Carbon has 2 electrons in its first shell and 4 in its second shell.Check me out: http://www.chemistnate.com. On a weight basis, carbon is 19th in order of elemental abundance in Earth’s crust, and there are estimated to be 3.5 times as many carbon atoms as silicon atoms in the universe. Only hydrogen, helium, oxygen, neon, and nitrogen are atomically more abundant in the cosmos than carbon. For example, an atom of carbon is absorbed from the air into the ocean water where it is used by little floating plankton doing photosynthesis to get the nutrition they need. There is the possibility that this little carbon atom becomes part of the plankton’s skeleton, or a part of the skeleton of the larger animal that eats it, and then part.

1. Carbon Chemical Series
2. Carbon Atomic Symbol
3. Carbon Atomic Number
4. Carbon Atomic Mass

The nomenclature is a very important part of organic chemistry. The names are not given only to compounds but also to the carbon atoms that make up this compound.

Thus, we can classify carbon atoms as primary, secondary, tertiary, or quaternary. These terms refer to the substitution level that a given carbon has in a molecule. In other words, these terms are used to describe how many other carbons a given carbon is attached to. This classification applies only to saturated carbons.

• Primary (1°) carbon atom – bonded to one other carbon atom,
• Secondary (2°) carbon atom – bonded to two other carbon atoms,
• Tertiary (3°) carbon atom – bonded to three other carbon atoms,
• Quaternary (4°) carbon atom – bonded to four other carbon atoms.

This can be explained by one of the important properties of carbon and is its tetravalency. Carbon is a strict octet follower, which means it needs a maximum of 8 electrons to form stable compounds. Since a carbon atom has 4 valence electrons, it can form up to 4 bonds with different elements. Part of the reason why there are millions of compounds of carbon is its ability to form a very stable bond with another carbon atom.

The same terminology is used for carbocations. A primary carbocation is attached to one other carbon, a secondary to two, and a tertiary to three. A quaternary carbocation does not exist without violating the octet rule.

For example, you get the following compound to determine which primary, secondary, tertiary, or quaternary carbons are. As mentioned above, a primary is attached to one carbon atom, a secondary to two, a tertiary to three, and a quaternary to four other carbon atoms. For each carbon atom, you need to count how many carbon atoms next to it that particular carbon atom is connected to.

There is another rule:

1. Primary carbon atoms are always at the end;
2. Secondary carbon atoms are in the middle (between two other carbon atoms);
3. Tertiary carbon atoms are branched out in three different ways;
4. Quaternary carbon atoms have the most carbon atoms around (max 4).

OK. These are carbon atoms. But what about the hydrogen atoms which are bonded to these carbon atoms? Yes, they can also be primary, secondary, and tertiary. It depends on the carbon atoms they are attached to. So follow the next rule for hydrogens:

1. Primary hydrogen atoms are attached to primary carbon atoms;
2. Secondary hydrogen atoms are attached to secondary carbon atoms;
3. Tertiary hydrogen atoms are attached to tertiary carbon atoms.

In our example, we have a total of 18 primary hydrogens. Because each primary carbon has 3 hydrogen atoms, and we have 6. Secondary hydrogen atoms have a total of 4 (2 hydrogens per secondary carbon atom), and tertiary 2 (1 hydrogen per tertiary carbon atom).
Let’s go back to the carbons. Let’s look at what are called carbons that are bonded to other atoms and atomic groups such as halides, hydroxides, amines.

Alkyl halides

It should also count here how much carbon atoms are attached to a particular carbon. Halides (fluorine, chlorine, bromine, or iodine) are not counted. Thus, the primary alkyl halide is one that has only one carbon atom bound to itself. The secondary has two carbon atoms and a halide, and the tertiary has three carbon atoms and a halide bonded to itself. The quaternary alkyl halides don’t exist because that would involve breaking the octet rule.

Alcohols

The rules apply the same way for alcohols as it does for alkyl halides. For the most groups like alcohols, alkyl halides, and hydrogen atoms to determine if it’s primary, secondary, or tertiary, look at the carbon atom that bears those atoms, ignore this atom or group and count how many carbons are attached to it.

