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3.11: Organic Compounds

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    Learning Objectives
    • To recognize the composition and properties typical of organic and inorganic compounds.

    Organic substances have been used throughout this text to illustrate the differences between ionic and covalent bonding and to demonstrate the intimate connection between the structures of compounds and their chemical reactivity. You learned, for example, that even though NaOH and alcohols (ROH) both have OH in their formula, NaOH is an ionic compound that dissociates completely in water to produce a basic solution containing Na+ and OH ions, whereas alcohols are covalent compounds that do not dissociate in water and instead form neutral aqueous solutions. You also learned that an amine (RNH2), with its lone pairs of electrons, is a base, whereas a carboxylic acid (RCO2H), with its dissociable proton, is an acid.

    Scientists of the 18th and early 19th centuries studied compounds obtained from plants and animals and labeled them organic because they were isolated from “organized” (living) systems. Compounds isolated from nonliving systems, such as rocks and ores, the atmosphere, and the oceans, were labeled inorganic. For many years, scientists thought organic compounds could be made by only living organisms because they possessed a vital force found only in living systems. The vital force theory began to decline in 1828, when the German chemist Friedrich Wöhler synthesized urea from inorganic starting materials. He reacted silver cyanate (AgOCN) and ammonium chloride (NH4Cl), expecting to get ammonium cyanate (NH4OCN). What he expected is described by the following equation.

    \[AgOCN + NH_4Cl \rightarrow AgCl + NH_4OCN \label{25.1.1} \]

    Instead, he found the product to be urea (NH2CONH2), a well-known organic material readily isolated from urine. This result led to a series of experiments in which a wide variety of organic compounds were made from inorganic starting materials. The vital force theory gradually went away as chemists learned that they could make many organic compounds in the laboratory.

    Today organic chemistry is the study of the chemistry of the carbon compounds, and inorganic chemistry is the study of the chemistry of all other elements. It may seem strange that we divide chemistry into two branches—one that considers compounds of only one element and one that covers the 100-plus remaining elements. However, this division seems more reasonable when we consider that of tens of millions of compounds that have been characterized, the overwhelming majority are carbon compounds.

    The word organic has different meanings. Organic fertilizer, such as cow manure, is organic in the original sense; it is derived from living organisms. Organic foods generally are foods grown without synthetic pesticides or fertilizers. Organic chemistry is the chemistry of compounds of carbon.

    Carbon is unique among the other elements in that its atoms can form stable covalent bonds with each other and with atoms of other elements in a multitude of variations. The resulting molecules can contain from one to millions of carbon atoms. We previously surveyed organic chemistry by dividing its compounds into families based on functional groups. We begin with the simplest members of a family and then move on to molecules that are organic in the original sense—that is, they are made by and found in living organisms. These complex molecules (all containing carbon) determine the forms and functions of living systems and are the subject of biochemistry.

    Organic compounds, like inorganic compounds, obey all the natural laws. Often there is no clear distinction in the chemical or physical properties among organic and inorganic molecules. Nevertheless, it is useful to compare typical members of each class, as in Table \(\PageIndex{1}\).

    Table \(\PageIndex{1}\): General Contrasting Properties and Examples of Organic and Inorganic Compounds
    Organic Hexane Inorganic NaCl
    low melting points −95°C high melting points 801°C
    low boiling points 69°C high boiling points 1,413°C
    low solubility in water; high solubility in nonpolar solvents insoluble in water; soluble in gasoline greater solubility in water; low solubility in nonpolar solvents soluble in water; insoluble in gasoline
    flammable highly flammable nonflammable nonflammable
    aqueous solutions do not conduct electricity nonconductive aqueous solutions conduct electricity conductive in aqueous solution
    exhibit covalent bonding covalent bonds exhibit ionic bonding ionic bonds

    Keep in mind, however, that there are exceptions to every category in this table. To further illustrate typical differences among organic and inorganic compounds, Table \(\PageIndex{1}\) also lists properties of the inorganic compound sodium chloride (common table salt, NaCl) and the organic compound hexane (C6H14), a solvent that is used to extract soybean oil from soybeans (among other uses). Many compounds can be classified as organic or inorganic by the presence or absence of certain typical properties, as illustrated in Table \(\PageIndex{1}\).

    Key Takeaway

    • Organic chemistry is the study of carbon compounds, nearly all of which also contain hydrogen atoms.


