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emeralddinosaur281Lv1

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Thin Layer Chromatography

Since this lab is to be commenced and concluded in the same day, please answer the following questions in your lab notebook as a SEPARATE SECTION of your Pre-Lab discussion.

Discuss the theory behind Thin Layer Chromatography (TLC).

Why do you need to be careful not to get fingerprints on the plates?

What is the purpose of the UV lamp? What is the purpose of the Iodine stain?

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Hi Iâve been struggling with my lab report and in need of some help. Here is everything you might need the lab report and data recorded in my notebook. I need help in the report questions please

QUALITATIVE STUDIES OF OXIDATION-REDUCTION REACTIONS Your objectives in this experiment include determining the products means of experimental tests, experimentally determining the relative ability of chlorine, and iodine to act as oxidizing agents, and designing an experiment to test an of a chemical reaction by bromine d rank a group of in order of their strength as reducing agents. All these objectives will require you to think logically in both your approach and your analysis of the results. Pre-Lab Questions: 1. In this lab you will be mixing hexane with aqueous (water) solutions. Which layer will be the water layer - top or bottom? Explain what property allows you to determine this. 2. Write a balanced chemical equation for the reaction of calcium metal with hydrochloric acid. What visible changes do you expect to see? Safety and Disposal: 1. Hexane is a volatile and flammable solvent. No open flames during this laboratory. When corked test tubes are shaken, pressure may develop, especially when a volatile solvent is one of the components. Remember to release the pressure intermittently by removing the cork slowly 2. Hydrochloric acid is corrosive. Wash your hands well with soap and water after working with it. 3. All solutions containing hexane must be placed in a container for recovery. Do not discard hexane down the sink. Do not put metals in the hexane recovery container. Part 1: The halogens Non-metals, such as the halogens, have relatively high electron affinities and as a result tend to react by gaining electrons, which we call becoming reduced, to form anions. In this experiment we will use the difference in solubility of the halogens (Cl2, Br2, and 12) as compared to the halides (Cr'. Br, and I') to test the reactivity of the elements The elemental halogens are non-polar and therefore are not very soluble in water. As a resul solutions of the halogen s in water are not very brightly colored. However, if an aqueous solution is mixed with a non-polar solvent, such as hexane, C&H14, the halogen is usually ferentially extracted into the non-polar solvent. Since the non-polar solvent is water, the halogen color is easily visible as a not miscible with separate colored layer

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