Pchem test 3.txt

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Pchem test 3.txt
2012-04-09 19:20:52

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    • author "Ljdankov"
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    • fileName "Pchem test 3"
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    • Lambda
    • Wavelength
  1. V
  2. Frequency and wavelength relation
    Lambda v = c
  3. Frequency unit
    Hertz s(-1)
  4. Period
    Reciprocal of frequency (time between peaks)
  5. Spring force
  6. Why use sin with spring constant?
    Twice differentiated is equal to sin
  7. Where is natural frequency iused
    Simple harmonic motion
  8. Node
    Intersection of wave with 0
  9. Antinode
    Waves peak
  10. Period
    Time between peaks, inverse frequency
  11. When is sin =0
    For any integer*pi and for 0
  12. Where is energy maximized?
  13. What is h
    Plancks constant. Ties wavelength to energy per packet.
  14. Work function
    Hv= kinetic energy of electron+work to remove electron
  15. Threshhold frequency
    Minimum frequency (w/h) to remove electron from surface
  16. Stationary mode
    Energy level at which electron emit no energy
  17. How is hv tied to changes in energy state?
  18. Ionization energy
    Energy needed to move an electron to infinity
  19. Rydberg constant
    Value used in deriving wavelength average from mjultiple spectral lines?
  20. Crystals are distinguished from amorphous solids by
    Representative unit of molecular structure repeated at fixed intervals.
  21. Basis
    Structural init of a crystal
  22. Lattice
    Unifor arangement of points in space repeatyed in cristal styructure.
  23. Crystal lattice
    3d lattice
  24. Space lattice
    2 d lattice
  25. Primitive cell
    Minimum volume of the 3d crystal
  26. Molecular bonding
    Held together by temporary van der waal forces
  27. Ionic bonding
    Held together by interaction of shared ions
  28. Covalent boonding
    Atoms with similair charges share electrons to comlete orbital
  29. Hydrogen bonding
    Partial charges bresponsible for bonds of this type.
  30. Intermediate type bonding.
    A large anions field of electrons is disturbed by a nearby ion
  31. Metal bonding.
    Sea of electron
  32. Lattice energy (inc E_c)
    The energy of a crystal lattice
  33. Speed of light
  34. Energy
  35. Momentum operator
    H/i d/dx= -ihd/dx
  36. Hamiltonian operator
  37. How do we determine if gtwo functions orthoganol?
    Integral of a*b dtau =0
  38. Energy of sublimation
    Energu to go from solid to gas
  39. Order of lattice strength
    Van der waal- hydrogen-metalic-covalent -ionic
  40. London vanderwaal bond energy
    Sum of forces modelled by leonard jones method. Based on partial charges as function of (1?r)^12 -(1/r) ^6
  41. Bond energy of metal
    Enthalpy of sublimation to mono atomic gas. Found as function of vapor pressure
  42. Intermolecular
    Between molecules
  43. Ntramolecular
    Inside the molecule
  44. Melting point increases with
    Bond strength
  45. Bond energy of hbond or dipole dipole
    Based on partial charges as function of (1/r) ^6
  46. Bond energy of cobvalent solids
    Enthalpy to convert into gas phase, can be calculated with density functional theory
  47. Ionic solid crystal lattice energy
    Calculated using hesss law
  48. Hesss law steps (5)
    • 1) calculate metals heat of sublimation
    • 2) calculate metal gas ionization energy per chatge
    • 3) if gas is diatomic, calculate dissociation energy
    • 4) calculatge gass electron affi nity for charge number
    • 5) sum and subtract solids enthalpy of formation
  49. Ionic crystal internal bond energy
    (Chargeanion)(charge cation)/r
  50. Physiadsorption
    Adsorption onto a surface caused by van der waals forces. Typically week and unimporgtant. Can however occur quickly and spontaneously
  51. Chemiadsorption
    Covalent adsorption onto a surface modelled by langmuir. Slow and rarely spontaneous due to high activation energy
  52. When does surface become saturated in langmuir model?
    High vapor pressure leads to 100% unilayer coverage
  53. What is sign of enthalphy h of adsorption
  54. What is sign of entropy s of adsorption
  55. What is sign of gibbs for adsorption
  56. Difference between graph of langmuir vs bet coverage.
    • Langmuir reaches a flat surface at 100% coverage by monolayer.
    • BET can have multiple layers so aftwr initial asymptote starts rising again
  57. Langmuir hinschelwood.
    Bimolecular reaction catalyzed by surfacwe. At some level (stoich ratio) rate peaks and then tapers off if conc of one increases while other stay constant
  58. Langmuir hinschelwood if one or both sunstance sorb weak
    Then that substance will drop out of bottom of eqjatipon
  59. Langmuir rideal
    Competitive adsorption, but b need bond surface and a must be gas for reaction
  60. Linier momentum operator
  61. Kinetic energy operator
    -(h_hat^2/2m) DEL^2
  62. Hamiltonian operator
    -i-hat^2/2m del^2 + E_HAT_P
  63. Blackbody average energy
    E_bar = k_b T
  64. Stationary state.
    State n in which electron emitsz no radiatoin
  65. Change in energy between state 1 and 2
    Planck*frequency = E2-E1
  66. Ionization energy
    Energy needed to remove elecytron
  67. Rhydberg formula
    Shows average frequency (1/wavelength) of an emission spectra
  68. Energy to momentum relations
    • Momentum * speed of light
    • Momentim*wavelength*frequency
  69. Wavelength to plank relations (2)
    • Wavelength=planck/momentum
    • =planck/massvel
  70. Heisenburg 3 forms
    • Inc location* inc momentum >= H_BAR/2
    • incE Inc t >=h_bar/2
    • Incq incu=h-bar/2m

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