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Electron’s in Atoms

Electron’s in Atoms. How Electrons are Configured in Energy Shells. Electron’s Lowest State.

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Electron’s in Atoms

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  1. Electron’s in Atoms How Electrons are Configured in Energy Shells

  2. Electron’s Lowest State • The lowest energy arrangement of electrons is the most stable. When electrons are arranged in the lowest possible energy arrangement it is called the electron’s ground-state electron configuration.

  3. Rules for Placing Electrons in Energy Shells • Three rules (principles) define how electronsare arrangedin orbit around an atom’s nucleus. • First Rule: • Aufbau’s principalstates that each electron occupies the lowest energy orbital available.

  4. 2nd & 3rd Rule • Pauli’s exclusion principalstates that a maximum of two electrons may occupy a single atomic orbital but only if they spin in oppositedirections. • Hund’s Rule states that single electrons with the same spin must each occupy an equal-energy orbital before additional electrons with different spins can occupy the same orbitals.

  5. Energy Levels & Sublevels • There are seven principal energy levels (shells). • Each principal energylevel contains sublevels. • Each sublevel contains orbitals. The orbitals are where the electronsreside. • Each orbital allows only two electrons.

  6. s & p Sublevels • The sublevels are designated s, p, d and f. • The s sublevels are spherical, contain one orbital, and can hold a total of twoelectrons. • The p sublevels resemble dumbbells. There are three p orbitals each allowing two electrons. The total number of electrons able to occupy the p sublevels is six.

  7. d & f Sublevels • The shapes of the d and the f sublevels become more complicated. The d sublevels have fiveorbitalsand can hold a maximum of 10 electrons while fsublevels contains 7 orbitals and can hold a maximum of 14 electrons. • The superscripts inform us how many electrons are residing in an orbital.

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