Experiment 1 and 2

1. Decide if the mineral is metallic or non-metallic based on its luster and streak.

Metal is responsible for the colour produced in the flame test for that salt. All salts contain

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

The main purpose of this experiment was to show that single displacement reactions between metals according to their reactivity, with more reactive elements having the power to displace less reactive elements and take their place in a chemical compound (Beran, 2014). This was supported by the results of the experiment, where solid metals were combined with aqueous solutions that contained another element, and reactions only took place when the solid metal was more reactive than the other element in the compound. Only three attempted trials resulted in a failure to produce a reaction, namely the combinations of copper with hydrochloric acid, and copper with nickel sulfate. The outcomes of these trials are justifiably reasonable because copper is ranked lower in the

In doing so, the identity of the unknown solutions was determined through comparing the colors of the unknown to that of the known, which were dependent on the varying energy transitions the electrons went through. Therefore, the purpose of the experiment was successfully achieved. Since LiNO3 and Sr(NO3)2 were red/red orange in color, it was determined that lithium ions and strontium ions have the least amount of energy due to the fact that red has the longest wavelength in the spectrum, and colors with longer wavelengths have lower energies. The energy of each the other metallic ions increased in accordance with the energy of the wavelength emitted from that color based on the color spectrum. Potassium had the highest energy emitted, since violet is at the opposite end of the spectrum and has the shortest wavelength and highest

For the organic layer, we had a melting point range of 240-243°C. For the IR spectra, we did note the C-Cl bond although there was not an OH bond present.

And copper (II) ions were reduced to copper because it gained electrons and its oxidation number changed from +2 in copper (II) ions to 0 in copper.

I started with elemental copper metal and then reactions occur step by step as follows:

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 result from the IR spectra for Trans-[Bis(inosinato)palladium(II)], and inosine are summarized in Table 2 and 3. It is important to note that Trans-[Bis(inosinato)palladium(II)] compound had an extra carbonyl peak at 1712.21 cm-1 which is from inosine impurity.

To achieve this, the Heaven Lab uses computational chemistry and laser spectroscopy. For computational chemistry, they use ECP (Effective Core Potential) to correct the mass of the electron and the Darwin term for the actinide elements; following the theories of configuration interaction, density functional theory, and active space methods. Also, Thorium oxide (a specific actinide detectable through spectroscopy) has been tested using laser ablation of an actinide rod with Laser induced fluorescence, REMPI, PFI, PFI-ZEKE, and MCP. Ultimately, they have found that computational chemistry and laser spectroscopy are significant tools in identifying bonding properties of

Experimental approach: In the first reaction, copper metal turnings oxidize when put in contact with nitric acid and become copper nitrate.

Copper is a transition metal with 29 protons and electrons this maintains an electronic balance within the atom (Bentor). The average atomic mass for copper is 63.546 amu. Coppers’

In the fourth reaction, 15 mL of 6.0 M sulfuric acid was added to the copper (II) oxide while stirring. The balanced equation for this reaction is as follows: