Chap. 11- Modern Atomic Theory

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Jpadawanj
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186542
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Chap. 11- Modern Atomic Theory
Updated:
2012-12-11 21:08:26
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Chemistry Mid Term
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made week of 12/2
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  1. wavelength 
    • - λ(lambda) 
    • - the distance between 2 consecutive wave peaks 
  2. frequency 
    • - ν 
    • - the # of waves that pass a specific point in 1 sec. 
    • (Hertz) 
  3.  equals 
    speed of light 
  4. equation for speed of light 
  5.  are directly/inversely proportional? 
    inversely proportional 
    • -Plank's constant 
    •  (Jules) 
  6. Energy is measured by
    Jules(J) 
  7. What equation connects energy to frequency?
  8. What equation connects enery to lambda? 
  9. E and  are _______ proportional 
    inversely
  10. Balmer's equation
    • - n= the orbit in which the electron falls on
    • - allows us to calculate the wavelengths of the lines in the visible spectrum 
  11. What did Bohr conlude from Balmer's equation?
    • e's orbit the nucleus at a fixed distance and the orbit's has a dixed energy 
    •  must absorb a fix amount of energy to tranfer to the next orbit
    • thinks like it is like a solar system
  12. color from lvl 3 to lvl 2
    red
  13. color from lvl 4 to lvl 2 
    blue/green
  14. color from lvl 5 to lvl 2
    violet
  15. When electrons falls into level 2 from any orbit. it will ALWAYS fall in to the _______ wavelengths
    visible
  16. fall into lvl 1---->
    ultraliviolet
  17. fall into lvl 5---->
    radio waves 
  18. quantized
    • only certain values are allowed 
    • orbits can only be in a certain fixed postitions 
  19. Schrodinger's eqution
    • l
    • m
    • s
  20. n(QN)
    • tells us size and energy 
    • allowed values: 1,2,3,4,5.....
  21. l(QN) 
    • 2nd azimothal QN
    • tells us shape
    • allowed values: 0.......n-1
  22. sublevels of l
    • s
    • p
    • d
    • f
  23. s orbital
    • =0
    • sperical 
    • can hold 2 electrons
  24. p orbital
    • dumbell
    • =1
    • two nodes don't touch
    • a place of zero probability of finding an electron
    • can hold 6 electrons 
  25. d orbital 
    • double dumbells 
    • =2
    • can hold 10 e's 
  26. f orbital
    • =3
    • nest of eggs
    • double dumbells 
    • can hold 14 e's 
  27. m(QN) 
    • tells us orientation of the orbitals with the respect to axes 
    • - magnectic QN
    • allowed values: -l......0......+l
  28. s(QN)
    allowed values:  or - 
  29. orbital energy diagram
    in lowest to increasing enegy level 
  30. column 1 & 2: QN? 
    s block
  31. column 3-12: QN? 
    d block 
  32. column 13-18: QN? 
    p block except He which is in S block
  33. those seperatee bottom electrons: QN? 
    f block except Thorium and Cesium
  34. Abreviated written electronic configuration
    labled to prededing noble gas and the number of electrons (including the element from)  to take to go to noble gas 
  35. corre. to Ionization energy, going down a family....
    less energy required to lose electron to gaseous state 
  36. corre. to Ionization energy, going across a series from left to right....
    generally increases because are nonmetals-less reactive

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