NCERT Solutions Class 10th Science Chapter – 3 Metals and Non-metals
| Textbook | NCERT |
| Class | 10th |
| Subject | Science |
| Chapter | 3rd |
| Chapter Name | Metals and Non-metals |
| Category | Class 10th Science |
| Medium | English |
| Source | Last Doubt |
| NCERT Solutions Class 10th Science Chapter – 3 Metals and Non-metals Notes What are the example of metal and non metal?, What are the 17 non-metals?, Which are the 11 non-metals?, What is called metal?, What is metal explain?, What are the main types of metals?, What are 5 uses of metals?, What are metal elements?, Is carbon a metal?, What are 22 nonmetals?, Is A Diamond a metal?, What are the 3 types of metals?, Is coal a metal?, Why are metals called?, How metal is made?, Why is metal important?, Which group is metal?, What is the symbol of metal? and What is metal and example? etc. |
NCERT Solutions Class 10th Science Chapter – 3 Metals and Non-metals
Chapter – 3
Metals and Non-metals
Notes
1. Metal
| Properties of Metal • Solid • Ductile • Malleable • Lusturous • Sonorous • Good conductor Reaction with • Air • Water • Acids • Compounds of other metals • Reactivity series |
2. Non-Metal
| Properties of Non-Metal • Solids, Liquids or Gases • Brittle • Bad Conductor • Non-Malleable • non-Lustrous • Non-Sonorous Reaction with Air |
3. Alloys
| Importance and Uses – Prevent corrosion Changed resistivity changed melting point Some alloys are Steel, Stainless steel, brass, bronze, solder and amalgam etc. |
4. Metallurgy
| Ore Enrichment ↓ Conversion of ore into Metal oxide: Roasting/Calcination ↓ Conversion of Metal oxide into metal: ↓ Heating Using Coke ↓ More reactive metal ↓ Electrolytic reduction ↓ Refining of Metals |
5. Ionic Compounds
| Formation by electron transfer from metal to non-metal. Physical properties • Solid state, brittle • High melting point • Soluble in water, insoluble in organic solvents • Good conductor in aqueous solution and in molten state |
6. Corrosion
| Prevention of Rusting/Corrosion by galvanization, painting and anodizing etc. (1) Rusting of Iron – Air and moisture are required to form rust (hydrated oxide of iron) Fe2O3. xH2O. (2) Silver – Reacts with H2S to form black Ag2S. (3) Copper – Reacts with Moisture and CO2 to Form green basic CUCO3, Cu(OH)2. |
Metals and Non Metals
| Metal • About 118 elements are known till date. There are more than 90 metals, 22 non metals and few metalloids. • Sodium (Na), Potassioum (K), Calcium (Ca), Magnesium (Mg), Iron (Fe), Aluminium (AI) are some metals. Metals around us Part of machines and defense equipments Making bridges, buildings, railway tracks Utensils and coins Jewellery and Ornaments Manufacturing of trains, cars, ships, aeroplanes Non-Metal Oxygen (O), Nitrogen (N), Hydrogen (H), Sulphur(S), Phosphorus (P), Fluorine (F), Bromine (Br) are a few non metals. Non-Meatal arounds us Carbon – as fuel, in nutrients, electrodes and jewellery. Hydrogen – in hydrocarbons, making of fertillzers and vegetable ghee, as fuel. Oxygen – in respiration, in fuel combustion. Nitrogen – in preventing rancidity, in tyres and making of acids, fertillizers and explosives. |
Different between Metal and Non-Metal
|
| Chemical Properties of Metals – 1. Reaction with air 2. Reaction with water 3. Reaction with dilute acids 4. Reaction with other metal compounds 5. Reaction between metals and non-metals |
1. Reaction with air
