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In the final review session, Lyndon said that H2Se has a greater boiling point (and therefore stronger bonds) because it has greater London dispersion forces than H2S does. However, in the chemistry textbook version 6 p.484, H2Se is expected to be a stronger acid than H2S because H2Se has weaker bonds. Does having more london dispersion forces make a molecule stronger, or more likely to ionize? And which explanation would be correct?
Bigger london dispersion forces do lead to higher boiling points when a molecule exhibits no hydrogen bonds, is not polar or when the polarity is almost the same between two molecules. The bigger the atom, the greater the shift in electrons to create a temporary dipole and makes H2Se a stronger acid
LDF is found in every bond because its the most basic form of molecular attraction. Since electrons are constantly moving, at any given time, one atom will be more electronegative than the other atom. Thus, there will always be some degree of induced dipole-induced dipole (also known as LDF).
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