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Warm Up 9/20
•Draw the Bohr Model for Aluminum
•What is the difference between a hypothesis and a theory?
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The Quantum Mechanical Model Chemistry
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Bohr’s Model
•Bohr energized hydrogen electrons
(1 e- per atom)
•Energized electrons jumped certain distances from the nucleus
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Bohr’s Model
•Bohr saw 4 colors
•Each color has a specific wavelength
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Bohr’s Model
•Each wavelength corresponds to a distance from the nucleus
•These distances are called “shells” or “energy levels”
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Bohr was wrong
•While Bohr’s theory worked for hydrogen, it could not be applied to any other element because they all have more than one electron
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Werner Heisenberg• 1927, Germany• Heisenberg
Uncertainty Principle = It is impossible to determine simultaneously both position and velocity off an electron or any other particle
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Heisenberg’s Uncertainty Principle• It’s impossible to
determine where any one electron is at any point in time.
•Scientists talk about probabilities of electrons locations (electronic cloud).
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Erwin Schrödinger
•Physicist from Austria
•Late 1920’s•Wrote an equation
to describe the probable location of an electron
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Quantum Mechanical Model
•Current Electron Theory
•Created by Schrödinger
•Involves Quantum Numbers
•Can be shown using Electron Configurations (ex: 1s22s22p5)
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Quantum Numbers• Each electron is
located in an energy level (n), which is within a sub-level with a shape (l).
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Quantum Numbers• A sub-level is made of
orbitals. Different electrons within the same sub-level will have a different orientation (ml) depending on the orbitals orientation within the sub-level.
• Each orbital can have 2 electrons max, but they have opposite spin (ms)
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Quantum Mechanical Model • Electrons are
arranged into Energy Levels or Shells (1, 2, 3, 4, …).
• The “Principal Quantum Number” (symbolized by n) indicates the main energy level occupied by the electron
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Quantum Mechanical Model• Energy Levels contain
sub-levels (s, p, d, f)
• The “Azimuthal or Angular Momentum Quantum Number” (symbolized by l) indicates the shape of the sub-level
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NRG Sub-level “s”Azimuthal Quantum Number 0
“s” sub-level
• l = 0•Sphere shape•Contains 2 e-•One Orbital
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NRG Sub-level “p”Azimuthal Quantum Number 1
“p” sub-levell = 1
Contains maximum 6 e-3 orbitals
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NRG Sub-level “d”Azimuthal Quantum Number 2
“d” sub-levell = 2
Maximum 10 e-5 orbitals
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NRG Sub-level “f”Azimuthal Quantum Number 3
“f” sub-levell= 3
Maximum 14 e-7 orbitals
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Quantum Numbers• Magnetic Quantum
Number (ml) indicates the orientation of an orbital around the nucleus
• For example, the sub-level “p” is composed of 3 different orbitals (px, py, and pz)
• Scientists use the values -1, 0, and +1 to tell the orbitals apart.
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Practice with Magnetic Quantum Numbers• What would be the
magnetic quantum number used for the s sub-level?
• What would be the magnetic quantum numbers used for the d sub-level?
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Spin Quantum Number, ms
• A maximum of 2 electrons can fit into each orbital. BUT electrons don’t like each other (repel)
• 2 spins = +1/2 (up) and -1/2 (down)