Allotropes of Carbon

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Allotropes are DIFFERENT STRUCTURAL forms of the SAME ELEMENT in the same physical state.

Here are examples of different allotropes of Carbon:

Formed from CARBON ATOMS each sharing four COVALENT BONDS in a rigid, three-dimensional structure.
DIAMOND is very hard, with a high melting point. This is because of the LARGE NETWORK of covalent bonds that require a LARGE AMOUNT of ENERGY to overcome.
It does not conduct electricity as it has NO FREE MOVING ELECTRONS OR IONS.

Composed of LAYERED structures of HEXAGONAL RINGS, with each carbon atom bonded to THREE other atoms with COVALENT BONDS.
Carbon has FOUR electrons in its outer shell, so the fourth electron that is NOT used for bonding is DELOCALISED.
This means GRAPHITE is a good CONDUCTOR of electricity, as its delocalised electrons can carry a charge (just like metals).
It is SOFT, and used as a LUBRICANT due to weak forces between layers, causing the layers to SLIDE over one another.

Graphene ia a SINGLE LAYER of graphite, and is strong and light.
It is a good CONDUCTOR of HEAT and ELECTRICITY due to its DELOCALISED ELECTRONS, so is used in ELECTRONICS and composite materials.

FULLERENES are molecules with hollow shapes, such as spheres or tubes.
The structure of fullerenes is based on hexagonal rings of Carbon atoms but they may also contain rings with five or seven Carbon atoms.
They can ENCAPSULATE other molecules and are used in drug delivery and as INDUSTRIAL CATALYSTS.

Nanotubes

Carbon nanotubes are CYLINDRICAL fullerenes with very HIGH length to diameter ratios.
Their properties make them useful for nanotechnology, electronics and materials.
They are good CONDUCTORS of HEAT and ELECTRICITY as they have DELOCALISED ELECTRONS, meaning they can be used in ELECTRONICS and nanotechnology.
They have a very high TENSILE STRENGTH without much MASS meaning they are useful for certain materials, such as the ones used in TENNIS RACKETS.

Allotropes are DIFFERENT STRUCTURAL forms of the SAME ELEMENT in the same physical state.

Here are examples of different allotropes of Carbon:

Formed from CARBON ATOMS each sharing four COVALENT BONDS in a rigid, three-dimensional structure.
DIAMOND is very hard, with a high melting point. This is because of the LARGE NETWORK of covalent bonds that require a LARGE AMOUNT of ENERGY to overcome.
It does not conduct electricity as it has NO FREE MOVING ELECTRONS OR IONS.

Composed of LAYERED structures of HEXAGONAL RINGS, with each carbon atom bonded to THREE other atoms with COVALENT BONDS.
Carbon has FOUR electrons in its outer shell, so the fourth electron that is NOT used for bonding is DELOCALISED.
This means GRAPHITE is a good CONDUCTOR of electricity, as its delocalised electrons can carry a charge (just like metals).
It is SOFT, and used as a LUBRICANT due to weak forces between layers, causing the layers to SLIDE over one another.

Graphene ia a SINGLE LAYER of graphite, and is strong and light.
It is a good CONDUCTOR of HEAT and ELECTRICITY due to its DELOCALISED ELECTRONS, so is used in ELECTRONICS and composite materials.

FULLERENES are molecules with hollow shapes, such as spheres or tubes.
The structure of fullerenes is based on hexagonal rings of Carbon atoms but they may also contain rings with five or seven Carbon atoms.
They can ENCAPSULATE other molecules and are used in drug delivery and as INDUSTRIAL CATALYSTS.

Nanotubes

Carbon nanotubes are CYLINDRICAL fullerenes with very HIGH length to diameter ratios.
Their properties make them useful for nanotechnology, electronics and materials.
They are good CONDUCTORS of HEAT and ELECTRICITY as they have DELOCALISED ELECTRONS, meaning they can be used in ELECTRONICS and nanotechnology.
They have a very high TENSILE STRENGTH without much MASS meaning they are useful for certain materials, such as the ones used in TENNIS RACKETS.