CARBON COMPOUND

CARBON COMPOUND

CHEMISTRY OF CARBON COMPOUNDS
The chemistry of carbon is subjugated by three features.

1. Carbon forms extraordinarily strong carbon-carbon (C-C) single bonds, carbon-carbon (C=C) double bonds, and carbon-carbon triple bonds.

2. The electronegativity of carbon (EN) = 2.55 is very small to permit carbon to form C4- ions with the largest part of metals and very large for carbon to form C4+ ions when it reacts with nonmetals. Carbon as a result forms covalent bonds with countless other elements.

3. Carbon forms strong double and triple bonds with many other nonmetals, which includes N, O, P, and S.

Chemistry of Carbon
Organic chemistry involves structures and reactions of mostly carbon and hydrogen. Inorganic chemistry involves every other pure element apart from carbon. The inorganic chemistry of carbon is as well known as inorganic carbon chemistry. It is the chemistry of carbon that does not fall into the category of the organic chemistry sector.

Inorganic Chemistry of Carbon
Inorganic carbon chemistry is carbon that is extracted from ores and minerals, in opposition to organic carbon originate in nature through plants and living things. A few instances of inorganic carbon are carbon oxides like carbon monoxide and carbon dioxide; polyatomic ions, cyanide, cyanate, thiocyanate, carbonate and carbide in carbon. Carbon is an element that is exceptional in itself. Carbon forms strong single, double and triple bonds and for that reason it normally requires extra energy to break these bonds than when carbon is bonded to another element.

For carbon monoxide the reaction is denoted with the equation below:

2C(s) + O2 → 2CO(g) Enthalpy of -110.52 kJ/mol CO

C(s) + O2 → CO2(g) Enthalpy of -393.51 kJ/mol CO2

CO and CO2 are together gases. CO has no smell or taste and can be deadly to living organisms if in contact at even extremely small amounts of one thousandth of a gram. This is due to the fact that CO will react with the hemoglobin that carries oxygen in the blood. CO2 is not deadly except the living organisms are exposed to bigger amounts of it, in relation to 15%. CO2 manipulates the atmosphere and also the temperature via the effect of the greenhouse gas. While heat is caged in the atmosphere by CO2 gases, the temperature of the Earth's increases. The main supply for CO2 in our atmosphere, in the midst of scores of them is volcanoes.

Allotropes of carbon
Examples of the inorganic chemistry of carbon allotropes are diamond, graphite and fullerenes.

• Inorganic carbon may exist in the form of diamond. Diamond is crystal clear, isotropic crystal. It is the hardest naturally existing substance on earth. Diamond has four valence electrons, and when each one of the electrons forms bonds with another carbon it forms a sp3-hybridized atom. The boiling point of diamond is 4827°C.

• Unlike diamond, graphite is opaque, spongy, dull and hexagonal. Graphite can act as a conductor (electrodes) or merely as pencils. Graphite is made up of planes of sp2 hybridized carbon atoms in which each carbon is linked to the other three carbons.

• Fullerenes are carbon cages that are denoted with the formula C2n where n > 13. The most available fullerene is the sperical C60. Fullerene might have atoms or molecules within the cage (endohedral fullerenes) or covalently linked outside (exhoedral or adduct fullerenes).

Formulas of Inorganic and Organic Compounds
A chemical formula is an arrangement utilized to convey the structure of atoms. The formula shows which elements and the number of every element that are available in a compound. Formulas are written with the help of the elemental symbol of every atom and a subscript to signify the number of elements.

The most widespread elements available in organic compounds are carbon, hydrogen, oxygen, and nitrogen. With carbon and hydrogen available, other elements, like phosphorous, sulfur, silicon, and the halogens, might be present in organic compounds. Compounds that do not follow this regulation are called inorganic compounds.

Chemical Formulas
Chemical formulas can be further sub divided into empirical formula, molecular formula, and structural formula. Structural formular can be written complete or in its condensed form. Chemical symbols of elements in the chemical formula stand for the elements available and subscript numbers correspond to mole proportions of the scheduled elements.

H H | | H-C-C-O-H | | H H
Structural formular of CH3CH3OH

C6H12

A structural formula showcases the way the atoms in a molecule or ion are bonded. For instance, ethanol can be represented by CH3CH2OH. This is a condensed or simple way to illustrate the complicated structure above.

Molecular Geometry and Structural Formula
The knowledge of the way atoms in molecules are arranged and the way they are bonded together is extremely essential in providing the molecule with an identity. Isomers are compounds with the same number of atoms, and thus the same molecular formula, but which have entirely different physical and chemical properties due to the differences in their structural formula.

