Chemical Changes

Whole Topic PLC

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Whole Topic PLC

Describe how metals react with oxygen and state the compound they form, define oxidation and reduction
Describe the arrangement of metals in the reactivity series, including carbon and hydrogen, and use the reactivity series to predict the outcome of displacement reactions
Recall and describe the reactions, if any, of potassium, sodium, lithium, calcium, magnesium, zinc, iron and copper with water or dilute acids
Relate the reactivity of metals to its tendency to form positive ions and be able to deduce an order of reactivity of metals based on experimental results
Recall what native metals are and explain how metals can be extracted from the compounds in which they are found in nature by reduction with carbon
Evaluate specific metal extraction processes when given appropriate information and identify which species are oxidised or reduced
HT ONLY: Describe oxidation and reduction in terms of loss and gain of electrons
HT ONLY: Write ionic equations for displacement reactions, and identify which species are oxidised and reduced from a symbol or half equation
HT ONLY: Explain in terms of gain or loss of electrons that the reactions between acids and some metals are redox reactions, and identify which species are oxidised and which are reduced (Mg, Zn, Fe + HCl & H2SO4)
Explain that acids can be neutralised by alkalis, bases and metal carbonates and list the products of each of these reactions
Predict the salt produced in a neutralisation reaction based on the acid used and the positive ions in the base, alkali or carbonate and use the formulae of common ions to deduce the formulae of the salt
Describe how soluble salts can be made from acids and how pure, dry samples of salts can be obtained
Required practical 1: preparation of a pure, dry sample of a soluble salt from an insoluble oxide or carbonate using a Bunsen burner to heat dilute acid and a water bath or electric heater to evaporate the solution
Recall what the pH scale measures and describe the scale used to identify acidic, neutral or alkaline solutions
Define the terms acid and alkali in terms of production of hydrogen ions or hydroxide ions (in solution), define the term base
Describe the use of universal indicator to measure the approximate pH of a solution and use the pH scale to identify acidic or alkaline solutions
HT ONLY: Use and explain the terms dilute and concentrated (in terms of amount of substance) and weak and strong (in terms of the degree of ionisation) in relation to acids
HT ONLY: Explain how the concentration of an aqueous solution and the strength of an acid affects the pH of the solution and how pH is related to the hydrogen ion concentration of a solution
Describe how ionic compounds can conduct electricity when dissolved in water and describe these solutions as electrolytes
Describe the process of electrolysis
Describe the electrolysis of molten ionic compounds and predict the products at each electrode of the electrolysis of binary ionic compounds
Explain how metals are extracted from molten compounds using electrolysis and use the reactivity series to explain why some metals are extracted with electrolysis instead of carbon
Describe the electrolysis of aqueous solutions and predict the products of the electrolysis of aqueous solutions containing single ionic compounds
Required practical 3: investigate what happens when aqueous solutions are electrolysed using inert electrodes
HT ONLY: Describe the reactions at the electrodes during electrolysis as oxidation and reduction reactions and write balanced half equations for these reactions