25 cm3 volumetric pipette and filler. CC9f Reactions of C3.11 Explain the general reactions 1) Place a strip of Students investigate reactions Summarise the two acids with metals of aqueous solutions of acids magnesium ribbon in a of acids with metals and different methods of and carbonates with (a) metals and (d) metal few cm3 of dilute sulfuric carbonates to test for carbon preparing soluble salts - carbonates to produce salts. acid in a test tube. and hydrogen. from an insoluble C3.12 Describe the chemical test Students should observe reactant and an acid Students will find that for (a) hydrogen; (b) carbon the effervescence (using metal, base or magnesium, zinc and iron dioxide (using limewater) (fizzing). Ask what is in carbonate) and from a effervesce with both dilute the bubbles. soluble reactant and an acids, although iron may not acid. Include the produce enough hydrogen to Equipment: eye general steps in the pop the lighted splint. Copper protection, test tube in a methods and the does not react with dilute acids. test-tube rack, piece of general equations. All the metal carbonates react magnesium ribbon with both dilute acids to provide (about 3 cm), dilute Digital Ionic equations bubbles of a gas that turns sulfuric acid about 5 cm3 presentation limewater turns milky. of 0.4 mol dm-3) Equipment: for each group: eye protection, Bunsen burner 2) Remind students and heat resistant mat, dropper about ions and ionic pipettes, spatula, test tubes, bonding. An ion is a test-tube rack, wooden splints, charged particle. Cations limewater, small pieces of are formed by the loss of copper e.g. foil or turnings, electron(s) and have a magnesium ribbon (1 cm positive charge. Anions length), granulated zinc (this are formed by the gain of works better if it is ‘dirty’), electron(s) and have a copper carbonate (few grams), negative charge. The magnesium carbonate (few ions are held together by grams), dilute hydrochloric acid electrostatic forces of
25 cm3 volumetric pipette and filler. CC9f Reactions of acids with metals and carbonates C3.11 C3.12 Explain the general reactions of aqueous solutions of acids with (a) metals and (d) metal carbonates to produce salts. Describe the chemical test for (a) hydrogen; (b) carbon dioxide (using limewater) 1) Place a strip of magnesium ribbon in a few cm3 of dilute sulfuric acid in a test tube. Students should observe the effervescence (fizzing). Ask what is in the bubbles. Equipment: eye protection, test tube in a test-tube rack, piece of magnesium ribbon (about 3 cm), dilute sulfuric acid about 5 cm3 of 0.4 mol dm-3) 2) Remind students about ions and ionic bonding. An ion is a charged particle. Cations are formed by the loss of electron(s) and have a positive charge. Anions are formed by the gain of electron(s) and have a negative charge. The ions are held together by electrostatic forces of Students investigate reactions of acids with metals and carbonates to test for carbon and hydrogen. Students will find that magnesium, zinc and iron effervesce with both dilute acids, although iron may not produce enough hydrogen to pop the lighted splint. Copper does not react with dilute acids. All the metal carbonates react with both dilute acids to provide bubbles of a gas that turns limewater turns milky. Equipment: for each group: eye protection, Bunsen burner and heat resistant mat, dropper pipettes, spatula, test tubes, test-tube rack, wooden splints, limewater, small pieces of copper e.g. foil or turnings, magnesium ribbon (1 cm length), granulated zinc (this works better if it is ‘dirty’), copper carbonate (few grams), magnesium carbonate (few grams), dilute hydrochloric acid Summarise the two different methods of preparing soluble salts - from an insoluble reactant and an acid (using metal, base or carbonate) and from a soluble reactant and an acid. Include the general steps in the methods and the general equations. Digital Ionic equations presentation
gcse-science-planning-document-term-3.docx