Transcript chapter 4 carbon and the molecular diversity of life

CHAPTER 4
CARBON AND THE
MOLECULAR
DIVERSITY OF LIFE
-THE IMPORTANCE OF CARBON
-FUNCTIONAL GROUPS
Although water is the universal medium for life on Earth, most of the chemicals that make up living organisms are
based on the element carbon. Of all chemical elements, carbon is unparalleled in its ability to form molecules that
are large, complex, and diverse, and this molecular diversity has made possible the diversity of organisms that
have evolved on Earth. The protein shown in the computer graphic image above is an example of a large,
complex molecule based on carbon (the green atoms). Proteins are a major topic of Chapter 5. In this chapter, we
focus on smaller molecules, using them to illustrate a few concepts of molecular architecture that highlight
carbon’s importance to life and the theme that emergent properties arise from the organization of the matter of
living organisms.
THE IMPORTANCE OF CARBON
Although a cell is composed of 70-95% water, the rest consists mostly of carbon-based compounds. Proteins,
DNA, carbohydrates, and other molecules that distinguish living matter from inanimate material are all composed
of carbon atoms bonded to one another and to atoms of other elements. Hydrogen (H), oxygen (O), nitrogen (N),
sulfur (S), and phosphorus (P) are other common ingredients of these compounds, but it is carbon (C) that
accounts for the large diversity of biological molecules.
Carbon
Organic chemistry is the study of carbon compounds
Compounds containing carbon are said to be organic, and the branch of chemistry that specializes in the study of
carbon compounds is called organic chemistry. Once thought to come only from living things, organic
compounds range from simple molecules, such as carbon dioxide (CO2) and methane (CH4), to colossal ones,
such as proteins, with thousands of atoms and molecular weights in excess of 100,000 daltons. Most organic
compounds contain hydrogen atoms.
The overall percentages of the major elements of life--C, H, O, N, S, and P--are quite uniform from one organism
to another. Because of carbon’s versatility, however, this limited assortment of atomic building blocks, taken in
roughly the same proportions, can be used to build an inexhaustible variety of organic molecules. Different
species of organisms, and different individuals within a species, are distinguished by variations in their organic
molecules.
Since the dawn of human history, people have used other organisms as sources of valued substances--from foods
to medicines and fabrics. The science of organic chemistry originated in attempts to purify and improve the yield of
such products. By the early 19th century, chemists had learned to make many simple compounds in the laboratory
by combining elements under the right conditions. Artificial synthesis of the complex molecules extracted from
living matter seemed impossible, however. It was at that time that the Swedish chemist Jöns Jakob Berzelius first
made the distinction between organic compounds, those that seemingly could arise only within living organisms,
and inorganic compounds, those that were found in the nonliving world. The new discipline of organic chemistry
was first built on a foundation of vitalism, the belief in a life force outside the jurisdiction of physical and chemical
laws.
Jöns Jakob Berzelius
Chemists began to chip away at the foundation of vitalism when they learned to synthesize organic compounds in
their laboratories. In 1828, Friedrich Wöhler, a German chemist who had studied with Berzelius, attempted to
make an inorganic salt, ammonium cyanate, by mixing solutions of ammonium (NH4+) and cyanate (CNO-) ions.
Wöhler was astonished to find that instead of the expected product, he had made urea, an organic compound
present in the urine of animals. Wöhler challenged the vitalists when he wrote, "I must tell you that I can prepare
urea without requiring a kidney or an animal, either man or dog." However, one of the ingredients used in the
synthesis, the cyanate, had been extracted from animal blood, and the vitalists were not swayed by Wöhler’s
discovery. However, a few years later, Hermann Kolbe, a student of Wöhler’s, made the organic compound acetic
acid from inorganic substances that could themselves be prepared directly from pure elements
Hermann Kolbe
Friedrich Wöhler
The foundation of vitalism finally crumbled after several more decades of laboratory synthesis of increasingly
complex organic compounds. In 1953, Stanley Miller, then a graduate student at the University of Chicago, helped
bring this abiotic (nonliving) synthesis of organic compounds into the context of evolution. Miller used a laboratory
simulation of chemical conditions on the primitive Earth to demonstrate that the spontaneous synthesis of organic
compounds could have been an early stage in the origin of life.
