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WorksheetsUnit 3 Part 2 LM Questions
Total questions: 48
Worksheet time: 24mins
What is the main cause of non-ideality in gases?
Attractions between gas molecules.
The individual volumes of each gas molecule.
High temperatures that rip electrons from atoms.
Gases are ideal.
Both intra- and intermolecular forces are considered what kind of attraction?
Gravitational
Coulombic
Nuclear
None of these answers
Which of the following is considered an intramolecular bond?
Hydrogen bond
Polar covalent bond
Dipole-dipole bond
Van der Waal's forces
Which of the following is true regarding the origin of dipole forces between molecules?
They result from interactions between highly electronegative atoms like nitrogen, oxygen, and fluorine attached to hydrogen.
They result from the attraction of the permanent positive and negative ends of separate polar molecules.
The result from the attraction of temporary regions of positive and negative charges that arise in the molecules.
They result from the attraction between positive and negative ions.
The strength of dipole interactions are mostly determined by what?
The difference in electronegativity between the two bonded atoms.
The difference in sizes between the two bonded atoms.
The difference in the phase the bonded molecule is in.
Highly electronegative atoms like nitrogen, oxygen, and fluorine directly bonded to hydrogen.
Which of the following energies would be comparable to the energy contained in a hydrogen bond?
22 kJ/mol
2 kJ/mol
150 kJ/mol
600 kJ/mol
Why is ionic bonding considered both inter- and intramolecular bonding?
Once a salt is dissolved in water, the individual cations and anions can form IMFs with surrounding molecules.
Ionic solids form directly from gases one atom at a time.
Ionic bonds are strictly intermolecular forces.
Ionic bonds are strictly intramolecular bonds. Each lattice is a single large molecule of some substance.
All of the following are intermolecular forces exist in different types of molecular compounds. Which of the following exists in all molecules?
Dispersion forces
Dipole-dipole
Ion-dipole
Hydrogen bonding
What is the approximate energy contained in a dipole-dipole intermolecular interaction?
15 kJ/mol
1 kJ/mol
200 kJ/mol
1500 kJ/mol
Which of the following has a permanent dipole?
BF3, CF4, PF3
BF3
PF3
CF4
All of these have permanent dipoles.
Which of the following molecules only exhibits dispersion forces?
C2H6
NH3
CH3Cl
PCl4-
Rank the following based on increasing intermolecular forces?
C2H6, C4H10, C6H14, C8H18
C2H6 < C8H18 < C6H14 < C4H10
C2H6 < C4H10 < C6H14 < C8H18
C6H14 < C4H10 < C2H6 < C8H18
C8H18 < C6H14 < C4H10 < C2H6
In the graph above (boiling point vs. period) why do the dots on the left side of the graph break the trend?
Those three dots exhibit hydrogen bonding.
Those three dots all have a permanent dipole.
Those three dots don't break any trend.
We try and ignore those three dots because they are uninteresting.
Which of the following exhibits hydrogen bonding?
HF, CH3F, CHF3, HCl
HF only
HF, CH3F, and CHF3
All four exhibit hydrogen bonding.
HF and HCl
What is the dominant intermolecular force in the following molecule:
Hint: the molecule above has more than one of the forces below. Which one is the strongest?
Van der Waals
Permanent Dipole
Hydrogen Bond
Ionic Forces
What is the dominant intermolecular force in the following module:
XeF4
Permanent Dipole
Dispersion
Hydrogen Bonding
Covalent Bonding
What liquid property describes the resistance to flow? Think honey vs rubbing alcohol.
High boiling point
High surface tension
High capillary action
High viscosity
Which of the following molecules would have the largest capillary action?
H2O, Hg, N2, CH4
N2
Hg
H2O
CH4
Rank the following molecules based on increasing heat of vaporization.
CH3OH, CH3CH2OH, CH3CH2CH2OH, CH3CH2CH2CH2OH
CH3OH < CH3CH2CH2OH < CH3CH2OH < CH3CH2CH2CH2OH
CH3OH < CH3CH2OH < CH3CH2CH2OH < CH3CH2CH2CH2OH
CH3OH < CH3CH2CH2CH2OH < CH3CH2OH < CH3CH2CH2OH
CH3CH2CH2CH2OH < CH3CH2CH2OH < CH3CH2OH < CH3OH
Which of the solutions above has the lowest boiling points?
C2H6
H2O
CH4
NH3
Rank the 4 solutions based on increasing viscosity (lowest first).
