9 2 reactivity series and corrosion of metals

The general equation for a metal reacting with an acid is: metal + acid → salt + hydrogen

True. Only metals above hydrogen in the reactivity series will react with dilute acids.

A salt is the ionic compound produced when a metal reacts with an acid.

The equation for the reaction of calcium with water is: Ca (s) + 2H2O (l) → Ca(OH)2 (aq) + H2 (g)

False. Copper is less reactive than hydrogen.

False. Magnesium reacts very slowly with cold water.

False. Potassium is more reactive than sodium.

If a metal-acid reaction is described as "vigorous", it means the reaction is rapid and intense

True. Potassium reacts violently with water and acid.

A metal that is above carbon in the reactivity series is:

A metal that is below hydrogen in the reactivity series is:

Zinc is more reactive than iron.

Aluminium is more reactive than zinc.

One mnemonic to remember the reactivity series is: “Please send lions, cats, monkeys and cute zebras into hot countries signed Gordon” Potassium, sodium, lithium, calcium, magnesium, carbon, zinc, iron, hydrogen, copper, silver and gold

False. The most reactive metal is found at the top of the reactivity series.

Displacement occurs when a more reactive substance takes the place of a less reactive substance.

False. Reactivity is determined by the tendency of the metal atoms to lose electrons.

True. Magnesium can displace copper from copper sulfate solution.

When a more reactive metal displaces a less reactive one, the less reactive metal coats the surface or falls out as a solid.

Observations made when copper sulfate solution reacts with magnesium:

True. Reactivity is determined by the tendency of the metal atom to form positive ions.

False. Metals higher up the reactivity series, lose electrons more easily.

The products formed when iron reacts with silver nitrate solution are iron(II) nitrate and silver.

Aluminium does not readily react with water and acids because it has a protective layer of aluminium oxide.

Rust is the hydrated iron(III) oxide that forms on iron when it corrodes.

Rusting specifically refer to the corrosion of iron.

The word equation for the rusting of iron is: iron + water + oxygen ⟶ hydrated iron(III)oxide

Two conditions needed for rusting of iron to occur are water and oxygen.

Examples of barrier methods that can prevent rusting are:

Nail A will rust because it is exposed to oxygen AND water.

True. Rusting weakens the structure and integrity of iron over time as more iron is lost.

False. Galvanising is the method of coating iron with a layer of zinc.

Sacrificial protection is when a more reactive metal is intentionally allowed to corrode to protect the metal it is covering.

Zinc is used to protect iron from corrosion because it is more reactive than iron so will react more readily with oxygen.

Iron / steel is galvanised with zinc by:

False. A metal more reactive than iron can be used for galvanising.