Quiz7key - equally paramagnetic although individual properties of each molecule may influence their magnetism(d picture of 1 g picture of 2 g 2

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CHEMISTRY 131 Quiz #7 Friday, March 17, 2006 Name: ___________Key_______________________ 1. For the molecules F 2 + and N 2 + : (a) Draw the MO diagram and determine which molecule has the strongest bond; (2 points) (b) Determine the molecular electron configuration; (2 points) (c) Determine the magnetic properties of the molecules; (2 points) (d) Draw the picture of the highest occupied molecular orbital (HOMO). (2 points) (a) 1 σ g 1 σ u 2 σ g 1 π u 1 π g 2 σ u 2s 2p 2s 2p F F F 2 + 1 σ g 1 σ u 2 σ g 1 π u 1 π g 2 σ u 2s 2p 2s 2p N N N 2 + bond order for F 2 + : (8 – 5)/2 = 1.5; for N 2 + : (7 – 2)/2 = 2.5. Therefore, since N 2 + has the higher bond order, it has the strongest bond. (b) MO config for F 2 + : (1 σ g ) 2 (1 σ u ) 2 (2 σ g ) 2 (1 ! u ) 4 (1 ! g ) 3 ; for N 2 + : (1 σ g ) 2 (1 σ u ) 2 (1 ! u ) 4 (2 σ g ) 1 . (c) Since each molecule contains an unpaired electron, each one is paramagnetic. Technically, they should be
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Unformatted text preview: equally paramagnetic although individual properties of each molecule may influence their magnetism. (d) picture of 1 g picture of 2 g 2. Briefly explain why the valence orbitals for F are lower in energy than the valence orbitals for N. (2 points) Z* is higher for F than for N, since F has more protons than N. Although it also has more electrons, these electrons do not completely screen the increased nuclear charge, so that Z* builds up for the valence electrons. This increased Z* in turn causes an increased electrostatic interaction between the valence electrons and the nucleus, which decreases the energies of these orbitals....
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This homework help was uploaded on 04/18/2008 for the course CHEM 131 taught by Professor Landry during the Spring '08 term at Vermont.

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