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The Quantum Mechanical Model

The Quantum Mechanical Model. The nucleus is found inside a blurry “electron cloud” A area where there is a high probability of finding an electron. Electron Configuration. Principal Quantum Number (n) = the energy level of the electron. (max # e- = 2n 2 )

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The Quantum Mechanical Model

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  1. The Quantum Mechanical Model • The nucleus is found inside a blurry “electron cloud” • A area where there is a high probability of finding an electron.

  2. Electron Configuration • Principal Quantum Number (n) = the energy level of the electron. (max # e- = 2n2 ) • Sublevels- like theater seats arranged in sections (s,p,d,f)(# of sublevels = n ) • Within each energy level, the complex math of Schrodinger’s equation describes several shapes. • These are called atomic orbitals - regions where there is a high probability of finding an electron *No more than 2 electrons in each orbital*

  3. Summary # of orbitals Max electrons Starts at energy level sublevel s 1 2 1 p 3 6 2 5 10 3 d 7 14 4 f

  4. Relative sizes of the spherical 1s, 2s, and 3s orbitals of hydrogen.

  5. Diagram of principal energy levels 1 and 2.

  6. The shapes and labels of the five 3d orbitals.

  7. Electron Configurations • The way electrons are arranged in atoms. • Three main “guiding” principles: • Aufbau principle- electrons enter the lowest energy first.

  8. Electron Configurations • Pauli Exclusion Principle- at most 2 electrons per orbital Why only 2 electrons per orbital? like charges repel each other, but… electrons spin on axis, clockwise or counterclockwise, creating magnetic polarization ( ↑↓ )

  9. Hund’s Rule- When electrons occupy orbitals of equal energy (same sublevel ) they don’t pair up until they have to. - one electron enters each orbital until all orbitals contain one electron with spins parallel.

  10. Writing Electron Configurations (Letter - number designation) # of e- H 1s1 Sublevel Principle Energy Level

  11. Orbital Diagrams Show each orbital as a circle, box, or line. Show each electron as an arrow, ↑ or ↓ spin. Label electron configuration (letter –number). ↑ ↓ ↑ ↓ ↑ ↑ ↑ N 7 1s 2s 2p 2 2 3

  12. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s Orbital (Aufbau) diagram

  13. Example • Let’s determine the electron configuration & orbital diagram for Phosphorus • Need to account for 15 electrons

  14. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s 1s2 2s2 2p6 3s2 3p3

  15. Orbitals being filled for elements in various parts of the periodic table.

  16. Remember… • When we write electron configurations, we are writing the lowest energy (ground state) configuration. Do Problems 21-24 pg 160 *** # 21 draw orbital diagrams, not just e- configurations

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