Reactions of Metals Displacement Reactions: Extraction of iron from iron oxide using displacement by carbon. Iron oxide + carbon  iron + carbon dioxide 2Fe2O3 + 3C  4Fe + 3CO2 Key definitions: Properties of metals: Shiny Malleable Ductile Sonorous Dense Solid (expect Hg) Conduct electricity Conduct heat Hard Displacement a reaction when a more reactive metal can push a less reactive metal from a compound., Reactivity series list of metals placed in order from most reactive to least reactive. Salt chemical formed form the reaction of an acid with a base, metal or alkali Malleable can be bent into shape Ductile can be stretched into wires Acid chemical with a pH of <7 which releases hydrogen ions (H+ ions) into solution. Corrosion damage caused to a metal by another chemical This is completed in a BLAST FURNACE. Zinc, Tin, Lead and Copper can also be extracted using this method. Reactivity Series & Extraction methods: extracted from their ores by displacement by carbon (low reactivity metals). extracted from their ores by electrolysis (highly reactive metals). Exist as pure metals in the ground (unreactive metals). Reactions with water: Metal + water  metal hydroxide + hydrogen. Reactions with oxygen: Metal + oxygen  metal oxide Reactions with acids: Metal + acid  salt + hydrogen Naming Salts: First part – use the metal name from the metal compound. Second part – the acid determines this. Hydrochloric acid chloride Sulphuric acid sulphate Nitric acid nitrate