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Flashcards

Chem 112 Ch 7

Josephine Brok Chemistry English 83 cards

Cards in this deck (83)

  1. 1line spectruma spectrum showing only a certain discrete wavelengths
  2. 2quantum model for hydrogen atomproposed that the electron in a hydrogen atom moves around the nucleus only in certain orbits
  3. 3change in energy equalsenergy of final state minus energy of initial state
  4. 4atoms has lost energy and is now in a more stable statenegative sign
  5. 5radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum (ex. light form sun, energy to cook food, x-rays, etc.)electromagnetic radiation
  6. 6the distance between two consecutive peaks or troughs in a wavewavelength (lambda)
  7. 7the number of waves (cycles) per second that pass a given point in spacefrequency (nu)
  8. 8waves have a ______ relationship, short wavelength has high frequency and long wavelength have low frequencyinverse
  9. 9the constant relating the change in energy for a system to the frequency of the electromagnetic radiation absorbed or emitted; equal to 6.626 x 10^-34 J times sPlanck's Constant
  10. 10speed of lightC (3.0 x 10^8 m/s)
  11. 11formula for wavelength, frwquncy, and speed of lightc = frequency times wavelength
  12. 12change in energy of a system formulaE = n x h x frequency
  13. 13concept that energy can occur only in discrete units called quanta (discrete units of hv)quantized
  14. 14a quantum of electromagnetic radiationphotons
  15. 15energy of a phhotonE = hc/wavelength
  16. 16phenomenon inn which electrons are emitted from the surface of a metal when light strikes itphotoelectric effect
  17. 17energy has mass (E = mc^2) or (m = h/wavelength x c)special theory of relativity (Einstein)
  18. 18statements that light exhibits both wave and particulate behaviordual nature of light
  19. 19λ = h/mvdebroglies equation
  20. 20the scattering of light from a regular array of points or lines, producing constructive and destructive inferenceDiffraction
  21. 21the interference that occurs when two waves combine to make a wave with increased intensity (brighter spot)Constructive interference
  22. 22The interference that occurs when two waves combine to make a wave with a smaller amplitude. Waves are out of phase troughs and peaks coincide to result in decreased intensity of a wave (dark spot)destructive interference
  23. 23the result is that all matter exhibit both _______ ____ _______ propertiesparticulate and wave
  24. 24a spectrum that exhibits all the wavelengths visible light (results when white light passes through a prism)continuous spectrum
  25. 25a spectrum showing only a certain discrete wavelengthsline spectrum
  26. 26proposed that the electron in a hydrogen atom moves around the nucleus only in certain orbitsquantum model for hydrogen atom
  27. 27the lowest possible energy state of an atom or molecule ( E=-2.178 x 10^-18 J)ground state
  28. 28_____ electron has more energy than it does for n = 6, means that the electron is more tightly bound in the smallest allowed orbitn = 1
  29. 29change in energy equalsenergy of final state - energy of initial state
  30. 30atom has lost energy and is now in a more stable statenegative sign
  31. 31as electron is brought ______ to the nucleus, energy is released from the systemcloser
  32. 32_____ _____ did not work when applied to atoms other than hydrogen. Electrons in orbits around nucleus and only certain "orbits" are allowed. Never in between, jumps.Bohr Model
  33. 33a stationary wave as on a string of a musical instrument, in the wave mechanical model, the electron in the hydrogen atom is considered to be a _____ _______standing wave
  34. 34a function of the coordinates of an electrons position in three-dimensional space that describes the properties of the electronwave function
  35. 35a specific wave function for an electron in an atom. the square of this function gives probability distribution for the electronorbital
  36. 36a model for the hydrogen atom in which the electron is assumed to behave as a standing wavequantum (wave) mechanical model
  37. 37lowest energy for the hydrogen atom1s orbital
  38. 38a principle stating that there is a functional limitation to how precisely both the position and momentum of a particle can be known at a given time. (built in the universe is uncertainty)(cannot know or measure both position and momentum simultaneously perfectly for a particle)Heisenberg Uncertainty Principle
  39. 39the square of the wave function indicating the probability of fining an electron at a particular point in spaceprobability distribution
  40. 40as n increases, means ____ energy because the electron is less tightly bound to nucleus and energy is less negativehigher
  41. 41the quantum number relating to size and energy of an orbital; it can have any positive integer valueprinciple quantum number (n)