     Learning Objectives
    • Identify alkanes, alkenes, alkynes, and aromatic compounds.
    • List some properties of hydrocarbons.

    The simplest organic compounds are those composed of only two elements: carbon and hydrogen. These compounds are called hydrocarbons. Hydrocarbons themselves are separated into two types: aliphatic hydrocarbons and aromatic hydrocarbons.

    Aliphatic hydrocarbons are hydrocarbons based on chains of C atoms. There are three types of aliphatic hydrocarbons. Alkanes are aliphatic hydrocarbons with only single covalent bonds. Alkenes are hydrocarbons that contain at least one C–C double bond, and Alkynes are hydrocarbons that contain a C–C triple bond. Occasionally, we find an aliphatic hydrocarbon with a ring of C atoms; these hydrocarbons are called cycloalkanes (or cycloalkenes or cycloalkynes).

    Aromatic hydrocarbons have a special six-carbon ring called a benzene ring. Electrons in the benzene ring have special energetic properties that give benzene physical and chemical properties that are markedly different from alkanes. Originally, the term aromatic was used to describe this class of compounds because they were particularly fragrant. However, in modern chemistry the term aromatic denotes the presence of a six-membered ring that imparts different and unique properties to a molecule.

    The simplest alkanes have their C atoms bonded in a straight chain; these are called normal alkanes. They are named according to the number of C atoms in the chain. The smallest alkane is methane:

    Bond line structure of methane.
    Figure \(\PageIndex{1}\) - Three-Dimensional Representation of Methane.
    Three-Dimensional Representation of Methane molecule.
    Figure \(\PageIndex{1}\) Three-Dimensional Representation of Methane © Thinkstock. The methane molecule is three dimensional, with the H atoms in the positions of the four corners of a tetrahedron.

    The next-largest alkane has two C atoms that are covalently bonded to each other. For each C atom to make four covalent bonds, each C atom must be bonded to three H atoms. The resulting molecule, whose formula is C2H6, is ethane:

    Structural formula of ethane.

    Propane has a backbone of three C atoms surrounded by H atoms. You should be able to verify that the molecular formula for propane is C3H8:

    structural formula of propane.

    The diagrams representing alkanes are called structural formulas because they show the structure of the molecule. As molecules get larger, structural formulas become more and more complex. One way around this is to use a condensed structural formula, which lists the formula of each C atom in the backbone of the molecule. For example, the condensed structural formula for ethane is CH3CH3, while for propane it is CH3CH2CH3. Table \(\PageIndex{1}\) - The First 10 Alkanes, gives the molecular formulas, the condensed structural formulas, and the names of the first 10 alkanes.

    Table \(\PageIndex{1}\) The First 10 Alkanes
    Molecular Formula Condensed Structural Formula Name
    CH4 CH4 methane
    C2H6 CH3CH3 ethane
    C3H8 CH3CH2CH3 propane
    C4H10 CH3CH2CH2CH3 butane
    C5H12 CH3CH2CH2CH2CH3 pentane
    C6H14 CH3(CH2)4CH3 hexane
    C7H16 CH3(CH2)5CH3 heptane
    C8H18 CH3(CH2)6CH3 octane
    C9H20 CH3(CH2)7CH3 nonane
    C10H22 CH3(CH2)8CH3 decane

    Because alkanes have the maximum number of H atoms possible according to the rules of covalent bonds, alkanes are also referred to as saturated hydrocarbons.

    Alkenes have a C–C double bond. Because they have less than the maximum number of H atoms possible, they are unsaturated hydrocarbons. The smallest alkene—ethene—has two C atoms and is also known by its common name ethylene:

    Structural formula of ethylene.

    The next largest alkene—propene—has three C atoms with a C–C double bond between two of the C atoms. It is also known as propylene:

    Structural formula of propylene.

    What do you notice about the names of alkanes and alkenes? The names of alkenes are the same as their corresponding alkanes except that the ending is -ene, rather than -ane. Using a stem to indicate the number of C atoms in a molecule and an ending to represent the type of organic compound is common in organic chemistry, as we shall see.

    With the introduction of the next alkene, butene, we begin to see a major issue with organic molecules: choices. With four C atoms, the C–C double bond can go between the first and second C atoms or between the second and third C atoms:

    2 structural formulas for butene, with the first butene having the double bond on the first and second carbon from the left and the latter having its double bond on the second and third carbon from the left. 

