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
Related Questions
Van der Waals’ forces are applied to:
All atoms and molecules
Only polar molecules
Only non-polar molecules
Only ionic compounds
The gases in the liquid form are held together by a weak attraction among the molecules, called as:
Nuclear attraction
Bond attraction
Van der Waals’ attraction
Gravitational attraction
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
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
Which factor has the LEAST influence on the strength of London Dispersion Forces?
Dipole moment
Number of electrons
Molecular shape
Molecular size
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
London Dispersion Forces are present in:
Polar molecules only
Nonpolar molecules only
All molecules
Ionic compounds only
Which of the following substances is expected to have the highest boiling point based on the strength of its intermolecular forces?
CH4
CH3Cl
CH3OH
CH3SH
Surface tension is a phenomenon caused by:
Adhesive forces between liquid and container
Cohesive forces between liquid molecules
Repulsive forces between liquid molecules
Gravitational forces acting on the liquid
Which of the following substances is expected to have the highest viscosity at room temperature?
Glycerol ()
Acetone ()
Ethanol ()
Diethyl ether ()
