Redirected from Allotropes
Some classic examples of elements that have allotropes, are phosphorus (in "red" and "white" forms) and carbon (in the form of graphite, diamond, or fullerenes). The term allotropes may also be used to refer to the molecular forms of an element (such as a diatomic gas), even if there is only one such additional form.
Allotropy specifically refers to the chemical bond structure between atoms of the same kind and should not be confused with the existence of multiple physical states, such as with water, which can exist as a gas (steam), a liquid (water), or a solid (ice). These phases of water are not allotropes, since they are caused by changes in the physical bonding between water molecules, rather than changes in the chemical bonding of the water molecules themselves. Allotropes of an element can be in any state, gaseous, liquid, or solid.
Allotropy usually refers to pure elemental solids, while Polymorphism may refer to elemental solids or more generally to any material having multiple crystal structures.
As can be seen with the example of carbon allotropes, certain physical properties can vary dramatically from allotrope to allotrope. In diamond, carbon atoms are connected each to four other carbon atoms in a tetrahedral lattice structure, whereas in graphite, each carbon atom is firmly bonded to just three other carbon atoms in hexagonal sheets. These hexagonal sheets are then more loosely coupled to one another in stacks. The structure of fullerenes (a carbon allotrope found in soot) resembles that of graphite, except that instead of hexagons of carbon atoms, smaller polygons are formed, such as a mix of hexagons and pentagons, such that the sheet can fold back onto itself into closed spheroids, as with the seams of a soccer ball. Allotropes not only show dramatic differences in physical properties but also show differences in chemical properties. Graphite can be oxidized by nitric acid to give compounds related to benzene whereas diamond does not give compounds related to benzene.