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Electron Configurations

Electron Configurations . Schrodinger’s Quantum Model . Principal Energy Levels - A region around the nucleus of an atom where the electron is likely to be moving . The principal energy levels (n) are assigned values in order of increasing energy

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Electron Configurations

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  1. Electron Configurations

  2. Schrodinger’s Quantum Model • Principal Energy Levels - A region around the nucleus of an atom where the electron is likely to be moving. • The principal energy levels (n) are assigned values in order of increasing energy • The average distance of the electron from the nucleus increases with increasing energy levels. (1 is closest to nucleus.) • There are 7 energy levels = 7 periods.

  3. Energy Sublevels • Energy sublevels can be thought of as a section of seats in a theater. The rows that are higher up and farther from the stage contain more seats, just as energy levels that are farther from the nucleus contain more sublevels.   • The number of energy sublevels is the same as the number of principal energy levels. 7 • Sublevels are labeled __s___ , ___p__ , __d___ , and __f___according to the shapes of the atom’s orbitals

  4. Atomic Orbitals • Atomic orbitals represent the electron probability clouds of an atom’s electrons. • Each orbital may contain at most ____2____ electrons. • All s orbitals are spherical • All p orbitals are dumbbell-shaped • 4 out 5 d orbitals are flower-shaped and one has a unique shape • 7 f orbitals have different and very complex shapes

  5. Shortcuts – Noble Gas Notation method – used to represent electron configurations of noble gases using bracketed symbols. • Practice: • Use shortcut method to write e-configurations for Ar and P.

  6. Ar: [Ne] 3s2 3p6 or [Ar] • P: [Ne] 3s2 3p3

  7. Ground State vs. Excited State • Ground State – The most stable, lower energy arrangement of the electrons in an atom. • (The electrons are in the correct order of orbitals.) • Excited State – When atom gains energy the electrons jump into higher energy level. • Identify the following atoms and describe their state. (Ground or Excited) • 1s22s22p63s23p64s13d104p3 • 1s22s22p63s23p64s23d104p5 • 1s22s22p63s23p64s23d104p65s24d8

  8. Electron Configuration – How to show the arrangement of electrons Aufbau Principle – Electrons enter orbitals of lower energy first. 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p Pauli Exclusion Principle – No more than __2______ electrons can occupy the same orbital AND they must spin in opposite direction (Opposite spins help hold e- in an orbital by creating magnetic attraction.) Hund’sRule – Orbitals of equal energy must EACH have _1____ electron with thesame ____spin______ before any orbital is occupied by a 2nd electron. Energy Level Increase

  9. In your book. • Copy table 5-2 on p. 134 • Copy Figure 5-17 on p. 135

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