Explain Chemical properties of metal and non metal
Answers
Explanation:
Chemical Properties of Metals
The density of metals is usually high.
Metals are malleable and ductile.
Metals form an alloy with other metals or non – metals.
Some metals react with air and corrode. ...
Metals are good conductors of heat and electricity. ...
Generally, metals are in a solid state at room temperature.
Chemical Properties of Nonmetals
Nonmetals are poor conductors of heat and electricity. ...
Unlike metals, nonmetals aren't malleable and ductile.
Nonmetals react more with metals than with nonmetals.
Usually, nonmetals react with other nonmetals in high temperature.
Most nonmetals do not react with air in room temperature.
Explanation:
Comparison of physical and chemical properties of metals and non – metals:-
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.
Comparison of Chemical Properties of Metals and Non-metals:-
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)