    (A double bond between the third and fourth C atoms is the same as having it between the first and second C atoms, only flipped over.) The rules of naming in organic chemistry require that these two substances have different names. The first molecule is named 1-butene, while the second molecule is named 2-butene. The number at the beginning of the name indicates where the double bond originates. The lowest possible number is used to number a feature in a molecule; hence, calling the second molecule 3-butene would be incorrect. Numbers are common parts of organic chemical names because they indicate which C atom in a chain contains a distinguishing feature.

    The compounds 1-butene and 2-butene have different physical and chemical properties, even though they have the same molecular formula—C4H8. Different molecules with the same molecular formula are called isomers. Isomers are common in organic chemistry and contribute to its complexity.

    Example \(\PageIndex{1}\)

    Based on the names for the butene molecules, propose a name for this molecule.


    A structural formula of a five carbon molecule with a double bond on the third and fourth carbon from the left. There are ten hydrogen atoms in total.

    With five C atoms, we will use the pent- stem, and with a C–C double bond, this is an alkene, so this molecule is a pentene. In numbering the C atoms, we use the number 2 because it is the lower possible label. So this molecule is named 2-pentene.

    Exercise \(\PageIndex{1}\)

    Based on the names for the butene molecules, propose a name for this molecule.

    A structural formula of a six carbon molecule with a double bond on the third and fourth carbon from the left. There are twelve hydrogen atoms in total.



    Alkynes, with a C–C triple bond, are named similarly to alkenes except their names end in -yne. The smallest alkyne is ethyne, which is also known as acetylene:

    Structural formula of acetylene.

    Propyne has the structure

    Structural formula showing three carbon molecules with a triple bond present between the first and second carbon atom. The appropriate number of hydrogen atoms is attached to each carbon atom.

    With butyne, we need to start numbering the position of the triple bond, just as we did with alkenes:

    Two structural formula of butyne. One butyne has a triple bond between the first and second carbon atom, while two butyne has the triple bond between the second and third carbon atom.  

    Aromatic compounds contain the benzene unit. Benzene itself is composed of six C atoms in a ring, with alternating single and double C–C bonds:

    The six carbons are arranged in a hexagon pattern with one hydrogen atom emerging outwards from each carbon atom. The presence of a double bond is alternated between every other carbon atom. 

    The alternating single and double C–C bonds give the benzene ring a special stability, and it does not react like an alkene as might be suspected. Benzene has the molecular formula C6H6; in larger aromatic compounds, a different atom replaces one or more of the H atoms.

    As fundamental as hydrocarbons are to organic chemistry, their properties and chemical reactions are rather mundane. Most hydrocarbons are nonpolar because of the close electronegativities of the C and H atoms. As such, they dissolve only sparingly in H2O and other polar solvents. Small hydrocarbons, such as methane and ethane, are gases at room temperature, while larger hydrocarbons, such as hexane and octane, are liquids. Even larger hydrocarbons are solids at room temperature and have a soft, waxy consistency.

    Hydrocarbons are rather unreactive, but they do participate in some classic chemical reactions. One common reaction is substitution with a halogen atom by combining a hydrocarbon with an elemental halogen. Light is sometimes used to promote the reaction, such as this one between methane and chlorine:

    \[CH_{4}+Cl_{2}\overset{light}{\rightarrow} CH_{3}Cl+HCl\nonumber \]

    Halogens can also react with alkenes and alkynes, but the reaction is different. In these cases, the halogen reacts with the C–C double or triple bond and inserts itself onto each C atom involved in the multiple bonds. This reaction is called an addition reaction. One example is


    Structural formula showing the reaction of ethylene with a chlorine molecule to form ethylene dichloride.

    The reaction conditions are usually mild; in many cases, the halogen reacts spontaneously with an alkene or an alkyne.

