CHEM 1301 Chapter Notes - Chapter 8.2: Caesium, Chemical Polarity, Molar Mass
22 Nov 2017
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Document Summary
Predicting the relative magnitudes of intermolecular forces and their effects on physical properties of substances. Larger the charge of the interacting particles = stronger attraction. Longer the distance between the interacting particles = weaker attraction. However these intermolecular attractive forces are small relative to the bonding forces between atoms (intramolecular forces) The strongest intermolecular (interparticle) forces ae when only ions are involved in bonding (ionic bond) Only polar molecules with a permanent dipole exhibit this force: hydrogen bonding force- a type of dipole-dipole force that arises between molecules that have a h atom bonded to a small, highly electronegative atoms with lone pairs: o, When an ionic substance dissolves in water, the ion and a nearby polar water molecular attracts each other via an ion-dipole interaction. Ions from an ionic compound are pulled towards the dipole of polar molecules. The power of the ion-dipole attraction is one of the key factors that governs the solubility of ionic compounds in water.
