Dipole-dipole forces act between molecules possessing:
  • No dipole moment
  • Electronic charges
  • Permanent dipole
  • Induced dipole
Partial charges are involved in:
  • Dipole-dipole forces
  • London forces
  • Dipole-induced dipole forces
  • Vander waals forces
Interaction energy associated with London force is
  • Proportional to the third power of the distance between two interacting particles.
  • Proportional to the sixth power of the distance between two interacting particles.
  • Inversely proportional to the sixth power of the distance between two interacting particles.
  • Inversely proportional to the third power of the distance between two interacting particles.
The force of attraction between two permanent dipoles is known as
  • Dipole - dipole force
  • London force
  • Repulsive force
  • Dipole Induced dipole force
Dipole-dipole interaction energy between stationary polar molecules is:
  • Inversely proportional to the third power of the distance between two interacting particles
  • Directly proportional to the third power of the distance between two interacting particles
  • Directly proportional to the sixth power of the distance between two interacting particles
  • Inversely proportional to the sixth power of the distance between two interacting particles
For dipole-induced dipole forces, interaction energy is:
  • Inversely proportional to the third power of the distance between two interacting particles
  • Directly proportional to the third power of the distance between two interacting particles
  • Inversely proportional to the sixth power of the distance between two interacting particles
  • Directly proportional to the sixth power of the distance between two interacting particles
London forces are important only at:
  • Distance between the two particles
  • Long distances
  • Short distances
  • Infinite distance
The strength of London forces do not increase with the increase in
  • The distance between two interacting particles
  • Surface area of molecule
  • Number of electrons
  • Molecular size
London forces are also known as
  • vander Waals forces
  • Dipole-dipole forces
  • Dispersion forces
  • Keesom forces
In dipole-induced dipole forces, the dipole moments (μ) of polar and non polar molecules are
  • μ = 0 and μ < 0
  • μ > 0 and μ = 0
  • μ < 0 and μ > 0
  • μ = 0 for both
The influence of permanent electrical dipole in dipole-Induced Dipole forces
  • Depend on the ionic radii
  • Decreases with the decrease in size of the molecule
  • Increases with the increase in size of the molecule
  • Does not depend on the size of the molecule
Magnitude of repulsion rises as the distance separating the molecules:
  • Remains constant
  • Increases
  • Has no effect on repulsion
  • Decreases
A strong type of dipole-dipole interaction is:
  • Electrostatic bond
  • Covalent bond
  • Ionic bond
  • Hydrogen bond
High polarisability increases the strength of:
  • Dipole-dipole forces
  • Dipole-induced dipole forces
  • Vander waals forces
  • London forces
The force of attraction between the polar molecules having permanent dipole and the molecules lacking permanent dipole is
  • Dipole Induced dipole force
  • Dipole - dipole force
  • Repulsive force
  • London force
Atoms and non-polar molecules are electrically:
  • Polarized
  • Ionized
  • Symmetrical
  • Unsymmetrical
Among the following, the force that is not included in vander Waals forces is
  • Dipole-dipole forces
  • Dipole-induced dipole forces
  • London forces
  • Covalent bond
A polar and a non-polar molecule interact by:
  • London forces
  • Dipole-induced dipole forces
  • Hydrogen bond
  • Dipole-dipole forces
The partial charges present on an atom are
  • Equal to the unit charge
  • Greater than the unit charge
  • Less than the unit charge
  • Does not depend on the unit charge
Dipole-dipole forces are:
  • Equal in strength to London forces
  • Stronger than London forces
  • Not comparable to London forces
  • Weaker than London forces
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