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Oxidation & Electrons | Appearance & Characteristics Reactions | Compounds | Radius | Conductivity Abundance & Isotopes | References | Cite this Page 
Models of carbon nanotube structure. |
General:
| Name: Carbon | Symbol: C |
| Type: Non-Metal, Carbon group | Atomic weight: 12.011 |
| Density @ 293 K: 2.267 g/cm3 (graphite), 3.513 g/cm3 (diamond) | Atomic volume: 5.31 cm3/mol (graphite), 3.42 cm3/mol (diamond) |
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Discovered: Carbon has been known since ancient times in the form of soot, charcoal, graphite and diamonds.
Ancient cultures did not of course realize that these substances were different forms of the same element.
'Carbon' is derived from the Latin carbo, meaning charcoal.
Antoine Lavoisier named carbon and he carried out early experiments to reveal its nature. In 1694 he pooled resources with other chemists to buy a diamond, which they placed in a closed glass jar. They focused the sun's rays on the diamond with a magnifying glass and the diamond burnt and disappeared. Lavoisier noted that the overall weight of the jar was unchanged. He concluded the diamond was composed of the same element as charcoal was - carbon. When it burnt, the diamond had combined with oxygen to form carbon dioxide. (1), (2) In 1779 Carl Scheele showed that graphite burnt to form carbon dioxide and so must be a form of carbon.(3) In 1796 Smithson Tennant established that diamond was pure carbon and not a compound of carbon and it burnt to form only carbon dioxide. Tennant also proved that when equal weights of charcoal and diamonds were burnt, they produced the same amount of carbon dioxide. (4) In 1855 Benjamin Brodie produced pure graphite from carbon in his laboratory, proving it was a form of carbon.(4) Although it had been previously attempted, in 1955 Francis Bundy and coworkers at General Electric finally demonstrated that graphite could be transformed to diamond at high temperature and high pressure.(5) In 1985 Robert Curl, Harry Kroto and Richard Smalley discovered fullerenes, a new form of carbon in which the atoms are arranged in soccer-ball shapes.(6), (7) |
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States
| State (s, l, g): solid | |
| Melting point: 3823 K (3550 oC) | Boiling point: 4300 K (4027 oC) |
| Note: At normal pressures, carbon does not melt when heated, it sublimes - i.e. when heated, carbon undergoes a phase change directly from solid to gas, much like dry ice (solid carbon dioxide) does. The melting point quoted above is under a pressure of 10 atmospheres. | |
Energies
| Specific heat capacity: 0.71 J g-1 K-1 (graphite), 0.5091 J g-1 K-1 (diamond) | Heat of atomization: 717 kJ mol-1 |
| Heat of fusion: 117 kJ mol-1 (graphite) | Heat of vaporization: 710.9 kJ mol-1 |
| 1st ionization energy: 1086.5 kJ mol-1 | 2nd ionization energy: 2352.6 kJ mol-1 |
| 3rd ionization energy: 4620.5 kJ mol-1 | Electron affinity: 121.55 kJ mol-1 |
Oxidation & Electrons
| Shells: 2,4 | Electron configuration: [He] 2s2 2p2 |
| Minimum oxidation number: -4 | Maximum oxidation number: 4 |
| Min. common oxidation no.: -4 | Max. common oxidation no.: 4 |
| Electronegativity (Pauling Scale): 2.55 | Polarizability volume: 1.8 Å3 |
Appearance & Characteristics
| Structure: hexagonal layers (graphite), tetrahedral (diamond) | Color: black (graphite), transparent (diamond) |
| Hardness: 0.5 mohs (graphite), 10.0 mohs (diamond) |
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Right: Diamonds (crystalline carbon). We thought about taking a picture of combusting diamonds - they combust at about 800 oC - but we couldn't afford it! 
Carbon based lifeforms, such as these, dominate our planet. 
DNA. The famous double-helix molecule is made possible by carbon's ability to form long molecular chains. 
