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ELECTRON CONFIGURATION The arrangement of electrons in an atom Each element has a distinct electron configuration Electron configuration describes the relationship between energy and stability

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ELECTRON CONFIGURATION Electrons and nucleus interact to make the most stable arrangement possible (lowest energy) The lowest arrangement is the “ground-state electron configuration”

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ELECTRON CONFIGURATION There are three rules for electron configurations Aufbau principle Pauli exclusion principle Hund’s rule

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ELECTRON CONFIGURATION AUFBAU PRINCIPLE Electrons occupy the orbitals of lowest energy first

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ELECTRON CONFIGURATION Aufbau order filling

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ELECTRON CONFIGURATION Pauli exclusion principle One orbital may describe at most 2 electrons To occupy the same orbital, the two electrons must have opposite spins ↑↓

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ELECTRON CONFIGURATION Hunds rule When filling orbitals of equal energy, One electron occupies each orbital

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ELECTRON CONFIGURATION HUNDS RULE cont. Until all orbitals contain one electron with the same spin direction Then they can be paired ↑↑↑↑↑↑↓↑↑

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ELECTRON CONFIGURATION Exceptions Half-filled sublevels are less stable than filled sublevels but more stable than other configurations

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ELECTRON ARRANGEMENT Orbital notation Electron configuration notation Noble gas configuration

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ORBITAL NOTATION Beryllium Nitrogen

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ORBITAL NOTATION Fluorine Phosphorous

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ELECTRON CONFIGURATION NOTATION Contains only the sublevel notation and Superscripts to indicate the number of electrons in the sublevel

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ELECTRON CONFIGURATION NOTATION 1s 2 2s 2 2p 1 has a total of 5 electrons (2+2+1=5) In ground state = 5 protons = Atomic number 5= Boron

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ELECTRON CONFIGURATION NOTATION 1s 2 2s 2 2p 6 = 1s 2 2s 2 2p 6 3s 1 = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 =

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NOBLE GAS CONFIGURATION Find the noble gas (group 18) before the element you are arranging Write that noble gas configuration as [symbol] [He], [Ne], [Ar] Then continue to write the electron configuration from that point

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NOBLE GAS CONFIGURATION Practice

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