Chemistry (Reactivity of Metals)

Chemistry (Reactivity of Metals) - Ch em i st r y React i v...

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C h e m i s t r y R e a c t i v i t y o f M e t a l s
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Aim: To compose an activity series via the determination of each metal tested reactivity.
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Hypothesis: The activity series formation of the reactivity of metal is constructed according to the relative ability of these metals to lose electrons. The ease of lose of electrons is due to the period and the outer shells capacity of electrons e.g. the greater the number of shells and lesser the number of valence electrons, the greater the reactivity of the metal, similarly the lesser number of shells and larger number of electrons, the lesser the reactivity. Hence the experiments results expectance is to follow the same order of the real activity series. ( http://www.nelsonthornes.com/secondary/science/scinet/scinet/react ion/react/metal.htm ) Apparatus: Refer to Appendix 1 Procedure: The metals Copper, zinc and magnesium were polished accordingly until they were clean and shiny. Two test tubes were then labeled with the numbers 1 and 2. In test tube 1, 5 drops of lead nitrate solution was added. In test tube 2, 5 drops of silver nitrate solution was added. To each test tube an equal sized polished piece of copper metal was added to the solutions. The observations were recorded. Furthermore, three additional test tubes were labeled with the numbers 3,4 and 5. In test tube 3, 5 drops of copper sulphate solution was added. In test tube 4, 5 drops of lead nitrate was added. Lastly in test tube 5, 5 drops of magnesium chloride solution was added. Subsequently, in each of the test tubes 3,4 and 5, an equal sized polished piece of zinc was added to the solution. The observations were recorded.
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6,7 and 8. In test tube 6, 5 drops of zinc chloride solution was added. In test tube 7, 5 drops of sodium chloride solution was added. Lastly, in test tube 8, 5 drops of potassium chloride solution was added. In each test tube, an equal sized piece of magnesium metal was added to the solution. The observations were recorded. Results: Refer to Appendix 1 Data Analysis: The results indicate the following reactions occurred, copper and silver nitrate, zinc and copper sulphate, zinc and lead nitrate, magnesium and zinc chloride. The reaction among copper metal and silver nitrate solution, provides the following balanced chemical equation: oxidises Cu + 2Ag + -----> 2Ag + Cu 2+ reduces For the above balanced equation, it signifys the loss of electrwons for the copper metal (oxidizes) and the reduction in the silver by gaining an electron. The half reactions are shown below:
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This note was uploaded on 10/18/2010 for the course CRE 16002 taught by Professor Harmon during the Spring '10 term at Creative Studies.

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Chemistry (Reactivity of Metals) - Ch em i st r y React i v...

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