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Transcript
Electron configuration is a shorthand notation that shows electron arrangement within orbitals. Electron configuration can be written in one of 3 methods: 1. Energy-Level Diagrams (orbital diagram) 2. Complete electron configuration 3. Condensed electron configuration (AKA noble gas configuration) Atomic spectra conclude that electrons in an atom have different energies Under normal conditions (i.e., ground state), an energy-level diagram can show the relative energies of electrons in various orbitals The number of electrons in an atom is equal to the atomic number Each added electron will enter the orbitals in the order of increasing energy Orbitals of lowest energy are filled first An orbital cannot take more than 2 electrons. Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied All electrons in singly occupied orbitals have the same spin. Analogy: “The Bus Seat Rule” – when boarding the bus, you would take an empty seat rather than sit beside someone. Convey the same information, but in a more condensed form In a single line, all orbitals and electrons are listed in order of increasing energy level There is, of course, a trend seen in the periodic table for electron configuration The n-value for s and p orbitals correspond to the row numbers on the periodic table The l-values correspond to the columns s block: Groups 1 & 2 p block: Groups 13-18 d block: Transition elements f block: inner transition elements Lanthanides (elements #57-70) Actinides (elements #89-102) To find the electron configuration of a given element, simply locate its position on the periodic table Determine the electron configuration of gallium As electron configurations can also be long and tedious, there is a shorthand form that conveys the same information This involves looking at the most recent noble gas (since they are stable and all orbitals are full) and then continuing the electron configuration from there Cl: 1s2 2s2 2p6 3s2 3p5 Sn: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2 →Sn: [Kr] 5s2 4d10 5p2 → Cl: [Ne] 3s2 3p5 Anions Simple! Simply add the correct number of “extra” electrons Try it for Br1- Cations Subtract electrons from the highest principal quantum number (n) To do so, it’s best to write the configuration for the neutral atom first Try it for Ga3+ Read Pages 185-193 On Page 191, #1-4 On Page 194, #6-11