BITESIZE GCSE REACTIVITY SERIES

For example, sodium reacts rapidly with cold water: Non-metals in the reactivity series It is useful to place carbon and hydrogen into the reactivity series because these elements can be used to extract metals. The method used to extract a metal from its ore depends upon the stability of its compound in the ore, which in turn depends upon the reactivity of the metal. In this reaction, magnesium is oxidised – it gains oxygen to form magnesium oxide – and water is reduced – it loses oxygen to form hydrogen. Evaluate the hazards and the precautions needed to reduce the risk of harm. When a metal reacts with a dilute acid , a salt and hydrogen are formed. Platinum will not react with dilute acids. A metal cannot displace itself, so no reaction would take place.

Reduction by carbon or carbon monoxide. A metal’s relative resistance to oxidation is related to its position in the reactivity series – in general, the lower down a metal is, the greater its resistance to oxidation. The method used to extract a metal from its ore depends upon the stability of its compound in the ore, which in turn depends upon the reactivity of the metal. When a metal reacts with water, a metal hydroxide and hydrogen are formed. This is because its protective aluminium oxide layer makes it appear to be less reactive than it really is. A metal below hydrogen in the reactivity series will not react with dilute acids. Predict its reaction with dilute acids and explain your answer. Non-metals in the reactivity series It is useful to place carbon and hydrogen into the reactivity series because these elements can be used to extract metals.

However, if steam is passed over hot magnesium, a vigorous reaction happens: It does not need to be chemically separated. For example, sodium reacts rapidly with cold water: In general, the more reactive the metal, the more rapid the reaction is.

This protects the metal and stops it reacting. Gces surface naturally forms a very thin layer of aluminium oxide that keeps water away from the metal below. The reactivity series of metals The reactivity series of metals is a chart showing metals in order of decreasing reactivity.

The reactivity series of metals is a chart showing metals in order of decreasing reactivity.

This table summarises some reactions of metals in the reactivity series. Magnesium reacts slowly when it is first added to water, but a layer of reactjvity magnesium hydroxide forms. In general, the more reactive a metal is: Non-metals in the reactivity series It is useful to place carbon and hydrogen into the reactivity series because these elements can be used to extract metals.

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In a reactivity series, the most reactive element is placed at the top and the least reactive element at the bottom. The method used to extract a metal from its ore depends upon the stability of its compound in the ore, which in turn depends upon the reactivity of the metal. Examples of ores include: More slowly than zinc. This includes the safe use and careful handling of substances.

Reactivity series and extraction of metals

One way to remember the order of metals in the reactivity series is to think of a phrase or sentence, which uses the first letter of each metal in the series. More reactive metals have a greater tendency to lose electrons and form positive ions. A metal cannot displace itself, so no reaction would take place. Metals below hydrogen in the reactivity series do not react with dilute acids, and both gold and platinum are placed below hydrogen.

Less reactive nitesize, such as reactivty, form less stable oxides and other compounds. When a metal reacts with water, a metal hydroxide and hydrogen are formed.

The reactivity series of metals – Revision 1 – GCSE Chemistry (Single Science) – BBC Bitesize

A metal’s relative resistance to oxidation is related to its position in the reactivity series – in general, the lower down a metal is, the greater its resistance to oxidation. There are a number of ways that you could investigate a displacement reaction.

Reactions of metals with water When a metal reacts with water, a metal hydroxide and hydrogen are formed. It is important in this practical activity to use appropriate apparatus and methods. Metals more reactive than carbon, such as aluminium, are extracted by electrolysis, while metals less reactive than carbon, such as iron, may be extracted by reduction with carbon.

When this layer is removed, the observations are more reliable.

Magnesium is the most reactive metal because a displacement reaction takes place with all the salt solutions. The reactivity series In a reactivity series, the most reactive element is placed at the top and the least reactive element at the bottom. Specified practical – metal displacement reactions Displacement in solutions There are a number of ways that you could investigate a displacement reaction.

A reactivity series of metals could include any elements. For example, magnesium reacts rapidly with dilute hydrochloric acid: This is because its protective aluminium oxide layer makes it appear to be less reactive than it really is.

Aims To investigate displacement reactions and produce a reactivity series for metals. Reduction by carbon or carbon monoxide. Here is the reactivity series including carbon and hydrogen: Note that aluminium can be difficult to place in the correct position in the reactivity series during these experiments. Carefully wipe up spills and wash hands.

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Reduction with carbon is often used to extract these metals and requires less energy to reduce them to extract the metal.

Platinum is placed below gold in the reactivity series. As gold is so unreactive, it is found as the native metal and not as a compound.

Metals – Revision 1 – KS3 Chemistry – BBC Bitesize

However, copper can be extracted using carbon or hydrogen. A metal below hydrogen in the reactivity series will not react with dilute acids.

Electrolysis is commonly gcxe to extract these metals and requires a lot of electric current energy to reduce them to extract the metal. Metal Method Potassium Electrolysis Sodium Electrolysis Calcium Electrolysis Magnesium Electrolysis Aluminium Electrolysis Carbon Non-metal Zinc Reduction by carbon or carbon monoxide Iron Reduction by carbon or carbon monoxide Tin Reduction by carbon or carbon monoxide Lead Reduction by carbon or carbon monoxide Hydrogen Non-metal Copper Various chemical reactions Silver Various chemical reactions Gold Various chemical reactions Platinum Various chemical reactions Metals more reactive than carbon, such as aluminium, are extracted by electrolysis, while metals less reactive than carbon, such as iron, may be extracted by reduction with carbon.

Question Platinum is placed below gold in the reactivity series. Some students did not test combinations of the same metal, such as magnesium and magnesium sulfate solution.

Reactivity and extraction method The table displays some metals in decreasing order of reactivity and the methods used to extract them.

The table displays some metals in decreasing order of reactivity and the methods used to extract them. The tables show how the elements react with water and dilute acids: In this reaction, magnesium is oxidised – it gains oxygen to form magnesium oxide – and water is reduced – reactviity loses oxygen to form hydrogen.

It is useful to place carbon and hitesize into the reactivity series because these elements can be used to extract metals.