4.16 - Intermolecular Forces - 2015
Complete the quiz using ONLY a calculator and your Reference Tables.
- 1.Determine the main type of intermolecular forces in CaO (aq).
- A.
London Dispersion Forces
- B.
Ion-Dipole Forces
- C.
Dipole-Dipole Forces
- D.
Hydrogen Bonds
- 2.Determine the main type of intermolecular forces in C2H5OH.
- A.
London Dispersion Forces
- B.
Ion-Dipole Forces
- C.
Dipole-Dipole Forces
- D.
Hydrogen Bonds
- 3.Determine the main type of intermolecular forces in PH3.
- A.
London Dispersion Forces
- B.
Ion-Dipole Forces
- C.
Dipole-Dipole Forces
- D.
Hydrogen Bonds
- 4.Determine the main type of intermolecular forces in CCl4.
- A.
London Dispersion Forces
- B.
Ion-Dipole Forces
- C.
Dipole-Dipole Forces
- D.
Hydrogen Bonds
- 5.
Based on the ion shown, which side of water molecules should be touching the ion?- A.
The partial negative end must be touching the Br^- ion, since like charges between partial negative end (O) in water and the negative ion attract.
- B.
The partial negative end must be touching the Br^- ion, since opposite charges between partial positive end (O) in water and the negative ion attract.
- C.
The partial positive end must be touching the Br^- ion, since opposite charges between partial positive end (H) in water and the negative ion attract.
- D.
None of the above
- 6.At standard pressure, NH3 has a boiling point of 240 K, AsH3 has a boiling point of 211 K, and PH3 has a boiling point of 186 K. What accounts for the higher boiling point of NH3?
- A.
NH3 has a higher boiling point, because it contains London forces.
- B.
NH3 has a higher boiling point, because it contains hydrogen bonds.
- C.
NH3 has a higher boiling point, because it contains dipole-dipole forces.
- D.
NH3 has a higher boiling point, because it contains ion-dipole forces.
- 7.At standard pressure, HF has a higher boiling point than HCl, HBr, or H2 does. What accounts for the higher boiling point of HF?
- A.
HF has a higher boiling point, because it contains London forces.
- B.
HF has a higher boiling point, because it contains hydrogen bonds.
- C.
HF has a higher boiling point, because it contains dipole-dipole forces.
- D.
HF has a higher boiling point, because it contains ion-dipole forces.
- 8.Compounds like CuO and NaHCO3 are soluble in water. Compare the boiling point of a solution of CuO to the boiling point of water at standard pressure.
- A.
The solution of CuO has a higher boiling point than water does.
- B.
Water has a higher boiling point than the CuO solution does.
- 9.A mixture contains hydrogen fluoride and ammonia. Identify a strong intermolecular force of attraction between hydrogen fluoride and ammonia.
- A.
Dipole-Dipole Forces
- B.
Hydrogen Bonding
- C.
Ion-Dipole Forces
- D.
London Dispersion Forces
- 10.Rank the following molecules in order of increasing boiling point: NaF (aq), H2S, HF, CO2.
- A.
NaF (aq) < H2S < HF < CF4
- B.
H2S < CO2 < HF < NaF (aq)
- C.
CO2 < H2S < HF < NaF (aq)
- D.
CO2 < HF < H2S < NaF (aq)
- 11.Rank the following molecules in order of increasing boiling point: CH3Cl, CH3OH, Na2O (aq), CF4.
- A.
CF4 < CH3OH < CH3Cl < Na2O (aq)
- B.
CF4 < CH3Cl < CH3OH < Na2O (aq)
- C.
CF4 < Na2O (aq) < CH3Cl < CH3OH
- D.
CF4 < Na2O (aq) < CH3OH < CH3Cl
- 12.Which element combines with hydrogen to form a compound with the strongest hydrogen bonding between its molecules?
- A.
Sulfur
- B.
Tellurium
- C.
Selenium
- D.
Oxygen
- 13.Substance A has a boiling point of 13 degrees Celsius, Substance B has a boiling point of 20 degrees Celsius, Substance C has a boiling point of 23 degrees Celsius, Substance D has a boiling point of 12 degrees Celsius. Which substance has the strongest intermolecular forces?
- A.
Substance A
- B.
Substance B
- C.
Substance C
- D.
Substance D
- 14.At standard pressure, HF and NH3 have higher boiling points than HBr and CH4 do. What accounts for the higher boiling point of HF?
- A.
NH3 and HF have higher boiling points, because they contain London Forces.
- B.
NH3 and HF have higher boiling points, because they contain hydrogen bonds.
- C.
NH3 and HF have higher boiling points, because they contain dipole-dipole forces.
- D.
NH3 and HF have higher boiling points, because they contain ion-dipole forces.
- 15.At standard pressure, H2Se and CO have higher boiling points than CF4 and CO2 do. What accounts for the higher boiling point of HF?
- A.
H2Se and CO have higher boiling points, because they contain London Forces.
- B.
H2Se and CO have higher boiling points, because they contain hydrogen bonds.
- C.
H2Se and CO have higher boiling points, because they contain dipole-dipole forces.
- D.
H2Se and CO have higher boiling points, because they contain ion-dipole forces.
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