4.16 - Intermolecular Forces - 2015

15 Questions | By Regentschemistry | Last updated: Mar 22, 2022 | Total Attempts: 561

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4.16 - Intermolecular Forces - 2015 - Quiz

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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.