Abiotic synthesis of organic compounds under "early Earth" conditions.
Here Stanley Miller re-creates his 1953 experiment, a laboratory simulation
demonstrating that environmental conditions on the lifeless, primordial Earth
allowed the spontaneous synthesis of some organic molecules. Miller used
electrical discharges (simulated lightning) to trigger reactions in a primitive
"atmosphere" of H2O, H2, NH3 (ammonia), and CH4 (methane)--some of the
gases released by volcanoes. From these ingredients, Miller’s apparatus made a
variety of organic compounds that play key roles in living cells. Similar chemical
reactions may have set the stage for the origin of life on Earth, a hypothesis we
will explore in more detail in Chapter 26.
The pioneers of organic chemistry helped shift the mainstream of biological thought from vitalism to mechanism,
the belief that all natural phenomena, including the processes of life, are governed by physical and chemical laws.
Organic chemistry was redefined as the study of carbon compounds, regardless of their origin. Most naturally
occurring organic compounds are produced by organisms, and these molecules represent a diversity and range of
complexity unrivaled by inorganic compounds. However, the same rules of chemistry apply to inorganic and
organic molecules alike. The foundation of organic chemistry is not some intangible life force, but the unique
chemical versatility of the element carbon.
Carbon atoms are the most versatile building blocks of molecules
The key to the chemical characteristics of an atom, as you learned in Chapter 2, is in its configuration of electrons,
because electron configuration determines the kinds and number of bonds an atom will form with other atoms.
Carbon has a total of 6 electrons, with 2 in the first electron shell and 4 in the second shell. Having 4 valence
electrons in a shell that holds 8, carbon has little tendency to gain or lose electrons and form ionic bonds; it would
have to donate or accept 4 electrons to do so. Instead, a carbon atom usually completes its valence shell by
sharing electrons with other atoms in four covalent bonds. Each carbon atom thus acts as an intersection point
from which a molecule can branch off in up to four directions. This tetravalence is one facet of carbon’s versatility
that makes large, complex molecules possible.
In Chapter 2, you also learned that when a carbon atom forms single covalent bonds, the arrangement of its four
hybrid orbitals causes the bonds to angle toward the corners of an imaginary tetrahedron (see FIGURE 2.15c).
The bond angles in methane (CH4) are 109° (FIGURE a), and they are approximately the same in any group of
atoms where carbon has four single bonds. For example, ethane (C2H6) is shaped like two tetrahedrons joined at
their apexes (FIGURE b). In molecules with still more carbons, every grouping of a carbon bonded to four other
atoms has a tetrahedral shape. But when two carbon atoms are joined by a double bond, all bonds around those
carbons are in the same plane. For example, ethene is a flat molecule; its atoms all lie in the same plane
(FIGURE c). It is convenient to write all structural formulas as though the molecules represented were flat, but it is
important to remember that molecules are three-dimensional and that the shape of a molecule often determines its
function.
The shapes of three simple
organic molecules.
The electron configuration of carbon gives it covalent compatibility with many different elements. The figure below
reviews the valences of the four major atomic components of organic molecules: carbon and its most frequent
partners--oxygen, hydrogen, and nitrogen. We can think of these valences as the rules of covalent bonding in
organic chemistry--the building code that governs the architecture of organic molecules.
Valences for the major elements of organic molecules.
Valence is the number of covalent bonds an atom will usually form. It is generally equal to the number of electrons required to
complete the atom’s outermost (valence) electron shell.
