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Metals and thier Reactivity (Seperating from their oxides (Extraction…
Metals and thier Reactivity
Reactivity Series
For metals how easily they lose electrons
compares reactivity with water or acid
C & H
how metal will react with them
Metals less reactive than C can be extracted from their ores
metal less reactive than H will not react with acids
Metal reactions
with acids
how react tells you about their reactivity
more reactive, faster the reaction
very reactive to Ca, react explosively
in general copper won't react with cold dilute acids
can use burning splint test to confimr H2 production
with water
K, Na, Li & Ca will react
Zn, Fe, Cu won't react
Seperating from their oxides
most not in pure form
reactive so form compounds that need extracting
E.g Al, Fe form oxides, in ore
ore, rock that contain metal compounds
Formation of metal ore, oxidation=gain of oxygen
extraction of metal, reduction = loss of oxygen
Extraction
Reduction with C
ore is reduced
C oxidised
E.g Iron oxide reduced in blast furnace
Redox reactions
Also for transfer of electrons
loss of electron is oxidation
gain of electron called reduction
occur same time so REDOX
Example
metal with acids
Iron is oxidised by the hydrogen ions
Halogen Displacement Reactions
Chlorine is reduced by the bromide ions
metal displacement reactions
more reactive metal will displace less
reactive metal from its compound
E.g Iron in solution of copper sulfate
Ionic equations
only show particles that react and products they form