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Quantum Theory Suggested Reading Pages 104 - 110 I II III Section 4-2 Quantum Theory Came about because classical physics couldn’t explain everything. Why does a metal emit invisible radiation first (IR – heat) and then glow red, and then yellow, and then white? Quantum Mechanics Heisenberg’s Uncertainty Principle There is a limit to just how precisely we can know both the position and velocity of a particle at a given time. de Broglie – electrons have wave-like properties. Diffraction: The bending of a wave as it passes by the edge of an object or through a small opening. Interference: occurs when waves overlap. Atomic Orbital's (electron clouds) Regions around the nucleus of an atom where an electron with a given energy is likely to be found. Quantum Numbers Describe orbital's and electrons in them 1st Quantum # = main energy level (n) 2nd Quantum # = shape (l) 3rd Quantum # = which way it’s pointing(m l ) 4th Quantum # = which way it’s spinning(ms) principal quantum number “n” Main Energy Level Higher “n” = more energy = farther from nucleus Angular momentum quantum number “ l” Has to be lower than 1st quantum # Indicates shape l = 0 s shaped contains 1 orbit l=1 p shaped contains 3 orbits l = 2 d shaped contains 5 orbits l = 3 f shaped contains 7 orbits Shapes of Orbitals s orbitals Shapes of Orbitals p orbitals Shapes of Orbitals d orbitals Shapes of Orbitals f orbitals Magnetic quantum number “m ” l Tells which way it’s pointed Possible Values of ml s = 0 p = -1, 0, +1 d = -2, -1, 0, +1, +2 f = -3, -2, -1, 0, +1, +2, +3 Spin quantum numbers ms Represented with up or down arrow Can only be +½ (pointed up) or -½ (pointed down) Pauli exclusion principle The rule states that no two electrons may ever have the same four quantum numbers. 4 Minute Review