Lecture 3 and 4

Lecture 3 and 4 - Lectures 3-4: Structure of Large Atoms...

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Lectures 3-4: Structure of Large Atoms Demonstration: fluorescence of minerals and laser dyes—compounds have quantized energies Buildup of electronic structures Shells (n=1 ,2, 3, etc.) describe energy and average distance. They correspond to n in the Rydberg expressions. This is the first “quantum number”. The energy of a single electron is the same for all orbitals in a particular shell. s, p, d, and f orbitals arise because of a second angular quantum number l . There are as many classes of orbitals (subshells, labeled s, p, d, f) in a shell as the shell number There are variations (specific orbitals) in each subshell (orbital class) because of a third, “magnetic” quantum number m: 1 kind of s, 3 kinds of p, 5 kinds of d, 7 kinds of f , labeled by x, y, z axis combinations (note—this is not the same as the spin quantum number; the term “magnetic” comes from the fact that their energy differences are observed in magnetic fields. Wikipedia has a good explanation of this: http://en.wikipedia.org/wiki/Magnetic_quantum_number) shapes of orbitals: s is spherical, p are figure-8 on each axis, d are in-plane/off- axis (3), in-plane/on-axis (1), extended figure 8 (1) the extents of the orbitals do get smaller as more electrons are added to the
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This note was uploaded on 09/29/2009 for the course ME 530.230 taught by Professor Katz during the Spring '09 term at Johns Hopkins.

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Lecture 3 and 4 - Lectures 3-4: Structure of Large Atoms...

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