Investigation: Developing an Activity Series for Metal Copper (Ii), Magnesium and Nickel

3. Common observations of a chemical reaction are described in the introduction section. For each observation, name a common or everyday occurrence that must involve a chemical reaction?

Procedure: In this experiment, various chemicals were mixed together, to determine a reaction. Using two drops from chemical 1 and two drops of chemical two, unless otherwise stated, then recording the type of physical reaction or color changes that occurred.

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 mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

An elements¡¦ reaction to certain substances may be predicted by its placement on the Periodic Table of Elements. Across a period, an element on the left will react with more vigor than one on the right, of the same period. Vertically, as elements are sectioned into groups, the reaction of each element increases

Solutions of 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, and 1.0 M of NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, and 1M Cu(NO3)2 were given in separate test tubes. The color of possible precipitates, ions, acid-base behaviour, odor and solubility rules were conducted and were reported in Table 1. The key information about a mixture of two solutions was

In some instances lead reacted very similarly with the alkaline earth metal but very different in the other reactions such as with iodide. This is due to lead’s position on the periodic table as compared to those of the alkaline earth metals. The position on the periodic table correlates to an element’s atomic radius, ionization energy, and electron affinity. All of these properties affect an element’s chemical properties such as solubility. A systematic error occurred during my experiment when I observed a reaction between barium and iodide. There should have been no reaction. This error is probably the result of using a test tube that was not cleaned properly prior to combining Ba(NO3)2 with NaI. This experiment reinforced the concepts introduced in Chapter 8 of our textbook.

The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

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

Refer to the reaction of iron nails with a copper solution assignment in Module 3, Section assignment 3.4 Part F of the Chemistry 11 course.

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

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

Purpose: The purpose of this experiment was to find the specific heat of an unknown metal, the heat of a reaction, and the heat of neutralization. Conclusion: Concepts covered in the lab were using formulas to find changes in temperatures, the heat capacity of water, molar masses of a metal, the change in enthalpy for a reaction, and the heat of solution per gram of a solid sample. Therefore, we learned how to apply these concepts into given materials and instructions in order for us calculate the heat capacity of a metal sample and how heat (energy) affects the system depending on certain surroundings.

This lab mainly focused on presenting 10 elements (2 unknown) that could be analyzed and then grouped together predominantly by metallic character. Each element was observed thoroughly and the findings can be seen in the above data table. By viewing the periodic table and observations, each element was labeled as either a metal, nonmetal, or metalloid, providing insight towards each element's physical properties and behavior with the two solutions, hydrochloric acid and copper chloride. The nonmetals, sulfur and carbon, did not undergo a chemical reaction with either solution.

As you go down the periodic table you can clearly see that the reaction decreases and this can be because the metals don’t really react as they should, this can be because when they get into contact with any of the substances they don’t really have a chemical reaction to them, this can be because they don’t react as they should when placed in acid. Aluminium –Copper there wasn’t really a reaction and this is because these metals didn’t really have any acid base substance in them. The other thing is that From this you can see that potassium reacted with everything and every substance that it was mixed to clearly showed a major reaction, this can be because of where it is placed in the periodic table, the fact that this is the last one from group 1 means that it is a metal that reacts really quickly because of the ion bonds it has on its outer layers, lithium is found at the top of the group 1 metals and this one clearly shows that it doesn’t really react that quickly and this can be because it isn’t a strong metal like potassium, the other thing you can see from lithium is that on all of them you can see there was a slow reaction this can be because of the ion bonds it may have and because this is a small metal it may not be stronger like the others. So clearly from the group 1 metals