Intermolecular Forces
Phase Changes
Solubility and Bond Enthalpy
Cumulative Miscellaneous
Cumulative Miscellaneous
100
This force is attributed to random electron movements about an atom creating temporary dipole moments
London Dispersion Forces
100
This is the phase change of going from a gas to a solid
Deposition
100
Fill in the blank for this common phrase about solubility:
_____ dissolves _____
Like dissolves like
Also acceptable:
polar dissolves polar
AND
nonpolar dissolves nonpolar
100
This is the electron and molecular geometry of Sulfur Tetrafluoride
Electron: trigonal bipyramidal
Molecular: Seesaw
100
A photon with a wavelength of 450 nm has this many joules of energy
h = 6.626e-34 j*s
c = 3e8 m/s
4.41e-19 Joules
E=(Planck's Constant)(Speed of Light)/(Wavelength)
200
Rank the forces from weakest to strongest:
Hydrogen Bonding
Ion-Dipole
London Disperson
Dipole-Dipole
London Dispersion
Dipole-Dipole
Hydrogen Bonding
Ion-Dipole
200
Pressure is held constant at 1. As temperature increases from 5 to 10, this phase change occurs
Sublimation
200
This is the bond enthalpy in 2 moles of carbon tetrachloride
2 moles * 4 (C-Cl)
2*4(328)
2*1312 kJ
2624 kJ
200
This is the electron geometry and molecular geometry of bromine pentafluoride
Electron: octahedral
Molecular: Square pyramidal
200
2C8H18 (l) + 25O2 (g) > 16CO2 (g) + 18H2O (g)
7.46 moles of C8H18 react with 8.28 moles of O2. How many moles of carbon dioxide form?
O2 is limiting, solve it to get 5.2992 moles of CO2
300
These are the intermolecular forces that exist in ammonia
London Dispersion
Hydrogen bonding (dipole-dipole)
300
If pressure is held at 3 and temperature is increased from 0 to 25, these are the 2 phase changes which will occur
Melting then vaporization
300
Rank the following from least to most soluble in water:
CH3(CH2)6Cl
CH3(CH2)6OH
HO(CH2)2OH
1) Least soluble 3) most soluble
1. CH3(CH2)6Cl
2. CH3(CH2)6OH
3. HO(CH2)2OH
300
An electron has an l value of 2. These are the possible values of ml
-2, -1, 0, 1, 2
300
An electron has an n value of 4. These are the possible l values.
0, 1, 2, 3
400
Rank the following from least to greatest boiling point:
Cl2, CBr4, Ar
Ar < Cl2 < CBr4
400
This is the phase(s) that this substance exists in at a pressure of 2 and temperature of 10
Solid, liquid, gas
400
This value is the reaction enthalpy when 1 mole of propane reacts with 5 moles of oxygen gas to create 3 moles of carbon dioxide and 4 moles of water
ΔH = bonds broken (reagents) - bonds formed (products)
Reagents:
Propane: 2(C-C) + 8(C-H) = 2(348) + 8(413)
Oxygen Gas: 5(O=O) = 5(495)
Products:
Carbon Dioxide: 6(C=O) = 6(799)
Water: 8(O-H) + 8(463)
ΔH = (5x495 + 2x348 + 8x413) - (8x463 + 6x799)
ΔH = -2023 kJ
400
This is the net ionic equation for the reaction of aqueous Aluminum Sulfate with aqueous Lead (II) Nitrate.
(remember charges and phase changes and balanced coefficients)
Al2(SO4)3 (aq) + 3Pb(NO3)2 (aq) -> 2Al(NO3)3 (aq) + 3PbSO4 (s)
Pb2+ (aq) + SO42- (aq) -> PbSO4 (s)
400
CNO- (arranged C-N-O where N is the central atom), has 3 resonance structures where octet rule is obeyed, although the 3 are not equally preferred. This is the number of pi bonds between the nitrogen and oxygen in the primary/preferred resonance structure
C≡N-O THIS IS PREFERRED, 0 pi bonds
C=N=O
C-N≡O
500
Rank the following from least to greatest vapor pressure:
Kr, CF4, H2, N2, CBr4, CBr2F2
CBr2F2 < CBr4 < CF4 < Kr < N2 < H2
500
Increasing temperature or pressure beyond point C creates this type of substance
Supercritical fluid
500
Rank the following from least to most soluble in hexanes:
CH3(CH2)6OH
CH3(CH2)6CH3
HO(CH2)2OH
1) Most soluble 2) least soluble
1. CH3(CH2)6CH3
2. CH3(CH2)6OH
3. HO(CH2)2OH
500
Ammonia and oxygen gas react to form nitrogen monoxide and water. 1.01 g of ammonia and 1.72 g of oxygen gas react together. This is how many grams of water form from the reaction.
1.16 grams
(see slideshow for answer key)
500
This is the energy output of a light source that emits photons at a rate of 819 photons per second with wavelengths of 158 nm. (note units)
h = 6.626e-34 j*s
c = 3e8 m/s
Ephoton = hc/λ
Ephoton = (6.626e-34)(3e8)/(158e-9)
Ephoton = 1.2581e-18 J/photon
Output:
1.2581e-18 J/photon x 819 photons/sec =
1.03e-15 J/s