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Electron Configurations

Electron Configurations. A shorthand to write orbital diagrams Eliminates the boxes and arrows and just replaces them with superscripts Ex. 1s 2s 2p 3s 3p Electron configuration is: 1s 2 2s 2 2p 6 3s 2 3p 2. Example 1: Write electron configurations for

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Electron Configurations

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  1. Electron Configurations • A shorthand to write orbital diagrams • Eliminates the boxes and arrows and just replaces them with superscripts Ex. 1s 2s 2p 3s 3p Electron configuration is: 1s22s22p63s23p2

  2. Example 1: Write electron configurations for • 23V • 35Br • 20Ca Answer: • 23e-  1s22s22p63s23p64s23d3 • 35e-  1s22s22p63s23p64s23d104p5 • 20e-  1s22s22p63s23p64s2

  3. Abbreviated form • We are only concerned with outermost electron(s) in the valence (outermost) shell – called valence electrons • The inner electrons called core or kernel electrons are not significant  can be abbreviated Ex. Na  1s22s22p63s1 but 1s22s22p6 is the e.c. of neon so Na can be written as [Ne]3s1 Mg [Ne]3s2

  4. [X] represents the electron configuration of a noble gas • Always choose the electron configuration of the noble gas that directly precedes the element

  5. Unexpected E.C. • Some elements need one electron to half-fill or completely fill a d-orbital; they will ”borrow” an electron from the s-orbital to complete its shell • Ex. Cu  [Ar]3d94s2 one short ofbeing filled • So actually [Ar]3d104s1

  6. Cr  [Ar]3d44s2 Actually [Ar]3d54s1 • Half-filled and filled d-subshells have some special stability that makes borrowing energetically favorable • Applies to these elements • group VIB (6) Cr, Mo, W • group 1B (11) Cu, Ag, Au

  7. Electron configurations of atoms in the Excited State • If the electron config. is not in its “normal” state, then you know it’s in an excited state • You recognize it because electron are found in higher orbital before the lower ones are filled e.x. 1s22s12px22py22pz1 An electron jumped up to a higher orbital

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