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Unformatted text preview: the positive end of one molecule is near the negative end of another moderately strong (ca. 10 kJ/mol) Important for mixtures of polar gases (HCl, HBr, etc.) with each other, in liquefied polar gases, and in solu-tions of polar molecules in polar solvents (H 2 O, NH 3 ) Hydrogen bond attractive forces that exists between a hydro-gen atom covalently bound to a very electro-negative atom, X , and a lone pair of electrons on another atom Y . moderately strong (ca. 5–40 kJ/mol) Important when X is F, O, or N. Responsible for the high boiling points of H 2 O, NH 3 . Can exist in the gas, liquid and solid phases of matter. Ion-dipole attractive forces be-tween an ion and a molecule with a perma-nent dipole strong Important in cases of solu-tions of ionic compounds in polar solvents (e.g., NaCl in H 2 O, where [Na(OH 2 ) x ] + is found) *Compare these to the strength of the H–H bond in H 2 (432 kJ/mol)...
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This note was uploaded on 03/17/2010 for the course CHEM chem102 taught by Professor Adamlist during the Spring '10 term at Vanderbilt.
- Spring '10