![]() Lead(II) oxide is formed.Ĭopper glows faintly. The residue is brown when hot and yellow when cold. Iron has a medium reactivity with oxygen. The residue is reddish- brown when hot and cold. The residue is yellow when hot and white when cold. Magnesium has a very high reactivity with oxygen. Magnesium burns brightly with a very brilliant white flame. Steps 1 to 4 are repeated using zinc powder, iron filings, lead powder and copper powder, one at a time, in place of magnesium powder.How vigorously magnesium reacts with oxygen and the colour of the residue when it is hot and when it is cold are observed. Then, the solid potassium manganate(VII) is heated. The magnesium powder is heated strongly.One spatulaful of magnesium powder is placed on a piece of asbestos paper and is put into the tube.The tube is clamped horizontally as shown in Figure. Some glass wool is pushed into the tube.One spatulaful of solid potassium manganate(VII) is put into a boiling tube.Materials: Magnesium powder, zinc powder, iron filings, lead powder, copper powder, solid potassium manganate(VII), asbestos paper, glass wool.Īpparatus: Boiling tube, retort stand and clamp, Bunsen burner, spatula, forceps.Īsbestos paper and glass wool are hazardous and should be handled with care. Reactivity Series of Metals with Oxygen ExperimentĪim: To investigate the reactivity of metals with oxygen. Oxidation and Reduction in Chemical Cells.Oxidation and Reduction in Electrolytic Cells.Application of the reactivity series of metals in the extraction of metals.Redox Reactions by Transfer of Electrons at a Distance.Displacement of Halogen From Halide Solution.Redox reaction in the displacement of metals from its salt solution.Changing of iron(II) ions to iron(III) ions and vice versa.This series of metals is quite similar to the electrochemical series because the reactivity of a metal with oxygen is closely linked to its ability to lose electrons. The reactivity series of metals towards oxygen is a list of metals according to their reactivity with oxygen.Hence, by observing how vigorously the metals react with oxygen, we can arrange the metals according to their reactivity towards the oxygen.The more reactive a metal is towards oxygen, the more vigorously it burns in oxygen.(c) Thus, metal acts as the reducing agent while oxygen acts as the oxidising agent in the formation of metal oxide. Its oxidation number decreases from 0 to -2. (b) Oxygen undergoes reduction to form oxide ions. Its oxidation number increases from zero to a positive value. (a) Metal undergoes oxidation to form positive ions. The formation of metal oxide is a redox reaction. One of the common compounds formed by metals is metal oxide.Aluminium, potassium and sodium have very high reactivity, and therefore exist as compounds in nature.Gold has very low reactivity and therefore can be found in its metallic state in nature.In fact, the form in which a metal occurs in nature depends on its reactivity. The reactivity of metals differs from one metal to another.The Reactivity Series of Metals Towards Oxygen ![]()
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