State the method used to extract metals that are above carbon in the reactivity series.

State the method used to extract metals that are below carbon in the reactivity series.

Explain why molten ore (not dissolved in water) must be used during the electrolysis of aluminium oxide.

Iron is extracted in a blast furnace. State the name of the reducing agent used and write a word equation for the reduction of iron(III) oxide.

Gold is found uncombined in the Earth's crust. State why gold does not need to be extracted from an ore.

Which metal is found uncombined (native) in the Earth's crust? (A) Sodium (B) Iron (C) Gold (D) Aluminium

Explain why aluminium cannot be extracted by heating its ore (aluminium oxide) with carbon.

Sodium is extracted by electrolysis of molten sodium chloride. State which electrode sodium is produced at, and explain why.

Copper can be extracted by heating copper(II) oxide with carbon, but potassium cannot. Explain this difference.

Write a balanced chemical equation, with state symbols, for the reduction of copper(II) oxide by carbon at high temperature.

Describe the relationship between a metal's reactivity and the ease of extracting it from its ore.

Explain, in terms of electrons, why the extraction of metals from their ores is a reduction process.

Zinc can be extracted by heating zinc oxide with carbon. Titanium cannot be extracted this way. (a) Suggest why zinc can be extracted this way. [1] (b) Suggest why titanium cannot be extracted this way. [1] (c) State the method used to extract titanium and identify the reducing agent. [1]

A student states: 'All metals above hydrogen in the reactivity series must be extracted by electrolysis.' Evaluate this statement.

Compare the extraction of iron and aluminium. In your answer, include: the method of extraction, the reason the method is chosen, and the economic or environmental impact of each method.