What is the molecular formula for carbon and hydrogen?

Covalent chemical bond between hydrogen and carbon atoms

In chemistry, the carbon-hydrogen bond (C−H bond) is a chemical bond between carbon and hydrogen atoms that can be found in many organic compounds.[1] This bond is a covalent, single bond, meaning that carbon shares its outer valence electrons with up to four hydrogens. This completes both of their outer shells, making them stable.[2]

Carbon–hydrogen bonds have a bond length of about 1.09 Å (1.09 × 10−10 m) and a bond energy of about 413 kJ/mol (see table below). Using Pauling's scale—C (2.55) and H (2.2)—the electronegativity difference between these two atoms is 0.35. Because of this small difference in electronegativities, the C−H bond is generally regarded as being non-polar. In structural formulas of molecules, the hydrogen atoms are often omitted. Compound classes consisting solely of C−H bonds and C−C bonds are alkanes, alkenes, alkynes, and aromatic hydrocarbons. Collectively they are known as hydrocarbons.

In October 2016, astronomers reported that the very basic chemical ingredients of life—the carbon-hydrogen molecule (CH, or methylidyne radical), the carbon-hydrogen positive ion (CH+) and the carbon ion (C+)—are the result, in large part, of ultraviolet light from stars, rather than in other ways, such as the result of turbulent events related to supernovae and young stars, as thought earlier.[3]

Bond length

The length of the carbon-hydrogen bond varies slightly with the hybridisation of the carbon atom. A bond between a hydrogen atom and an sp2 hybridised carbon atom is about 0.6% shorter than between hydrogen and sp3 hybridised carbon. A bond between hydrogen and sp hybridised carbon is shorter still, about 3% shorter than sp3 C-H. This trend is illustrated by the molecular geometry of ethane, ethylene and acetylene.

Molecule	Ethane	Ethylene	Acetylene
Formula	C2H6	C2H4	C2H2
Class	alkane	alkene	alkyne
Structure
Hybridisation of carbon	sp3	sp2	sp
C-H bond length	1.094 Å	1.087 Å	1.060 Å
Proportion of ethane C-H bond length	100%	99%	97%
Structure determination method	microwave spectroscopy	microwave spectroscopy	infrared spectroscopy

Reactions

Main article: Carbon–hydrogen bond activation

The C−H bond in general is very strong, so it is relatively unreactive. In several compound classes, collectively called carbon acids, the C−H bond can be sufficiently acidic for proton removal. Unactivated C−H bonds are found in alkanes and are not adjacent to a heteroatom (O, N, Si, etc.). Such bonds usually only participate in radical substitution. Many enzymes are known, however, to affect these reactions.[5]

Although the C−H bond is one of the strongest, it varies over 30% in magnitude for fairly stable organic compounds, even in the absence of heteroatoms.[6][7]

See also

• Carbon–carbon bond
• Carbon–nitrogen bond
• Carbon–oxygen bond
• Carbon–fluorine bond

References

1. ^ March, Jerry (1985), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (3rd ed.), New York: Wiley, ISBN 0-471-85472-7
2. ^ "Life Sciences Cyberbridge". Covalent Bonds. Archived from the original on 2015-09-18. Retrieved 2015-09-15.
3. ^ Landau, Elizabeth (12 October 2016). "Building Blocks of Life's Building Blocks Come From Starlight". NASA. Retrieved 13 October 2016.
4. ^ CRC Handbook of Chemistry and Physics, 88th edition
5. ^ Bollinger, J. M. Jr., Broderick, J. B. "Frontiers in enzymatic C-H-bond activation" Current Opinion in Chemical Biology 2009, vol. 13, page 51-7. doi:10.1016/j.cbpa.2009.03.018
6. ^ "Bond Energies". Organic Chemistry, Michigan State University. Archived from the original on 29 August 2016.
7. ^ Yu-Ran Luo and Jin-Pei Cheng "Bond Dissociation Energies" in CRC Handbook of Chemistry and Physics, 96th Edition

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The tremendous variety and diversity of organic chemistry is due to the ability of carbon atoms to bond with each other in a variety of straight chains, branched chains, and rings and of adjacent carbon atoms to be joined by single, double, or triple bonds. This bonding ability can be illustrated with the simplest class of organic chemicals, the hydrocarbons consisting only of hydrogen and carbon. Figure 6.1 shows some hydrocarbons in various configurations. Hydrocarbons are the major ingredients of petroleum and are pumped from the ground as crude oil or extracted as natural gas. They have two major uses. The first of these is combustion as a source of fuel. The most abundant hydrocarbon in natural gas, methane, CH4, is burned in home furnaces, electrical power plants, and even in vehicle engines,

\[\ce{CH4 + 2O2 \rightarrow CO2 + 2H2O + heat energy}\]

to provide energy. The second major use of hydrocarbons is as a raw material for making rubber, plastics, polymers, and many other kinds of materials. Given the value of hydrocarbons as a material, it is unfortunate that so much of hydrocarbon production is simply burned to provide energy, which could be generated by other means.

