Hydrocarbons

HydrocarbonsFrom Indonesian Wikipedia, the free encyclopediaPending changes shown on page iniBelum CheckedJump to: navigation, searchModel replica of the molecule methane, CH4. Methane is one example of the hydrocarbons in the category of an alkane, have only one kind of bond only.
In chemistry, a hydrocarbon is a compound composed of the elements carbon (C) and hydrogen atoms (H). The entire chain hydrocarbons having carbon and hydrogen atoms bonded to the chain. The term is used also as a sense of aliphatic hydrocarbons.
For example, methane (swamp gas) is a hydrocarbon with one carbon atom and four hydrogen atoms: CH4. Ethane is a hydrocarbon (more specifically, an alkane) consisting of two carbon atoms are united by a single bond, each of which binds to three carbon atoms: C2H6. Propane has three C atoms (C3H8) and beyond (CnH2 · n +2).
Types of hydrocarbons
Classification of hydrocarbons, which are grouped by organic nomenclature is:

    Hydrocarbon saturated / saturated (alkanes) are the simplest hydrocarbon. Hydrocarbons is composed entirely of a single bond and bound with hydrogen. The general formula for saturated hydrocarbons is CnH2n +2. [1] is the main composition of saturated hydrocarbons in fossil fuels and is found in the form of straight or branched chain. Hydrocarbons with the same molecular formula but different structural formulas called structural isomers. [2]
    Unsaturated hydrocarbons / is not saturated hydrocarbons which have one or more double bonds, either duplicate or triplicate. Hydrocarbons having double bonds called alkenes, with the general formula CnH2n. [3] hydrocarbons that have a triple bond are called alkynes, with general formula CnH2n-2. [4]
    Cycloalkanes are hydrocarbons containing one or more carbon rings. The general formula for saturated hydrocarbons is CnH2n ring with 1. [2]
    Aromatic hydrocarbons, also known as the arena, are hydrocarbons that have at least one aromatic ring.
Gaseous hydrocarbon (eg methane and propane), liquids (eg hexane and benzene), waxes or solids with a low boiling point (eg paraffin wax and naphthalene) or polymers (eg, polyethylene, polypropylene and polystyrene).Common traits
Because of its molecular structure is different, then the empirical formula of the hydrocarbon was also different: the amount of hydrocarbon bound to alkenes and alkynes definitely less because carbon atoms bonded duplicate.
The ability of hydrocarbons to bond with itself called katenasi, and cause hydrocarbons can form compounds that are more complex, such as cyclohexane or benzene arena. This ability is obtained due to the characteristics of the bonds between carbon atoms are non-polar.
In accordance with the valence bond theory, the carbon atom must satisfy the rule "4-hydrogen" which states the maximum number of atoms that can be bonded to the carbon, because carbon has four valence electrons. Judging from the valence electrons, the carbon has four electrons that can form covalent bonds or dative bonds.
Hydrocarbons are hydrophobic and are included in the lipid.
Some hydrocarbons are available in abundance in the solar system. Lakes containing liquid methane and ethane have been found on Titan, the largest natural satellite of Saturn, as stated by the Cassini-Huygens mission. [5]
Simple hydrocarbons and its variationsNumber of atomsCarbon Alkanes (1 bonds) alkenes (2 ties) alkyne (3 ties) Cycloalkanes Alkadiena1 Methane Metena Metuna -2 Ethane Ethene (ethylene) ethyne (acetylene) -3 Propane propene (propylene) Propuna (metilasetilena) Cyclopropane Propadiena (alena)4 Butane Butene (butylene) Butuna Siklobutana ButadienePentane 5 Pentena Pentuna Pentadiena cyclopentane (piperylene)6 Hexane Cyclohexane hexene Heksuna Heksadiena7 heptane Heptena Heptuna Sikloheptana Heptadiena8 octane octene Oktuna Siklooktana Oktadiena9 Nonana Nonena Nonuna Siklononana Nonadiena10 decane Dekena Dekuna Siklodekana DekadienaUse
Hydrocarbons are one of the most important sources of energy on earth. The main use is as a fuel source. In solid form, hydrocarbons are one forming composition asphalt. [6]
Hydrocarbons had also been used for the manufacture of chlorofluorocarbons, a substance used as a propellant in spray mosquito. Currently chlorofluorocarbons are no longer used because it has a bad effect on the ozone layer.
Methane and ethane are gases at room temperature and is not easily liquefied by pressure away. Propane is easier to be melted, and are usually sold in tubes in liquid form. Butane is very easily melted, making it safer and is often used for cigarette lighters. Pentane clear liquid at room temperature, typically used in industry as a solvent for waxes and greases. Hexane is also used as chemical solvents and are included in the composition of gasoline.
Hexane, heptane, octane, nonana, decane, including some with alkenes and cycloalkanes is an important component in gasoline, naphtha, jet fuel, and industrial solvents. With increasing carbon atoms, the hydrocarbon in the form of linear viscosity properties and will have a higher boiling point, with a darker color.
Burning hydrocarbonsCurrently, hydrocarbons are energy sources of electricity and thermal energy in the world because it produces when burned. [7] hydrocarbon energy is usually often used directly for heating in homes, in the form of oil and natural gas. Hydrocarbons were burnt and the heat is used to evaporate water, which later spread to the rest of the steam room. A similar principle is used in power plants.
General characteristics of the hydrocarbons are generating vapor, carbon dioxide, and heat during combustion, and the oxygen necessary for combustion reactions can take place. Here is an example of the methane combustion reaction:

    CH4 + 2 O2 → 2 CO2 + H2O + Energy
If poor air oxygen gas, it will form carbon monoxide (CO) and water:

    2 CH4 + 3 O2 → 2CO + 4H2O
Another example, propane combustion reaction:

    C3H8 + 5 O2 → 4 CO2 + H2O + 3 Energy

    CnH2n +2 ​​+ (3n +1) / 2 O2 → (n +1) n CO2 + H2O + Energy