| Metals can either burn, react or don’t react with air Metal + Oxygen → Metal oxide Example – (i) 2Na + 02 → Na2O (ii) 2Mg + 02 → MgO (iii) 2Cu + 02 → CuO (black) (iv) 3Fe + 202 → Fe304 Some metals like Na and K are kept immersed in kerosene as they react vigorously with air. Metals like Mg, AI, Zn and Pb react slowly with air and form a protective layer. Magnesium can burn in air but combine with oxygen to form oxide. Fe and Cu does not burn in air but combine with oxygen to form their oxides. Iron filings burn when sprinkled in the flame of burner. Silver, platinum and gold show no reaction with air. Amphoteric oxides – These are metal oxides which react with both acids as well bases. Example: ZnO, Al2O3 (i) Al2O3 + 6HCl → 2AlCl3 + 3H20 (ii) Al2O3 + 2NaOH → 2NaAlO2 + H2O Sodium aluminate = NaAlO2 Anodizing of metals – In Anodizing, Aluminium is made anode and graphite as cathode, oxygen gas is released by the electrolysis of Sulphuric acid, which reacts with aluminium to form a thick protective oxide layer on the surface of metal. |
2. Reaction with water
| Metals react with water differently and Not all metals react with water. Example – (i) 2K + 2H20 → 2KOH + H2 (ii) Ca + 2H2O → Ca(OH)2 + H2 (iii) Mg + 2H20 → Mg(OH)2 + H2 Three Condition of Water form react with metal Metal React with cold water Example: Na, K, Ca Metal React only with steam Example: Fe, Al Metal React with hot water Example: Mg • In case, of Ca and Mg, the metal starts floating due to bubbles of hydrogen gas sticking to its surface. Example – (i) 2Al + 3H2O → Al2O3 + 3H2 (ii) 3Fe + 4H2O → Fe3O4 + 4H2 |
3. Reaction with dilute acids
| (i) Most metals react with dilute HCl and dilute H2SO4, to form salt and hydrogen gas. Metal + dilute acid → salt + hydrogen gas Example – (a) Mg + 2HCl → MgCl2 + H2 (b) Al + 6HCl → 2AlCl3 + 3H2 (c) Zn + H2SO4 → ZnSO4 + H2 Important thing – Copper(Cu), Mercury(Hg) and Silver(Ag) don’t react with dilute acids. (ii) With dilute nitric acid – As metals react with dilute nitric acid, hydrogen gas produced is oxidised to water. Mg and Mn are exceptions. Mg + 2HNO3 → Mg(NO3)2 + H2 Aqua Regia – It is a mixture of concentrated HCl and concentrated HNO3 in a 3:1 ratio. It dissolves gold and platinum. |
4. Reaction with other metal compounds
| Metal A + Salt solution of metal B → Salt solution of Metal B + Metal A More reactive metals can displace less reactive metals from their compounds in solution. This forms the basis of reactivity series of metals. Reactivity series of metals – It is an arrangement of metals in decreasing order of their reactivity. (i) K> Na > Ca > Mg > Al > Zn > Fe > Pb > H> Cu > Hg > Ag > Au → Decreasing reactivity (ii) Copper being more reactive displace Silver Example: Cu + 2AgNo3 → Cu(NO3)2 + 2Ag |
5. Reaction between metals and non-metals
| Reactivity of elements can be understood as a tendency to attain a completely filled valence shell arrangement. Atom of metals lose valence electron to form cations (+ve ions) Atoms of non-metals can gain electron in valence shell to form anions (-ve ions) Oppositely charged ions attract each other forming an ionic compound. Formation of MgCl2 Mg → Mg2+ + 2e– (2,8,2) → (2,8) 2Cl + 2e– → 2Cl– (2,8,7) → (2,8,8)  Properties of Ionic compounds – Are solid and mostly brittle. Have high melting and boiling points. More energy is required to overcome the strong inter-ionic force of attraction. Generally soluble in water, but insoluble in inorganic solvents like kerosene, petrol etc. Conduct electricity in aqueous solutions and in molten state. In both cases, free ions are formed and conduct electricity. |
Occurance of Metals
| (1) Minerals – Compounds of metals present in earth’s crust can be termed as minerals. (2) Ores – Mineral from which metal can be economically extracted is called an ore. Example – sulphide ores, carbonate ores, oxide ores. Not all the minerals are ores. Metals at the bottom of reactivity series like gold, platinum, silver, copper occur in free state. But copper and silver also occur in sulphide and oxide ores. Metals of moderate reactivity (Zn, Fe, Pb) occur mainly as oxide, sulphide or carbonate ores. Metals of high reactivity (K, Na, Ca, Mg, AI) are found in combined states. (3) Gangue – Ores are found mixed with earthly impurities like soil, sand, etc. known as gangue. The gangue is removed from the ore. (4) Metallurgy – It is the step-wise process of obtaining metal from its ore. These steps are 1. Enrichment of ore. 2. Obtaining metal from enriched ore. 3. Refining of impure metal to obtain pure metal. |
