Amino-Polyalcohol Ligands Essay

1 Copper (II) Nitrate Crystals in vial, Copper Metal - 6-8 pc. in bag 2"x 3"

When the red Co(NO3)2*6H2O crystal was added to the white NH4 crystal, and water was added to dissolve, the solution turned blue in color. As the solution was nixed, the color changed to that of a blue-purple and a blue precipitate formed. When the 6 M NH3 began to be added, the color shifted to dark purple color after 15 mL of ammonia and the amount of the precipitate was less. After 20 mL of ammonia, the solution became a red brown with very little of the blue precipitate. After 30 mL of ammonia, the solution was similar in color to an iodine solution, a dark brown-red, almost black in color. At this point there was no visible precipitate on the surface of the solution. After 40 mL of the ammonia had been added, the solution was the same iodine like color as before. When closely examined, there was a black precipitate that had settled on the bottom of the beaker. At this point, hydrogen peroxide, 3% H2O2, was added to solution. After 4 mL of the H2O2 was added, the solution was the same color and the precipitate had not changes. After 8 mL of the H2O2, there was not noticeable change. After 12 mL of the H2O2, the solution was slightly redder in color but the precipitate had not changed. After 15 mL of H2O2, the solution was the same color and no changes had occurred to the precipitate. At 17 mL, the solution began to effervesce slightly, though there

The product was then suspended in 2 ml of water with a stir rod in a 50 ml Erlenmeyer flask and heated to boiling. Water was added in one milliliter increments until all the product was dissolved (18 ml added total). The saturated solution was allowed to slowly cool, and gradual white crystal formation was observed. Recrystallized product was collected once more by suction filtration with the Hirsch funnel once crystallization ceased. Collected product dried on a watch glass for a week, weighed 0.14 g (1.2 mmol), and the melting point was 139°-141°

The product obtained had a melting point of approximately 107 °C and a weight of .324 grams. Some of the product would not dissolve in water and so was removed through vacuum filtration, which left .141 g not dissolved in solution. It took 13.2 mL of sodium hydroxide to turn the solution of the product dissolved in water pink. A molecular weight of 138.63 g/mol was calculated from the data. These results indicate that the product was 2-methylbenzoic acid, the Grignard reagent was 2-methylphenylmagnesium bromide, and the unknown bromide solution was 2-methylbromobenzene. Calculations showed that the limiting reagent of the Grignard preparation was magnesium and that the experiment had a 23.13 % yield.

Describe what you believe is implied by the term “engagement risk.” What are the key factors likely considered by Deloitte and other audit firms when assessing engagement risk? How, if at all, are auditors’ professional responsibilities affected when a client proposes a higher than normal degree of engagement risk?

7. NiSO4, nickel sulfate was in the past very valuable and it is recognized by its “envious” green nature.

The compound was tested for the presence of ammonium, carbonate, sulfate, chloride, and nitrate, as seen in Table 2. The nitrate test produced a precipitate, indicating the presence of the nitrate ion in the compound. At this point it was hypothesized that our unknown compound was calcium nitrate.

Documentation: 28 August & 1 September 2015 C4C Lauren Truax was my lab partner and we worked together to discover the results of the unknown mineral and calculations.

The pipet was put into the top of the condenser and leaving no open spaces. The vacuum served to get rid of the nitrogen oxide gases that were formed during the oxidation reaction. The solution was heated for 30 minutes, beginning the time when the first sign of nitrogen oxide fumes were observed. After the 30 minutes, the solution was removed and cooled for a few minutes. The solution turned was a brownish-yellow color and all the crystal were dissolved, leaving a liquid. The solution was then transferred, using a Pasteur pipet, to 3 mL of water in a beaker. The reaction flask was rinsed to remove the remainder of the solution. The solution was stirred with a glass rod until room temperature of the solution was achieved. A yellow solid was to form, but instead the solution remained aqueous in the case of the specific experiment explained here. With additional scraping of the solution with a glass rod, no crystals formed at all. The next procedure, if the crystals had formed was to crush the solid with the glass rod and filter the solid until the crystals were dry. The mass would then be weighed and the crystals were to be recrystallized with 95% ethanol. The crystals were to be cooled in ice water to get full crystallization and then the crystals were to be filtered and air dried, then weighed.

Aim: To classify unknown substances according to their structure type and to observe how the structure of materials affects their uses.

Questions like What is a Ligand, or What is a antagonists role in the body are completely open ended and can lead to many different answers among students. Our game displays what role each section of the processes within the body does in a simple method using simple tetras like shapes. Instead of students trying to memorize a textbook definition and struggling to remember medical terms, students who play this game will figure out the roles of each part of the process naturally. No student wants to spend hours attempting to understand complex concepts. Our games goal is to motivate people to learn about these complex concepts. Giving students a means to study that does not feel like studying.

Comparison of the Behaviour of Halides Purpose: to compare the properties of halides and relate them to the position of halogens in the periodic table. To use these properties to identify an unknown halide. Hypothesis: The halogens that are further down the group are more reactive than those that are further up. Also, Unknown substance C will be sodium iodide.

Introduction: The purpose of this lab was to use different spectra to determine the structure of an unknown compound. The mass spectrum showed that the molecular ion had a mass value of 138. Because the molecular ion is the same as the molecular mass of the compound, then the mass of the molecular ion can be used to find the molecular formula of the unknown compound. Additionally, because the mass of the molecular ion is even, then this indicates that there is an even number of nitrogen atoms in the compound- with zero being considered as an even number.

The synthesized pellets of La1-xSrxMnO3, (x=0.3, 0.4 and 0.5) manganites are shown in figure

Olmsted, John III; Williams, Greg; Burk, Robert C. Chemistry, 1st Canadian ed.; John Wiley and Sons Ltd: Mississauga, Canada, 2010, pp 399 - 406