Experiment 2 - Chemical Nomenclature of Ionic Compounds Learning chemistry is mu

Question

Experiment 2 - Chemical Nomenclature of Ionic Compounds Learning chemistry is much like learning a language. To communicate effectively within this discipline, a scientist must first learn to name chemical compounds. In this experiment you will examine a number of ionic compounds. Ionic compounds contain itively charged ions (cations) and negatively charged ions (anions). Rules for naming ionic compounds are outlined in the Chemical Nomenclature Flow Chart that follow. Procedure: In this experiment, you will be asked to do two things 1. Given the formula of each compound, write its name. 2. Determine the color of the ions. Colors of the ions can be determined by using the information you will obtain in the first part of this experiment about the colors of various compounds. For example: Na,SO, is observed to be white or colorless. Therefore, both Nat and so.2 must be colorless. FeSOs is green. Conclusion, since sulfate is colorless, the color in iron (II) sulfate cannot be due to the sulfate, but must be due to the iron in the compound. Thus iron (II) must be green. Note: Some compounds are colored when they should be white or have a darker color than would be expected based on the individual ions they contain. Pbs is black, even though Pb2 and S2 are both colorless. Note these compounds with unexpected colors or your report form. Safety The only danger is if you open or break a sample container. Many of the compounds are toxic and corrosive. Do NOT open any of the containers. If you have a spill or breakage, see your instructor and warn your colleagues. When you finish, return all containers to their proper place in the chemical hood.

Explanation / Answer

Answer:

31 Copper (II) sulphate Pentahydrate.

Chemical Formula: CuSO4. 5H2O.

Splitting of ions to know colour: Cu2+ SO42- 5 H2O

Blue Colorless colourless

Hence overall colour of CuSO4 5H2O is Blue. Known as Blue Sulphate.

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