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At standard temperature and pressure, it resists all but the strongest oxidizers.
It does not react with sulfuric acid, hydrochloric acid, chlorine or any alkalis.
Carbon's covalent radii are normally taken as 77.2 pm (C–C), 66.7 pm (C=C) and 60.3 pm (C≡C), although these may vary depending on coordination number and what the carbon is bonded to.
In general, covalent radius decreases with lower coordination number and higher bond order.
The most common oxidation state of carbon in inorganic compounds is 4, while 2 is found in carbon monoxide and transition metal carbonyl complexes.
It is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds.
This gives graphite its softness and its cleaving properties (the sheets slip easily past one another).
Because of the delocalization of one of the outer electrons of each atom to form a π-cloud, graphite conducts electricity, but only in the plane of each covalently bonded sheet.
At normal pressures, carbon takes the form of graphite, in which each atom is bonded trigonally to three others in a plane composed of fused hexagonal rings, just like those in aromatic hydrocarbons.
The resulting network is 2-dimensional, and the resulting flat sheets are stacked and loosely bonded through weak van der Waals forces.