~~ Chem 207 Lab - Report 6 - Results and Discussion: Lab 6...

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Results and Discussion: Lab 6 Part A For Part A, directions from the Chem 207 lab manual were carefully followed in order to construct a NH 3 molecule and a SF 4 molecule. The Spartan program was used in building the molecules and was also used to verify each molecule’s bond angles, bond lengths, and dipole moments given on pages 38-40. The observations made in lab perfectly match was listed for both NH 3 and SF 4 Part B For Part B, CH 3 Cl, PCl 5 , and NO 3 - molecules were built and optimized using the Spartan program in lab. For each molecule, a number of observations were made and compared to prelab Lewis structure, formal charge, molecular shape, and molecular polarity predictions. For the CH 3 Cl molecule, the predictions and actual lab observations are seen below. Prelab Predictions Actual Lab Observations Lewis Structure Carbon in center, single bonded to three separate hydrogen atoms and one chlorine atom. Carbon in center, single bonded to three separate hydrogen atoms and one chlorine atom. Formal Charges (FC) or Actual Charge (Q) FC of H 1 = 0 FC of H 2 = 0 FC of H 3 = 0 FC of C = 0 FC of Cl = 0 Overall FC = 0 Q of H 1 = 0.134 Coulombs Q of H 2 = 0.133 Coulombs Q of H 3 = 0.133 Coulombs Q of C = -0.222 Coulombs Q of Cl = -0.178 Coulombs Overall Q = 0 0.133 (2) + 0.134 - 0.222 - 0.178 = 0 C Bond angles All about 109º H-C-H = 110.46º H-C-Cl = 108.46º Molecular Shape Tetrahedral Tetrahedral Polarity Polar Dipole moment towards the chlorine atom. Polar Dipole moment towards the chlorine atom. (2.25 debyes) Bond Length N/A C-H = 1.078 A C-Cl = 1.785 A As shown above, all of my predictions were correct. Although I predicted a zero FC on each individual atom (when there was really a partial charge), in the end, the overall charge for the CH 3 Cl molecule was zero. When
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~~ Chem 207 Lab - Report 6 - Results and Discussion: Lab 6...

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