Do now!

Can you fill in the observations of the

“Rusting” experiment?

Last lesson

• Conditions needed for rusting

• Rust protection

• Sacrificial protection

Rusting

Rust is a form of iron oxide. It has water bonded loosely to it. It is called hydrated iron oxide

Learn!

In order for iron to rust

Both air and water’s a must,

Air alone won’t do

Without water there too,

So protect it, or get a brown crust!

It’s actually the oxygen in air

Learn too!

Protecting from rust

Painting is a barrier method

But what about

sacrificial protection?

Sacrificial protection

Zinc is electrically connected to the iron. Any water or oxygen reacts with the zinc (or magnesium) instead of the iron. Coating in zinc is called galvanization and it works even when the zinc coating is scratched.

Copy!

Today’s lesson

• The extraction of iron from iron ore using a blast furnace

• Extraction method and position in the reactivity series

Ores

Most metals are found naturally in rocks called ores. They are in compounds, chemically bonded to other elements

iron ore

Native

Some unreactive metals can be found as elements. They are called native metals.

Roasting

Some unreactive metals can be extracted from a compound simply by heating. This is called roasting.

Roasting copper sulphide

Copper sulphide + oxygen copper + sulphur dioxide

Cu2S(s) + O2(g) 2Cu(s) + SO2(g)

Mr Porter will give you some slides to stick in

Roasting lead sulphide

Roasting lead sulphide produces lead oxide, NOT lead.

The more reactive a metal is, the more difficult it is to extract from its ore.

Can you copy please?

Heating with carbon

Extracting metals with carbon

Carbon is higher than some metals in the reactivity series. It can be used to extract medium reactive metals.

Extracting metals with carbon

lead oxide + carbon lead + carbon dioxide

2PbO(s) + C(s) 2Pb(s) + CO2(g)

Reduction and oxidation

lead oxide + carbon lead + carbon dioxide

2PbO(s) + C(s) 2Pb(s) + CO2(g)

carbon is oxidised

lead oxide is reduced

Reduction and oxidation

lead oxide + carbon lead + carbon dioxide

2PbO(s) + C(s) 2Pb(s) + CO2(g)

carbon is oxidised

lead oxide is reduced

Oxidation is the gain of oxygen, reduction is the loss of oxygen

Mr Porter will give you some slides to stick in

The Blast furnace

1000°C

1500°C

1900°C

Iron ore (haematite), coke (carbon) and limestone (calcium carbonate)

Hot waste gases (recycled to heat furnace)

Blasts of hot airBlasts of hot air

Molten iron

YouTube - Steelmaking: Blast Furnace

Reactions in the furnace

The coke (carbon) reacts with oxygen in the hot air to make carbon dioxide

C(s) + O2(g) CO2(g)

Reactions in the furnace

The carbon dioxide reacts with more hot coke to form carbon monoxide

CO2(g) + C(s) 2CO(g)

Reactions in the furnace

The carbon monoxide then reduces (takes oxygen away) the iron oxide to iron

Fe2O3(s) + 3CO(g) 2Fe(l) + 3CO2(g)

Reactions in the furnace

Limestone reacts with the impurities to form slag.

CaCO3(s) + SiO2(s) CaSiO3(s) + CO2(g)

Can you fill in the gaps?

YouTube - Steelmaking: Blast Furnace

YouTube - Blast furnace

HomeworkRead pages 188 to 191 for next lesson

(Friday)