Intermolecular Forces Quizz 1. Dipole-dipole forces act between molecules possessing: No dipole moment Electronic charges Permanent dipole Induced dipoleQuestion 1 of 202. Partial charges are involved in: Dipole-dipole forces London forces Dipole-induced dipole forces Vander waals forcesQuestion 2 of 203. 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.Question 3 of 204. The force of attraction between two permanent dipoles is known as Dipole – dipole force London force Repulsive force Dipole Induced dipole forceQuestion 4 of 205. 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 particlesQuestion 5 of 206. 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 particlesQuestion 6 of 207. London forces are important only at: Distance between the two particles Long distances Short distances Infinite distanceQuestion 7 of 208. 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 sizeQuestion 8 of 209. London forces are also known as vander Waals forces Dipole-dipole forces Dispersion forces Keesom forcesQuestion 9 of 2010. 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 bothQuestion 10 of 2011. 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 moleculeQuestion 11 of 2012. Magnitude of repulsion rises as the distance separating the molecules: Remains constant Increases Has no effect on repulsion DecreasesQuestion 12 of 2013. A strong type of dipole-dipole interaction is: Electrostatic bond Covalent bond Ionic bond Hydrogen bondQuestion 13 of 2014. High polarisability increases the strength of: Dipole-dipole forces Dipole-induced dipole forces Vander waals forces London forcesQuestion 14 of 2015. 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 forceQuestion 15 of 2016. Atoms and non-polar molecules are electrically: Polarized Ionized Symmetrical UnsymmetricalQuestion 16 of 2017. Among the following, the force that is not included in vander Waals forces is Dipole-dipole forces Dipole-induced dipole forces London forces Covalent bondQuestion 17 of 2018. A polar and a non-polar molecule interact by: London forces Dipole-induced dipole forces Hydrogen bond Dipole-dipole forcesQuestion 18 of 2019. 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 chargeQuestion 19 of 2020. Dipole-dipole forces are: Equal in strength to London forces Stronger than London forces Not comparable to London forces Weaker than London forcesQuestion 20 of 20 Loading…