1. Types of chemical reactions STUDY GUIDE V2.0 Background In chemistry there are many different types of chemical reactions. Chemists use chemical equations as shorthand representations for reactions. The purpose of this experiment is to observe several important types of chemical reactions and to write equations for these reactions. Equipment required Balance Spatula Bunsen Metal tongs Wax taper Dropper Beaker (100 mL) Steel wool Zinc strips (two) Copper strip (one) Copper(II) carbonate [CuCO 3 ] (2 g) Calcium carbonate [CaCO 3 ] marble chips (2 g) Magnesium ribbon (two 3 cm strips) Silver nitrate solution [AgNO 3 ] 0.1 mol L -' (30 mL) Sodium bromide solution [NaBr] 0.1 mol L -' (5 mL) Copper(II) sulfate solution [CuSO 4 ] 0.1 mol L -' (30 mL) Sodium hydroxide solution [NaOH] 2 mol L -I (5 mL) Sodium hydroxide solution [NaOH] 0.1 mol L -' (30 mL) Hydrochloric acid [HC1] 2 mol L-' (10 mL) Hydrochloric acid [HCI] 0.1 mol L-' (30 mL) Limewater [Ca(OH) 2 ] saturated (10 mL) Universal indicator (5 drops) Lead(II) nitrate solution [Pb(NO 3 ) 2 ] 0.1 mol L ' (25 mL) This work must be completed by Friday 29th Feb 2008 Complete all questions/research on the GREY PAGES

2. Procedure #1 Prepare a table including space for reactants, observations and products for the following reactions. Decomposition of a carbonate by heating #2 Place a spatula of copper(II) carbonate into a large test tube and fit the test tube with a stopper and delivery tube. Heat the test tube with a bunsen and pass any gas evolved through 5 mL of limewater in another test tube. Decomposition of a carbonate with an acid #3 Place a spatula of calcium carbonate (marble chips) into a large test tube, add 2 mol L-' hydrochloric acid to a depth of about 2-3 cm, and fit the test tube with the stopper and delivery tube as before. Again note the effect of any gas evolved on limewater solution. Oxidation of a metal #4 Place a protective mat on the laboratory bench. Cut a 3 cm strip of magnesium ribbon. Hold the ribbon in some tongs and heat in a bunsen flame above the mat. Reaction of a reactive metal with a dilute acid #5 Place another 3 cm strip of magnesium in a small test tube and add 2 mol L-' hydrochloric acid to a depth of about 3 cm. Note the reaction and collect any gas evolved by inverting another small test tube and holding it directly above the reaction tube. Test the gas evolved by placing a lighted taper in the inverted test tube. Precipitation reactions #6 Place 2-3 mL of 0.1 mol L ' AgNO 3 solution into a test tube and add about the same volume of 0.1 mol L ' NaBr solution. #7 Place 2-3 mL of 0.1 mol L-' CuSO 4 solution into a test tube and add about the same volume of 2 mol L-' NaOH solution. From Practical guide

3. Metal displacement reactions #8 Place about 25 mL of 0.1 mol L ' CuSO 4 solution into a 100 mL beaker and place into the beaker a freshly cleaned zinc strip. #9 Place about 25 mL of 0.1 mol L-' Pb(NO 3 ) 2 solution into a 100 mL beaker and place into the beaker a freshly cleaned zinc strip. #10 Place about 25 mL of 0.1 mol L-' AgNO 3 solution into a 100 mL beaker and place into the beaker a freshly cleaned copper strip. Neutralisation reaction - reaction of an acid and a base #11 Place about 20 mL of 0.1 mol L ' HCI into a beaker and add 5 drops of universal indicator. Using a dropper gradually add 0.1 mol L' NaOH solution until about 25 mL of the base has been added. Note any colour changes which take place. Processing of results, and questions 1 Write word equations and balanced chemical equations for each of the reactions observed. 2 Write word equations and balanced chemical equations for the following reactions. a heating magnesium carbonate

4. Mg+0 2 Calcium + oxygen Sodium + oxygen reactive metal oxygen metal oxide + complete this and convert into chemical equation x 3

5. Metal + acid-> salt + hydrogen Note 2, dilute acids will not react with metals from copper down in the reactivity series Zinc/sulphuric acid iron/ nitric acid Note 1, do not add dilute acid to the most reactive metals. (list + why?) magnesium hydrochloric acid magnesium chloride hydrogen + + complete this and convert into chemical equation x 3 Also find a reactivity series of metals Chromium + phosphoric acid REACTIVE METALS + DILUTE ACIDS

6. Find a solubility table. Some salts are insoluble sodium bromide + silver nitrate silver 'bromide(s) + sodium nitrate(aq) lead nitrate copper sulphate + complete this and convert into chemical equation potassium iodide lead nitrate + complete this and convert into chemical equation Precipitation reactions

7. Find a definition of the term salt metal carbonate + acid = salt + water + carbon dioxide calcium carbonate + hydrochloric acid = calcium chloride + water + carbon dioxide complete this and convert into chemical equation lead carbonate + nitric acid sodium carbonate + sulphuric acid

8. Copper Carbonate ZnCO 3 look up a reactivity series for metals metal carbonate = metal oxide + carbon dioxide note carbonates containing reactive metals (Na K etc) tend to be thermally stable CuCO 3 = CuO + CO 2 Al 2 (CO 3 ) 3 complete these and convert into chemical equation

9. M + MX salt M X + M M is more reactive than M magnesium + copper sulphate zinc + copper sulphate = copper + zinc sulphate gold + copper sulphate = ? copper + silver nitrate = ? complete these and convert into chemical equation

10. Research these write a general reaction and three specific examples using three different acids and three different bases