Hydrocarbons are organic compounds with the general formula CₓHy. As a rule of thumb, many carbon atoms in a hydrocarbon molecule give higher boiling and melting points. For example, buthane C₄H₁₀ is a gas at room temperature whereas the compound octane C₈H₁₈ is a liquid. All of them are flammable and often used as fuels in various applications. For example buthane is found in LPG, liquefied petroleum gas and octane is the major hydrocarbon in gasoline. Hydrocarbons are also common for fabrication of plastics and as solvents. Hydrocarbons are divided into four main groups:
- Saturated, alkanes; only single bonds
- Unsaturated, alkenes or alkynes; double or triple bonds
- Aromatic, arenes; based upon benzene or other aromatic molecules
- Cyclic, cycloalkanes; ringformed hydrocarbons with no double bonds
Propane, C₃H₈, is a typical alkane with three carbon atoms. Ethene, C₂H₄, is the smallest alkene, with one C=C double bond.
Next is two variants of drawings of the most typical arene benzene, C₆H₆. The example to the right is more common, showing that all electrons are equally shared between six carbon atoms in a flat ring.
Lewis structure may become cumbersome and hard to read in the case of more complex molecule structures. As a response to this simplifications (such as the simplified depiction) has been developed. These are based on the fact that carbon always take four bonds (and hydrogen only takes one bound) and thus forming the rings seen in the example above.
Regardless of the molecule formula or exact composition of a hydrocarbon mixture, the hydrocarbons have a peak at 3.4 µm. The C-C stretchings from alkane chains absorb in weak broad bands between 7.7 – 12.5 µm. Besides, there are strong peaks from --CH₃ or --CH₂ groups at 6.7 – 7.7 µm due to C-H bending. Typical alkane peaks for hexane are shown in graph above.
A double bond in an alkene gives C=C stretching at 6.1 µm. A sharp vibration band near 6.7 µm indicates presence of a benzene ring in an arene.
Ethene (C₂H₄), formerly called ethylene, has a typical C=C double bond in a flat molecule.
C₂H₄ is a colorless gas with a slightly sweet smell. The vapor can cause tiredness or dizzyness and gives a high risk for suffocation. Ethene is very flammable and could easily be ignited by sparks. Ethene is well-known for its ability to stimulate ripening of fruits. In nature the gas is produced during plant metabolism and it's classified as a plant hormone. Also it's used for producing plastics such polyethene (polyethylene) and polyvinyl chloride (PVC).
IR of spectrum ethene C₂H₄
The IR spectrum of ethene is rather uncomplicated due to its simple structure. It has a strong band at 11 µm due to H-C-H out- off-plane wagging. Also, ethene has relatively weak absorption peaks at 7.1 µm from H-C-H scissoring and 3.2 µm from C-H assymetric stretching. Note that the C=C double bond in the C₂H₄ molecule cannot absorb IR radiation, because it has a totally symmetric vibration. Such a bond is called IR inactive.
Liquified petroleum gas (LPG)
Liquified petroleum gas (LPG) is a mixture of hydrocarbons mostly propane and butane, with formulae C₃H₈ and C₄H₁₀, respectively. In large concentrations LPG may cause asphyxiation. Examples of LPG are propane, n-butane and isobutane.
In addition to any LPG mixture there is always an odorant so that a leakage can be discovered. Often the odorant is a terribly smelling thiol, an organic molecule with a --SH group which has a very low threshold for human detection (on the level of ppb, parts per billion). Liquified petroleum gas is extremely flammable and thus suitable for burners, heating appliances, and vehicles. Also, it is used as aerosol propellants and as refigrerants instead of freons.
Methane (CH₄), the smallest hydrocarbon, is an uncolored and non-smelling gas. It has a symmetrical non-polar structure, where the carbon atom is surrounded by four hydrogen atoms in a perfectly tetrahedral arrangement.
CH₄ is regarded as non-toxic for humans but may displace oxygen in a closed space and cause a risk for suffocation. CH₄ is extremely flammable and may form explosive mixtures with air.
Normally the gas is formed in swamps or other oxygen-poor environments such as soil, manure or sewage plants. Other major methane sources are mining, processing and use of coal, oil and natural gas. The IR spectrum of methane is less complicated than spectra from larger hydrocarbons because it has a simpler structure.
Unfortunately, methane is a powerful greenhouse gas. Methane emissions are expressed in carbon dioxide equivalents using its global warming potential (GWP). Then one kg CH₄ is more than 20 times as effective at trapping heat in the earth´s atmosphere as one kg of CO₂, within a time horizon of 100 years.
IR spectrum of methane CH₄
In the IR spectrum of methane there are two strong absorption bands consisting of many overlapping peaks. They are found at 3.3 µm and 7.7 µm due to C-H stretching and bending modes, respectively.