Topic 2 - Metals and the Reactivity series Flashcards
(21 cards)
Ores
Metal compounds that contain a high enough percentage of the metal to make it economically viable to extract
Most reactive to Least Reactive
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Potassium
How are metals above carbon extracted
Through electrolysis
In a displacement reaction
Metals below carbon can be heated with carbon
copper oxide + carbon =
copper + carbon dioxide
Reduction
When oxygen is removed from the metal by carbon
Native metals
Metals like silver and gold are found as pure substances in the Earth’s crust
Properties of Metals (non - pure)
- Hard
- Strong
- Ductile
- Malleable
- Sonorous
- Lustrous
- Dense
Pure Metals
Soft and Malleable because layers of atoms can slide over each other when a force is applied
Alloys
Mixtures of metals plus one or other elements; harder than pure metals
How do different size atoms disrupt the regular arrangements of atoms?
Layers of atoms can no longer slide over each other when a force is applied
metal + acid =
salt + hydrogen
Metals above hydrogen in the reactivity series will displace
hydrogen from acids form a salt and hydrogen
A salt formed is named after …
the metal and the type of acid.
e.g. calcium + nitric acid = calcium nitrate
Displacement Reactions
When a metal is added to a compound containing a metal lower down in the reactivity series, the more reactive metal displaces. This results in the formation of a different compound
Metal + salt =
e.g. potassium + silver chloride =
salt + metal
e.g. potassium chloride + silver
More reactive metals also react with
water.
group 1 metals are unusual because
they are soft and very reactive; they are stored in oil as they react quickly with oxygen in the air
metal + water =
metal hydroxide + hydrogen
Universal indicator turns an alkali
purple (metal hydroxides are alkaline)
When testing for hydrogen
Burning splint - pops when placed in hydrogen
