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Electron Configuration & Orbital Writing

Electron Configuration & Orbital Writing. Pre AP Chemistry. Electron Configuration / Energy Levels. Electrons are arranged around the nucleus in specific regions called shells.

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Electron Configuration & Orbital Writing

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  1. Electron Configuration & Orbital Writing Pre AP Chemistry

  2. Electron Configuration / Energy Levels • Electrons are arranged around the nucleus in specific regions called shells. • Electrons of lower energy are located near the nucleus and electrons of higher energy are in the highest shell and are called valence electrons. • Each shell is broken down into subshells or orbitals (s, p, d, f) which are three dimensional regions around the nucleus that indicate the probable location where electrons are likely to occur. • Elements located in the same group on the periodic table have their highest energy electrons arranged in the same way and that makes them chemically similar.

  3. Electron Configuration • the phone number or address of an atom. • 1st = energy level of the e-. • represented by rows ( Period) on the periodic table • 1 = lowest, 7 = highest • 2nd = shape of sub-level • 4 different shapes…found on each energy level • S, P, D, F • 3rd = orientation of orbital in space. • - number of electrons, each element represents 1 • electron • - S has 1 orbital with a total of 2 electrons • - P has 3 orbitals with a total of 6 electrons • - D has 5 orbitals with a total of 10 electrons • - F has 7 orbitals with a total of 14 electrons

  4. Single atom orbital http://www.bing.com/images/search?q=electron+cloud+model+picture&qpvt=electron+cloud+model+picture&FORM=IGRE&adlt=strict

  5. Electron Configurations • In e- configurations, you must represent (in order), the: • energy level # (electron shell), subshell orbital (s,p,d or f) and e- # for the atom. • Always read left to right, top to bottom.

  6. II. Electron Arrangement in AtomsA. Electron Configurations

  7. Hydrogen 1s1 • first number =the energy level. • letter = the orbital location • superscript = number of electrons

  8. Helium Number of electrons 1s2 Electron shell (energy level) Type of subshellorbitals

  9. Lithium Number of electrons 1s22s1 Electron shell (energy level) Type of subshellorbitals

  10. Beryllium Number of electrons 1s22s2 Electron shell (energy level) Type of subshellorbitals

  11. Period 2 • Boron = 1s22s22p1 • Carbon = 1s22s22p2 • Nitrogen = 1s22s22p3 • Oxygen = 1s2 2s22p4 • Fluorine = 1s2 2s22p5 • Neon = 1s2 2s22p6 • Remember that the superscript numbers must equal the atomic number

  12. Write out the correct e- configuration for Na (Z = 11) • 1s2 2s22p6 3s1 • Write out the correct e- configuration for Mg (Z = 12) • 1s2 2s2 2p6 3s2 • Write out the correct e- configuration for P (Z = 15) • 1s2 2s2 2p6 3s2 3p5 • ‘d’ orbitals are so large that they reach into the next energy level. Therefore, the 1st ‘d’ orbital belongs to the 3rd energy level…even though we don’t see it until the 4th row of the P.T.! • Write out the correct e- configuration for Br (Z = 35) • 1s2 2s2 2p6 3s2 3p54s2 3d10 4p5 • ‘f’ orbitals are so large that they reach into the next 2 energy levels. Therefore, the 1st ‘f’ orbital belongs to the 4th energy level…even though we don’t see it until the 6th row of the P.T.!

  13. Heisenberg Uncertainty Principle • Impossible to know exactly where an electron is at any moment. http://www.bing.com/images/search?q=electron+cloud+model+picture&qpvt=electron+cloud+model+picture&FORM=IGRE&adlt=strict

  14. Orbital Filling- Aufbau Principle • Aufbauprinciple.1. Electrons enter at the lowest energy level. 2. Some energy levels overlap into the adjacent principal energy level.

  15. Orbital Filling- Pauli Exclusion Principle • Pauli exclusion principle.1. Spectral data shows that only 2 electrons can exist in the same orbital. 2. Electrons behave as if they were spinning about their own axis. 3. When electrons occupy the same orbital – they are said to spin in opposite directions (assign +1/2 and – 1/2).

  16. Orbital Filling- Hund’s Rule • Hund’sRule.1. Also with the principle, you must have all orbital filled with one electron before you can add the other electron with opposite spin to the orbital. 2 . All elements would like to have a completely filled orbital and the maximum number of electrons that can exist in a filled orbital is eight

  17. Orbital Filling

  18. Electron Arrangement in AtomsExceptional Electron Configurations • 1. Filled sublevels are more stable than partial filled or half-filled sublevels. • 2. But sometimes half-filled may be more stable than other configurations. • 3 Example: Iron, Copper, and Chromium • 1s22s22p63s23p64s23d5 • 1s22s22p63s23p64s13d10 This is more stable because the higher energy sublevel is completely filled. • *1s22s22p63s23p64s13d5 3d and 4s are very close together indeed in the transition series, so filled shell or half filled shell stability (Cr, 4s13d5) is enough to tip the balance. • *http://answers.yahoo.com/question/index?qid=20090425034031AAOJJUQ

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