Electrolysis and Reactivity Series by Nicholas Law https://padlet.com/hknick/11TCo4 en-us 2016-09-04 14:59:04 UTC 2016-09-05 04:40:47 UTC hello@padlet.com Reactivity series  https://padlet.com/hknick/11TCo4/wish/121532692 2.29 - Potassium -> Sodium ->  Lithium -> Calcium -> Magnesium -> Aluminium -> Zinc -> Iron -> Copper -> Silver -> Gold
2.30 - React with water, acid. Most hydrogen produced = higher in reactivity series. 
2.31 - A metal higher in the reactivity series would displace one lower down.
2.32 - oxidation is loss of electrons, and gain of oxygen. 
Reduction is gain of electrons, loss of oxygen 
OILRIG 
2.33 - Redox( a reaction in which both oxidation and reduction happen) 
Oxidizing agent - reduces, helps the other in oxidizing
Reducing agent - oxidizes, helps the other in reducing
2.34 - iron needs water and oxygen
2. 35 - It can act as a physical barrier and prevent the oxygen/ water reaching the iron
2. 36 - Galvanizing, Zinc, is more reactive than iron, gives iron the electrons, prevents it from corroding

]]> 2016-09-05 04:27:21 UTC https://padlet.com/hknick/11TCo4/wish/121532692 React https://padlet.com/hknick/11TCo4/wish/121532911 2016-09-05 04:30:25 UTC https://padlet.com/hknick/11TCo4/wish/121532911 React with water: K, Na, Li, Ca https://padlet.com/hknick/11TCo4/wish/121532916 React with acids: Mg, Al, Zn, Fe
React with O2: Cu, Ag
Not reactive: Au]]> 2016-09-05 04:30:27 UTC https://padlet.com/hknick/11TCo4/wish/121532916 Electrolysis https://padlet.com/hknick/11TCo4/wish/121533158 1.48
Electric current is the flow of electrons
1.49
Covalent compounds do not conduct electricity because they don't have any free electrons. Covalent compounds share electrons so the electrons are not free to move around.
1.50
Ionic compounds can conduct electricity when it's molten or solution because when the ionic compound is a solid, there are ]]> 2016-09-05 04:33:47 UTC https://padlet.com/hknick/11TCo4/wish/121533158 Extraction and uses of Metal https://padlet.com/hknick/11TCo4/wish/121533405 5.1
-Anything below carbon can be displaced from its ore by carbon.
-Anything above carbon can't so is extracted by electrolysis.
5.2
-Bauxite is purified into aluminium oxide.
-This is then dissolved in molten cryolite to bring down the boiling point
-The walls of the tank are the negative electrode; here aluminium is made
-The aluminium sinks to the bottom and is tapped off
-Oxygen is formed at the positive electrode
-The oxygen formed reacts with the graphite anode to from carbon dioxide; so the anode has to be replaced
-It is very expensive to supply the electricity needed for this electrolysis.
5.3
-Al3+ + 3e- > Al
-2O2- → O2 + 4e-
5.4
-Iron is displaced from its ore (haematite) by carbon (from coke):
 2Fe2O3 + 3C > 4Fe + 3CO2
-It is also displaced by carbon monoxide
 Fe2O3 + 3CO > 2Fe + 3CO2
-Limestone reacts with impurities to from 'slag' which is tapped off.
-Air allows burning to take place (of coke.)
5.5
-Aluminium is 'low density' and does not corrode so is used for the bodies of planes.
Iron is used in electromagnets as it is a soft magnetic material. 
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