Obtaining Metals low in the reactivity series
| These metals can be obtained by heating the ore in air at high temperature. (i) Mercury from cinnabar  (ii) Copper from copper sulphide 2Cu2S + 302 heat → 2Cu2O + 2SO2 ↑ 2Cu2O + Cu2S heat → 6Cu + SO2 ↑ |
Extracting Metals in the middle of Activity series
| Metals are easier to obtain from oxide ores, thus, sulphide and carbonate ores are converted into oxides. Metal ore heated strongly in excess of air (Roasting) Example: 2ZnS + 302 heat → 2ZnO + 2SO2 Metal ore heated strongly in limited supply of air (Calcination) Example: ZnCO3 heat → ZnO + CO2 Reduction of metal oxide – 1. Using coke – Coke as reducing agent. Example – ZnO + C heat → Zn + CO 2. Using Displacement Reaction – highly reactive metal like Na, Ca and Al are used to displace metals of lower reactivity from their compounds. Example – (i) MnO2 + 4Al heat → 3Mn + 2Al2O3 + heat (ii) Fe2O3 + 2Al heat → 2Fe + Al2O3 + heat In the above reaction Molten iron is formed and is used to join railway tracks. This is called thermit reaction. |
Extracting Metals at the top of Activity Series
| These metals Have more affinity for oxygen than carbon These metals are obtained by electrolytic reduction. Sodium is obtained by electrolysis of its molten chloride NaCI → Na+ + CI– As electricity is passed through the solution metal gets deposited at cathode and non-metal at anode. (i) At cathode: Na+ + e– → Na (ii) At anode: 2CI– → CI2 + 2e– |
Refining of Metals
| Impurities present in the obtained metal can be removed by electrolytic refining. Copper is obtained using this method. Following are present inside the electrolytic tank. • Anode-slab of impure copper • Cathode-slab of pure copper • Solution-aqueous solution of copper sulphate with some amount of dilute Sulphuric acid. • From anode copper ions are released in the solution and equivalent amount of copper from solution is deposited at cathode. • Insoluble impurities containing silver and gold gets deposited at the bottom of anode as anode mud.  |
Corrosion
| Metals are attacked by substances in surroundings like moisture, acids, and moist air. Silver- it reacts with H2S in air to form silver sulphide and articles become black. Copper-reacts with moist carbon dioxide in air and gains a green coat of basic copper carbonate. Iron-acquires a coating of a brown flaky substance called rust. Both air and moisture are necessary for rusting of iron. |
Prevention of Corrosion
| • Rusting of iron is prevented by painting, oiling, greasing, galvanizing, chrome plating, anodising and making alloys. • In galvanization iron or steel is coated with a layer of zinc because zinc is preferably oxidized than iron. • Alloys – these are mixture of metals with metals or non-metals Adding small amount of carbon makes iron hard and strong. • Stainless steel is obtained by mixing iron with nickel and chromium. It is hard and doesn’t rust. Mercury is added to other metals to make amalgam. • Brass – alloy of copper and zinc. • Bronze – alloy of copper and tin. • In brass and bronze, melting point and electrical conductivity is lower than that of pure metal. • Solder – alloy of lead and tin has low melting point and is used for welding electrical wires.  |
Alloys
| These are homogeneous mixture of metals with metals or non-metals. Adding small amount of carbon makes iron hard and strong.
|
| NCERT Solution Class 10th Science All Chapters Notes |
| NCERT Solution Class 10th Science All Chapters Question & Answer |
| NCERT Solution Class 10th Science All Chapters MCQ |
You Can Join Our Social Account
| Youtube | Click here |
| Click here | |
| Click here | |
| Click here | |
| Click here | |
| Telegram | Click here |
| Website | Click here |