Reactivity Series of Metals Flashcards
Metal + H2O
Metal Hydroxide + H2
. Metal + H2O (g=water vapour)
Metal Oxide + H2
Metal + Acid
Salt+H2
Poisoned
Sausages
Can
Make
A
Zulu
Ill
Therefore
Let
Highly
Clever
Men
Slaughter
Good
Pigs
Potassium (MR)
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Mercury
Silver
Gold
Platinum (LR)
Method of extraction for PSCMA
Electrolysis of molten compound
Method of extraction for ZITLHCMS
Heating with Carbon
Method of extraction for SGP
Found naturally uncombined
PSC reactions
React with cold water and steam. Reaction becomes less vigorous down the group.
React with acid to form salt and hydrogen.
Magnesium reaction
Magnesium reacts very slowly with cold
water, but explodes in steam.
React with acid to form salt and hydrogen.
Aluminium reaction
React with acid to form salt and hydrogen.
ZILTL reactions
No reaction with cold water;
heated metal reacts with steam.
React with acid to form salt and hydrogen.
CMSGP reactions
No reaction
Why aluminium cannot react with water?
Protected by layer of oxide to prevent reaction with water.
Format for answering displacement reactions
MORE reactive metal displaces LESS REACTIVE metal from its COMPOUND.
Extraction of Iron in the Blast Furnace
Substances added from top of furnace:
1. Iron ore (haematite), Fe2O3
2. Coke (carbon), C
3. Limestone, CaCO3 [to remove acidic impurities]
* Hot air pumped in near bottom of furnace.
* Molten slag and iron are removed at the bottom, iron sinks
to the bottom and slag floats on top of it.
Reactions in the Blast Furnace
1) Coke burns in air to form carbon dioxide. C + O2 → CO2
2) Carbon dioxide reacts with more coke to produce carbon monoxide. CO2 + C → 2CO
3) Carbon monoxide (reducing agent) reacts with iron (III) oxide to form iron and carbon dioxide.
3CO + Fe2O3 → 2Fe + 3CO2
4) Limestone is decomposed to form calcium oxide and carbon dioxide. CaCO3 → CaO + CO2
5) Calcium oxide reacts with acidic impurities like silicon dioxide (sand) to produce slag (calcium
silicate).
CaO + SiO2 → CaSiO3(slag)
Pure metals texture
soft
Alloys texture
stronger and harder
Pure metals
Atoms of the same size
Atoms of pure metals movement
When a force is
applied, atoms can
slide over each
other easily
Alloys movement
The atoms from the other metals are of
different sizes. They disrupt the orderly
arrangement of the metals and prevent the atoms from sliding over each other making alloys stronger and harder.
Alloys
Mixture of metal and other metals/non-metals
Reasons for Recycling Metals
1) Recycling costs less than extracting new metals from their ores.
2) There are only limited amounts of metals in the ‘Earth’s surface, recycling will conserve resources.
3) Recycling avoids the land pollution caused by disposal of metals in landfill sites or caused by mining.
Explain why alloys are harder than metals.
The addition of another element
disrupts the orderly arrangement of metal due to difference in size.
Hence, the particles are not able to
slide over one another easily.
State the condition for rusting.
Oxygen and water need to be present for rusting to occur.
Explain why more
energy is required for the extraction of sodium from its chloride than any other metals.
Sodium is high in the reactivity series and forms strong bonds
in its compounds.
Hence it can only be extracted by electrolysis which requires more energy.
How is silver extracted?
Silver is found naturally uncombined in the ground.
Suggest why silver, but not magnesium is found in the Earth’s crust as
the unreacted element
Silver is low in the reactivity series
and while magnesium is high in the reactivity series.
Hence, magnesium tends to react with other elements like
oxygen to form compounds, but
silver is unreactive and does not react easily.
Name waste gases that are possibly produced in the extraction of iron.
Carbon monoxide, carbon dioxide,
nitrogen (due to hot air being introduced)
