How are metals with different reactivities extracted?

what charge do metals form when they become ions

positive charge

reactivity series of metals

potassium

sodium

lithium

calcium

magnesium

carbon

zinc

iron

hydrogen

copper

what are the most reactive metals

group 1 metals

how do we measure reactivity of metals

react metal with either acid or water to see how violent reactivity is

metal+acid

salt and hydrogen

potassium+hydrochloric acid

potassium chloride+hydrogen

explosive reaction

reactions as you go down the series

get less violent

temperature change of most reactive metals produce

most heat

how to ensure testing reactivity of metals is fair

same mass/SA of metal

same type/conc of acid

metal+water

metal hydroxide+hydrogen

lithium+water

lithium hydroxide+hydrogen

which metals are likely to react with water

the most reactive ones i.e potassium lithium and sodium

displacement reactions

more reactive metals displace less reactive metals

magnesium+iron sulphate

magnesium sulphate+iron

magnesium displaces iron

Bacterial extraction

- some bacteria absorb metal compounds

- produce solutions called leachates which contain metals

Phytomining

Using plants to absorb metal compound

Plants can be burned to produce ash that contains the metal compounds

Phytomining advantages

Carbon neutral

Does not cause destruction that mining does

Phytomining disadvantages

Requires electricity for electrolysis

Slow process

Requires sulphuric acid that needs to be manufactured

Oxidation

gain of oxygen

loss of electrons

reduction

loss of oxygen

gain of electrons

which metals don’t react with oxygen

unreactive metals like gold

metal oxide+carbon

pure metal+carbon dioxide

copper oxide+carbon

copper+carbon oxidised

copper was reduced and carbon was oxidised

which metals can we extract with carbon

metals that are less reactive than carbon i.e zinc iron and copper

what do we use to extract metals more reactive than carbon

electrolysis

mining for iron

rocks containing iron have different iron ores-metal rich compounds

reduce iron oxides in rock using carbon

Redox

A combination of reduction and oxidation reactions.

OILRIG refers to

electrons

ionic equations only show

only show the ions that change in the reaction and show the gain or loss of electrons

spectator ions

ions that do not change in a reaction and charges stay the same

they are removed in ionic equations

half equations

show gain and loss of electrons for each element

write two half equations when sodium reacts with iron sulphate

Fe²+ + 2e^- —> Fe

Na—>Na^+ + e^-

half equation for calcium when it loses two electrons

Ca—> Ca^2+ + 2e^-