In this experiment, students build a spectrometer to explore infrared radiation and greenhouse gases in an inquiry-based investigation to introduce climate science in a general chemistry lab course. The lab is based on the exploration of the thermal effects of molecular absorption of infrared radiation by greenhouse and non-greenhouse gases. A novel feature of the experiment has students building an infrared spectrometer, using a hot plate as an IR source, a sample compartment employing a plastic cuvette holder with open sides (to standardize the path length), and a low-cost infrared thermometer. Students, working in groups, (1) explore a PhET simulation; (2) design a set of experiments in response to a scientific question, “comparing the absorption of infrared light in the presence and absence of each different sample of gas, are there any significant differences that can be observed experimentally?”; (3) reflect on climate science and their experimental results by visiting the American Chemical Society Climate Science Toolkit; and (4) communicate their results in lab by constructing and presenting a poster. Assessment of student responses to a pre- and postexperiment question suggests that the lab has a positive influence on student understanding of the concepts involved in identifying greenhouse gases. Results from postexperiment questions also provide information for what aspects of the online resources students found useful.
The mechanism of gold(i)-thiolate, disulfide exchange was investigated by using initial-rate kinetic studies, 2D ((1)H-(1)H) ROESY NMR spectroscopy, and electrochemical/chemical techniques. The rate law for exchange is overall second order, first order in gold(i)-thiolate and disulfide. 2D NMR experiments show evidence of association between gold(i)-thiolate and disulfide. Electrochemical/chemical investigations do not show evidence of free thiolate and are consistent with a mechanism involving formation of a [Au-S, S-S], four-centered metallacycle intermediate during gold(i)-thiolate, disulfide exchange.
Phosphine gold(I) thiolate complexes react with aromatic disulfides via two pathways: either thiolate-disulfide exchange or a pathway that leads to formation of phosphine oxide. We have been investigating the mechanism of gold(I) thiolate-disulfide exchange. Since the formation of phosphine oxide is a competing reaction, it is important for our kinetic analysis to understand the conditions under which phosphine oxide forms.
The concentration of dimethyl sulfide (DMS) in seven different samples of research grade dimethyl sulfoxide (DMSO), including one deuterated sample, was measured by GC-MS. The average concentration of DMS is 0.48 AE 0.14 mM (range: 0.44-0.55 mM) and ca. 0.35 mM in DMSO-d 6 . The presence of DMS in DMSO is potentially problematic for compounds that are susceptible to reaction with DMS and are present at mM-mM concentrations. Standard methods of purification of DMSO were unsuccessful in removing all traces of DMS.Dimethyl sulfoxide (DMSO) is an aprotic, polar solvent that is widely used in chemistry and biology. It dissolves hydrophobic and hydrophilic solutes, 1-4 is used as a cryoprotectant for biological samples, 5 and is a component in drug delivery. 6 Researchers have taken advantage of the miscibility of DMSO with water, organic solvents, and ionic liquids (IL) to solubilize polymers and enhance reaction chemistry. For example, recent reports describe the benecial effects of a DMSO : IL co-solvent as a green solvent for hydrolysis of cellulose; 7 and a DMSO : water co-solvent to promote thiol-disulde dynamic combinatorial chemistry. 8 DMSO can also participate in reactions. Some examples include: playing an essential role as a ligand for transition metal catalysts, 9,10 an oxidant for the oxidation of thiols or alcohols, 11,12 and a participant in the oxidation of gold phosphine complexes. 13 We have employed DMSO as a solvent in our kinetic studies of the inuence of solvent dielectric on metal thiolate-disulde exchange reactions. 14-16 Our interest lies in comparing metalmediated thiolate-disulde exchange to metal-free thioldisulde exchange, the latter of which proceeds at a slower rate in high dielectric solvents, such as water or DMSO, than in low dielectric solvents such as THF or CH 2 Cl 2 . 17 Since the metal thiolate complexes and disuldes employed in our kinetic studies are not water-soluble, DMSO was selected as a solvent with a high dielectric constant (3 ¼ 46.45) 1 for these studies. During the course of kinetic investigations, we observed that addition of bis(4-nitrophenyl)disulde to DMSO, in the absence of any metal thiolate, formed a pale red solution with an absorbance near 500 nm. Bis(4-nitrophenyl)disulde is isolated as a pale yellow solid aer recrystallization from boiling nbutanol. When the disulde is dissolved in solvents such as CH 2 Cl 2 , CH 3 CN, acetone, or THF, the solution does not turn red (i.e. there is no absorbance at 500 nm). We suspected that the species responsible for the color in solutions of DMSO was 4-nitrophenylthiolate because addition of base (NEt 3 ) to a DMSO solution of 4-nitrophenylthiol produced a similar red solution with l max ¼ 502 nm. 18 Over the course of time, we observed that when bis(4-nitrophenyl)disulde is dissolved in a variety of DMSO solvents obtained from different commercial suppliers, a similar red color was produced. Thus, we hypothesized that an impurity in DMSO reacts with the disulde to form 4-nitrophenylthiolate. DMSO is an odorle...
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