PPT-8.4-8.6 Electron Configuration, The Explanatory Power of the Quantum Mechanical Model,

Electron Configurations Valence Electrons and the Periodic Table The periodic table is arranged by grouping elements with similar chemical properties connection between electron configuration and chemical properties. 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. Advanced Chemistry. Ms. Grobsky. Shortcomings of the Bohr Model. Bohr’s model was too simple. Worked . well with only hydrogen because H only has one . electron. C. ould . only approximate spectra of other elements with more than one . 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. cont’d. 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. Chapter 5. The scale model shown is a physical model. However, not all models are physical. In fact, several theoretical models of the atom have been developed over the last few hundred years. You will learn about the currently accepted model of how electrons behave in atoms.. 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.. Two regions. Nucleus . protons and neutrons. Electron . cloud. region where you might find an electron. Modern View. . . . . . . .. Dalton (1803). Thomson (1904). (positive and negative charges). Should create electron structures for given atoms.. Could work out . Ar. of given elements.. ------------------------------------------------. Starter: What is abundance?. Fill in the table. Subatomic. The Periodic Table got its name because of the repeating pattern of chemical & physical . properties. .. Mendeleev ordered his periodic table with elements arranged in order of increasing atomic . Part 1. Outline. Introduction. Problems of classical physics. Black-body Radiation. experimental observations. Wien’s displacement law. Stefan – Boltzmann law. Rayleigh - Jeans. Wien’s radiation law. 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.. Unit 5. Electrons. Rutherford described the dense center of the atom called the nucleus.. But the Electrons spin around the outside of that nucleus.. Provide the chemical properties of the atoms.. Responsible for color and reactivity.. Section 6.1. . Development of the Modern Periodic Table. Section 6.2. . Classification of the Elements. Section 6.3. . Periodic Trends. Exit. Click a hyperlink or folder tab to view the corresponding slides..