There are several major class of hydrocarbons, all consisting of only hydrogen and carbon. Alkanes have only single bonds between carbon atoms. Cyclohexane, n-heptane, and 3-ethyl-2,5-dimethylhexane in Figure 6.1 are alkanes; the cyclohexane is a cyclic hydrocarbon. Alkenes, such as propene shown in Figure 6.1, have at least one double bond consisting of 4 shared electrons between two of the carbon atoms in the molecule. Alkynes have at least one triple bond between carbon atoms in the molecule as shown for acetylene in Figure 6.1. Acetylene is an important fuel for welding and cutting torches; otherwise, the alkynes are of relatively little importance and will not be addressed farther. A fourth class of hydrocarbon consists of aromatic compounds which have rings of carbon atoms with special bonding properties as discussed later in this chapter

The molecular formulas of non-cyclic alkanes are CnH2n+2. By counting the numbers of carbon and hydrogen atoms in the molecules of alkanes shown in Figure 6.1, it is seen that the molecular formula of n-heptane is C7H6 and that of 3-ethyl-2,5-dimethylhexane is C10H22, both of which fit the general formula given above. The general formula of cyclic alkanes is CnH2n; that of cyclohexane, the most common cyclic alkane, is C6H12. These formulas are molecular formulas, which give the number of carbon and hydrogen atoms in each molecule, but do not tell anything about the structure of the molecule. The formulas given in Figure 6.1 are structural formulas which show how the molecule is assembled. The structure of n-heptane is that of a straight chain of carbon atoms; each carbon atom in the middle of the chain is bound to 2 H atoms and the 2 carbon atoms at the ends of the chain are each bound to 3 H atoms. The prefix hep in the name denotes 7 carbon atoms and then-indicates that the compound consists of a single straight chain. This compound can be represented by a condensed structural formula as CH3(CH2)5CH3 representing 7 carbon atoms in a straight chain. In addition to methane mentioned previously, the lower alkanes include the following:

Ethane: CH3CH3 Propane: CH3CH2CH3 Butane: CH3(CH2)2CH3 n-Pentane: CH3(CH2)3CH3

For alkanes with 5 or more carbon atoms, the prefix (pen for 5,hex for 6,hept for 7,oct for 8,non for 9) shows the total number of carbon atoms in the compound and n-may be used to denote a straight-chain alkane. Condensed structural formulas may be used to represent branched chain alkanes as well. The condensed structural formula of 3-ethyl-2,5-dimethylhexane is

CH3CH(CH3)CH(C2H5)CH2CH(CH3)CH3

In this formula, the C atoms and their attached H atoms that are not in parentheses show carbons that are part of the main hydrocarbon chain. The (CH3) after the second C in the chain shows a methyl group attached to it, the (C2H5) after the third carbon atom in the chain shows an ethyl group attached to it, and the (CH3) after the fifth carbon atom in the chain shows a methyl group attached to it.

Compounds that have the same molecular formulas but different structural formulas are structural isomers. For example, the straight-chain alkane with the molecular formula C10H22 is n-decane

which is a structural isomer of 3-ethyl-2,5-dimethylhexane.

The names of organic compounds are commonly based upon the structure of the hydrocarbon from which they are derived using the longest continuous chain of carbon atoms in the compound as the basis for the name. For example, the longest continuous chain of carbon atoms in 3-ethyl-2,5-dimethylhexane shown in Figure 6.1 is 6 carbon atoms, so the name is based upon hexane. The names of the chain branches are also based upon the alkanes from which they are derived. As shown below,

the two shortest-chain alkanes are methane with 1 carbon atom and ethane with 2 carbon atoms. Removal of 1 of the H atoms from methane gives the methyl group and removal of 1 of the H atoms from ethane gives the ethyl group. These terms are used in the name 3-ethyl-2,5-dimethylhexane to show groups attached to the basic hexane chain. The carbon atoms in this chain are numbered sequentially from left to right. An ethyl group is attached to the 3rd carbon atom, yielding the “3-ethyl” part of the name, and methyl groups are attached to the 2nd and 5th carbon atoms, which gives the “2,5-dimethyl” part of the name.