A couple of additional examples will show how the rules of covalent bonding apply to carbon atoms with partners
other than hydrogen. In the carbon dioxide molecule (CO2), a single carbon atom is joined to two atoms of oxygen
by double covalent bonds. The structural formula for CO2 is OCO. Each line (bond) in a structural formula
represents a pair of shared electrons. Notice that the carbon atom in CO2 is involved in four covalent bonds, two
with each oxygen atom. The arrangement completes the valence shells of all atoms in the molecule. Because
carbon dioxide is a very simple molecule and lacks hydrogen, it is often considered inorganic, even though it
contains carbon. Whether we call CO2 organic or inorganic is an arbitrary distinction, but there is no ambiguity
about its importance to the living world. Taken from the air by plants and incorporated into sugar and other foods
during photosynthesis, CO2 is the source of carbon for all the organic molecules found in organisms.
Another relatively simple molecule is urea, CO(NH2)2. This is the organic compound found in urine that Wöhler
learned to synthesize in the early 19th century. The structural formula for urea is shown on the following
page.
Again, each atom has the required number of covalent bonds. In this case, one carbon atom is involved in both
single and double bonds.
Both urea and carbon dioxide are molecules with only one carbon atom. But as the figure above shows, a carbon
atom can also use one or more of its valence electrons to form covalent bonds to other carbon atoms, making it
possible to link the atoms into chains of seemingly infinite variety.
Variation in carbon skeletons contributes to the diversity of organic molecules
Carbon chains form the skeletons of most organic molecules. The skeletons vary in length and may be straight,
branched, or arranged in closed rings. Some carbon skeletons have double bonds, which vary in number and
location. Such variation in carbon skeletons is one important source of the molecular complexity and diversity that
characterize living matter. In addition, atoms of other elements can be bonded to the skeletons at available sites.
Variations in carbon skeletons.
Hydrocarbons, organic molecules consisting only of carbon and hydrogen, illustrate the diversity of the carbon skeletons of organic
molecules.
All the molecules shown in the figure below are hydrocarbons, organic molecules consisting only of carbon and
hydrogen. Atoms of hydrogen are attached to the carbon skeleton wherever electrons are available for covalent
bonding. Hydrocarbons are the major components of petroleum, which is called a fossil fuel because it consists of
the partially decomposed remains of organisms that lived millions of years ago.
Although hydrocarbons are not prevalent in living organisms, many of a cell’s organic molecules have regions
consisting of only carbon and hydrogen. For example, the molecules known as fats have long hydrocarbon tails
attached to a nonhydrocarbon component. Neither petroleum nor fat mixes with water; both are hydrophobic
compounds because the bonds between the carbon and hydrogen atoms are nonpolar. Another characteristic of
hydrocarbons is that they store a relatively large amount of energy. The gasoline that fuels a car consists of
hydrocarbons, and the hydrocarbon tails of fat molecules serve as stored fuel for animal bodies.
The role of hydrocarbons in fats.
(a) A fat molecule consists of a headpiece and three hydrocarbon tails. The tails store energy and account for the hydrophobic
behavior of fats. (Black = carbon; gray = hydrogen; red = oxygen) (b) Mammalian adipose cells stockpile fat molecules as a fuel
reserve. Each adipose cell in this micrograph is almost filled by a large fat droplet, which stockpiles a huge number of fat molecules.
Isomers
Variation in the architecture of organic molecules can be seen in isomers, compounds that have the same
molecular formula but different structures and hence different properties. Compare, for example, the two butanes
in FIGURE a. Both have the molecular formula C4H10, but they differ in the covalent arrangement of their carbon
skeletons. The skeleton is straight in butane, but branched in isobutane. We will examine three types of isomers:
structural isomers, geometric isomers, and enantiomers.
Structural isomers differ in the covalent arrangements of their atoms. The
number of possible isomers increases tremendously as carbon skeletons
increase in size. There are only two butanes, but there are 18 variations of C 8H18
and 366,319 possible structural isomers of C20H42. Structural isomers may also
differ in the location of double bonds.
