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Unformatted text preview: possible to achieve a minimal energy state. However, the shows that the ions are actually repelled at small distances. To explain this observation, remember that the ions' nuclei are both positively charged. When the nuclei approach each other, they repel strongly--accounting for the steep rise in potential as the ions get closer than the bond length. Figure %: Plot of potential energy versus distance for oppositely charged ions The depth (y-axis) of the minimum in the potential energy curve above represents the bond strength, and the distance (x-axis) at the energy minimum is the bond length. Using Coulomb's law and the bond length, one can actually predict with some accuracy the strength of an ionic bond. Performing a series of these calculations you find that ionic compounds formed by ions with larger charges create stronger bonds and that ionic compounds with shorter bond lengths form stronger bonds....
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This note was uploaded on 11/14/2011 for the course CHEM ch 101 taught by Professor - during the Fall '10 term at Montgomery.
- Fall '10