Chlorine

When combined Sodium Bicarbonate and Hydrochloric Acid, Carbon Dioxide is produced. The two chemicals do not undergo a change in color but a chemical change when CO2 is produced.

Unknown white compound (823U) was discovered in the lab. In order to dispose of it correctly, the substance and its physical and chemical properties had to be identified. The unknown white compound was one of a list of 15 compounds. 5g of the unknown compound were given in order to correctly identify and discover its physical and chemical properties. In order to do so, a solubility test, a flame test, and ion tests were conducted. From the results of these initial tests and the given list of compounds, the unknown white compound was thought to be composed of sodium and a halide (I-, Br-, or Cl-). Of the list, NaCl was the appropriate compound, however NaC2H3O3 was also tested out of skepticism. To verify the identity of the substance, the solubility and flame tests were performed again along with a pH test. The pH tests of NaCl and NaC2H3O2 did not match that of the unknown white compound. The list of compounds had been entirely ruled out. The identity of the unknown white compound was revealed to be calcium chloride. To synthesize at least a gram (calculated to produce 1.2g) of CaCl2, the following reaction was completed.

| Combustion product reacted by becoming cold, dissolving, and no gas formation with an end product is clear colorless solution.

Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. The magnesium displaces the hydrogen in the acid, so it forms magnesium chloride and hydrogen gas.

Potassium Chloride is a metal halide salt composed of potassium and chlorine. In its pure state, it is odorless and has a white or colorless vitreous crystal appearance. It is commonly used in fertilizer.

But, as the concentration of HCl was increased, pungent gas was evolved. 4. Reaction with

In the set that was exposed to light, Ethylbenzene was the first to react. It turned from a dark orange color to a colorless liquid. Next, toluene turned colorless. After that, none of the other solutions turned colorless. However,

the element chlorine picks up one electron to form an ion. Chlorides ions help keep the

Chemiluminescence is the release of light without heat due to a chemical reaction. The release of light is from bonds that are broken, formed, or restructured2. A similar process, known as fluorescence, also produces an illumination. This chemical process on the other hand, gets its energy for light from the absorbance and release of light at different frequencies.

Some physical properties are its greenish-yellow color (only is gas form). Its disagreeable, suffocating smell, solubility in water, and a boiling point of -34.05°C. It also has a melting point of -101°C, a density of 3.214 g/l, and a gravity of -33.6°C. These properties are physical and not chemical because when observed, they do not change the chemical makeup of that matter (in this case chlorine). The properties are also easily observed with the 5 senses. But how does chlorine get its physical properties? Chlorine gets its properties from the number of protons in the nucleus. Different elements have different numbers of protons, which means they have different chemical/physical

Titanium is not found on its own, but in compounds with other elements where can it later be separated through various ways of extraction. One way which is commonly used is to extract titanium from its ore, rutile (TiO2) and to turn it into titanium chloride (which is done by the two substances reacting together). Then the titanium chloride is minimised using either magnesium (Mg) or sodium (Na) to then form the titanium metal, this method is known as Kroll's process, below is a more detailed diagram of the overall process.

When reacting to oxygen (O2) a chemical reaction occurs causing Sodium (Na) to become Sodium Oxide (Na¬2O) presenting a white crystallised substance. Burns with oxygen to provide a bright yellow flame

When mixed with hydrochloric acid (appendix 4), they react violently, hence why only a small portion was allowed for this experiment. This supports the hypothesis, that is, it was predicted that such a reaction would occur as these metals are highly reactive, hence why the hydrogen gas produced was clearly visible (appendix 5). Tin is less reactive, however, according to the Metal Reactivity Series, reacts with acids at an extremely slow rate. This was evident in the experiment; however, more of a reaction would have occurred if the time frame was expanded. The metal was only left in the acid for five minutes; therefore, it had no reaction but could of, had it been left a while longer. Magnesium and Calcium are both alkaline earth metals which means that they all have an oxidation number of ‘+2’, making them highly reactive. Calcium is more reactive than Magnesium even though it is located below it on the periodic table (appendix 6) because its electron configuration is ‘2,8,8,2’ while Magnesium’s is ‘2,8,2’. This means that Calcium has more shells which, therefore, means that there is less of an attraction to the nucleus. This makes it easier for Calcium to lose electrons and react more so than Magnesium. According to the Metal Reactivity Series, in order from the most reactive to the least reactive, tin is located at around the middle of the

result in the formation of chloramines. These appear as residual chlorine but in the form of

In this experiment, a nucleophilic substitution was performed, where a chloride nucleophile substituted a tertiary hydroxyl group on 2-methyl-2-butanol. In a nucleophilic substitution reaction, an electron rich nucleophile attacks a positively or partially positively charged electrophile, and replaces a leaving group. In this reaction, chloride ions are the nucleophile, the tertiary carbon in 2-methyl-2-butanol is the electrophile, and water is the leaving group. In the mechanism for this reaction, the oxygen from the hydroxyl group of the 2-methyl-2-butanol attacks the hydrogen of the HCl, causing heterolytic cleavage of the HCl, resulting in a chloride ion, and in the oxygen bonding to an extra hydrogen, and becoming positively charged.