Open main menu


chemical element with the atomic number of 6

Carbon is a very important chemical element, with a chemical symbol of C. All known life on Earth needs it. Carbon has atomic mass 12 and atomic number 6. It is a nonmetal, meaning that it is not a metal.

Carbon,  6C
Graphite (left) and diamond (right), two allotropes of carbon
General properties
Allotropesgraphite, diamond
Appearancegraphite: black
diamond: clear
Standard atomic weight (Ar, standard)[12.009612.0116] conventional: 12.011
Carbon in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson


Atomic number (Z)6
Groupgroup 14 (carbon group)
Periodperiod 2
Element category  reactive nonmetal, sometimes considered a metalloid
Electron configuration[He] 2s2 2p2
Electrons per shell
2, 4
Physical properties
Phase at STPsolid
Sublimation point3915 K ​(3642 °C, ​6588 °F)
Density (near r.t.)amorphous: 1.8–2.1 g/cm3[1]
graphite: 2.267 g/cm3
diamond: 3.515 g/cm3
Triple point4600 K, ​10,800 kPa[2][3]
Heat of fusiongraphite: 117 kJ/mol
Molar heat capacitygraphite: 8.517 J/(mol·K)
diamond: 6.155 J/(mol·K)
Atomic properties
Oxidation states−4, −3, −2, −1, 0, +1,[4] +2, +3,[5] +4[6] (a mildly acidic oxide)
ElectronegativityPauling scale: 2.55
Ionization energies
  • 1st: 1086.5 kJ/mol
  • 2nd: 2352.6 kJ/mol
  • 3rd: 4620.5 kJ/mol
  • (more)
Covalent radiussp3: 77 pm
sp2: 73 pm
sp: 69 pm
Van der Waals radius170 pm
Color lines in a spectral range
Spectral lines of carbon
Other properties
Natural occurrenceprimordial
Crystal structuregraphite: ​simple hexagonal
Simple hexagonal crystal structure for graphite: carbon

Crystal structurediamond: ​face-centered diamond-cubic
Diamond cubic crystal structure for diamond: carbon

Speed of sound thin roddiamond: 18,350 m/s (at 20 °C)
Thermal expansiondiamond: 0.8 µm/(m·K) (at 25 °C)[7]
Thermal conductivitygraphite: 119–165 W/(m·K)
diamond: 900–2300 W/(m·K)
Electrical resistivitygraphite: 7.837 µΩ·m[8]
Magnetic orderingdiamagnetic[9]
Magnetic susceptibility−5.9·10−6 (graph.) cm3/mol[10]
Young's modulusdiamond: 1050 GPa[7]
Shear modulusdiamond: 478 GPa[7]
Bulk modulusdiamond: 442 GPa[7]
Poisson ratiodiamond: 0.1[7]
Mohs hardnessgraphite: 1–2
diamond: 10
CAS Number7440-44-0
DiscoveryEgyptians and Sumerians[11] (3750 BCE)
Recognized as an element byAntoine Lavoisier[12] (1789)
Main isotopes of carbon
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
11C syn 20 min β+ 11B
12C 98.9% stable
13C 1.1% stable
14C trace 5730 y β 14N
| references

When iron is alloyed with carbon, hard steel is formed. Carbon in the form of coal is an important fuel.


Chemistry of carbonEdit

A whole type of Chemistry, organic chemistry, is about carbon and its compounds. Carbon makes many types of compounds. Hydrocarbons are molecules with carbon and hydrogen. Methane, Propane, and many other fuels are hydrocarbons. Many of the substances that people use daily are organic compounds.

Carbon, hydrogen, nitrogen, oxygen, and some other elements like sulfur and phosphorus together form most life on earth (see List of biologically important elements). Carbon forms a very large number of organic compounds because it can form strong bonds with itself and with other elements. Because of the amounts of carbon living things have, all organic things are considered "carbon-based". Each carbon atom can form four single covalent bonds. These bonds allow carbon to form long chain-shaped molecules, called polymers, such as plastics.


