Metals:

• Write balanced half equations and ionic equations
• 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
• Describe oxidation and reduction in terms of loss and gain of electrons
• Write ionic equations for displacement reactions, and identify which species are oxidised and reduced from a symbol or half equation
• 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
• Explain that acids can be neutralised by alkalis, bases and metal carbonates and list the products of each of these reactions
• 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 reactions at the electrodes during electrolysis as oxidation and reduction reactions and write balanced half equations for these reactions
• Name and describe alternative biological methods for extracting metals, including phytomining and bioleaching
• Evaluate alternative methods for extracting metals