Which of the following best explains the high viscosity of glycerol (C3H8O3)?
High molecular weight
London Dispersion Forces
Extensive hydrogen bonding network
Dipole-dipole interactions
Related Questions
Amongst and the one with highest B.P is
because of lower molecular weight
because of higher molecular weight
because of H-bonding
because of lower molecular weight
The attraction that non-polar molecules have for each other is primarily caused by:
Hydrogen bonding
Difference in electronegativities
High ionisation energy
Van der Waals’ forces
Amongst and the one with highest B.P is
because of lower molecular weight
because of higher molecular weight
because of H-bonding
because of lower molecular weight
In case of hydrogen and helium the van der Waals’ forces are:
Strong
Very strong
Weak
None of these
Arrange the following compounds in order of increasing vapor pressure: CH3CH2OH, CH3OCH3, CH3CH2CH3.
CH3CH2CH3 < CH3OCH3 < CH3CH2OH
CH3CH2OH < CH3OCH3 < CH3CH2CH3
CH3OCH3 < CH3CH2CH3 < CH3CH2OH
CH3CH2CH3 < CH3CH2OH < CH3OCH3
Consider the following statements regarding intermolecular forces:
I. Dipole-induced dipole forces are stronger than London Dispersion Forces.
II. Ion-dipole forces are weaker than hydrogen bonds.
III. London Dispersion Forces are present in all molecules.
Which of the above statements is/are TRUE?
I and II only
II and III only
I and III only
I, II, and III
Which of the following molecules is most likely to exhibit dipole-dipole interactions?
CH4
CO2
HCl
Cl2
Which force is strongest?
Dipole-dipole forces
Ion-ion forces
Ion-dipole forces
Ion-induced dipole forces
Which of the following substances is expected to have the highest viscosity at room temperature?
Glycerol ()
Acetone ()
Ethanol ()
Diethyl ether ()
The unusually high boiling point of HF compared to other hydrogen halides is primarily attributed to:
Strong hydrogen bonding
Larger dipole moment
Higher molar mass
Greater London Dispersion Forces