Amines

Here is a slightly different story. Amines are named according to the number of carbons attached to nitrogen. Primary, secondary, and tertiary amines are nitrogens bound to one, two and three carbons, respectively. They also form quaternary amines, since the nitrogen has a lone pair and it possible to form another bond to carbon. They bear a positive charge on nitrogen and are not at all basic. They are often referred to as quaternary ammonium salts.

Numbers of carbon atoms attached to carbon atoms also govern how they will react.

For carbocations, that is cations if carbons, carbons with more carbons attached on (i.e. tertiary) tend to be less electron-deficient due to hyperconjugation from nearby C-H bonds. Therefore, tertiary carbocations are more stable compared to secondary, primary, and methyl, respectively.

Another case is that of alcohols. Primary alcohols can be oxidized to aldehydes and carboxylic acids (two levels). Secondary alcohols can go only one level of ketones, and tertiary alcohols cannot be oxidized at all.

The Element Carbon

Carbon is the chemical element in the periodic table that has the symbol C and atomic number 6. An abundant nonmetallic, tetravalent element, carbon has several allotropic forms:

• diamonds (hardest known mineral). Binding structure: 4 electrons in 3-dimensional so-called sp3-orbitals
• graphite (one of the softest substances). Binding structure: 3 electrons in 2-dimensional sp2-orbitals and 1 electron in s-orbitals.
• Covalent bound sp1 orbitals are of chemical interest only.

Fullerite (fullerenes) are nanometer-scale molecules. In the simple form 60 carbon atoms form a graphitic layer which is bent to a 3-dimensional structure, similar to a soccer ball.

Lamp black consists of small graphitic areas. These areas are randomly distributed, so the whole structure is isotropic.

So-called 'glassy carbon' is isotropic and as strong as glass. Unlike normal graphite, the graphitic layers are not arranged like pages in a book, but are crumpled like crumpled paper.

Carbon fibers are similar to glassy carbon. Under special treatment (stretching of organic fibers and carbonization) it is possible to arrange the carbon planes in direction of the fiber. Perpendicular to the fiber axis there is no orientation of the carbon planes. The result are fibers with a higher specific strength than steel.

The element carbon occurs in all organic life and is the basis of organic chemistry. This nonmetal also has the interesting chemical property of being able to bond with itself and a wide variety of other elements, forming nearly 10 million known compounds. When united with oxygen it forms carbon dioxide which is absolutely vital to plant growth. When united with hydrogen, it forms various compounds called hydrocarbons which are essential to industry in the form of fossil fuels. When combined with both oxygen and hydrogen it can form many groups of compounds including fatty acids, which are essential to life, and esters, which give flavor to many fruits. The isotope carbon-14 is commonly used in radioactive dating.

Notable characteristics

Carbon is a remarkable element for many reasons. Its different forms include one of the softest (graphite) and one of the hardest (diamond) substances known to man. Moreover, it has a great affinity for bonding with other small atoms, including other carbon atoms, and its small size makes it capable of forming multiple bonds. Because of these properties, carbon is known to form nearly ten million different compounds. Carbon compounds form the basis of all life on Earth and the carbon-nitrogen cycle provides some of the energy produced by the sun and other stars.

Carbon was not created in the big bang due to the fact that it needs a triple collision of alpha particles (helium nuclei) to be produced. The universe initially expanded and cooled too fast for that to be possible. It is produced, however, in the interior of stars in the horizontal branch, where stars transform a helium core into carbon by means of the triple-alpha process.

Applications

The element carbon is a vital component of all known living systems, and without it life as we know it could not exist (see carbon chauvinism). The major economic use of carbon is in the form of hydrocarbons, most notably the fossil fuels methane gas and crude oil. Crude oil is used by the petrochemical industry to produce, amongst others, petroleum, gasoline and kerosene, through a distillation process, in so-called refineries. Crude oil forms the raw material for many synthetic substances, many of which are collectively called plastics.

