SeF4 or SeF6 ion-dipole III. CS2 or H2S. The strongest intermolecular forces in methanol are hydrogen bonds ( an especially strong type of dipole-dipole interaction). The two "C-Cl" bond dipoles in the plane of the paper have a resultant pointing to the right at an angle of 54.75° from the vertical. From each pair below, select the molecule that will display weaker intermolecular dipole-dipole forces in a sample of the pure substance. Molecular Dipole Moments. Each of the following substances is a liquid at –50°C. hydrogen bonding A) I, II, III, and IV B) I and III C) I, III, and IV D) I and II E) II and IV Ans: C . (B) AsCl3 and BCl3 are both non-polar, but AsCl3 is a larger molecule and has more electrons. A polar bond is a bond between two atoms of varying electronegativity. 6.68 Place each set of molecules in order of decreasing strength of intermolecular forces: (a) AsCl3, CS, Kr (b) BeCl2, BC1z, CCL (c) HF, CF4, CF2H2 . Relevance. I. dipole-dipole II. In contrast, intramolecular forces act within molecules. 5) Describe the intermolecular forces that must be overcome to convert each of the following from a liquid to a gas: a) Br 2 b) CH 3 OH c) H 2 S. 6) What kind of attractive forces must be overcome to a) melt ice b) boil HCl c) sublime I 2 d) vaporize CH 3 Cl 7) Which member of the following pairs has the larger London dispersion forces? 9 46. You previously learned how to calculate the dipole moments of simple diatomic molecules. In more complex molecules with polar covalent bonds, the three-dimensional geometry and the compound’s symmetry determine whether there is a net dipole moment. Smark. Intermolecular Dipole-Dipole Forces? It is therefore subject to greater London forces, and BCl3 has weaker London forces. From each pair below, select the molecule that will display stronger intermolecular dipole-dipole forces in a sample of the pure substance. 2 Answers. Answer Save. "CCl"_4 is a tetrahedral molecule with a "Cl-C-Cl" bond angle of 109.5°. ethandm. Previous question Next question Transcribed Image Text from this Question. CF4 or CHF3. 1.CS2 / H2O 2.AsCl3 / … when you look at the dot diagram it has a single electron pair on the As does that make it polar? dispersion IV. yes. Intermolecular forces act between molecules. Examples of intermolecular forces include the London dispersion force, dipole-dipole interaction, ion-dipole interaction, and van der Waals forces. 1 decade ago. AsCl3 or BCl3. (C) CH4 is non-polar, so its dipole-dipole forces of attraction are much weaker than those of CHF3, which is polar. Favorite Answer. The intermolecular forces present in CH 3 NH 2 include which of the following? Decreasing strength of intermolecular forces: 1) Kr > AsCl3> CS2 2) BeCl2> BCl3> CCl4 3) HF > CF4> CF view the full answer. Is AsCl3 polar or non-polar? ; Intermolecular forces are weaker than intramolecular forces. (Wikipedia) Polarity is dependent upon the relative electronegativity of the atoms in a molecule. Its strongest intermolecular forces are London dispersion forces. The more electronegative element will attract electron density towards itself, resulting in uneven charge distribution. Answer = AsCl3 (Trichloroarsine) is Polar ... Polar molecules interact through dipole–dipole intermolecular forces and hydrogen bonds. Lv 6. 1 decade ago. Polarity underlies a number of physical properties including surface tension, solubility, and melting and boiling points." Intermolecular forces in #"CCl"_4# The #"C-Cl"# bonds are polar but, because of the tetrahedral symmetry, the bond dipoles cancel each other. 0 1.