Physical Properties of Non-metals
Below are the properties of non metals:
Physical state: Most
of the non-metals exist in two of the three states of matter at room
temperature: gases (oxygen) and solids (carbon). These have no metallic
lustre, and do not reflect light.
Nature: Non-metals are very brittle, and cannot be rolled into wires or pounded into sheets.
Conduction: They are poor conductors of heat and electricity.
Electronegative Character: Non-metals have a tendency to gain or share electrons with other atoms. They are electronegative in character.
Reactivity: They generally form acidic or neutral oxides with oxygen.
Metals and Non-Metals - Compared
A detailed comparison of properties of metals and non-metals is given in table:
Property | Metals | Non-metals |
State of matter | These are usually solid, except mercury, which is a liquid at room temperature. Gallium and Caesium melt below 30. So if room temperature is around 30, they may also be in liquid state | These exist in all the three states. Bromine is the only liquid. |
Density | They usually have high density, except for sodium, potassium, calcium etc. | Their densities are usually low. |
Melting point | They usually have a high melting point except mercury, cesium, gallium, tin, lead. | Their melting points are low. |
Boiling point | Their boiling points are usually high. | Their boiling points are low. |
Hardness | They are usually hard, except mercury, sodium, calcium, potassium, lead etc. | They are usually not hard. But the exception is the non-metal diamond, the hardest substance. |
Malleability | They can be beaten into thin sheets. | They are generally brittle. |
Ductility | They can be drawn into thin wires, except sodium, potassium, calcium etc. | They cannot be drawn into thin wires. |
Conduction of heat | They are good conductors of heat. | They are poor conductors of heat. |
Conduction of electricity | They are good conductors of electricity. | They are non-conductors, except for carbon in the form of graphite and the gas carbon. |
Lustre | Newly cut metals have high lustre. Some get tarnished immediately. | Usually not lustrous, except iodine and diamond - the most lustrous of all the substances. |
Alloy formation | They form alloys. | Generally, they do not form alloys. However carbon, phosphorus, sulphur etc. can be present in some alloys. |
Tenacity | These usually have high tensile strength except sodium, potassium, calcium, lead etc. | These have low tensile strength. |
Brittleness | They are hard but not brittle, except zinc at room temperature. | They are generally brittle. |
Electronic configuration | They usually have 1, 2 or 3 electrons in their valence shell. The greater the number of shells and lesser the number of valence electrons, the greater is the reactivity of the metal. | They usually have 4, 5, 6 or 7 electrons in the valence shell. If it has 8 electrons, it is called a noble gas. Lesser the number of shells and greater the number of valence electrons, greater is the reactivity of the non-metal. |
Ionization | They always ionize by losing electrons: | They always ionize by gaining electrons: |
Charge of ions | Positively charged. | Negatively charged. |
Type of valency | Metals always exhibit electrovalency. | Non-metal exhibit both electrovalency or covalency. |
Deposition during electrolysis | They are always deposited at the cathode. | They are always deposited at the anode. |
Redox reaction | These lose electrons and hence get oxidized. | These gain electrons and hence get reduced. |
Redox agents | They are reducing agents. | They are oxidizing agents. |
Nature of oxides | They generally form basic oxides, some of which are also amphoteric, such as aluminium oxide, zinc oxide, lead oxide etc. | They generally form acidic oxides. Some oxides are neutral, such as nitrous oxide, nitric oxide, carbon monoxide water etc. |
Hydrides | They usually do not form hydrides except those of sodium, potassium and calcium. | They do form hydrides, e.g. NH3, PH3, HCl, HBr, HI, H2S, H2O etc. |
Atomicity | These are always monatomic. | These can be mono, di, tri, or polyatomic. |
Solubility | They do not dissolve in solvents except by chemical action. | They dissolve in solvents and can be re-obtained by evaporation. Example: Sulphur in carbon disulphide. |
Action with chlorine | They produce chlorides, which are electrovalent. | They produce chlorides, which are covalent. |
Action with dilute acids | On reaction with dilute acids they give respective salt and hydrogen. | They do not react with dilute acids. |
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