Notes of chapter carbon and its compound
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Carbon is a chemical element with symbol C and atomic number 6. It is nonmetallic and tetravalent — making four electrons available to form covalent chemical bonds. It belongs to group 14 of the periodic table. Three isotopes occur naturally, 12C and 13C being stable, while 14C is a radionuclide, decaying with a half-life of about 5,730 years.
Carbon is one of the few elements known since antiquity.
Carbon compounds form the basis of all known life on Earth, and the carbon–nitrogen cycle provides some of the energy produced by the Sun and other stars.
The most common oxidation state of carbon in inorganic compounds is +4, while +2 is found in carbon monoxide and transition metal carbonyl complexes.
The largest sources of inorganic carbon are limestones, dolomites and carbon dioxide, but significant quantities occur in organic deposits of coal, peat, oil, and methane clathrates. Carbon forms a vast number of compounds, more than any other element, with almost ten million compounds described to date, and yet that number is but a fraction of the number of theoretically possible compounds under standard conditions.
For this reason, carbon has often been referred to as the "king of the elements".
The allotropes of carbon include graphite, one of the softest known substances, and diamond, the hardest naturally occurring substance.
It bonds readily with other small atoms including other carbon atoms, and is capable of forming multiple stable covalent bonds with suitable multivalent atoms.
Carbon is known to form almost ten million different compounds, a large majority of all chemical compounds. Carbon also has the highest sublimation point of all elements.
Carbon is the 15th most abundant element in the Earth's crust, and the fourth most abundant element in the universe by mass after hydrogen, helium, and oxygen.
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