WorksheetsLearning Modules 43-48
Total questions: 13
Worksheet time: 7mins
All of the following are intermolecular forces exist in different types of molecular compounds. Which of the following exists in all molecules?
Van der Waals
Dipole-Dipole
Hydrogen Bonding
Ionic
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 exhibits hydrogen bonding?
HF, CH3F, CHF3, HCl
HF only
HF and HCl
All 4 Compounds
HF, CH3F, and CHF3
Surface tension describes
the inward forces that must be overcome in order to expand the surface area of a
liquid.
The resistance to flow of a liquid
Adhesive forces between molecules
the forces of attraction between surface molecules of a solvent and the solute
molecules
Rank the compounds
NH3 , N2 , C2 H6 , NCl3 , H2
in terms of decreasing capillary action in a glass tube.
NH3 > NCl3 > C2 H6 > N2 > H2
H2 > N2 > C2 H6 > NCl3 > NH3
NH3 > N2 > C2 H6 > NCl3 > H2
NH3 > C2 H6 > N2 > NCl3 > H2
Rank the liquids
I) C6 H6
II) CH3 CH2 OH
III) CH2 OHCHOHCH2 OH
IV) CH2 OHCH2 OH
V) H2 O
in order of increasing viscosity at 25°C.
I < V < II < IV < III
II < IV < I < V < III
IV < V < II < I < III
I < IV < II < V < III
Which one of the following substances is INCORRECTLY matched with the kind of solid that it forms?
diamond: molecular
calcium fluoride: ionic
iron: metallic
carbon dioxide: molecular
Which of these is NOT a property of network solids
Relatively low melting points
Insoluble in water
brittle
rigid
Arrange the following compounds in order from highest to lowest melting point C(s), CO2(s), LiBr(s), MgF2(s)
C(s) > MgF2(s) > LiBr(s) > CO2(s)
CO2(s) > MgF2(s) > LiBr(s) > C(s)
CO2(s) > LiBr(s) > MgF2(s) > C(s)
C(s) > LiBr(s) > MgF2(s) > CO2(s)
In theory, 1.00 mol of water vapor in a 10.0 L container at 400 K should have pressure of 3.28 atm, according to the ideal gas law. However, the observed pressure is actually 3.24 atm. Which of the following is the best justification for why the observed pressure is slightly less than the predicted value?
Water molecules experience intermolecular attractive forces with each other.
Water molecules tend to travel at faster speeds that other gas molecules.
Water molecules tend to bounce off each other with a large repulsive force.
Water molecules experience adhesion with the walls of the container.
Boiling point trends are usually attributed to the strength of the intermolecular forces in the liquid. As the strength of the intermolecular force increases, the boiling point of the liquid increases. Which of the following accounts for why Br2 is a nonpolar molecule with a boiling point of 59°C, while HF is a polar molecule with a boiling point of 19.5°C
The hydrogen bonds in HF are weaker than the London dispersion forces in Br2.
The London dispersion forces in HF are weaker than the dipole-dipole forces in Br2
The London dispersion forces in Br2 are weaker than the hydrogen bonds in HF.
The London dispersion forces in Br2 are weaker than the London dispersion forces in HF.
Which of the following is TRUE regarding the origin of dipole forces between molecules?
They result from the attraction of the positive and negative ends of separate polar molecules.
It comes from strong charges in molecules due to highly polar bonds between hydrogen and oxygen, hydrogen and fluorine, or hydrogen and nitrogen.
They result from the interaction of temporary regions of positive and negative charges that arise in molecules.
They result from the interactions between positive and negative ions.
Which molecules of the following gases will have the greatest average kinetic energy?
All of the molecules have the same kinetic energy.
N2 at 1 atm and 298 K
H2 at 0.5 atm and 298 K
CO2 at 0.1 atm and 298 K