Molecular Formula
The molecular formula is derived from the authentic makeup of the compound. Even though the molecular formula can occasionally be same with the empirical formula, molecular compounds have the tendency to be more useful. Nevertheless, they do not illustrate the way the atoms are put together. Molecular compounds are as well deceptive when handling with isomers, which possess identical number and types of atoms.

Example-The Molecular Formula of Ethanol is C2H6O.

Empirical Formula
The empirical formula formular of a compound shows the simplest formular of the compound. Empirical formulas exhibit the number of atoms of every element in a compound in the most simplified form with the help of integers or whole numbers. Empirical formulas have the tendency to show a little consigning a compound as it is not possible to know the structure, shape, or properties of a compound without the knowledge of its molecular formula. The worth or value of the empirical formula is less due to the fact that a lot of chemical compounds can posses the same empirical formula.

Example-To find the empirical formula of C8H16O2.

To get the answer, you divide each and every one of the subscript by 2 to get the smallest ratio of whole numbers.

Structural Formula
A structural formula showcases the atoms in a molecule in the order they are bonded. It also depicts the way the atoms are bonded to one another just like in single, double, and triple covalent bond. Covalent bonds are illustrated with the help of lines. The numbers of dashes illustrates if the bond is a single, double, or triple covalent bond. Structural formulas are of a great help due to the fact that they give details about the properties and structure of the compound which empirical and molecular formulas cannot constantly showcase.

Condensed Structural Formula
Condensed structural formulas illustrate the order of atoms as you would obtain in a structural formula other than they are written just in a single line to economize space and make it additionally suitable and quicker to write. Condensed structural formulas are as well useful when illustrating that a group of atoms is associated with one atom in a compound. When this occurs, parenthesis is utilized just about the group of atoms to illustrate that they are together.

Example of Condensed Structural Formula-The condensed structural formula of Ethanol: CH3CH2OH (Molecular Formula for Ethanol C2H6O).

A homologous series
The homologous series of compounds with comparable general formula regularly vary by one parameter like the length of a carbon chain. Examples of a homologous series are the straight-chained alkanes (paraffins), the akenes with double bonds and alkynes with triple bonds and some of their derivatives like the primary alcohols, aldehydes, and mono carboxylic acids. Another homologous series is the single-ring un-branched cycloalkanes.

Elemental Forms of Carbon: Graphite, Diamond, Coke, and Carbon Black

Carbon exists as a diversity of allotropes. The various allotropes of carbon are two crystalline forms- diamond and graphite and a lot of amorphous or non crystalline forms, like charcoal, coke, and carbon black.

The properties of diamond are a reasonable significance of its structure. In a diamond Carbon, with its four valence electrons, forms covalent bonds to four adjoining carbon atoms prearranged near the corners of a tetrahedron, every one of the sp3-hybridized atoms are then bonded to 4 other carbon atoms, which in turn form bonds to 4 other carbon atoms, and the bond continues in like manner. Owing to this, an ideal diamond can be considered of as one giant molecule. The might of each individual C-C bonds and their organization in space results to the abnormal properties of diamond.

In a number of ways, the properties of graphite are similar to those of diamond. Both diamond and graphite boil at 4827oC, for instance. But graphite is as well extremely dissimilar to diamond. Diamond with the density of (3.514 g/cm3) is denser than graphite with the density of 2.26 g/cm3. While diamond is the hardest known substance, graphite is one of the softest substances available. Diamond is an brilliant insulator, with minimal or zero inclination to allow the passage of electric current through it. Graphite is an excellent conductor of electricity and as a result, electrodes made with graphite are made use of in the construction of electrical cells.

The physical properties of graphite can be implicit from the structure of the solid.

Graphite is composed of extended planes of sp2-hybridized carbon atoms with every one of the carbon atom firmly bound to three other carbon atoms.

The reason for the high melting point it possesses is due to the strong bonds linking carbon atoms within every plane. The distance flanked between these planes of atoms, nevertheless, is very much bigger than the distance between the atoms inside the planes. Since the bonds between planes are weak, it is very simple to distort the solid by permitting one plane of atoms to shift in relation to the other. Owing to this, graphite is very soft and is being used in pencil and as a form of lubricant in motor oil.

"Lead" pencils do not, by the way, contain lead which is very good due to the fact that a lot of people chew up pencils and lead compounds are poisonous. Lead pencils are made with graphite or "black lead as it was formally called with a mixture of clay 20% to 60% by weight and subsequently baked to form a ceramic rod. An increase in the percentage of clay makes the pencil harder, so that smaller amount of graphite is place on the paper.