Other uses:

• The isotope ¹⁴C, discovered February 27th, 1940, is used in radiocarbon dating.
• Some smoke detectors use tiny amounts of a radioactive isotope of carbon as source of ionizing radiation (Most smoke detectors of this type use an isotope of Americium)
• Graphite is combined with clays to form the 'lead' used in pencils.
• Diamond is used for decorative purposes, and also as drill bits and other applications making use of its hardness.
• Carbon is added to iron to make steel.
• Carbon is used for control rods in nuclear reactors.
• Graphite carbon in a powdered, caked form is used as charcoal for cooking, artwork and other uses.
• Charcoal pills are used in medicine in pill or powder form to adsorb toxins or poisons from the digestive system.

The chemical and structural properties of fullerenes, in the form of carbon nanotubes, has promising potential uses in the nascent field of nanotechnology.

History

Carbon (Latin carbo meaning 'charcoal') was discovered in prehistory and was known to the ancients, who manufactured it by burning organic material in insufficient oxygen (making charcoal). Diamonds have long been considered rare and beautiful. The last-known allotrope of carbon, fullerenes, were discovered as byproducts of molecular beam experiments in the 1980's.

Allotropes

Four allotropes of carbon are known to exist: amorphous, graphite, diamond and fullerenes. The discovery of a fifth form was announced on March 22, 2004 [1] (http://www.nature.com/nsu/040322/040322-5.html).

In its amorphous form, carbon is essentially graphite but not held in a crystalline macrostructure. It is, rather, present as a powder which is the main constituent of substances such as charcoal and lamp black (soot).

At normal pressures carbon takes the form of graphite, in which each atom is bonded to three others in a plane composed of fused hexagonal rings, just like those in aromatic hydrocarbons. The two known forms of graphite, alpha (hexagonal) and beta (rhombohedral), both have identical physical properties, except for their crystal structure. Graphites that naturally occur have been found to contain up to 30% of the beta form, when synthetically-produced graphite only contains the alpha form. The alpha form can be converted to the beta form through mechanical treatment and the beta form reverts back to the alpha form when it is heated above 1000 °C.

Because of the delocalization of the pi-cloud, graphite conducts electricity. The material is soft and the sheets, frequently separated by other atoms, are held together only by van der Waals forces, so easily slip past one another.

At very high pressures carbon has an allotrope called diamond, in which each atom is bonded to four others. Diamond has the same cubic structure as silicon and germanium and, thanks to the strength of the carbon-carbon bonds, is together with the isoelectronic boron nitride (BN) the hardest substance in terms of resistance to scratching. The transition to graphite at room temperature is so slow as to be unnoticeable. Under some conditions, carbon crystallizes as Lonsdaleite, a form similar to diamond but hexagonal.

Fullerenes have a graphite-like structure, but instead of purely hexagonal packing, also contain pentagons (or possibly heptagons) of carbon atoms, which bend the sheet into spheres, ellipses or cylinders. The properties of fullerenes (also called 'buckyballs' and 'buckytubes') have not yet been fully analyzed. All the names of fullerenes are after Buckminster Fuller, developer of the geodesic dome, which mimics the structure of 'buckyballs'.

Occurrence

There are nearly ten million carbon compounds that are known to science and many thousands of these are vital to life processes and very economically important organic-based reactions. This element is abundant in the sun, stars, comets, and in the atmospheres of most planets. Some meteorites contain microscopic diamonds that were formed when the solar system was still a protoplanetary disk. In combination with other elements, carbon is found the earth's atmosphere and dissolved in all bodies of water. With smaller amounts of calcium, magnesium, and iron, it is a major component of very large masses carbonate rock (limestone, dolomite, marble etc.). When combined with hydrogen, carbon form coal, petroleum, and natural gas which are called hydrocarbons.

Graphite is found in large quantities in New York and Texas, the United States; Russia; Mexico; Greenland and India.

Natural diamonds occur in the mineral kimberlite found in ancient volcanic 'necks,' or 'pipes'. Most diamond deposits are in Africa, notably in South Africa, Namibia, Botswana, the Republic of the Congo and Sierra Leone. There are also deposits in Canada, the Russian Arctic, Brazil and in Northern and Western Australia.