    Hydrogen can also be added across a multiple bond; this reaction is called a hydrogenation reaction. In this case, however, the reaction conditions may not be mild; high pressures of H2 gas may be necessary. A platinum or palladium catalyst is usually employed to get the reaction to proceed at a reasonable pace:

    \[CH_{2}=CH_{2}+H_{2}\overset{metal\: catalyst}{\rightarrow} CH_{3}CH_{3}\nonumber \]

    By far the most common reaction of hydrocarbons is combustion, which is the combination of a hydrocarbon with O2 to make CO2 and H2O. The combustion of hydrocarbons is accompanied by a release of energy and is a primary source of energy production in our society (Figure \(\PageIndex{2}\) - Combustion). The combustion reaction for gasoline, for example, which can be represented by C8H18, is as follows:

    \[2C_{8}H_{18}+25O_{2}\rightarrow 16CO_{2}+18H_{2}O+\sim 5060kJ\nonumber \]

    A tower in the middle of a desert with a large flame emerging from the top.
    Figure \(\PageIndex{2}\) Combustion © Thinkstock. The combustion of hydrocarbons is a primary source of energy in our society.

    Key Takeaways

    • The simplest organic compounds are hydrocarbons and are composed of carbon and hydrogen.
    • Hydrocarbons can be aliphatic or aromatic; aliphatic hydrocarbons are divided into alkanes, alkenes, and alkynes.
    • The combustion of hydrocarbons is a primary source of energy for our society.
    Exercise \(\PageIndex{2}\)
    1. Define hydrocarbon. What are the two general types of hydrocarbons?
    2. What are the three different types of aliphatic hydrocarbons? How are they defined?
    3. Indicate whether each molecule is an aliphatic or an aromatic hydrocarbon; if aliphatic, identify the molecule as an alkane, an alkene, or an alkyne.
      1. Structural formula of butane.
      2. Structural formula of toluene.
      3. Structural formula of 2 butene.
    4. Indicate whether each molecule is an aliphatic or an aromatic hydrocarbon; if aliphatic, identify the molecule as an alkane, an alkene, or an alkyne.
      1. Structural formula of 2 butyne.
      2. Structural formula of naphthalene, a polycyclic aromatic compound.
      3. Structural formula of ethylene.
    5. Indicate whether each molecule is an aliphatic or an aromatic hydrocarbon; if aliphatic, identify the molecule as an alkane, an alkene, or an alkyne.
      1. Structural formula of cyclopropane.
      2. Structural formula of cyclopropene.
      3. Structural formula of 1, 2, 4 trimethylbenzene.
    6. Indicate whether each molecule is an aliphatic or an aromatic hydrocarbon; if aliphatic, identify the molecule as an alkane, an alkene, or an alkyne.
      1. Structural formula of three hexene.
      2. Structural formula of phenalene.
      3. Structural formula of 1,4 pentadiyne.
    7. Name and draw the structural formulas for the four smallest alkanes.
    8. Name and draw the structural formulas for the four smallest alkenes.
    9. What does the term aromatic imply about an organic molecule?
    10. What does the term normal imply when used for alkanes?
    11. Explain why the name 1-propene is incorrect. What is the proper name for this molecule?
    12. Explain why the name 3-butene is incorrect. What is the proper name for this molecule?
    13. Name and draw the structural formula of each isomer of pentene.
    14. Name and draw the structural formula of each isomer of hexyne.
    15. Write a chemical equation for the reaction between methane and bromine.
    16. Write a chemical equation for the reaction between ethane and chlorine.
    17. Draw the structure of the product of the reaction of bromine with propene.
    18. Draw the structure of the product of the reaction of chlorine with 2-butene.
    19. Draw the structure of the product of the reaction of hydrogen with 1-butene.
    20. Draw the structure of the product of the reaction of hydrogen with 1-butene.
    21. Write the balanced chemical equation for the combustion of heptane.
    22. Write the balanced chemical equation for the combustion of nonane.

    1. an organic compound composed of only carbon and hydrogen; aliphatic hydrocarbons and aromatic hydrocarbons
      1. aliphatic; alkane
      2. aromatic
      3. aliphatic; alkene
      1. aliphatic; alkane
      2. aliphatic; alkene
      3. aromatic
    5. Structural formula of methane, ethane, propane, and butane.
    7. Aromatic means that the molecule has a benzene ring.
    9. The 1 is not necessary. The name of the compound is simply propene.
    11. Structural formula of 1 pentene and 2 pentene.
    13. CH4 + Br2 → CH3Br + HBr
    15. Structural formula of 1 2 dibromopropane.
    17. Structural formula of butane.
    19. C7H16 + 11O2 → 7CO2 + 8H2O

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