  42. 42as n increases, the orbital becomes _______ and the electron spends more time farther away from the nucleuslarger
  43. 43the quantum number relating to the shape of an atomic orbital which can assume any integer value 0 to n-1 for each value of n (related to shape of atomic orbital)angular momentum quantum number (l)
  44. 44l = 0s subshell, spherical shape
  45. 45l = 1p subshell, dumbell shape
  46. 46l = 2d subshell, shape different than s or p
  47. 47l = 3f subshell
  48. 48the quantum number relating to the orientation of an orbital in space relative to the other orbitals with the same L quantum number. it can have integral values between l and -l including zero. (ex. orbital where n=2, l=1 is 2p)magnetic quantum number (ml)
  49. 49an area of an orbital having zero electron probabilitynodes
  50. 50a group of orbitals with the same energydegenerate
  51. 51a quantum number representing one of the two possible values for the electron spin; either +1/2 or -1/2electron spin quantum number
  52. 52in a given atom no two electrons can have the same set of four quantum numbersPauli Exclusion Principle
  53. 53a atom with more than one electronpolyelectronic atoms
  54. 54is given most credit for the periodic table, predicted existence of and properties of still unknown elements (lists by atomic number)mendeleev
  55. 55as protons are added one by one to the nucleus to build up elements, electrons are similarly added to those hydrogen like orbitalsAufbau Principle
  56. 56the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli Exclusion principle in a particular set of degenerate orbitals, with all unpaired electrons having parallel spinsHund's Rule
  57. 57the electrons in the outermost principle quantum numbervalence electrons
  58. 58an inner electron in an atom; one not in the outermost (valence) principle quantum levelcore electrons
  59. 59elements in the same _____ have the same valence electron configuration. Elements with same valence electron configuration show similar chemical behaviorgroup
  60. 60several series of elements in which inner orbitals (d or f) are being filledtransition metals
  61. 61[Ar] 4s1 3d5Cr
  62. 62[Ar] 4s1 3d10Cu
  63. 63the first ionization energy is the energy require to remove the highest-energy electron of an atomionization energy
  64. 64as we go across a period, ionization energy ________ (in same shell, adding charge pulling in orbital, harder to pull electron away from that positive charge)increases
  65. 65as we go down a group, ionization energy _________(easier to remove electron from a larger orbital)decreases
  66. 66used to determine the relative energies of electronsphotoelectron spectroscopy for atoms
  67. 67the energy change associate with the addition of an electron to a gaseous atom. the energy released when an electron is added to a gaseous atom. (decreases as o across a period, and increases as go down a group)electron affinity
  68. 68change in energy, when the addition of the electron is _________, the corresponding value of electron affinity if negativeexothermic
  69. 69half the distance between the nuclei in a molecule consisting of identical atomsatomic radius
  70. 70atomic radius _____ across a perioddecreases
  71. 71Atomic radius _______ down a groupincreases
  72. 72elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic propertiesmetalliods
  73. 73(very reactive) going down a group ionization energy decreases and atomic radius increasesalkalimetals
  74. 74_______ _______ is important for particles that are really fast or really smallwave behavior
  75. 75electrons behave like math says they behave (mass x velocity = h/4pi)fundamental limitation
  76. 76HΨ=EΨ, wave function, mathematical func., no physical meaning. H is Hamiltonian operator. E energy calculate of electron orbitalsSchrodinger equation
  77. 77Ψ^2 probability of finding an electron in a region of space around nucleus, 3 dimensional graphprobability function for electrons
  78. 78define orbitals as ___% probability. Orbital does not equal orbit90
  79. 792 elements with the same electron configuration (ex. f^-, gains an electron and becomes ________ to Ne)isoelectronic
  80. 80ability to attract electrons in covalent bonds (not like atomic radii and ionization they are physical things) (only relevant for covalent)electronegativity
  81. 81has largest electronegativity (increases across a row and decreases down a group)fluorine
  82. 82ionicmetal and nonmetal
  83. 83covalentnonmetal and nonmetal

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Chemistry Flashcards on Chem 112 Ch 7, created by Josephine Brok on 29/11/2022.
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Josephine Brok
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