in an atom B. John Newlands proposed an arrangement where elements were ordered by increasing atomic mass C. The second group contains Alkaline Earth Metals D. Werner Heisenberg believed that position could not be measured without disrupting movement R. Electron Behavior A. and F sublevels 1. The periodic table has metals. Moseley rearranged the table by increasing atomic number. Eventually evidence of atomic orbital was found T. Groups 3-12 are known as transitional elements VII. Valence electrons increase from left to right C. and resulted in clear patterns F. From left to right Ionization Energy increases but it will decrease from top to bottom . Noble gases (group 18) are very non-reactive G. P. the S sublevel has one orbital 2. The Elements A. Classification A. Groups 1-2 and 13-18 are know as representative elements D. the F sublevel has seven orbitals IV. Non-metals are elements that are brittle or gaseous E. From left to right Atomic Size will decrease but it will increase from top to bottom B. Alkali Metals (first group) create explosive reactions C. and metalloids B. In the 1700s. Halogens (group 17) are very reactive F. D. Electrons orbit the nucleus in S. the Pauli Exclusion Principle states that a maximum of two electrons can occupy an orbital and only if they have opposite spins V. Metalloids Contain properties of metals and non-metals VIII. Antoine Lavoisier listed and studied all the know elements of the time B. Ions in aqueous solutions that conduct electricity are Electrolytes J. Chemical Bonds are the forces that hold two atoms together C. Pi Bonds are when atoms have double or triple covalent bonds F. This allows the atoms in a compound to gain stability C. Symbols used in chemical equations 1. Diatomic Molecules are molecules made of two of the same atoms that bond to each other naturally 1. All atoms try to form the octet and become stable B. “(g)” refers to a gaseous compound 6. The positively charged ion becomes the Cation E. Color. A Coefficient is a number written before a reactant or a product that signifies the amount of the compound B. The electrons in a sea of electrons are call Delocalized Electrons N. Nitrogen. Chemical Reactions A. and Hydrogen D. so does the metal’s strength X. Sigma Bonds are when atoms have single covalent bonds E. The negatively charged ion becomes the Anion F. Gas (Bubbles). Sometimes it’s possible for atoms to ‘share’ electrons instead of ‘stealing’ them B. “→” means yields (like an equals sign) 2. Chlorine. The Law of Conservation of Mass states that the amount of atoms in the reactants of an equation must equal the amount of atoms in the product . Ionic Crystals are formed when a repeated packing of ions into a compound occurs H. Oxygen. Fluorine. Ionic Bonds form between the positive charges of one atom’s nucleus and the other atom’s electrons D. From left to right Electronegativity will increase but it will decrease from top to bottom IX. Lewis Structures are used to describe these bonds G.D. Endothermic reactions absorb heat and Exothermic Reactions release heat K. As the number of delocalized electrons increases. Iodine. Ions A. Metals are so reactive because they lose valence electrons easily G. “(s)” refers to a solid compound 4. A Word Equation states the chemical equation in ‘sentence’ format D. Balancing a Chemical Equation A. “(l)” refers to a liquid compound 5. Bromine. The strongest ionic attractions form a Crystal Lattice I. “(aq)” refers to an aqueous compound C. Covalent Bonding A. XI. Heat B. Lattice Energy is used to break apart ions L. The Electron Sea Model proposed that all metal atoms contribute their valence electrons to forming a ‘sea of electrons’ M. A Skeleton Equation uses symbols to represent the elements and operations XII. Evidence of a reaction: Light. “+” signifies the combination of two separate compounds 3. a reaction in which the atoms of one element replace the atoms of another element 1. A + O2 → AO2 C. A + BX → AX + B E. The Molar Mass is the number of grams in one mole of a substance XV. C. Single Replacement . A + B → C B. Avogadro’s Number is 6. D. Percent Mass is the percent by mass of one individual element in a compound B.XIII.An exchange of ions between two compounds dissolved in aqueous solutions 1. Combustion . Decomposition .a reaction in which one compound breaks down into two or more elements or new compounds 1. Types of Reactions A. A Molecular Formula specifies the actual number of atoms of each element in a molecule or formula unit of a compound. Double Replacement . The Mole A.a reaction in which oxygen combines with a substance and releases heat and light 1. AB → A + B D. Molecular Mass is the .022 * 1023 B.a chemical reaction in which two or more substances react to produce a single product 1. AX + BY → AY + BX\ XIV. Synthesis . A mole is the SI base unit to measure the amount of any given substance C. An Empirical Formula is the smallest whole number mole ratio of elements in a compound. Compound Formulas A.