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Metal and Non-metal Class 10 Notes For Science Chapter 3

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Metals and NonMetals Class 10 Notes
NCERT CBSE Chapter 3 Chemistry Download pdf

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

Comparison of physical and chemical properties of metals and non – metals






Physical State

Metals are solid at room
temperature. Except mercury and gallium.

Non-metals generally
exist as solids and gases, except Bromine.


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.



Generally high.

Generally low.


Malleability and Ductility

Malleable and ductile.

Neither malleable nor


Electrical and thermal conductivity

Good conductors of heat
and electricity.

Generally poor
conductors of heat and electricity except graphite.



Poses shining luster.

Do not have luster
except iodine.


Sonorous sound

Give sonorous sound
when struck.

Does not give
sonorous sound.



Generally hard except
Na, K

Solid non-metals are
generally soft except diamond.

Comparison of Chemical Properties of Metals and Non-metals:-


Reaction with

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
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


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.


with dilute

Metal + Acid →Metal salt + Hydrogen

Mg(s) + 2HCl(aq)→ MgCl2(aq) + H2(g)
2Na(s) + H2SO2→ Na2SO4(aq) +H2(g)
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


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)


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



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


 Physical nature

:   solid and hard due to strong force of attraction.  (generally brittle)

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.


:   soluble in water and insoluble in kerosene and pertrol.           

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

metal properties


Elements or compounds, occuring naturally in the earth‘s crust


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

Enrichment of Ores

EXAMPLE Roasting Calcination

metal and non metals

Metals and NonMetals Class 10 Notes

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