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Electron Orbitals

Electron Orbitals. Cartoon courtesy of lab-initio.com. Quantum Mechanical Model of the Atom. Mathematical laws can identify the regions outside of the nucleus where electrons are most likely to be found . These laws are beyond the scope of this class…. Heisenberg Uncertainty Principle.

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Electron Orbitals

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  1. Electron Orbitals Cartoon courtesy of lab-initio.com

  2. Quantum MechanicalModel of the Atom Mathematical laws can identify the regions outside of the nucleus where electrons are most likely to be found. These laws are beyond the scope of this class…

  3. Heisenberg Uncertainty Principle “One cannot simultaneously determine both the position and momentum of an electron.” The more certain you are about where the electron is, the less certain you can be about where it is going. The more certain you are about where the electron is going, the less certain you can be about where it is. Werner Heisenberg

  4. Quantum Numbers Each electron in an atom has a unique set of 4 quantum numbers which describe it. • Principal quantum number • Angular momentum quantum number • Magnetic quantum number • Spin quantum number

  5. Electron Energy Level (Shell) Generally symbolized by n, it denotes the probable distance of the electron from the nucleus. “n” is also known as the Principle Quantum number Number of electrons that can fit in a shell: 2n2

  6. Electron Orbitals An orbital is a region within an energy level where there is a probability of finding an electron. Orbital shapes are defined as the surface that contains 90% of the total electron probability. The angular momentum quantum number, generally symbolized by l, denotes the orbital (subshell) in which the electron is located.

  7. sOrbital shape The s orbital (l = 0) has a spherical shape centered around the origin of the three axes in space.

  8. porbital shape There are three dumbbell-shaped porbitals(l = 1) in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.

  9. Things get a bit more complicated with the five d orbitals(l = 2) that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells” d orbital shapes …and a “dumbell with a donut”!

  10. Shape of f (l = 3) orbitals

  11. Energy Levels, Sublevels, Electrons

  12. Magnetic Quantum Number The magnetic quantum number, generally symbolized by m, denotes the orientation of the electron’s orbital with respect to the three axes in space.

  13. Orbital filling table

  14. Electron Spin The Spin Quantum Numberdescribes the behavior (direction of spin) of an electron within a magnetic field. Possibilities for electron spin:

  15. Pauli Exclusion Principle Two electrons occupying the same orbital must have opposite spins Wolfgang Pauli

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