Nasa: Carbon nanotubes have outstanding tensile strength - two orders of magnitude higher than graphite fibers, kevlar or steel. |
Harmful effects:
Pure carbon has very low toxicity. Inhalation of large quantities of carbon black dust (soot/coal dust) can cause irritation and damage to the lungs. Characteristics: Carbon can exist in several allotropes, including graphite, diamond, amorphous carbon, fullerines and nanotubes. (The structures of eight allotropes are shown at the bottom of this page.) Interestingly, graphite is one of the softest substances and diamond was thought, until recently, to be the hardest naturally occurring substance. An extremely rare allotrope of carbon, Lonsdaleite, has been calculated, in pure form, to be 58% stronger than diamond. Lonsdaleite is made when meteorites containing graphite hit another body, such as Earth. The high temperatures and pressures of the impact transform the graphite into Lonsdaleite, a diamond-like substance that retains graphite's hexagonal structure. Carbon has the highest melting/sublimation point of all the elements and, in the form of diamond, has the highest thermal conductivity of any element. This is the origin of the slang term "ice" - diamond, at room temperature, carries heat away from your warmer skin faster than any other material and so feels cold to touch. Uses: Carbon (coal) is used as a fuel. Graphite is used as a lubricant, for pencil tips, high temperature crucibles, dry cells and electrodes. Diamonds are used in jewelry and - because they are so hard - in industry for cutting, drilling, grinding, and polishing. Carbon black is used as the black pigment in printing ink. Carbon can form alloys with iron, of which the most common is carbon steel. The 14C radioactive isotope is used in archaeological dating. Carbon compounds are important in many areas of the chemical industry. Carbon forms a vast number of compounds with hydrogen, oxygen, nitrogen and other elements. Its ability to form long-chained, complex compounds has resulted in carbon acting as the basis of all life on Earth. The outstanding physical properties - for example thermal conductivity and strength - of new carbon allotropes, such as nanotubes, show enormous potential for future development. |
Reactions
| Reaction with air: vigorous, ⇒ CO2 | Reaction with 6 M HCl: none |
| Reaction with 15 M HNO3: mild, w/ht ⇒ C6(CO2H)6 (mellitic/graphitic acid) | Reaction with 6 M NaOH: none |
Compounds
| Oxide(s): CO , CO2 | Chloride(s): CCl4 |
| Hydride(s): CH4 and many CxHy |
Radius
| Atomic radius: 70 pm | Ionic radius (1+ ion): pm |
| Ionic radius (2+ ion): pm | Ionic radius (3+ ion): pm |
| Ionic radius (2- ion): pm | Ionic radius (1- ion): pm |
Conductivity
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Thermal conductivity: 25-470 W m-1 K-1 (graphite)
470 W m-1 K-1 (diamond) |
Electrical conductivity: 0.07 x 106 S cm-1 |
Abundance & Isotopes
| Abundance earth's crust: 200 parts per million by weight, 344 parts per million by moles | |
| Abundance solar system: 3,000 parts per million by weight, 300 parts per million by moles | |
| Cost, pure: $2.4 per 100g | |
| Cost, bulk: $ per 100g | |
| Source: Carbon can be obtained by burning organic compounds with insufficient oxygen. The four main allotropes of carbon are graphite, diamond, amorphous carbon and fullerines. Natural diamonds are found in kimberlite from ancient volcanoes. Graphite can also be found in natural deposits. Fullerenes were discovered as byproducts of molecular beam experiments in the 1980's. Amorphous carbon is the main constituent of charcoal, soot (carbon black), and activated carbon. | |
| Isotopes: 13 whose half-lives are known, with mass numbers 8 to 20. Of these, two are stable, 12C and 13C. Isotope 14C, with a half-life of 5730 years, is widely used to date carbonaceous materials such as wood, archeological specimens, etc for ages up to about 40,000 years. | |
References
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1. Robert E. Krebs, The history and use of our earth's chemical elements: a reference guide., (2006) p192. Greenwood Publishing Group
2. John Emsley, Nature's building blocks: an A-Z guide to the elements., (2002) p95. Oxford University Press. 3. Jessica Elzea Kogel, Industrial minerals & rocks: commodities, markets, and uses., (2006) p507. SME. 4. Amanda S. Barnard, The diamond formula: diamond synthesis--a gemmological perspective., (2000) p3. Butterworth-Heinemann 5. Robert M. Hazen, The diamond makers., (1999) p145. Cambridge University Press. 6. Jonathan W. Steed, Jerry L. Atwood, Supramolecular Chemistry., (2009) p423. Wiley. 7. Nobel Prize for Chemistry, 1996 |
Cite this Page
For online linking, please copy and paste one of the following:
<a href="http://www.chemicool.com/elements/carbon.html">Carbon</a>or <a href="http://www.chemicool.com/elements/carbon.html">Carbon Element Facts</a>To cite this page in an academic document, please use the following MLA compliant citation: "Carbon." Chemicool Periodic Table. <http://www.chemicool.com/elements/carbon.html>. |
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A wonderful image released by Michael Ströck under the GNU Free Documentation License: The structures of eight allotropes of carbon:
a) Diamond b) Graphite c) Lonsdaleite d) C60 (Buckminsterfullerene) e) C540 Fullerene f) C70 Fullerene g) Amorphous carbon h) Single-walled carbon nanotube |
