4 - 4 0.76 5 None of these 6 0.63 Explanation rAl = 53 pm...

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4. 0.76 5. None of these 6. 0.63 Explanation: rAl = 53 pm The energy Ep 1 rBe = 27 pm -|z| , so the ratio is r2 2 |zAl | rBe |3| (27 pm)2 EAl = 2 = |2| (53 pm)2 = 0.389284 EBe |zBe | rAl 001 (part 1 of 1) 10 points Identify the kinds of intermolecular forces that might arise between molecules of trans CHCl CHCl. 1. dipole-dipole 2. None of these 3. London forces, dipole-dipole, hydrogen bonding 4. London forces, dipole-dipole 5. London forces correct 6. hydrogen bonding Explanation: Cl C H C Cl H 003 (part 2 of 2) 10 points Which ion will attract a water molecule more strongly? 1. Al3+ 2. Equal attraction 3. Be2+ correct Explanation: The attraction of the Be2+ ion will be greater than that of the Al3+ ion. Even though the Be2+ ion has a lower charge, its radius is much smaller than that of Al3+ , making the attraction greater. 004 (part 1 of 1) 10 points Which of the following cations is likely to be hydrated in compounds? 1. Cs+ 2. K+ 3. Li+ correct 4. Rb+ 5. NH+ 4 Explanation: Li+ is the smallest. 005 (part 1 of 1) 10 points is non-polar. 002 (part 1 of 2) 10 points Calculate the ratio of the potential energies for the interaction of a water molecule with an Al3+ ion (of radius 53 pm) and with a Be2+ ion (of radius 27 pm). 1. 0.39 correct 2. 0.24 3. 0.52 Which of the following compounds is UNLIKELY to be commonly available and thus not found in the laboratory? 1. BaCl2 2H2 O 2. KCN 2H2 O correct 3. La(NO3 )3 6HO 4. Na2 CO3 10H2 O 5. CuSO4 5H2 O Explanation: K+ is only a +1 cation AND it is too large to substantially attract waters of hydration. +2 and +3 cations will generally form hydrates. Na+ will also attract water due to its smaller size. 006 (part 1 of 1) 10 points What would be the most significant type of intermolecular forces in a liquid sample of fluoroform (CHF3 )? 1. dispersion 2. dipole-dipole correct 3. covalent 4. hydrogen bonding 5. ionic Explanation: London forces, dispersion forces, van der Waals or induced dipoles all describe the same intermolecular force. London forces are induced, short-lived, and very weak. Molecules and atoms can experience London forces because they have electron
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clouds. London forces result from the distortion of the electron cloud of an atom or molecule by the presence of nearby atoms or molecules. Permanent dipole-dipole interactions are stronger than London forces and occur between polar covalent
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This note was uploaded on 01/12/2010 for the course BME 14345 taught by Professor Orlyalter during the Fall '09 term at University of Texas.

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4 - 4 0.76 5 None of these 6 0.63 Explanation rAl = 53 pm...

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