The name of carbon comes from Latin carbo, meaning charcoal. In many foreign languages the words for carbon, coal and charcoal are synonyms.

Types of carbonEdit

Carbon in nature is found in three forms called allotropes: diamond, graphite, and fullerenes. Graphite, with clay, is in pencils. It is very soft. The carbon atoms in it make rings, which are on top of each other and slide very easily. Diamonds are the hardest natural mineral. Fullerenes are a "soccer ball" shape of carbon. They are mostly of interest to science. A special, man-made, tube-shaped allotrope of carbon is the carbon nanotube. Carbon nanotubes are very hard, so they might be used in armor. Nanotubes might be useful in nanotechnology. There are 10 million known carbon compounds.

Some forms of carbon: a) diamond; b) graphite; c) lonsdaleite; d-f) fullerenes (C60, C540, C70); g) amorphous carbon; h) carbon nanotube.

Radiocarbon datingEdit

A radioactive isotope of carbon, carbon-14, can be used to figure out how old some objects are or when something died. As long as something is on the surface of the earth and taking in carbon, the amount of carbon-14 stays the same. When an object stops taking in carbon, the carbon-14 amount goes down. Because the half-life (how long it takes for half of a radioactive isotope to go away) of carbon-14 is 5730 years,[16] scientists can see how old the object is by how much carbon-14 is left.

Where carbon isEdit

Carbon is in many places in the universe. It was first made in old stars. Carbon is the fourth most common element in the sun.[16] The atmospheres of Venus and Mars are mostly carbon dioxide.[17]

Carbon is important to the human body and other living things, and it is the second most common element in the human body, at 23% of all body weight.[16] It is also a key part of many biological molecules (molecules used in life).

Most of the carbon on Earth is coal. Graphite is in many (typically desert) areas, including Sri Lanka, Madagascar, and Russia. Diamonds are rare and are found largely in Africa. Carbon is also in some meteorites.

Related pagesEdit


  1. Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
  2. Haaland, D (1976). "Graphite-liquid-vapor triple point pressure and the density of liquid carbon". Carbon 14 (6): 357. doi:10.1016/0008-6223(76)90010-5. 
  3. Savvatimskiy, A (2005). "Measurements of the melting point of graphite and the properties of liquid carbon (a review for 1963–2003)". Carbon 43 (6): 1115. doi:10.1016/j.carbon.2004.12.027. 
  4. "Fourier Transform Spectroscopy of the Electronic Transition of the Jet-Cooled CCI Free Radical" (PDF). Retrieved 2007-12-06.
  5. "Fourier Transform Spectroscopy of the System of CP" (PDF). Retrieved 2007-12-06.
  6. "Carbon: Binary compounds". Retrieved 2007-12-06.
  7. 7.0 7.1 7.2 7.3 7.4 Properties of diamond, Ioffe Institute Database
  8. "Material Properties- Misc Materials". Retrieved 12 November 2016.
  9. Magnetic susceptibility of the elements and inorganic compounds, in Handbook of Chemistry and Physics 81st edition, CRC press.
  10. Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  11. "History of Carbon and Carbon Materials - Center for Applied Energy Research - University of Kentucky". Retrieved 2008-09-12.
  12. Senese, Fred (2000-09-09). "Who discovered carbon?". Frostburg State University. Retrieved 2007-11-24.
  13. "Fourier Transform Spectroscopy of the System of CP" (PDF). Retrieved 2007-12-06.
  14. "Fourier Transform Spectroscopy of the Electronic Transition of the Jet-Cooled CCI Free Radical" (PDF). Retrieved 2007-12-06.
  15. "Carbon: Binary compounds". Retrieved 2007-12-06.
  16. 16.0 16.1 16.2 Emsley, John (2001). Nature's Building blocks. Oxford University Press. ISBN 0-19-850341-5. Check |isbn= value: invalid character (help).
  17. University of Sheffield and Webelements Ltd. (2007). "Chemistry : Periodic Table : carbon : key information".

Other websitesEdit