1. Reactions of Metals Displacement Reactions:
Extraction of iron from iron oxide using displacement by carbon.
Iron oxide + carbon  iron + carbon dioxide
2Fe2O C  4Fe CO2
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