CGP Topic 3 and 4 Reactivity Series Please à Potassium
Stop à Sodium
A more reactive metal will displace a less reactive metal in the solution. Calling à Calcium
The sulphate ion is a spectator ion. Me à Magnesium
Ionic Equations A à Aluminium
2HCL(aq) + Mg(OH)2(aq) à MgCl2(aq) + 2H2O(l) Careless à Carbon
2H+(aq) + 2Cl-(aq) + Mg2+(aq)+ 2OH(aq) à Mg2+(aq) + 2Cl-9aq) + 2Cl-(aq) + 2H2O(l) Zebra à Zinc
2H+(aq) + 2OH-(aq) à H2O(l) Instead à Iron
H+(aq) + OH-(aq) à H2O(l) Try à Tin
Learning à Lead
How à Hydrogen
Copper à Copper
Saves à Silver
Gold à Gold
https://www.
youtube.com/
watch?v=3nm
OY4CzRww
Finding ionic
charges of
transition
metals
Extracting Metals
The first metal discovered by man around 420BC
An ore is a metal oxide. It is a rock containing a high enough percentage of a metal to make it economically viable to
extract. Contain a high percentage of impurities such as silicon dioxide (sand).
Carbon + Zinc Oxide à Carbon dioxide + Zinc Carbon is oxidised because it gains oxygen
Displaces Zinc is reduced because it loses oxygen
It is better to extract iron by heating iron oxide with
carbon because electrolysis of molten iron oxide
requires more energy to keep the salt molten than for
the electrolysis than heating with carbon so it is more
expensive.
Electrolysis is chemical decomposition produced by
passing an electric current through a liquid or solution
containing ions.
If a metal is less reactive than carbon, it can be
extracted from its oxide by heating with carbon.
The carbon displaces the metal from the compound,
and removes the oxygen from the oxide
, Experiments
It is often difficult to tell if a metal has
been formed as it is coated in a black
charcoal powder.
To improve experiment:
Tip the mixture into water, the charcoal
should float on the top and as the
particles of the metal ore are denser they
will sink to the bottom.
Copper oxide + Copper à Carbon
dioxide + Copper
2CuO(s) + Cu(s) à CO2(g) + Cu(s)
Metal Oxide Observation Was metal formed?
Copper oxide Brown Copper
Ca(s) + HCL(aq) à CaCl2(aq) + H2(g)
Metal Reaction with dilute HCL
Copper No reaction
Magnesium Slight effervescence
Zinc Effervescence
Calcium Squeaky pop, dissolved to salt
Metal + water à metal hydroxide +
hydrogen
Sodium + water à sodium
hydroxide + hydrogen
2Na(s) + 2H2O(l) à 2NaOH(aq) + H2(g)
Metal + oxygen à metal oxide
Magnesium + oxygen à magnesium
oxide
2Mg(s) + O2(g) à 2MgO(s)
Metal + acid à salt + hydrogen
Calcium + sulphuric acid à calcium
sulphate + hydrogen
Ca(s) + H2SO49aq) à CaSO4(aq) + H2(g
Stop à Sodium
A more reactive metal will displace a less reactive metal in the solution. Calling à Calcium
The sulphate ion is a spectator ion. Me à Magnesium
Ionic Equations A à Aluminium
2HCL(aq) + Mg(OH)2(aq) à MgCl2(aq) + 2H2O(l) Careless à Carbon
2H+(aq) + 2Cl-(aq) + Mg2+(aq)+ 2OH(aq) à Mg2+(aq) + 2Cl-9aq) + 2Cl-(aq) + 2H2O(l) Zebra à Zinc
2H+(aq) + 2OH-(aq) à H2O(l) Instead à Iron
H+(aq) + OH-(aq) à H2O(l) Try à Tin
Learning à Lead
How à Hydrogen
Copper à Copper
Saves à Silver
Gold à Gold
https://www.
youtube.com/
watch?v=3nm
OY4CzRww
Finding ionic
charges of
transition
metals
Extracting Metals
The first metal discovered by man around 420BC
An ore is a metal oxide. It is a rock containing a high enough percentage of a metal to make it economically viable to
extract. Contain a high percentage of impurities such as silicon dioxide (sand).
Carbon + Zinc Oxide à Carbon dioxide + Zinc Carbon is oxidised because it gains oxygen
Displaces Zinc is reduced because it loses oxygen
It is better to extract iron by heating iron oxide with
carbon because electrolysis of molten iron oxide
requires more energy to keep the salt molten than for
the electrolysis than heating with carbon so it is more
expensive.
Electrolysis is chemical decomposition produced by
passing an electric current through a liquid or solution
containing ions.
If a metal is less reactive than carbon, it can be
extracted from its oxide by heating with carbon.
The carbon displaces the metal from the compound,
and removes the oxygen from the oxide
, Experiments
It is often difficult to tell if a metal has
been formed as it is coated in a black
charcoal powder.
To improve experiment:
Tip the mixture into water, the charcoal
should float on the top and as the
particles of the metal ore are denser they
will sink to the bottom.
Copper oxide + Copper à Carbon
dioxide + Copper
2CuO(s) + Cu(s) à CO2(g) + Cu(s)
Metal Oxide Observation Was metal formed?
Copper oxide Brown Copper
Ca(s) + HCL(aq) à CaCl2(aq) + H2(g)
Metal Reaction with dilute HCL
Copper No reaction
Magnesium Slight effervescence
Zinc Effervescence
Calcium Squeaky pop, dissolved to salt
Metal + water à metal hydroxide +
hydrogen
Sodium + water à sodium
hydroxide + hydrogen
2Na(s) + 2H2O(l) à 2NaOH(aq) + H2(g)
Metal + oxygen à metal oxide
Magnesium + oxygen à magnesium
oxide
2Mg(s) + O2(g) à 2MgO(s)
Metal + acid à salt + hydrogen
Calcium + sulphuric acid à calcium
sulphate + hydrogen
Ca(s) + H2SO49aq) à CaSO4(aq) + H2(g