Butane
Isobutane
Geometric isomers have the same covalent partnerships, but they differ in their
spatial arrangements. Geometric isomers arise from the inflexibility of double
bonds, which, unlike single bonds, will not allow the atoms they join to rotate
freely about the bond axis. The subtle difference in shape between geometric
isomers can dramatically affect the biological activities of organic molecules. For
example, the biochemistry of vision involves a light-induced change of rhodopsin,
a chemical compound in the eye, from one geometric isomer to another.
Enantiomers are molecules that are mirror images of each other. In the balland-stick models shown in FIGURE 4.6c, the middle carbon is called an
asymmetric carbon because it is attached to four different atoms or groups of
atoms. The four groups can be arranged in space about the asymmetric carbon
in two different ways that are mirror images. They are, in a way, left-handed and
right-handed versions of the molecule. A cell can distinguish these isomers
based on their different shapes. Usually, one isomer is biologically active and
the other is inactive.
Three types of isomers.
Compounds with the same molecular formula but
different structures, isomers are a source of
diversity in organic molecules.
The concept of enantiomers is important in the pharmaceutical industry because the two enantiomers of a drug
may not be equally effective. In some cases, one of the isomers may even produce harmful effects. This was the
case with thalidomide, a drug prescribed for thousands of pregnant women in the late 1950s and early 1960s. The
drug was a mixture of two enantiomers. One enantiomer reduced morning sickness, the desired effect, but the
other caused severe birth defects. (And unfortunately, even if the "good" thalidomide enantiomer is used in purified
form, some of it soon converts to the "bad" enantiomer in the patient’s body.) The differing effects of enantiomers
in the body demonstrate that organisms are sensitive to even the most subtle variations in molecular architecture.
Once again, we see that molecules have emergent properties that depend on the specific arrangement of their
atoms.
The pharmacological importance of enantiomers.
L-Dopa is a drug used to treat Parkinson’s disease, a
disorder of the central nervous system. The drug’s
enantiomer, the mirror-image molecule designated DDopa, has no effect on patients.
FUNCTIONAL GROUPS
The distinctive properties of an organic molecule depend not only on the arrangement of its carbon skeleton, but
also on the molecular components attached to that skeleton. We will now examine certain groups of atoms that
are frequently attached to the skeletons of organic molecules.
Functional groups contribute to the molecular diversity of life
The components of organic molecules that are most commonly involved in chemical reactions are known as
functional groups. If we think of hydrocarbons as the simplest organic molecules, we can view functional groups
as attachments that replace one or more of the hydrogens bonded to the carbon skeleton of the hydrocarbon.
(However, some functional groups include atoms of the carbon skeleton, as we will see.)
Each functional group behaves consistently from one organic molecule to another, and the number and
arrangement of the groups help give each molecule its unique properties. Consider the differences between
testosterone and estradiol (a type of estrogen). These compounds are male and female sex hormones,
respectively, in humans and other vertebrates (FIGURE 4.8). Both are steroids, organic molecules with a
common carbon skeleton in the form of four fused rings. These sex hormones differ mainly in the functional
groups attached to the rings. The different actions of these two molecules on many targets throughout the body
help produce the contrasting features of females and males. Thus, even our sexuality has its biological basis in
variations of molecular architecture.
A comparison of functional groups of female (estradiol) and male (testosterone) sex hormones.
The two molecules differ mainly in the attachment of functional groups to a common carbon skeleton of four fused rings. (The carbon
skeleton has been simplified here by omitting the carbons in the rings, as well as their hydrogens.) These subtle variations in
molecular architecture influence the development of the anatomical and physiological differences between female and male
vertebrates.
The six functional groups most important in the chemistry of life are the hydroxyl, carbonyl, carboxyl, amino,
sulfhydryl, and phosphate groups (TABLE). All are hydrophilic and thus increase the solubility of organic
compounds in water.
The ionized forms of the carboxyl and amino groups
prevail in cells. However, acetic acid and glycine are
represented here in their non-ionized forms.
