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Quantum Mechanical Model

AWESOME. Quantum Mechanical Model. February 28, 2007 Chem 102B. 1s Orbital ( ). Probability of electron in 3-D space around the nucleus. More “s” orbitals. The higher the energy level, the larger the size, and the more nodes that are present Note the Nodes. Nodes.

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Quantum Mechanical Model

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  1. AWESOME Quantum Mechanical Model February 28, 2007 Chem 102B

  2. 1s Orbital () • Probability of electron in 3-D space around the nucleus

  3. More “s” orbitals • The higher the energy level, the larger the size, and the more nodes that are present • Note the Nodes

  4. Nodes • Region of zero probablity

  5. “P” Orbitals • Dumbell shapes • Sets of 3

  6. The 3p orbital has 3 nodes

  7. “D” Orbitals

  8. “F” Orbitals

  9. Quantum Numbers • n - principalSize and Energy • integer values • l - angularShape • integral values from 0 to n-1 • ml - magneticOrientation • integral values from -l to l including 0 • ms - spinSpin • +1/2 or -1/2

  10. Pauli Exclusion Principle • Two electrons in the same orbital have opposing spins • In a given atom: No two electrons can have same QN’s!

  11. Aufbau Principle • “Building up” • Add electrons one at a time • Energy tells us what order to fill the electrons in the orbitals - Hund’s Rule • Lowest energy equals max number of “unpaired electrons”

  12. Periodic Table

  13. Ionization Energies • Energy required to completely remove an electron from an atom.

  14. Electron Affinity • The energy change associated with the addition of an electron to a gaseous atom • X(g) + e- X-(g) • Atoms that tend to form negative ions release more energy when an electron is added

  15. Atomic radius • Half the distance between the nuclei in a molecule consisting of identical atoms • Not exact measure!

  16. Radii trends • Down the group the atoms get larger, more electrons, bigger size. • Across the period the atoms get smaller, why?

  17. R Summary of Trends Too erratic to predict IE EA

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