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
Arrange the following compounds in order of increasing boiling point: , , , .
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 has the highest boiling point?
HCl
HBr
HI
HF
What is the reason for unusual high b.p. of water?
Extensive hydrogen bonding between water molecules
Strong van der Waals forces
High molecular weight of water
Its covalent nature
Which type of intermolecular force is responsible for the high boiling point of water?
London Dispersion Forces
Dipole-Dipole Interactions
Hydrogen Bonding
Ion-Dipole Interactions
HF has a higher boiling point than HCl despite Cl being more electronegative than F. What is the primary reason for this?
Larger size of Cl
Stronger hydrogen bonding in HF
Higher dipole moment of HCl
Higher polarizability of Cl
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
Which of the following substances is expected to have the highest viscosity at room temperature?
Glycerol ()
Acetone ()
Ethanol ()
Diethyl ether ()
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
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