Inorganic compounds

Carbon Chemical Series

The most prominent oxide of carbon is carbon dioxide, CO₂. This is a minor component of the Earth's atmosphere, produced and used by living things, and a common volatile elsewhere. In water it forms trace amounts of carbonic acid, H₂CO₃, but as most compounds with multiple single-bonded oxygens on a single carbon it is unstable. Through this intermediate, though, resonance-stabilized carbonate ions are produced. Some important minerals are carbonates, notably calcite. Carbon disulfide, CS₂, is similar.

The other oxides are carbon monoxide, CO, and the uncommon carbon suboxide, C₃O₂. Carbon monoxide is formed by incomplete combustion, and is a colorless, odorless gas. The molecules each contain a triple bond and are fairly polar, resulting in a tendency to bind permanently to hemoglobin molecules, so that the gas is highly poisonous. Cyanide, CN-, has a similar structure and behaves a lot like a halide ion; the nitride cyanogen, (CN)₂, is related.

With strong metals carbon forms either carbides, C^-, or acetylides, C₂^2-; these are associated with methane and acetylene, both incredibly pathetic acids. All in all, with an electronegativity of 2.5, carbon prefers to form covalent bonds. A few carbides are covalent lattices, like carborundum, SiC, which resembles diamond.

Carbon chains

It´s the atomic structure of hydrocarbons in which a series of carbon atoms, saturated by hydrogen atoms, form a chain. Volatile oils have shorter chains. Fats have longer chain lengths, and waxes have extremely long chains.

Carbon cycle

The continuous process of combining and releasing carbon and oxygen thereby storing and emitting heat and energy. Catabolism + anabolism = metabolism. See carbon cycle.

Isotopes

Carbon Atomic Symbol

In 1961 the International Union of Pure and Applied Chemistry adopted the isotope carbon-12 for basis for atomic weights.

• Carbon-14 is a radioisotope with a half-life of 5715 years and has been used extensively for radiocarbon dating wood, archaeological sites and specimens.

Carbon Atomic Number

Carbon has two stable, naturally-occurring isotopes: C-12 (98.89%) and C-13 (1.11%). Ratios of these isotopes are reported in ? relative to the standard VPDB (Vienna Pee Dee Belemnite from the Peedee Formation of South Carolina). The dC-13 of the atmosphere is -7?. During photosynthesis, the carbon that becomes fixed in plant tissue is significantly depleted in C-13 relative to the atmosphere.

There is two mode distribution in the dC-13 values of terrestrial plants resulting from differences in the photosynthetic reaction used by the plant. Most terrestrial plants are C3 pathway plants and have dC-13 values range from -24 to -34?. A second category of plants (C4 pathway plants), composed of aquatic plants, desert plants, salt marsh plants, and tropical grasses, have dC-13 values that range from -6 to -19. An intermediate group (CAM plants) composed of algae and lichens has dC-13 values range from -12 to -23?. The dC-13 of plants and organisms can provide useful information about sources of nutrients and food web relations.

Carbon Atomic Mass

Precautions

Compounds of carbon have a wide range of toxic action. Carbon monoxide (CO), which is present in the exhaust of combustion engines, and cyanide (CN^-), which is sometimes in mining pollution, are extremely toxic to mammals. Many other carbon compounds are not toxic and are in fact absolutely essential for life. Organic gases such as ethene (CH₂=CH₂), ethyne (HCCH), and methane (CH₄) are dangerously explosive and flammable when mixed with air.

External links

• WebElements.com – Carbon(http://www.webelements.com/webelements/elements/text/C/index.html)
• EnvironmentalChemistry.com – Carbon(http://environmentalchemistry.com/yogi/periodic/C.html)
• It's Elemental – Carbon(http://education.jlab.org/itselemental/ele006.html)
• – Carbon Fullerene and other Allotropes(http://www.vincentherr.com/cf/) models by Vincent Herr
• Carbon Module -- Edinformatics.com (http://www.edinformatics.com/math_science/c_module.htm)
  Los Alamos National Laboratory – Carbon(http://periodic.lanl.gov/elements/6.html)