CHM Test 3

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CHM Test 3
2013-04-16 18:58:02
Chemistry test MSU CHM105 106

Chapters 9 - 12
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  1. Atomic size
    • determined by the distance between the outermost electrons and the nucleus
    • atomic size decreases as you move to the right across a period
    • atomic size increases as you move down a column in the periodic table
    • Cs is largest
  2. Core electrons
    • electrons not in the outermost principle shell
    • not valence electrons
  3. valence electrons
    electrons in the outermost principal shell
  4. Quantum mechanical model
    Explains the manner in which electrons exist and behave in atoms
  5. electromagnetic radiation
    • composed of perpendicular oscillating waves, one for the electric field and one for the magnetic field
    • All electromagnetic waves move through space at the same, constant speed
  6. electric field
    a region where an electrically charged particle experiences a force
  7. Magnetic field
    a region where a magnetized particle experiences a force
  8. 3.00 x 108 m/s in a vaccum
    • the speed of light
    • C
  9. amplitude
    • height of the wave
    • measure of how intense the light is
    • larger the amplitude, the brighter the light
  10. wavelength
    • measure of distance covered by the wave
    • tells you what type of electromagnetic radiation it is
    • radio waves have the lowest energy and the longest wavelength
    • gamma rays have the highest energy and the shortest wavelength
  11. frequency
    the number of wavelengths that pass a point in a given period of time
  12. Rank the electromagnetic spectrum in order according to energy, from highest to lowest
    • gamma rays
    • xrays
    • ultraviolet
    • infrared
    • microwaves
    • radio waves
  13. rank the electromagnetic spectrum according to  wavelength, from longest to shortest
    • radio waves
    • microwaves
    • infrared
    • ultraviolet
    • xrays
    • gamma rays
  14. rank the electromagnetic spectrum according to frequency, from most frequent to least frequent
    • gamma rays
    • xrays
    • ultraviolet
    • infrared
    • microwaves
    • radiowaves
  15. how are energy levels labeled?
    • n
    • increase in energy as n increases
    • the electrons with the lowest energy are in n=1 and closest to the nucleus
  16. how many orbitals does the s level have?
    • 1 orbital
    • 2 electrons
  17. How many orbitals does the p level have?
    • 3 orbitals
    • 6 electrons
  18. how many orbitals does the d level have?
    • 5 orbitals
    • 10 electrons
  19. how many orbitals does the f level have?
    • 7 orbitals
    • 14 electrons
  20. Hunds rule
    when filling orbitals in the same subshell, maximize the number of parallel spins
  21. vapor
    changing liquid to gas
  22. condensation
    gas to liquid
  23. triple point
    where solid, liquid, gas exist at the same time
  24. deposition
    gas to solid
  25. sublimation
    • solid to a gas
    • ex: dry ice
  26. If the intermolecular force is strong, what is the vapor pressure?
    lower - stronger the intermolecular force, the lower the vapor pressure
  27. orbital
    the region around the nucleus of an atom where an electron is most likely to be found
  28. photon
    a particle of light or a packet of light energy
  29. principal quantum number
    a number that indicates the shell that an electron occupies
  30. ionization energy
    the energy required to remove an electron from an atom in the gaseous state
  31. when do we see colored light?
    when the specific wavelength that corresponds to that color is present
  32. In terms of absorbed and reflected light, why does a blue object appear blue?
    When we look at a blue object, it appears blue because the object reflects the wavelength corresponding to blue and absorbs all of the other wavelengths from the white light that illuminated the object.
  33. Bohr orbits have fixed ____  and fixed _____
    fixed energies and fixed distances
  34. In the Bohr model, what happens when an electron makes a transition between orbits?
    When an electron moves from a lower energy orbit to a higher energy orbit, energy is absorbed. When an electron relaxes from a higher orbit to a lower orbit, a photon of light is emitted that corresponds to the difference in orbit energy levels.
  35. In Charles Law, what is constant?
  36. With Boyle's Law, what is constant?
  37. Gay Lussac's law. What's constant?
  38. What is the Ideal Gas Law?
  39. The model that predicts the behavior of gases
    Kinetic Molecular Theory
  40. T/F: The frequency of electromagnetic radiation is directly proportional to its wavelength.
    False - the higher the frequency, the shorter the wavelength (it's inverse)
  41. VSPER
    Electrons don't like each other
  42. Paramagnetic
    • attracted to magnetic field
    • unpaired electrons
  43. diamagnetic
    • will not be attracted to unpaired electrons
    • no unpaired
  44. In molecular geometry, what shape/s are possible with two atoms?
    Only one- linear
  45. In molecular geometry, what shape/s are possible with three atoms?
    • linear or bent
    • bent only happens when you have unpaired electrons on the central atom
  46. In molecular geometry, what shapes are possible when you have four atoms?
    • Trigonal planar or trigonal pyramidal
    • trigonal pyramidal happens when you have unpaired electrons on the central atom
  47. In molecular geometry, what shapes are possible when you have five atoms?
  48. what three shape choices do you have with electronic geometry?
    linear, trigonal planar and tetrahedral