A) CBr4 c) C6H14 As the atomic mass of the halogens increases, so does the number of electrons and the average distance of those electrons from the nucleus. E) None, all of the above exhibit dispersion forces. E) None. Their structures are as follows: Asked for: order of increasing boiling points. Helium is nonpolar and by far the lightest, so it should have the lowest boiling point. A: A question based on properties of liquid that is to be accomplished. In order for this kind of bond to work, the molecules need to be very close to each other, like they are in a liquid. b. Which are likely to be more important in a molecule with heavy atoms? Since all compounds exhibit some level of London dispersion forces and compounds capable of H-bonding also exhibit dipole-dipole, we will use the phrase "dominant IMF" to communicate the IMF most responsible for the physical properties of the compound. The hydrogen bond is actually an example of one of the other two types of interaction. (a) How many mL will vaporize in an evacuated 1.50-L flask at 20C? {/eq}. C) Large nonpolar molecules C) (i) and (iii) What is the main difference between intramolecular interactions and intermolecular interactions? 2. In each case, identify the principal intermolecular forces involved forces and account briefly for your choice. Temperature and Pressure at Triple point = ? 2.11: Intermolecular Forces and Relative Boiling Points (bp) At 40 C? Because ice is less dense than liquid water, rivers, lakes, and oceans freeze from the top down. A) increases linearly with increasing temperature The intermolecular forces make it difficult for the molecules to move apart because they are so attracted to each other, so more energy is needed, which in turn makes the temperature at which something boils much higher. Lewis proposed the octet rule, which suggests that the electronic configuration of the noble gas represents the most stable state for an atom. 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