The Reactivity Series of Metals Flashcards
What is a reactivity series?
A list of elements in decreasing/increasing order of reactivity
Give the mnemonic for the reactivity series of metals
Please Send Little Charlie’s Monkeys And Zebras In Cages Securely Guarded
Give the reactivity series of metals.
Potassium Sodium Lithium Calcium Magnesium Aluminium Zinc Iron Copper Silver Gold
Give the reaction of Potassium, Sodium and Lithium with water.
Potassium-burst into lilac flame, floats, melts into a ball, moves
Sodium-melts into a ball, floats, fizzes, moves
Lithium, floats, fizzes, moves
Give the reaction of Calcium and Magnesium with water/steam
Calcium-sinks, fizzes, goes white, v. hot to the touch
Magnesium-in strip form w/ water nothing, in powder form, some reaction. w/ steam & boiling water v. vigorous
2Lithium/Sodium/Potassium + 2Water =
2Lithium/Sodium/Potassium Hydroxide + Hydrogen
Magnesium strip + acid
violent fizzing, heat, colour change, Mg disappears, squeaky pop when gas ignited
Zinc + acid
gentle fizzing, quite slow to start
Iron + acid
small bubbles, metallic smell
Copper + acid
No reaction
Define displacement reaction
When a more reactive metal displaces a less reactive metal from a solution of its salt.
What is a Thermite Reaction used for?
To produce molten iron to fix railway tracks
Give the equation for the Thermite Reaction
Aluminium + Iron (III) Oxide = Aluminium Oxide + Iron
2Al + Fe2O3 = Al2O3 + 2Fe
Where is carbon in the reactivity series? How is this useful?
Above Zn, Fe and Cu but below Al. So C can be used to extract Fe from its ore as it is more reactive.
C cannot extract Al or higher because it is less reactive.
In the blast furnace what happens?
Iron oxide is reacted with coke (nearly pure carbon) in a 3 step process.
Describe the 3 step process in the blast furnace
1)C + O2 = CO2 (exothermic reaction)
2)CO2 + C = 2CO (carbon monoxide)
3)Fe2O3 + 3CO = 3CO2 + 2Fe or sometimes Fe2O3 reacts directly with coke
2Fe2O3 + 3C = 3CO2 + 4Fe
Define oxidation and reduction
oxidation- when a substance loses oxygen/electrons
reduction-when a substance gains oxygen/electrons
Define oxidising and reducing agents
oxidising agent-gives oxygen/electrons to something else (so is reduced)
reducing agent- receives oxygen/electrons from something else (so is oxidised)
Describe 3 problems with iron
1) It rusts
2) If it doesn’t contain enough C(e.g is too pure), it is soft
3) If it contains too much C, it is brittle
What is rust? What are the conditions needed?
Hydrated Iron(III) Oxide. Water and Oxygen (sped up by salt)
Name and describe 3 methods of rust prevention
1) Galvanising-coat w/ zinc because zinc is more reactive than iron so reacts with oxygen and water in preference
2) Sacrificial Plating-place bags of a more reactive metal around the iron OR coat the iron in the metal
3) Barrier Methods-stop water and oxygen getting to the iron e.g oil/grease moving parts, coat iron in plastic or paint it
Define alloy
A metal with other elements, such as carbon or other metals, added to strengthen it.
Why is an alloy stronger?
The particles of the non-metal or other metal interrupt the layers of the metal, meaning they cannot slide over or past each other.
Name, give the percentage carbon and give the qualities and uses of 3 types of steel.
1) Low carbon steel-0.1-0.3% carbon, easily shaped and used in car bodies
2) High carbon steel-0.22-2.5% carbon, v. strong, inflexible, brittle and used in bridges
3) Stainless steel-Chromium/nickel added, corrosion resistant, hard and used in cutlery
