Cuo Nanoparticle Lab Report

The purpose of this lab was to determine the empirical formula of copper oxide compound. In the lab, hydrochloric acid and copper oxide compound was mixed until it formed a blue solution. An oxidation-reduction reaction, a reaction in which there is an exchange of electrons between elements, was performed by adding zinc to the solution to displace the copper in copper chloride. Zinc, in this case, was oxidized by losing two electrons (0 → 2+) while copper was reduced by gaining two electrons (2+ → 0). Also, when the copper was displaced, it became a precipitate, which is a substance that comes out of a solution as a solid due to insolubility.

After this, the solution was poured into a volumetric flask just about to the 1dm3 line and then it was left there to cool to the same temperature as the room before filling precisely to the 1dm3 line with distilled water. The molar mass of CuSO4.5H20 was 249.5 so that means 249.5g of copper sulphate was needed to dissolve, in order to make a standard solution, into 1dm3of distilled water. Following this, a linear dilution of the CuSO4.5H2O was made in order to be used to make a calibration curve after using the colorimeter to write down the absorbance of each sample. A linear dilution is diluted with distilled water in order for it to make the concentration weaker and weaker. For this investigation, the dilutions made ranged from 0.01 to 0.1 M/l . It was essential to only make up 10cm3

In this experiment an elemental copper was cycled a series of five reactions where it ended with pure elemental copper as well, but at different stages of the cycle the copper was in different forms. In the first reaction, elemental copper was reacted with concentrated nitric acid where copper changed the form from solid to aqueous. Second reaction then converted the aqueous Cu2+ into the solid copper II hydroxide (Cu(OH)2) through reaction with sodium hydroxide. The third reaction takes advantage of the fact that Cu(OH)2 is thermally unstable. When heated, Cu(OH)2 decomposes (breaks down into smaller substances) into copper II oxide and water. When the solid CuO is reacted with sulfuric acid, the copper is returned to solution as an ion (Cu2+). The cycle of reactions is completed with the

The purpose of performing the variety of tests that we did was to give more accurate results of what the unknown mineral was. By roasting the copper mineral, we obtained copper(II) oxide. This new sample came out of the crucible grayish-black. It was very brittle and full of cracks. This provided the percent composition that was necessary in finding the unknown mineral. When performing

Semiconductor Nano crystals or quantum dots are materials that are typically 2-20 nm in diameter, consisting of approximately twelve to fourteen thousand atoms. The effect of quantum confinement results, in the electrons and holes in the Nano crystal to exhibit quantized energy states; thus enabling them to exhibit novel physical properties that are not found in their bulk counterparts. Research in semiconductor quantum dots started with the realization that the optical and electronic properties of these particles were strongly dependent on particle size, due to quantum confinement of the charge carriers in small spaces.

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.

Before the synthesis of the Copper Iodine Compound, the identities provided (CuNO3)2 and Nal weighed 1.65 g and 4.7 g, respectively. After being weighed, the (CuNO3)2 exhibited a blue color, while the Nal, through observation, was a white color. However, when both identities were combined, the product turned into a brown and red rocky material. Once 20 mL of deionized water was added, the product quickly turned pale pink paste. After the solution was repeatedly washed with a total of an additional 100 mL of deionized water, the product was powdery and pink with small grains, and was left to air-dry. Once the product was air dried, it was observed to be a pale pink color, while the filter paper was stiff as the product was hard and dry. Therefore, the solid was scraped off onto a recrystallizing dish. However, the mass of an empty recrystallizing dish needed to be recorded in order to compare how much of the synthesized copper iodide was obtained. Within this case, the empty recrystallizing dish used weighed 32.01 g, the product on the empty dish weighed 1.03 g, having a total weight of 33.04 g.

The Spec 20 was turned on and set the wavelength for maximum absorbance for copper(II) solutions, 600 nm, 30 minutes prior to the start of the experiment. 12 test tubes were cleaned thoroughly and a tape label was added to the top identifying which solution would be placed within and then they were set in a test tube rack to dry. The amount of solid copper(II) sulfate pentahydrate (CuSO4 H2O ) needed to create 20.0 mL of 0.5 molarity solution was calculated, using the equation for molarity the molar mass, as 2.50g. The CuSO4 H2O and a 100 mL beaker were carried to the instrument room. Small amounts of solid CuSO4 H2O were placed onto a paper towel which was gently tapped over the beaker until exactly 2.50g was reached. Approximately 5

Chloride Equation: Ag+ (aq) + Cl- AgCl (s) Sliver Nitrate- Adding dilute nitric acid. (Sliver nitrate + dilute nitric acid.)

A 50 mL beaker was used to mix 15 mL of solution A with 15 mL of solution B inside the beaker. The reaction yield solution F which was used for the concentration and temperature experiments. The cuvettes were labeled at the top 1a, 2a, 3a, 4a and 1b, 2b, 3b, 4b (Wilson, et al 2015). The blank cuvette 1a was prepared as indicated in the mixing tables by blanking the spectrophotometer, which ensured an accurate reading at zero at 405 nm. The spectrophotometer was not blanked for the remainder of the

The Fe-Co deposit obtained from ethaline and reline was successfully deposited on a copper substrate by maintaining a steady potential of 3.0 V at 60℃ for 2 hours. The Fe-Co coating from reline was dark black in colour, whereas the Fe-Co coating from ethaline appeared to show a tint of grey on the surface. The Fe-Co deposits in both liquids were smooth and uniform. Figure 6.3 a and b show the SEM images of Fe-Co deposited from ethaline and reline. It is clear from the images that there is a variation in morphology from both liquids. The Fe-Co coating from reline appears to show a more nodular shaped structure which is evenly spread on the surface of the copper substrate when compared to Figure 6.3 a.

The reaction characteristics of basic copper carbonate 〖mCuCO〗_3⋅n〖Cu(OH)〗_2 were observed by changing the reaction mole ratio. The reaction mole ratio of sodium carbonate to copper chloride (II) was controlled from 1.08 to 1.68. Fig. 1 shows the XRD patterns of copper carbonate powder. At a reaction ratio of 1.08, paratacamite (Cu_2 Cl(OH)_3 ), beside alkali copper carbonate, was formed because of incomplete reaction at a copper content of 53.9 wt%. Lack of sodium carbonate may cause incomplete reaction with copper chloride (II) because of low pH (6.0) of the solution [12]. The copper content according to the reaction mole ratio were 57.7, 50.5, 58.8, 59.3, and 59.8 wt% at the reaction mole ratios of 1.20, 1.32, 1.44, 1.56, and 1.68, respectively.

2. Miller, F.; Wilkins, C. Infrared Spectra and Characteristic Frequencies of Inorganic Ions. Ph.D. Dissertation, Mellon Institute, Pittsburgh, PA, 1952.

When the sulfuric acid was added to copper (II) oxide, the solution turned blue. This was due to the formation of aqueous copper (II) sulfate, which produced the copper ions to change the color of the solution.

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