Chem 1C Quiz 2

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  1. Raoult's Law

    Addition of a nonvolatile solute to a pure solution ___ the vapor pressure of the solution
  2. Raoult's Law Formula

    Vapor pressure solution=(mol fraction of solvent)(vapor pressure of the pure solvent)
  3. What is the vapor pressure of water above a solution comprised of 3.40g of NaCl dissolved in 30.0g H2O at 25C if the vapor pressure of pure water at this temperature is 23.8 torr?
    22.2 torr
  4. NaCl ionizes to __ mole particles
  5. Calculate the grams of glucose that must be added to 2.85kg of H2O at 65C to lower the vapor pressure by 10.0 torr if the vapor pressure of pure H2O at this temperature is 188 torr
    1.62x10^3g C6H12O6
  6. If you increase solute concentration, you __ vapor pressure
  7. If you increase solute concentration, you __ the freezing point
  8. If you increase solute concentration, you __ the boiling point
  9. Vapor Pressure
    Pressure exerted by vapor that is in dynamic equilibrium with its liquid
  10. Nonvolatile
    Liquids not easily evaporated
  11. Vapor Pressure Lowering
    Vapor pressure of solvent containing a nonvolatile solute is lower than the vapor pressure of the pure solvent
  12. Vapor Pressure Lowering is dependent on __
    The # of ions that the molecule breaks apart into
  13. Pure Solvent- Equilibrium established between?
    Liquid and vapor
  14. In a solution, solute particles reduce the number of solvent particles able to __
    Escape the liquid (vaporize)
  15. The molecule with the most ions has the __ vapor pressure
  16. Freezing Point Depression
    Difference between the freezing points of the pure solvent and a nonelectrolyte solution in that solvent

    Is directly proportional to the molal concentration
  17. Freezing Point Formula

    Kf H2O

    1.86C kg H2O/ 1 mol solute
  18. What is the freezing point depression of water in 17.1g sucrose and 200g water?
  19. A water solution containing an unknown quantity of molar solute is found to have a freezing point of -0.23C. What is the molal concentration of the solution?
    0.124 mol/kg
  20. Boiling Point Elevation

    BP H2O

    Difference in temperature between boiling point of solution and boiling point of pure solvent

    0.512C kg H2O/1 mol solute

  21. Osmosis
    Movement of solvent from an area of lower solute concentration to an area of higher solute concentration
  22. Osmotic Pressure
    Pressure required to stop osmosis

  23. Calculate the osmotic pressure of a 0.0120M solution of NaCl in water at 0C. Assume the Van Hoff factor, i, is 1.94 for this solution
    0.522 atm
  24. How many s blocks/how many does s hold?
    How many d blocks/how many does d hold?
    How many p blocks/how many does p hold?
    How many f blocks/how many does f hold?
    • 7s, each holds 2
    • 6p blocks starting at 2, each holds 6
    • 4d blocks starting at 3, each holds 10
    • 2f blocks starting at 4, each f holds 14
  25. Noble gas configuration
    Get noble gas in row above. Get shells for that noble gas, put in [ ]. Then, put in all preceding shells until you get the total number of electrons
  26. For elements with a 4 or 9 d electron, remove an electron from __ orbital and add it to __ orbital
    s, d
  27. Forming Metal Ions

    Remove __ electrons first
  28. Complex
    Something with many interconnected pairs
  29. Ligands
    • Things bonded to metal by coordinate bond to a transition metal
    • Based on how many lone pairs it can donate to 1 metal ion
  30. Unidentate
    • 1 attachment site
    • 2 attachment sites
    • >2 attachment sites
  31. Coordination number
    How many ligands attached to metal ion that have formed coordinate bonds
  32. Complex Ion
    Transition metal bound to multiple ligands

    Carries a charge
  33. Counter Ions
    Ions that balance charge, not part of the complex ion
  34. Coordination Compounds don't follow __/__
  35. Naming transition metal compunds

    1) Name __ before __
    2) Name __ before __
    3) If ligand is an anion, put _ at end of name
    • 1) cation/anion
    • 2)ligands/metal ion
    • 3) "o"
  36. Naming Exceptions

    • 1) Aqua
    • 2) Ammine
    • 3) Carbonyl
    • 4) Nitrosyl
    • 5) Methylamine
  37. Simple ligand prefixes

    Complicated ligand prefixes

    -Same as always

    • -1) None
    • -2) Bis
    • -3) Tris
    • -4) Tetrakis
  38. Ligands go in __ order (excluding prefixes)
    Alphabetical order


  39. Metal complexes as anions

    Potassium hexafluorocobaltate(III)

    • 1)Cation first
    • 2) Add -ate to end of metal name
    • 3) if name ends with -ium, drop the -ium
  40. Isomers

    Coordination Isomerism

    Linkage Isomerism
    Molecules with same molecular formulas but different arrangements of atoms

    Different ligands in complex

    Different binding site on the ligand
  41. Geometric Isomers

    -Different arrangements of ligands around central atom

    • -Ligands are side-by-side/90 degree angle
    • -Ligands are across from each other/180 degree angle
  42. Optical Isomers
    • Non-superimposable mirror images
    • -Ex: hands
  43. Chiral Molecules

    Type of molecule that has a non-superimposable mirror image

    Pair of molecules that are non-superimposable mirror images

    Also called optical isomers
  44. Simple Model assumptions of Crystal Field Theory

    • 1) Ligands=negative point charges
    • 2) Metal=ligand bonds are ionic bonds
  45. How many possible d orbitals are there?

    In the absence of ligands, these orbitals are __

    Degenerate (equal in energy)
  46. dz2 and dx2-y2 (top orbitals)

    -Directed towards __
    __ Energy of these orbitals a lot
    • -Point charges
    • -Raise
  47. dx2, dxy, dy2 (bottom d orbitals)

    -Are ___ point charges
    -Energies of these orbitals are not __ by as much

  48. What gives transition metal complexes their color?

    Where is this typically located?
    • Delta E, energy of absorbed photon
    • E=hc/^

    -Located in visible region of the spectrum
  49. Color Wheel

    You observe the __ __ of the light absorbed by the complex

    -complementary color

    • 1)800-650 nm
    • 2)650-600nm
    • 3)600-560 nm
    • 4)560-490 nm
    • 5)490-430 nm
    • 6) 430-400 nm
  50. Spectrochemical series
    Ranks ligands from weakest field to strongest field

  51. Field Strength and Electron Spin

    1) Strong field case
    2) Weak field case
    • 1) Large delta E, cannot populate top 2, low electron spin
    • 2) Small delta E, can populate top 2, high electron spin
  52. D Splitting
    Order of split energy levels is opposite in tetrahedral case

    • Gap between energy is smaller for tetrahedral
    • All tetrahedral complexes have weak field/high spin
  53. Ligand Field Theory
    Crystal field theory assumes that ligand-metal bonds are ionic- inaccurate

    -Accounts for covalent bonding of ligands to metals
  54. In line-angle structure, hydrogen atoms bound to  carbon are __
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Chem 1C Quiz 2
2014-11-14 19:51:36

Chem 1C UCSB quiz 2
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