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Quantum Mechanical Model Electron Placement

Quantum Mechanical Model Electron Placement. Electron basics. Carries the negative charge of the atom Has mass of 0.0006 amu (6/10000 mass of a proton) Located in region around nucleus Has a spin that creates a magnetic field Either spins clockwise (“up”) Or counterclockwise (“down”)

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Quantum Mechanical Model Electron Placement

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  1. Quantum Mechanical Model Electron Placement

  2. Electron basics • Carries the negative charge of the atom • Has mass of 0.0006 amu (6/10000 mass of a proton) • Located in region around nucleus • Has a spin that creates a magnetic field • Either spins clockwise (“up”) • Or counterclockwise (“down”) • Atoms are electrically neutral, therefore, the number of electrons = number of protons.

  3. B.Electron Placement 1.Not Bohr Orbits • Electrons rarely, if ever, orbit in neatly defined circles.

  4. B.Electron Placement 2.Orbitals = Regions of Probability • Where electrons are likely to be found • Determined by electron density • Area of high density = many electrons are there = Orbital! • Area of low density = few electrons are there = Not Orbital!

  5. 2.Orbitals = Regions of Probability • Orbital Shapes: • s - spherical shape, centered on nucleus • p - dumb-bell shaped, with three possible orientations on x-, y- or z-axes. Dumb-bell “neck” centers on nucleus • d - clover shaped, with four possible orientations in xy, yz, zx, and x2 – y2 planes; also one dumb-bell-with-ring shape, on z-axis. Five total orbital orientations. • f – very complex shapes, with seven orbital orientations. (pictures don’t do this shape justice.)

  6. B.Electron Placement 3.Energy Levels • As Bohr theorized, we believe electrons have certain levels of energy (level = n = 1, 2, 3, etc.) • For each level of energy, there are sublevels of energy:

  7. 3.Energy Levels • Each level n has n sublevels • Each sublevel (s, p, d, f) corresponds to orbital shapes and orientations: • Sublevel s contains ones orbital • Sublevel p contains threep orbitals • Sublevel d contains fived orbitals • Sublevel f contains sevenf orbitals

  8. B.Electron Placement 4.Fitting electrons into place: Electron Configuration • Aufbau Principle: Electrons will inhabit the lowest possible energy level and sublevel. • Pauli Exclusion Principle: Each orbital holds a maximum of two electrons: one of each spin. • Hund’s Rule: Electrons will spread themselves out in a sublevel so that a maximum number of unpaired electrons result • If a sublevel were a bus, electrons wouldn’t share seats unless they had to.

  9. 3d 4s E N E R G Y 3p 3s 2p 2s 1s Electron Configuration Fluorine: 9 protons, 9 electrons 1s2 2s2 2p5

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