Online revision notes for CBSE Class 10 Science are created by askIITians Science experts to help you understand all the concepts of this chapter. Metals and nonmetals is an interesting chapter that includes information about how metals are extracted, what are the different properties of metals and non-metals, the reactivity series of metals, corrosion of metals and prevention of corrosion. The experts at askIITians have created the revision notes for this chapter covering all these topics in detail.
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Elements are classified as metals and non-metals based on different properties. The properties of metals and non-metals are given in the form of the table below-
Metals |
Non-metals |
Metals are lustrous, that is, they have a property to shine. |
They are not lustrous, that is, they do not have a shining surface except, graphite and iodine. |
All metals exist as solids except mercury which is liquid at room temperature. |
They are generally soft, except for diamonds. |
They can be drawn into wires, this is known as Ductility. |
They are non-ductile. |
Metals can be converted into sheets, this is known as Malleability, except mercury |
They are non-malleable |
They are good conductors of electricity and heat. Except for Lead and mercury. |
They are poor conductors of electricity and heat. Exception-graphite is a good conductor of electricity |
They have high density and high melting point. Exception-sodium and potassium have low melting points. |
They have low density compared to metals and low melting point except for Diamond which has a high melting point. |
For Example, Copper reacts with oxygen to form copper oxide.
Metal + O2 → Metal oxide
2Cu + O2 → 2CuO
4Al + 3O2 → 2Al2O3
Al2O3 + 6HCl → 2AlCl3 + H2O
2Na + 2H2O → 2NaOH + 1H2
2Al + 3H2O → Al2O3 + 3H2
Metal + Acid → Metal Salt + Hydrogen
Mg + 2HCl → MgCl2 + H2
Non-metal + Oxygen → Non-metal oxide
C + O2 → CO2
2 NaBr (aq) + Cl2(aq) → 2NaCl (aq) + Br2 (aq)
H2(g) + S(l) → H2S(g)
The series in which metals are arranged in the decreasing order of reactivity is known as the Reactivity Series.
Fig.1. Reactivity Series
Compounds formed due to the transfer of electrons from a metal to a non-metal are known as Ionic Compounds.
A bond is formed by the sharing of electrons between the two atoms. They share their valence electrons to gain stability.
Elements or compounds which occur naturally in earth crust are known as Minerals. Minerals from which pure metals can be extracted are known as Mineral Ores.
Extraction of pure metals from its ores/steps for extraction of metals from its ore
Gangue - Ores contain different impurities in it such as sand, soil etc. These impurities are known as Gangue.
Extracting Metals which are low in activity series
Metals which are low in the activity series are unreactive. The oxides of such metals can be reduced to metals by heating alone. For Example, Cinnabar (HgS)
Extracting Metals in the middle of the Activity Series
These metals are moderately reactive. They exist as sulphides or carbonates in nature. Before reduction, metal sulphides and carbonates must be converted into metal oxides. Sulphide ores are converted into oxides by heating strongly in the presence of excess air, this is known as Roasting. Carbonate ores are converted into oxides by heating in limited air. This is known as Calcination.
Roasting
Calcination
Reduction-metal oxides can be reduced to metals using a reducing agent such as Carbon.
Extracting metals towards the top of the activity series
The metals are highly reactive. They cannot be obtained by heating. For Example, Sodium, magnesium and calcium are obtained by the electrolysis of their molten chlorides.
At cathode Na+ + e- → Na
At anode 2Cl- → Cl2 + 2e-
Refining of impure metal is done using electrolytic refining. Impure copper is used as anode and a strip of pure copper is used as Cathode. Acidified copper sulphate is used as an electrolyte. When an electric current is passed through this, impure metal from the anode gets deposited in the electrolyte solution, whereas pure metal from the electrolyte is deposited at the cathode.
Deposition of insoluble residue formed from the dissolution of the anode during commercial electrolysis.
Fig.2. Electrolytic refining
When exposed to moist air for a long period of time, metals become corroded. This is known as Corrosion. For Example, Silver reacts with moist air and becomes black in colour due to silver sulphide coating.
Iron + oxygen → Iron (III) oxide
Fe + O 2 → Fe2O3
Mixture of two or more metals or metal and non-metal is known as Alloy. For Example,
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