PPT-Electron Configuration Electron configurations tells us in which orbitals the electrons

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. 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. Elements with high electronegativities (non-metals) will not give up electrons. Bonds are not formed by a transfer of electrons, they are formed by sharing electrons.. Molecules are neutral groups of covalently bonded atoms. The 2p. z. orbitals overlap in head-to-head fashion,. so these bonds are.... s. bonds.. -- the corresponding MOs are: . s. 2p. and . s. *. 2p. The other 2p orbitals (i.e., 2p. x. and 2p. y. ) overlap in. 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. 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. Configurations. Vocabulary:. Electron configuration. Aufbau Principle. Pauli Exclusion Principle. e. lectron . s. pin. Hund’s . Rule. Orbital diagram. Paul Klee, . Greeting. , 1922. American.. Subshells. 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.. Models of the Atom-History in Models. Democritus. (450BC, GR): smallest bit that is still that element.. Joseph Proust . (1794 FR): proposed that compounds form in definite proportions. Proust’s experiments and law influenced Dalton.. (1900):. Proposed that. amounts of energy are quantized. . only certain . E values . are allowed . Niels Bohr. (1913):. e. –. can possess . only certain amounts of energy, and. can therefore be only certain . Mrs. Medina. 1. Why do metals glow when heated?. 2. Models of the Atom. A model should explain not just what the material is made of (composition) but also how it is going to behave (changes).. Rutheford’s. use flame tests to provide evidence . that energy is absorbed or released in discrete units when electrons move from one energy level to another . explain how flame tests provide evidence . that energy is absorbed or released in discrete units when electrons move from one energy level to another . 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.. Fermi liquid theory.  (also known as . Landau–Fermi liquid theory. ) is a theoretical model of interacting . fermions.  that describes the normal state of most . metals.  at sufficiently low .