Flame Test, Electro Configuration火焰测试，电子组态.ppt

* * * * * * * The three 2p orbitals, 2px, 2py, 2pz x y z Once the 1s orbital is filled… The 2s orbital begins to fill Once the 2s orbital is filled… The 2p orbitals begin to fill Each 2p orbital intersects the 2s orbital and the 1s orbital Each 2p orbital gets one electron before pairing begins Once each 2p orbital is filled with a pair of electrons, then… The 3s orbital gets the next two electrons The 3s electrons have a higher energy than 1s, 2s, or 2p electrons 3s electrons are generally found further from the nucleus than 1s, 2s, or 2p electrons Exit Ticket Explain the mechanism behind different colored fireworks * * * * * * * * * * * * * * * * * * * * Flame Test, Electron Configuration Warm - Up What is a photon? How can we identify elements based on their emission spectrum? What is the Photoelectric Effect? Why do we say that light has a dual nature? Objective Today I will be able to: Analyze the emission of energy in metals by completing a flame test Calculate the electron configuration for elements on the periodic table Homework Electron Configuration Practice Agenda Warm – Up Flame Test Lab Electron Configuration Notes Electron Configuration Practice Exit Ticket Electron Configuration Electron Configuration Electron configuration – arrangement of electrons in an atom Electrons try to populate the lowest energy levels available – “ground state” Arrangement of Energy Levels Principal energy levels – represented by n As atoms get bigger, there are more electrons, therefore more energy levels Within each energy level, we have one or more sublevels These sublevels are made up of orbitals Energy Levels on the Periodic Table Orbitals According to modern atomic theory electrons are found in orbitals Orbital – 3-D region around the nucleus indicating the probable location of the electron There are 4 types of orbitals where the electrons can be found – s,p,d,f Order of energy from lowest to highest: s, p, d, f 3-D images of the orbitals Energy Sublevels Each