PPT-Electron Configuration

contd Ms McGrath Chemistry 11 Aufbau principle States that in going from a hydrogen atom to a larger atom you add protons to the nucleus and electrons to orbitals You start at the orbitals having the lowest energy level and fill them in order of increasing energy until you run out of electrons. Configuration . for Elements Above Atomic # 18. Electron Shells. Periods on the periodic table are similar because they have the same number of electron shells.. Within these shells there are layers called sublevels', a shell can have between 1 and 4 sublevels.. Energies in Relation to Periodic Table. 3d. 4f. 1s. 2p. http://www.docstoc.com. Energies of Orbitals. E. Hydrogen. ei. Everything other than Hydrogen. Questions: . What . is the difference between the two? Why do you think hydrogen is different?. Shielding and Penetration. Orbitals with radial probability closer to the nucleus are more . penetrating. . . The closer, more penetrating orbitals, are . shielding. the further orbitals from the nucleus. . Electron Configurations. The way electrons are arranged in atoms. Energy Levels (Principle Quantum Number – n). First energy level. Only s sublevel (1 s orbital). Only 2 electrons. 1s. 2. Second energy level. Finish Calculations. Start Quantum Numbers. Drill. Calculate the frequency and wavelength of a wave with E = 3.0 . x. 10. -15. J.. nu = 4.5 . x. 10. 18. Hz. lambda = 6.7 . x. 10. -11. . m. = 0.067 nm. Review. Electrons are the negatively charged part of the atom. Electrons are found in . orbitals. around the nucleus. We write the electron configuration of the element to see the different . orbitals. Quantum Atomic Theory. Heisenberg (1901-1976). Schrödinger (1887-1961). Einstein (1879-1955). Pauli (1900-1958). Plank (1858-1947). Bohr-Rutherford . vs. Quantum. Similarities. Electrons have discrete amounts of energy. In a normal chemical reaction, the nucleus of an atom remains unchanged. However, in nuclear reaction, the nucleus of an atom often changes. This reaction causes radiation to be given off.. Radioactivity. Electron Shells. Periods on the periodic table are similar because they have the same number of electron shells.. Within these shells there are layers called sublevels', a shell can have between 1 and 4 sublevels.. DO NOW. Pick . up your paperwork. Pick up two handouts. Get out Electron Configuration Notes, your Blank Periodic Table, and your green periodic table.. RULES. Aufbau. Principle. Each electron occupies the lowest energy orbital available. Electrons are added from the ground state up. Electrons fill in increasing energy order.. Lesson Objectives. Understand the relationship between the number of orbitals in various energy sublevels and the length of the periods in the periodic table.. Identify each block of the periodic table and be able to determine which block each element belongs to based on its electron configuration.. Gwyn P Williams 1-112X-Ray Emission EnergiesJeffrey B Kortright andAlbert C Thompson 1-813Fluorescence Yields For K and L ShellsJeffrey B Kortright 1-2814Principal Auger Electron Energi Three rules:. electrons fill orbitals starting with lowest n and moving upwards;. The order is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d etc.. Orbital Diagram. The . electron configuration. of an atom is a shorthand method of writing the location of electrons by sublevel.. Jun-ya HASEGAWA. Fukui Institute for Fundamental Chemistry. Kyoto University. 1. Prof. M. . Kotani. (1906-1993). 2. Contents. Molecular Orbital (MO) Theory. Electron Correlations. Configuration Interaction.