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Electron Configuration

Electron Configuration. What is it? A list of orbitals that contain electrons for an element. Ex. 1s 2 2s 2 2p 6 3s 1 What are the different ways: Orbital notation _______ 1s Complete configuration 1s 2 2s 2 2p 6 3s 1

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Electron Configuration

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  1. Electron Configuration • What is it? • A list of orbitals that contain electrons for an element. • Ex. 1s22s22p63s1 • What are the different ways: • Orbital notation _______ 1s • Complete configuration 1s22s22p63s1 • Abbreviated configuration(noble gas configuration) [He] 2s2

  2. S orbitals are spherical Lowest energy orbital

  3. P orbitals are dumbell shaped

  4. D orbitals

  5. F orbitals (highest energy orbital level)

  6. Rules of Electron Configuration • 1. Afbau principle • An electron occupies the lowest energy orbital that can receive it. • 2. Pauli exclusion principle • No two electrons in the same atom can have the same four quantum numbers. • 3. Hund’s rule • Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron and all electrons in singly occupied orbitals must have the same spin state.

  7. Notations • Orbital Notation- • An unoccupied orbital is represented by ____ • An orbital containing one electron is represented by ______ 1s • An orbital containing two electrons is represented by _______ 1s • Electron Configuration Notation • 1s2 2s2 2p6

  8. Steps • 1. determine the number of electrons to be “addressed”. • 2. Look at the template or periodic table and “count” • 3. You must fill “up” arrows in the orbitals before filling “down” arrows. • 4. The order of filling is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p (these are lowest energy to highest)

  9. Blocks on the periodic table • Can you find a pattern

  10. Electron configuration practice

  11. Additional items • Isoelectric • When these atoms lose or gain electrons, they would have the same number of electrons. • Outer shell configuration • Valence electrons orbitals and placement • Diamagnetic • When all of the electrons in orbitals are paired (up spin and down spin). If one is unpaired it is called paramagnetic)

  12. Quantum Theory and Electron Configuration

  13. Quantum model of the atom • Quantum theory of an atom • A theory that uses mathematical equations to describe wave properties of electrons and other small particles. • Quantum Numbers • These numbers completely describe orbitals.

  14. Quantum numbers • 4 sets of numbers house #, street, city, zip code area code, prefix, number, extension 1. Principal quantum number 2. Angular momentum quantum number 3. magnetic quantum number 4. spin quantum number

  15. Principal Quantum Number • Symbolized by n • Indicates the energy level of the electron • As n increases the electron’s energy and its distance from the nucleus increase. • 1-7

  16. Angular Momentum Quantum Number • Symbolized by l • Indicates the shape of the orbital in a specific energy level. • l = n-1 • For l=0, s orbital (spherical) • For l=1, p orbital (dumbbell) • For l=2, d orbital • For l=3, f orbital

  17. Magnetic Quantum Number • Symbolized by m • M numbers are whole, including 0 from –l to +l. • Indicates the orientation of an orbital around the nucleus. • S has only 1 possible orientation • P has 3 orientations • D has 5 orientations • F has 7 orientations

  18. Spin Quantum Number • Values are +1/2 and -1/2 • Indicates direction of spin • 2 electrons that are occupying the same orbital have to have opposite spins.

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