C2H6 < H2O < NH3 < CH4
C2H6 < CH4 < H2O < NH3
CH4 < C2H6 < NH3 < H2O
CH4 < C2H6 < H2O < NH3
Which of the followings has the lowest boiling point?
Ne
He
Ar
Kr
Which liquid property is related to why water beads up on a windshield but acetone does not?
Viscosity
Surface Tension
Boiling Point
Boiling Point
Which of the following compounds has the highest evaporation rate and vapor pressure?
He, H2O, NH3, HF
H2O
NH3
He
HF
As a little refresher, which of the following is the most polar covalent bond?
C-H
C-F
C-Cl
C-N
How many "buckets" would we need to separate the following compounds? Remember these are separated by the strongest intermolecular force present.
KCl, Br2, CaBr2, MgO, BCl3, CH3COOH (acetic acid), RbF
3
2
1
4
How many buckets (different kinds of IMF) would we need to separate these chemicals?
1
2
3
4
Of the compounds above, which one has the strongest IMFs, and what is the strongest IMF present in that compound?
NH3, Hydrogen bonding
NH3, Dipole-dipole
C2H6, Dipole-dipole
C2H6, dispersion forces
Rank the compounds above based on increasing intermolecular forces.
NH3 < CH3F < CH4 < C2H6
CH3F < NH3 < CH4 < C2H6
CH4 < C2H6 < CH3F < NH3
C2H6 < CH3F < CH4 < NH3
What is the dominant IMF in a mixture of HCl and CH3Cl?
dipole-dipole
ion-dipole
H bonding-dipole
dispersion
What is the dominant IMF in a mixture of NH3 and KCl?
ion-dipole
dipole-dipole
dipole-H bonding
ion-H bonding
Which answer below is best in describing dispersion forces in mixtures?
Dispersion forces are always present
Dispersion forces are present in non-polar mixtures.
Dispersion forces are present when at least one substance is non-polar.
There are no dispersion forces in mixtures.
Which of the following states of matter has the lowest internal energy?
Solids
Liquids
Gases
There is no way to tell without more information
IMF attractions are more likely to produce solids when
the temperature is high.
the temperature is low.
the pressure is low.
all the time under every circumstance.
What kind of solid is diamond?
Ionic solid
Covalent network solid
Molecular solid
Metallic solid
What kind of solid is CaCl2?
Ionic solid
Molecular solid
Network covalent solid
Metallic solid
Gold is a great example of a metallic solid. What solid properties would you expect gold to have?
Hard and brittle
Soluble in water
Electrically conductive
Low melting point.
What kind of solid is dry ice? Dry ice is solid carbon dioxide.
Ionic solid
Covalent molecular solid
Metallic solid
Covalent network solid
Which of the following two substances are made of the same element but conformed in different ways?
Graphene and coal
Calcium chloride and rock salt
Water ice and dry ice
Glass and salt slabs
Solid methane exists only at very cold temperatures. What kind of solid do you expect this to be?
Metallic solid
Ionic solid
Covalent molecular solid
Covalent network solid
In a sealed container with rigid walls, what happens to the pressure inside the container when the temperature is tripled?
The pressure is tripled.
The pressure increases by a factor of 9.
The pressure is reduced to 1/3 its original value.
Nothing happens to the pressure.
Which of the following statements is inconsistent with KMT?
Atoms in a gas do not interact with each other.
Gas molecules are mathematical points (they have no volume).
Gas molecules are polarizable.
Collisions are elastic.
Which of the following gases would be the least ideal?
CH3Cl
CH3CH2Cl
CH3CH2CH2Cl
CH3CH2CH2CH2Cl
We have two containers with an identical amount of gas in each. One gas is helium, the other is ammonia. Which would you expect to have the higher pressure?
Helium
Ammonia
They will have the same pressure.
There is no way to tell.
Which of the following have the strongest intermolecular forces?
CH4
CH3Cl
CHCl3
CCl4
Rank the following 4 compounds from weakest to strongest intermolecular forces?
NH3, BF3, BCl3, PH3
CH4
CH3Cl
CHCl3
CCl4
How many different IMFs are dominant in the substances below?
H2, CH3F, CH3COOH, CH3CH3, NaBr, CH3NH2
1
2
3
4
What kind of solid is a frying pan?
Metallic solid
Covalent network solid
Molecular solid
Ionic solid
