<p>Atom and Electrons Review People Democritus – suggests the existence of atoms 400BC Dalton – first Atomic Theory 1803 (Which of his postulates are considered true/false?) Avogadro – Avogadro’s Hypothesis – volumes of gases and number of particles Goldstein – Protons (anode rays) Thomson – Electrons and charge/mass ratio of the electron (cathode ray tube) Millikan – Oil Drop and the charge and mass of an electron Rutherford – Gold Foil and the nucleus Bohr – Orbits and Energy Levels Planck/Einstein – Particulate nature of light – Quantum Mechanics – photons and quanta DeBroglie – Wavelength of moving particles Heisenberg – Uncertainty Principle – to “see” electrons you have to hit them with light Schrodinger – Orbitals not Orbits – quantum numbers etc. Chadwick – Neutrons – solves the mystery of the missing mass</p><p>The Atom Definition of the Atom Nuclear Symbols Protons / Neutrons -- Both made up of quarks. Therefore both are hadrons. Atomic Number / Mass Number / Isotopes Electrons / Ions – How are they formed (cations and anions) The AMU / Atomic Mass / Average Atomic Mass The Periodic Table / Groups / Periods / Metals / Nonmetals / Metalloids What does “fundamental” mean? Which particles inside the atom are fundamental? What is a hadron? What is a quark?</p><p>Light and Light Math Spectrum of Electromagnetic Radiation Wavelength, Frequency, Energy – how are all of these related to each other? Inversely?? Directly?? 3 key equations: ______Quantum Mechanics – Energy comes in little quantifiable packets called quanta or photons (in the case of light) Alpha, Beta, Gamma Radiation Emission Spectrum vs. Absorbance Spectrum</p><p>Electrons in the Atom Can you label a Periodic Table for use with electron configurations? Energy Levels / Shells (energy level = n) Sublevels / Subshells (# sublevels in an energy level = n) Orbitals – shapes and number of each type in an energy level (# orbitals in an energy level = n2) Electrons – (# electrons which can fit in an energy level = 2n2) Degenerate Orbitals How are Hydrogen’s energy levels and sublevels different than all other atoms?</p><p>Quantum Numbers (n l ml ms) : What are they? What do they indicate? Orbital Diagrams Aufbau Principle / Pauli Exclusion Principle / Hund’s Rule Exceptions to Aufbau Principle (Where do we find these elements?) Electron Configurations Ground State vs. Excited State Configurations (How can electrons be excited?) Paired and unpaired electrons Shorthand Configurations / Valence Configurations Configurations of ions Isoelectronic ions/atoms. Dot Diagrams and Valence Electrons Magnetic vs Nonmagnetic Metals</p>