Define chemical element
Copper is a chemical element naturally reddish-brown. Apart from being a good conductor or electricity, the element is found in group two of the periodic table.It is found as a mineral of many mineral forms such as cuprite, bornite, azurite, and chalcocite. Copper also occurs in plants and animals. The commercial production of copper occurs through smelting as it is extracted from its natural ores. The element is highly reactive to oxidizing acids such as nitric acid as we shall see later in the experiment.
Some properties of copper include having an atomic number of 29, valence of 1 and 2, and atomic weight of 63.546.PurposeThe purpose the experiment is to observe various properties of copper and how it reacts with various components. 1.
It aims at cycling solid copper through a series of chemical forms via phase reactions2. Learn about different types of solvent reactions3. Calculate percentage concentration of copper.Experiment 1ProcedureThe first experiment involved the reaction of copper and concentrated nitric acid.
0.5g of copper was weighed and placed in a 250ml beaker. 5.0ml of concentrated nitric acid was then added. The nitric acid was poured until it covered the copper metals. The copper was allowed to dissolve.
ObservationThe colorless conc. Nitric acid is poured on the brown copper metals. A reddish brown gas is produced.4HNO3(l) + Cu(s) =Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)DiscussionThe Colorless liquid is the concentrated nitric acid. The gas produced is the Nitrogen (IV) Oxide. The solution formed is copper (II) nitrate.
The rationale behind the reaction is that concentrated nitric acid is a strong oxidizing agent. The experiment demonstrated the oxidization of Cu (s) to Cu+2 (aq). Experiment 2ProcedureThe next procedure was to add 20ml 6M NaOH onto the sample from experiment 1 above. ObservationThere is the production of a light blue precipitate EquationCU(NO3)2(aq) + 2NaOH(aq) = Cu(OH)2(s) + 2NaNO3(aq)DiscussionThe light blue precipitate is the copper (II) hydroxide.
The compound does not dissolve in water, for that reason, it forms a precipitate. Experiment 3Procedure involved putting the content f experiment 3 above in a hot water bath.ObservationThe blue precipitate changes to blackEquationCu(OH)2(s) + heat= CuODiscussionWhen Copper II Oxide is heated, it produces Copper II Oxide and water.Experiment 4ProcedureDilute sulphuric acid is added to copper II oxide.
ObservationA blue solution is formedCUO(s) + H2SO4(aq)= CUSO4(aq) + H20(l)DiscussionThe solution formed is called Copper II Sulphate. The reaction is neutralization reaction and involves a base and an acid.
