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

 

 

 

 

 

 

 

 

 

[MHS AP Chemistry page]

 

 

Colors, Wavelengths, and Frequencies


 
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

[MHS AP Chemistry page]