Periodic Table Lab Report

2. Obtained a 2-3 cm strip of magnesium metal ribbon and coiled it loosely into a small ball. Added the magnesium metal to the acid in the test tube.

During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the

When the tip of the rod touched the pH paper, the color of the pH paper became blue.

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

10) When HCl was added, the H⁺ ions reacted with the NH₃ to form NH₄⁺. This causes the [NH₃] to

In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The balanced formula for this is:

To study the nature of ionic reactions, write balanced equations, and write net ionic equations for precipitation reactions.

The purpose of this experiment is to identify the periodic trends in the solubility of the alkaline earth metals and compare the results to that of lead

Reaction with Magnesium sulfate: Few drops of Magnesium sulphate were added to the test tube. White precipitates were formed. 3. Reaction with HCl: Few drops of 06 molar HCl were added to the test tube. Reaction did not occur at low concentration of HCl.

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

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

Part A.1. Sodium metal is also readily oxidized by oxygen. If the product of the reaction were dissolved in water, what would be the color of the litmus for a litmus test? Explain. What is the product?

When applying the sodium hydroxide to the acidic solutions a dropper was used. This tool was very inaccurate in that it relied on human pressure to pipette a drop which caused issues with the trials for 1 M hydrochloric acid. Ideally, the values of the 1 M trials should be double those of the 0.5 M trials because it is double the concentration however the dropper caused variation in the data throughout the entire experiment (see figure 2). The dropper produces drops of varying size depending on the pressure applied. At certain points in the experiment the dropper produced large drops, at others hollow bubbles all of which were deemed one drop. To solve this, a burette should be used to apply the aqueous sodium hydroxide to the acidic solutions because it does not vary the size of its applications based on the pressure applied to it.

6. 3 drops of phenolphthalein were added to the vinegar solution. 7. The vinegar solution was placed under the burette and titration was started. 8.

C2H5Cl + :OH- C2H5OH + Cl- C2H5Br + :OH- C2H5OH + Br= C2H5I + :OH- C2H5OH + I- The mechanism for this reaction is: The free halide ions will then bond with the positive silver ions. The precipitation of the halides will occur as follows: Ag+(aq) + Cl-(aq) AgCl(s) Ag+(aq) + Br-(aq) AgBr(s) Ag+(aq)