Chemistry Lecture 1

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  1. Aufbau Principle
    For each new proton that is added to create a new element there is also a new electron added.
  2. Hund's Rule
    Electrons will not fill any orbital in the same subshell until all orbitals in that subshell contain at least one electron and the paired electrons will have parallel spins.
  3. Principle quantum number
    (n) - designates the shell level. The larger the number the greater the size and energy of the electron orbital. For Transition metals n lags behind the period.
  4. Azimuthal quantum number
    (l) - designates the subshell or orbital shapes such as s, p,d, and f
  5. Magnetic quantum number
    (m) - designates precise orbital of a given subshell each orbital will have values of that range from -l to +l
  6. Electron spin quantum number
    (ml) - can have values of -1/2 to +1/2
  7. Heisenberg Uncertainty Principle
    There is an inherent uncertainty in the product of the position of a particle and its momentum, and that uncertainty is on the order of Planck's constant.
  8. Pauli Exclusion Principle
    No two electrons in the same atom can have the same four quantum numbers.
  9. Photoelectric Effect
    There is a one-to-one photon to electron collision necessary to eject an electron. Shows that light is made of particles.
  10. Period in Periodic Table
    Each horizontal row
  11. Groups or Families
    The vertical columns
  12. Alkali Metals
    First Group
  13. Alkali Earth Metals
    Second Group
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Chemistry Lecture 1
2014-10-24 04:37:15
Atoms Molecules QM

Chemistry Lecture I: Atoms, Molecules and QM
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