MHS AP Chemistry
Syllabus 6

 Read Chapter 6 Take Notes from the board [my notes are on this page] Notice figures 6.13, 6.19, 6.20, 6.21, 6.28 Notice figure 6.17 (wasn't he suave?) Enjoy "Chemistry at Work" on page 200 Check Out Schroedinger's Cat (Thank you Caroline McNamara for the link) Problems 6.2, 6.6, 6.8abd 6.14, 6.18, 6.20 6.24, 6.26, 6.28c, 6.32a[b] 6.40, 6.44b, 6.46 6.54, 6.56 6.64, 6.66abdf, 6.68 Lab 31 Spectrophotometric Determination of Iron Other Possible Labs: Diffraction Grating Calibration Analysis of Hydrogen Spectrum

Colors, Wavelengths, and Frequencies

 color wavelength frequency l n [nm] [x1014 Hz] ultraviolet 200 to 400 15 to 7.5 violet 400 to 420 7.5 to 7.1 blue 420 to 490 7.1 to 6.1 green 490 to 580 6.1 to 5.2 yellow 580 to 590 5.2 to 5.1 orange 590 to 650 5.1 to 4.6 red 650 to 700 4.6 to 4.3 infrared > 700 < 4.3 radio 2200n7 m 0.0014

Notes
Define electromagnetic, spectrum
Wave stuff: c, l, n, nm, E = hn, c = ln
h = 6.63x10-34 J/Hz
c = 3.0x108 m/s
Frequency gives color
UV, IR, visible, etc.
Photons: energy packets - wave AND particle properties
"Quantum" & photoelectric effect
Line spectra, "n," emission & absorption spectra
equation 6.3
Bohr's model: equation 6.4
combined: equation 6.5  J

RH = 2.18x10-18 J = 313.6 kcal/mol
for Hydrogen:    n=x to n=1 gives UV
n=x to n=2 gives visible
n=x to n=3 gives IR
Electron: Wave?  Particle?  "Wavicle!"
DeBroglie: E = mc2  and E = hn  and c = ln combine to give
l = h/mv  for any particle (v = velocity)
Heisenberg & uncertainty principle
Wave functions, probability, orbitals
Quantum numbers & orbitals
 n = 1, 2, 3, ... energy level ("shell") l = 0, 1, 2, ...n-1 shape or # of nodes ("subshell") ml = –l, –l+1...l–1, l orientation in space s = ±½ spin ("up" or "down")
s, p, d, f orbitals   for l = 0, 1, 2, 3
"Degenerate"
Single electron vs. many electron
Screening effect
Electron structure 1s22s22p63s1 etc.  What atom is that?
Periodic table & electron structure