CHMA10H3 Lecture Notes - Lecture 11: Intermolecular Force, Atomic Orbital, Boiling Point
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CHMA10H3 Full Course Notes
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Chapter11 crystaline solid - e. g. salt and dimonds. Amorphous solids - e. g. plastic and glass non polar you don t have partial charges you can move electron clouds to one place to another - this is the primary way that thy react with each other. Stronger the intermolecular attraction you will have to add more heat to break the bond. The higher the normal boiling point of the liquid. When you push the electrons to one side you will get a partial negative and positive side. Larger molar mass= more electrons = larger electron cloud= increased polarizability=stronger attractions. More surface-to-surface contact = larger induced dipole = stronger attraction the stronger the attractive forces between the molecules the, higher the boiling point would be. Like disolves like as they have to have the same or similar bonds to be soluble. Ions from an ionic compound are attracted to the dipole of the polar molecules.
