3.3 Electron Configuration

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Presentation transcript:

3.3 Electron Configuration

1s 2 s 3 s 4 s 5 s 6 s 7 s 2 p 3 p 4 p 5 p 6 p 7 p 3 d 4 d 5 d 6 d 4 f 5 f 5d Color and label your blank periodic table 6d

Notes: Electron Configuration These three principles govern the filling of orbitals by electrons: Aufbau Principle: Electrons enter orbitals of lowest energy first. Pauli Exclusion Principle: An atomic orbital contains a maximum of two electrons. Hund’s Rule: When electrons occupy orbitals of equal energy, one electron enters each orbital until the orbital is filled.

There are a total of 7 energy levels (shells). Each energy level contains a sublevel made up of orbitals. These are the following sublevels (orbitals): orbitals (#) s (1) p (3) d (5) f (7) Maximum # of electrons 2 6 10 14

Orbital notation represents the number of electrons and their spin Orbital notation represents the number of electrons and their spin. Since only 2 electrons occupy the 1s orbital, and their spin is opposite, the orbital notation for helium is: written as “1s2” Arrows are used in opposite direction to show the opposite spin. The orbital notation for boron, atomic number 5, is: 1s2 2s2 2p1

Noble Gas Configuration: The last noble gas before the element of interest is the noble gas we put in the brackets. For example the element aluminum (atomic number 13) we write: [Ne] 3s2 3p1 Sulfur: [Ne] 3s2 3p4 Barium: [Xe] 6s2 Arsenic: [Ar] 4s2 3d10 4p3

Do not copy

Do not copy

Note the number of electrons and its energy level