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Bioinorganic Coordination Chemistry: Copper (II) Tetraphenylporphyrinate

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Introduction

Kristin Quinn Bioinorganic Coordination Chemistry: Copper (II) Tetraphenylporphyrinate February 17, 2005 Quinn 1 Kristin Quinn Intermediate Inorganic Lab 17 February 2005 Abstract This experiment uses H2TTP made during the last lab and hydrated copper (II) acetate to convert the H2TTP to Cu(TTP). The reaction proceeds by being refluxed for 30 minutes. The final product is a non-iridescent purple color, unlike the vivid, shimmering purple color of the starting H2TTP. Introduction Thin layer chromatography, or TLC, is used as a prerequisite for column chromatography. When performing types of chromatography, like TLC, the polarity of solvents is extremely important. This lab uses TLC plates, five solvents (hexane, toluene, ethyl acetate, dichloromethane, and acetone), and small evaporating dishes to determine which solvent would be best to use in column chromatography. The least polar solvent is hexane, which has a polarity index of 0.1. Toluene has a polarity index of 2.4, while ethyl acetate's is almost twice that at 4.4. By comparing the polarity indexes, you can tell what solvent will separate your dots of product on your TLC plates the best (Skoog 761). ...read more.

Middle

10. Dilute the product once again with dichloromethane and filter with a pipet stuffed with cotton. Make sure the product is a very light pink color; it will need to be very diluted. 11. Take a UV-vis spectrum of the product. Data By looking at the TLC plates (attached) of the starting and final products, it is easy to see that dichloromethane would be the best solvent for column chromatography. The ethyl acetate moved the final product up leaving just one spot near the top of the plate, but it left one wide band for the starting product. Toluene left two lines from top to bottom for both products, with no clear distinction of a certain spot. Hexane didn't move the products at all from the beginning line. Acetone separated the starting product, but not the final product. Dichloromethane clearly separated both products. The reason for this separation is because dichloromethane is more polar than the other solvents. Even though I accidentally spilled most of my product while pouring it into the separatory funnel, the product left was identical to everyone else's by comparison of the UV-vis spectrum. ...read more.

Conclusion

The reason for this is because of the acidity of the hydrogen atoms. Since the hydrogens are acidic, they want to "hold" onto the silica gel, which will cause them to elute after a longer time period. 2. The rates at which compounds elute from a silica gel column depend on any pretreatment of the silica gel. In which case would a compound elute faster: down a column made of silica gel that had been previously heated at 150 degrees Celsius under vacuum for 8 hours, or down a column made of silica gel that had been sitting open in the laboratory for a few days? Explain. When you heat silica gel, water evaporates off the gel leaving open sites where polar molecules can bond. When you let silica gel out in the open, it will collect water molecules on it. Compounds would elute faster down a column that has been heated at 150 degrees for 8 hours because the gel would be dry. 3. A mixture of cis and trans isomers of the neutral complex Cr(CO)4[P(C6H5]2 is loaded onto a silica gel and eluted with CHCl3. Which isomer would elute first, and why? The trans isomer would elute first. ...read more.

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