The names discussed above are systematic names, which are based upon the actual structural formulas of the molecules. In addition, there are common names of organic compounds that do not indicate the structural formulas. Naming organic compounds is a complex topic, and no attempt is made here to teach it to the reader. However, from the names of compounds given in this and later chapters, some appreciation of the rationale for organic compound names should be obtained.

Other than burning them for energy, the major kind of reaction with alkanes consists of substitution reactions such as,

\[\ce{C2H6 + 2Cl2 \rightarrow C2H4Cl2 + 2HCl}\]

in which one or more H atoms are displaced by another kind of atom. This is normally the first step in converting alkanes to compounds containing elements other than carbon or hydrogen for use in synthesizing a wide variety of organic compounds.

Alkenes

Four common alkenes are shown in Figure 6.2. Alkenes have at least one C=C double bond per molecule and may have more. The first of the alkenes in Figure 6.2, ethylene, is a very widely produced hydrocarbon used to synthesize polyethylene plastic and other organic compounds. About 25 billion kilograms (kg) of ethylene are processed in the U.S. each year. About 14.5 billion kg of propylene are used in the U.S. each year to produce polypropylene plastic and other chemicals. The two 2-butene compounds illustrate an important aspect of alkenes, the possibility of cis-trans isomerism. Whereas carbon atoms and the groups substituted onto them joined by single bonds can freely rotate relative to each other as though they were joined by a single shaft, carbon atoms connected by a double bond behave as though they were attached by two parallel shafts and are not free to rotate. So, cis-2-butene in which the two end methyl (-CH3) groups are on the same side of the molecule is a different compound from trans-2-butene in which they are on opposite sides. These two compounds are cis-trans isomers

Alkenes are chemically much more active than alkanes. This is because the double bond is unsaturated and has electrons available to form additional bonds with other atoms. This leads to addition reactions in which a molecule is added across a double bond. For example, the addition of H2O to ethylene

yields ethanol, the same kind of alcohol that is in alcoholic beverages. In addition to adding immensely to the chemical versatility of alkenes, addition reactions make them quite reactive in the atmosphere during the formation of photochemical smog. The presence of double bonds also adds to the biochemical and toxicological activity of compounds in organisms

Because of their double bonds, alkenes can undergo polymerization reactions in which large numbers of individual molecules add to each other to produce big molecules called polymers (see Section 6.5). For example, 3 ethylene molecules can add together as follows:

a process that can continue, forming longer and longer chains and resulting in the formation of huge molecules molecules of polyethylene

Aromatic Hydrocarbons

A special class of hydrocarbons consists of rings of carbon atoms, almost always containing 6C atoms, which can be viewed as having alternating single and double bonds as shown below:

These structures show the simplest aromatic hydrocarbon, benzene, C6H6. Although the benzene molecule is represented with 3 double bonds, chemically it differs greatly from alkenes, for example undergoing substitution reactions rather than addition reactions. The properties of aromatic compounds are special properties called aromaticity. The two structures shown above are equivalent resonance structures, which can be viewed as having atoms that stay in the same places, but in which the bonds joining the atoms can shift positions with the movement of electrons composing the bonds. Since benzene has different chemical properties from those implied by either of the above structures, it is commonly represented as a hexagon with a circle in the middle:

Many aromatic hydrocarbons have two or more rings. The simplest of these is naphthalene,

a two-ringed compound in which two benzene rings share the carbon atoms at which they are joined; these two carbon atoms do not have any H attached, each of the other 8 C atoms in the compound has 1 H attached. Aromatic hydrocarbons with multiple rings, called polycyclic aromatic hydrocarbons, PAH, are common and are often produced as byproducts of combustion. One of the most studied of these is benzo(a)pyrene,

found in tobacco smoke, diesel exhaust, and charbroiled meat. This compound is toxicologically significant because it is partially oxidized by enzymes in the body to produce a cancer-causing metabolite.

The presence of hydrocarbon groups and of elements other than carbon and hydrogen bonded to an aromatic hydrocarbon ring gives a variety of aromatic compounds. Three examples of common aromatic compounds are given below. Toluene is widely used for chemical synthesis and as a solvent. The practice of green chemistry now calls for substituting toluene for benzene wherever possible because benzene is suspected of causing leukemia, whereas the body is capableof metabolizing toluene to harmless metabolites (see Chapter 7). About 850 million kg of aniline are made in the U.S. each year as an intermediate in the synthesis of dyes and other organic chemicals. Phenol is a relatively toxic oxygen-containing aromatic compound which, despite its toxicity to humans, was the first antiseptic used in the 1800s.