These notes for CBSE Class 10 Science, Chapter 3, focus on Metals and Non-metals. They begin by classifying elements into metals, non-metals, and metalloids based on their properties. The document provides a detailed comparison of the physical properties of metals and non-metals, including their state, melting/boiling points, density, malleability, ductility, conductivity, luster, sonority, and hardness. It further elaborates on the chemical properties, detailing reactions with oxygen, water, dilute acids, salt solutions, chlorine, and hydrogen. The notes explain the formation of oxides, hydroxides, chlorides, and hydrides, highlighting the acidic or basic nature of oxides and the amphoteric nature of some metal oxides. The properties of ionic compounds, such as their physical nature, melting/boiling points, solubility, and electrical conductivity in different states, are also discussed. Finally, the notes touch upon the occurrence of metals, defining minerals and ores with examples like Bauxite and Haematite. These notes are ideal for students preparing for their exams.
Last optimized 10 Aug 2026
Jump to solutions, books, papers, or another subject — without leaving NCERT Help.
Elements are classified broadly into two categories on the basis of properties: Metals: Iron, Zinc, Copper, Aluminium etc.
Non – metals: Chlorine, Nitrogen, Hydrogen, Oxygen, Sulphur etc.Apart from metals and non-metals some elements show properties of both metals and non – metals, e.g. Silicon, Arsenic, Germanium .They are called metalloids
S.No |
Property |
Metals |
Non-Metals |
1 |
Physical State |
Metals are solid at room temperature. Except mercury and gallium. |
Non-metals generally exist as solids and gases, except Bromine. |
2 |
Melting and boiling points |
Metals generally have high m.pt and b.pt except gallium and cesium. |
Non-metals have low m.pt and b.pt except diamond and graphite. |
3 |
Density |
Generally high. |
Generally low. |
4 |
Malleability and Ductility |
Malleable and ductile. |
Neither malleable nor ductile. |
5 |
Electrical and thermal conductivity |
Good conductors of heat and electricity. |
Generally poor conductors of heat and electricity except graphite. |
6 |
Luster |
Poses shining luster. |
Do not have luster except iodine. |
7 |
Sonorous sound |
Give sonorous sound when struck. |
Does not give sonorous sound. |
8 |
Hardness |
Generally hard except Na, K |
Solid non-metals are generally soft except diamond. |
1 |
Reaction with Oxygen |
Metal + Oxygen?Metal oxide 4Na(s) + O2(g) ?2Na2O(s) 4Al(s) + 3O2(g) ?2Al2O3 Metals form basic oxides Zn and Al form amphoteric oxides (they show the properties of both acidic and basic oxides) Most of the metal oxides are insoluble in water Some of them dissolve to form Alkali Na2O(s) + H2O(l) ?2NaOH(aq) |
Non-metal + Oxygen ?Non-metal oxide C + O2 ?CO2 S + O2 ?SO2 Non-metals form acidic oxides CO and HO2O are neutral oxides(they are neither acidic nor basic in nature) Non- metal oxides are soluble in water They dissolve in water to form acids SO2 + H2O ?H2SO3 |
2 |
Reaction with water |
Metals react with water to form metal oxides or metal hydroxide and H2 gas is released. 2Na(s) + 2H2O(l) ?2NaOH + H2(g) + heat |
Non-metals do not react with water, steam to evolve hydrogen gas. Because Non-metals cannot give electrons to hydrogen in water so that it can be released as H2 gas. |
3 |
Reaction with dilute Acids |
Metal + Acid ?Metal salt + Hydrogen HCl Mg(s) + 2HCl(aq)? MgCl2(aq) + H2(g) H2SO4 2Na(s) + H2SO2? Na2SO4(aq) +H2(g) HNO3 Metal + HNO3? H2 gas is not displaced. Reason- HNO3 is strong oxidizing agent. |
Non-metals do not react with acids to release H2 gas Reason- Non-metals cannot loose electrons and give it to Hydrogen ions of acids so that the gas is released. Mn + 2HNO3? Mn(NO3)2 + H2 H2 gas from HNO3 |
4 |
Reaction with salt solutions |
When metals react with salt solution, more reactive metal will displace a less reactive metal from its salt solution. CuSO4(aq) + n(s)? ZnSO4(aq) + Cu(s) |
When non-metals react with salt solution, more reactive non-metal will displace a less reactive non-metal from its salt solution. 2NaBr(aq) + Cl2(g)? 2NaCl(aq) + Br2(aq) |
5 |
Reaction with Chlorine |
Metal + Chlorine? Metal Chloride ionic bond is formed. Therefore Ionic compound is obtained. 2Na+ Cl2 ? 2NaCl |
Non-metal + Chlorine?Non-metal Chloride covalent bond is formed. Therefore covalent compound is obtained. H2(g) + Cl2 ? 2HCl
|
| 6 | Reaction with Hydrogen |
Metals react with hydrogen to form metal hydride This reaction takes place only for most reactive metals. 2Na(s)+ H2(g) ? 2NaH(s) |
Non-metals react with hydrogen to form hydrides H2(g) + S(l) ? H2S(g) |
Properties of ionic compounds |
||||
| 1. | Physical nature |
: | solid and hard due to strong force of attraction. (generally brittle) | |
| 2. | Melting point and boiling point |
: | have high M.P and B.P, as large amount of heat energy is required to break strong ionic attraction. | |
| 3. | Solubility |
: | soluble in water and insoluble in kerosene and pertrol. | |
| 4. | Conduction of electricity |
: | ionic compounds in solid state-----does not conduct electricity. | |
Reason—Ions can not move due to rigid solid structure. Ionic compounds conduct electricity in molten state. |
||||
Reason-- Ions can move freely since the electrostatic forces of attraction between the oppositely charged ions are overcome due to heat. |
||||
Occurrence of metals. It occurs in Earths crust, sea-water
|
||||
Minerals Elements or compounds, occuring naturally in the earth‘s crust |
Ores Minerals that contain very high percentage of a perticular metal and these met als can be extracted economically on a large scale. e.g Bouxite ore ? Aluminium Haematite ? Iron |
|||
Elements are broadly classified into metals, non-metals, and metalloids based on their properties.
Mercury and Gallium are exceptions to metals being solid at room temperature; they are liquid.
Metals generally form basic oxides, although some like Zinc and Aluminium form amphoteric oxides.
Non-metals do not react with water or steam to evolve hydrogen gas because they cannot donate electrons to hydrogen.
Ionic compounds conduct electricity in the molten state because their ions can move freely.
Minerals are naturally occurring elements or compounds in the Earth's crust, while ores are minerals from which metals can be extracted economically on a large scale.
Generally, non-metals are poor conductors, but graphite is an exception and conducts heat and electricity.
Copyright @ ncerthelp.com A free educational website for CBSE, ICSE and UP board.
