INTERMOLECULAR ATTRACTIONS

INTERMOLECULAR ATTRACTIONS - covalent molecules containing...

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INTERMOLECULAR ATTRACTIONS Intermolecular forces are forces acting among the particles of a compound. If these forces did not exist, the condensed phases (liquid and solid) could not exist! These forces hold the particles close to one another in liquids and solids. Physical properties of compounds such as boiling point, melting point, vapor pressure… depend on these forces. There are four types of intermolecular forces: ION-ION INTERACTIONS: These are the forces of attraction among oppositely charged ions in ionic compounds. They are the strongest types of interactions. They are controlled by coulomb’s law: For ions of different charges, the ion-ion interaction increases as the charges on ions increase. NaF vs MgO For ions of similar charges, the ion-ion interaction increases, as the ions become smaller. NaF vs NaCl HYDROGEN BONDING: These are strong interactions that occur among polar
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Unformatted text preview: covalent molecules containing H directly attached to one of the three small electronegative elements: O, N, or F. DIPOLE-DIPOLE INTERACTIONS: These are strong interactions that occur between polar covalent molecules. They are due to the attraction of the + atoms of one molecule to the -atoms of another molecule. DISPERSION FORCES (LONDON FORCES): Very week attractive forces between short lived temporary dipoles. They are present for all types of molecules. They are the ONLY type of intermolecular forces for non-polar substances. Dispersion forces result from the attraction of the positively charged nucleus of one atom for the electron cloud of an atom in nearby molecules. This induces temporary dipoles in neighboring atoms or molecules. THEY ARE GENERALLY STRONGER FOR MOLECULES THAT ARE LARGE!!...
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INTERMOLECULAR ATTRACTIONS - covalent molecules containing...

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