You will see that we have so far shown that
#REACTIVITY OF CARBON SERIES#
Repeating the series from a previous page: most reactive The magnesium is more reactive than carbon and reacts with carbon dioxide, taking the oxygen from it. This excellent bit of video from the Royal Society of Chemistry shows that although you can use carbon dioxide to put out a petrol (gasoline) fire, you can't do the same thing with a magnesium fire. The reaction between magnesium and carbon dioxide You will meet that process later in the course. Carbon is above iron in the reactivity series, and will take oxygen from iron oxide.
It isn't actually used industrially to extract copper from copper ores, but is used to extract iron from iron oxide ores. The reason that carbon is included in the reactivity series is that it can be used to extract several metals from their oxide ores. The reaction shows that carbon is more reactive than copper, because it has taken the oxygen from the copper. The carbon dioxide escapes from the tube as a gas. The photo shows what the tube looks like after the experiment. The mixture turns brown as copper is formed. If you heat a mixture in a test tube, a red glow runs through the mixture showing that heat is being produced in the reaction in addition ot the heat from the Bunsen. The reaction between carbon and copper(II) oxideĬarbon powder and copper(II) oxide are both black. This second piece of video shows the use of the reaction in welding railway track together. Annoyingly it doesn't show the iron formed glowing red in the sand. The first piece of YouTube video shows the reaction in a lecture theatre. You will find the term "exothermic" used - an exothermic reaction is one which gives out heat. Do not try this reaction at home! It can go badly wrong, and put you at serious risk. I am going to give you two pieces of video about this reaction - one in the lab, and one showing an industrial use for the reaction. This competition between aluminium and iron again shows that the aluminium is the more reactive metal and takes the oxygen from the iron(III) oxide to leave metallic iron. The reaction between aluminium and iron(III) oxide In fact, because of the temperatures created, any that is formed is going to react with oxygen in the air to go back to copper(II) oxide again.īut the vigour of the reaction shows that magnesium is definitely higher in the reactivity series than copper. Unfortunately, the reaction is so violent, that it is impossible to see easily that any copper metal has been formed. There is clearly a very vigorous reaction as the magnesium takes the oxygen from the copper. Start by watching this very, very short bit of YouTube video showing what happens when you heat a mixture of magnesium and copper (II) oxide on a piece of ceramic paper on a tripod. The reaction between magnesium and copper(II) oxide Instead, we put metals in competition with each other over control of oxygen by giving one of the metals oxygen to start with, and seeing if another metal can grab it for itself. Too much depends on whether the metal is in a big chunk or a fine powder, or whether there is anything on the surface which prevents oxygen from getting at it. If you have read the introductory page about burning metals, you will know that you can't safely say anything precise about their reactivity just by heating them in air or oxygen. It assumes that you will already have read the page about burning metals and have seen the list of the reactivity series on this page. This page shows how you can build up a part of the reactivity series using reactions between metals and the oxides of other metals. Reactions between metals and metal oxides
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