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Quantum Numbers and Electron Configuration

Quantum Numbers and Electron Configuration. Pauli Exclusion Principle. No two electrons in an atom can have the same set of four quantum numbers (n, l, m l , and m s ) This means: no atomic orbital can contain more than two electrons. Hund’s Rule.

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Quantum Numbers and Electron Configuration

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  1. Quantum Numbers and Electron Configuration

  2. Pauli Exclusion Principle • No two electrons in an atom can have the same set of four quantum numbers (n, l, ml, and ms) • This means: no atomic orbital can contain more than two electrons

  3. Hund’s Rule • The most stable arrangement of electrons is that with the maximum number of unpaired electrons, all with the same spin direction

  4. Aufbau Principle • When filling orbitals, electrons go into the lowest energy orbital around the atom FIRST • The means that the atom will minimize it’s energy

  5. How we represent Electron Configuration • Orbital Diagrams • Each ‘box’ represents 1 orbital • s orbitals only have 1 box (1 orientation) • p orbitals have 3 boxes (3 orientations) • d orbitals have 5 boxes (5 orientations) • Each box can only contain 2 electrons of different spin (Pauli Exclusion Principle)

  6. Examples • Draw the orbital diagrams for: Hydrogen, Helium, Boron, and Magnesium

  7. Energy Level Diagrams • Another version of Orbital diagrams showing the distribution of energy • Draw the energy level diagrams for: Be, O, Si, Mn

  8. Electron Configuration • A way to simplify orbital diagrams (no drawing needed!) • Longhand: Identifying all the orbitals that are filled with electrons in order of increasing energy level • Shorthand: Using the closest noble gas and then identifying any other orbitals that are filled in order of increasing energy level

  9. Electron Configuration • Examples: Write the Longhand and Shorthand electron configurations of the following elements. • Magnesium • Iron • Iodine

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