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  1. principal
  2. threshold frequency
  3. radiancy
  4. Pauli exclusion principle
  5. incandescence
  6. orbital
  7. Stefan-Boltzmann law
  8. line absorption spectrum
  9. photoelectrons
  10. quanta
  11. unpredictable
  12. node
  13. vary continuously
  14. Compton effect
  15. quantized
  16. ground state
  17. visible light, radiation
  18. quantum theory
  19. wave mechanical model
  20. quantum numbers
  21. de Broglie's equation
  22. higher, lower
  23. model
  24. blackbody
  25. spin
  26. Wien's law
  27. complementarity
  28. photons
  29. saturation potential
  30. uncertainty principle
  31. subshell
  32. stopping potential
  33. wave-particle duality
  34. matter waves
  35. magnetic
  36. line emission spectra
  37. excited state
  38. wave function
  39. Niels Bohr
  40. photoelectric effect
  41. wavelengths
  42. work function
  1. a term for the luminal energy emitted per unit time from a unit area
  2. b the concept that every quantum system exhibits both particle and wave properties, but the demonstration of one property limits the demonstration of the other at the same moment
  3. c term for a certain potential at which the current in a collector ceases
  4. d The ____ quantum number (denoted m1) indicates the spatial orientation of an orbital.
  5. e term signifying that all the electrons within any atom are restricted to specific energy states
  6. f According to the wave equation, ψ gives the value of the ___ ___ under a given set of conditions.
  7. g the effect that occurs when a block of graphite is placed in the path of a narrow beam of xrays, and the x-rays scatter in such a way that, at any angle of scattering, they are most intense at two wavelengths: the incident wavelength and a longer wavelength that increases as the scaterring angle increases
  8. h Bohr postulated that light is emitted by the hydrogen electron only when it moves from a ___ energy state to a ___ one.
  9. i the equation which states that the wavelength of any material particle or body is equal to Planck's constant divided by the product of mass and velocity
  10. j A gas emits the same ____ that is absorbs.
  11. k the law that states that the most strongly emitted wavelength is a function of temperature
  12. l the discrete amounts in which radiation is emitted, according to Planck
  13. m term for the amount of work that must be done to remove an electron from the outermost orbit of an outlying atom to a distance infinitely far away
  14. n term for the lowest possible energy state of an electron
  15. o Bohr stated that the energy of a hydrogen atom's electron does not ___ ____.
  16. p term for the specific frequencies of radiation emitted by elements or compounds in gaseous form, which increase in intensity as a function of temperature
  17. q term for the electrons ejected from a surface exposed to ultraviolet light or other radiation
  18. r Heisenberg's principle which states that we know either an electron's position or momentum, but not both at the same time
  19. s term for a certain positive potential beyond which the current rises very little
  20. t term for the space beween two shells-- a place of low probablility for containing an electron
  21. u Bohr claimed that the jumps of the hydrogen electron are esentially ____.
  22. v the Danish physicist who constructed a model of a hydrogen atom in order to predict the behavior of its electron
  23. w term for the spectrum whose prominent lines are identical in location to the two prominent lines in the line emission spectrum of the same element
  24. x the theory that matter exists simultaneously as both waves and particles, the particles moving in a manner dictated by the waves
  25. y The ____ (denoted by l) indicates the possible orbitals within a given energy level.
  26. z The ____ quantum number (denoted n) indicates a specific energy level containing electrons at an average radius from the nucelus.
  27. aa Bohr proposed that light emited by the hydrogen electron during transition to a lower energy state takes the form a of a single photon with a frequency of ___ ___ or of ___ elsewhere on the spectrum.
  28. ab The ___ quantum number (denoted ms) differentiates the two electrons in the same orientation within the same orbital within the same energy level.
  29. ac term for the ejection of electrons from a surface exposed to ultraviolet light or any other radiation
  30. ad When a property like wavelength is a factor, matter may be viewed as ___ ___.
  31. ae term for the hollow, three-dimensional shape that shows positions of high probability for finding an electron around a nucleus
  32. af term for a theoretical picture of something
  33. ag term for an ideal absorber, which absorbs all the radiation that falls upon it
  34. ah term for the production of visible light by a heated body
  35. ai Max Planck's theory that radiation is emitted in discrete amounts when an electrically charged body oscillates
  36. aj term for the frequency above which photoemission occurs even if the light is extremely weak, and below which photemission never occurs
  37. ak Schrodinger's model which related an electron's energy state to a cyclical standing wave
  38. al term for the higher energy state of an electron
  39. am term for the particles of which light consists
  40. an the four numbers that provide a statistical description of an electron's likelihood to be found in a given region where they will demonstrate observed characteristics
  41. ao term for the relationship betweent the radiated energy and the temperature of a blackbody
  42. ap the principle which states that no two electrons within an atom can have the same set of quantum numbers