# 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
decreases
2. Raoult's Law Formula
PA=XAPA

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
2
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
decrease
7. If you increase solute concentration, you __ the freezing point
decrease
8. If you increase solute concentration, you __ the boiling point
increase
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
Lowest
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
deltaTf=mKf

1.86C kg H2O/ 1 mol solute
18. What is the freezing point depression of water in 17.1g sucrose and 200g water?
0.465C
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

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

0.512C kg H2O/1 mol solute

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

Pi=cRTi
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
s
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
Bidentate
Multidentate
• 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 __/__
Lewis/VSEPR
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)H2O
2)NH3
3)CO
4)NO
5)CH3NH2
• 1) Aqua
• 2) Ammine
• 3) Carbonyl
• 4) Nitrosyl
• 5) Methylamine
37. Simple ligand prefixes

Complicated ligand prefixes

1)
2)
3)
4)
-Same as always

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

[CoBr(NH3)5]SO4

Pentaaminebromocobalt(III)sulfate
39. Metal complexes as anions

K3[CoF6]
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

Molecules with same molecular formulas but different arrangements of atoms

Different ligands in complex

Different binding site on the ligand
41. Geometric Isomers

Cis
Trans
-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

Enantiomers
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)
2)
• 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 __
5

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
Between

Raised
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

1)red-orange
2)orange-yellow
3)yellow-green
4)green-blue
5)blue-violet
6)violet-red
-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

I-<Br-<Cl-<F-<OH-<H2O<NH3<en<NO2-<CN-
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 __
ignored

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 Author: Trekofstarsx ID: 289180 Filename: Chem 1C Quiz 2 Updated: 2014-11-14 19:51:36 Tags: Chem Folders: Description: Chem 1C UCSB quiz 2 Show Answers:

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