Experiment 1 and 2
Korleyfah Mouth
Chem 331 Thursday 2:00pm
Dr. Lijuan Li
20A Preparation of CuCl2~2DMSO
20B Preparation of RuCl2~4DMSO
Abstract In order to synthesize our metal complexes, we were able to make both Copper and Ruthenium metals. From this, we combined each metal complex with DMSO by refluxing the compound. The metal complexes were analyzed through their melting point and IR spectroscopy to determine whether the metal bonded to a Sulfur atom or an Oxygen atom of the DMSO. After analyzing the IR spectrum, it was determined that S=O shifted to a lower wavenumber in CuCl2~2DMSO and that S=O shifted to a higher wavenumber in RuCl2~4DMSO.
Introduction Depending on the metal, it will bond to DMSO through its oxygen or sulfur atom. This will cause the frequency of the S=O bond absorption to move depending on which atom it bonds to. For oxygen bond the frequency will be low due to the weakened interaction. As for sulfur bond the frequency will be higher because the metal donates the electrons as a back donation to the pi orbital in DMSO.
In the first experiment, I had to synthesized CuCl2~2DMSO to determine which DMSO atom; Sulfur or Oxygen, combined to Copper (II) Chloride. I was able to determine it base on finding the melting point and observing the Infrared Spectroscopy. Since copper is a hard metal, it will most likely bond to an oxygen atom because they are both hard. In the second experiment, I also synthesized RuCl2~4DMSO to determine which DMSO atom; Sulfur or Oxygen, combines to Ruthenium (III) to be reduced to Ruthenium (II). I was able to determine it based on finding the melting point and observing the Infrared Spectroscopy. Since ruthenium is a soft metal, it will most likely bond to Sulfur because they are both soft.
20A Preparation of CuCl2~2DMSO
Experimental We prepared the sample by synthesizing Copper Chloride with DMSO. 0.160 grams of CuCl2~2DMSO was added to a 10 mL Erlenmeyer flask with a magnetic stir bar. Than 1 mL of absolute ethanol
Chem 331 Thursday 2:00pm
Dr. Lijuan Li
20A Preparation of CuCl2~2DMSO
20B Preparation of RuCl2~4DMSO
Abstract In order to synthesize our metal complexes, we were able to make both Copper and Ruthenium metals. From this, we combined each metal complex with DMSO by refluxing the compound. The metal complexes were analyzed through their melting point and IR spectroscopy to determine whether the metal bonded to a Sulfur atom or an Oxygen atom of the DMSO. After analyzing the IR spectrum, it was determined that S=O shifted to a lower wavenumber in CuCl2~2DMSO and that S=O shifted to a higher wavenumber in RuCl2~4DMSO.
Introduction Depending on the metal, it will bond to DMSO through its oxygen or sulfur atom. This will cause the frequency of the S=O bond absorption to move depending on which atom it bonds to. For oxygen bond the frequency will be low due to the weakened interaction. As for sulfur bond the frequency will be higher because the metal donates the electrons as a back donation to the pi orbital in DMSO.
In the first experiment, I had to synthesized CuCl2~2DMSO to determine which DMSO atom; Sulfur or Oxygen, combined to Copper (II) Chloride. I was able to determine it base on finding the melting point and observing the Infrared Spectroscopy. Since copper is a hard metal, it will most likely bond to an oxygen atom because they are both hard. In the second experiment, I also synthesized RuCl2~4DMSO to determine which DMSO atom; Sulfur or Oxygen, combines to Ruthenium (III) to be reduced to Ruthenium (II). I was able to determine it based on finding the melting point and observing the Infrared Spectroscopy. Since ruthenium is a soft metal, it will most likely bond to Sulfur because they are both soft.
20A Preparation of CuCl2~2DMSO
Experimental We prepared the sample by synthesizing Copper Chloride with DMSO. 0.160 grams of CuCl2~2DMSO was added to a 10 mL Erlenmeyer flask with a magnetic stir bar. Than 1 mL of absolute ethanol
References: Boschmann, E; Wollaston, G.J. Chem. Edu. 1982, 59,57 Ebsworth, E. A. V.; Ranking, D.W.H.; Cradock, S., Structural Methods in Inorganic Chemistry, Blackwell: Oxford, 1987 Pike, M Ronald; Singh, M Mono; Szafran Zvi. Microscale Inorganic Chemistry; A Comprehensive Laboratory Experience. New York 1991, p218-222. Reynolds, W. R, “Dimethyl Sulfoxide in Inorganic Chemistry” in Progress in Inorganic Chemistry, S. J. Lippard, Ed., Interscience: New York, 1970, Vol 12, p. 1.