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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 |
Non-metals generally |
2 |
Melting and boiling points |
Metals generally have |
Non-metals have low |
3 |
Density |
Generally high. |
Generally low. |
4 |
Malleability and Ductility |
Malleable and ductile. |
Neither malleable nor |
5 |
Electrical and thermal conductivity |
Good conductors of heat |
Generally poor |
6 |
Luster |
Poses shining luster. |
Do not have luster |
7 |
Sonorous sound |
Give sonorous sound |
Does not give |
8 |
Hardness |
Generally hard except |
Solid non-metals are |
1 |
Reaction
with |
Metal + Oxygen→Metal oxide |
Non-metal + Oxygen →Non-metal oxide |
2 |
Reaction |
Metals react with water to |
Non-metals do not react |
3 |
Reaction |
Metal + Acid →Metal salt
+ Hydrogen HCl |
Non-metals do not react
with acids to release H2 gas |
4 |
Reaction |
When metals react with salt |
When non-metals react |
5 |
Reaction with Chlorine |
Metal + Chlorine→ Metal Chloride |
Non-metal + Chlorine→Non-metal Chloride covalent bond is formed. Therefore covalent compound is obtained. H2(g) + Cl2 → 2HCl
|
6 | Reaction |
Metals react with hydrogen |
Non-metals react with hydrogen to form hydrides H2(g) + S(l) → H2S(g) |
Properties of ionic compounds |
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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. |
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Reason-- Ions can move freely since the electrostatic forces of attraction between the oppositely charged ions are overcome due to heat. |
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Occurrence of metals. It occurs in Earths crust, sea-water |
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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. |
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