The Hydroxyl Group
In a hydroxyl group, a hydrogen atom is bonded to an oxygen atom, which in turn is bonded to the carbon
skeleton of the organic molecule. Organic compounds containing hydroxyl groups are called alcohols, and their
specific names usually end in -ol, as in ethanol, the drug present in alcoholic beverages. In a structural formula,
the hydroxyl group is usually abbreviated by omission of the covalent bond between the oxygen and hydrogen and
is written as--OH or HO--. (Do not confuse this functional group with the hydroxide ion, OH-, formed by the
dissociation of bases such as sodium hydroxide.) The hydroxyl group is polar as a result of the electronegative
oxygen atom drawing electrons toward itself. Consequently, water molecules are attracted to the hydroxyl group,
and this helps dissolve organic compounds containing such groups. Sugars, for example, owe their solubility in
water to the presence of multiple hydroxyl groups (see FIGURE 5.3).
The Carbonyl Group
The carbonyl group (
) consists of a carbon atom joined to an oxygen atom by a double bond. If the carbonyl
group is on the end of a carbon skeleton, the organic compound is called an aldehyde; otherwise the compound
is called a ketone. The simplest ketone is acetone, which is three carbons long. Acetone has different properties
from propanal, a three-carbon aldehyde. (Acetone and propanal are structural isomers.) Thus, variation in
locations of functional groups along carbon skeletons is a major source of molecular diversity.
Propanal (aldehyde)
Acetone (ketone)
The Carboxyl Group
When an oxygen atom is double-bonded to a carbon atom that is also bonded to a hydroxyl group, the entire
assembly of atoms is called a carboxyl group (--COOH). Compounds containing carboxyl groups are known as
carboxylic acids, or organic acids. The simplest is the one-carbon compound called formic acid (HCOOH), the
substance some ants inject when they sting. Acetic acid, which has two carbons, gives vinegar its sour taste. (In
general, acids taste sour.)
Why does a carboxyl group have acidic properties? A carboxyl group is a source of hydrogen ions. The covalent
bond between the oxygen and the hydrogen is so polar that the hydrogen tends to dissociate reversibly from the
molecule as an ion (H+). In the case of acetic acid, we have
Dissociation occurs as a result of the two electronegative oxygen atoms of the carboxyl group pulling shared
electrons away from hydrogen. If the double-bonded oxygen and the hydroxyl group were attached to separate
carbon atoms, there would be less tendency for the --OH group to dissociate because the second oxygen would
be farther away. Here is another example of how emergent properties result from a specific arrangement of
building components.
The Amino Group
The amino group (--NH2) consists of a nitrogen atom bonded to two hydrogen atoms and to the carbon skeleton.
Organic compounds with this functional group are called amines. An example is glycine, illustrated in TABLE 4.1.
Because glycine also has a carboxyl group, it is both an amine and a carboxylic acid. Most of the cell’s organic
compounds have two or more different functional groups. Glycine and similar compounds having both amino and
carboxyl groups are called amino acids; these are the molecular building blocks of proteins.
Glycine
The amino group acts as a base. You learned in Chapter 3 that
ammonia (NH3) can pick up a proton from the surrounding
solution. Amino groups of organic compounds can do the
same:
This process gives the amino group a charge of +1, its most
common state within the cell.
The Sulfhydryl Group
Sulfur is directly below oxygen in the periodic table; both have 6 valence electrons and form two covalent bonds.
The organic functional group known as the sulfhydryl group (--SH), which consists of a sulfur atom bonded to an
atom of hydrogen, resembles a hydroxyl group in shape (see TABLE 4.1). Organic compounds containing
sulfhydryls are called thiols. In Chapter 5, you will learn how sulfhydryl groups can interact to help stabilize the
intricate structure of a protein.
stabilizing
protein
structure
The Phosphate Group
Phosphate is an anion formed by dissociation of an inorganic acid called phosphoric acid (H3PO4). The loss of
hydrogen ions by dissociation leaves the phosphate with two negative charges. Organic compounds containing a
phosphate group (
) have a phosphate ion covalently attached by one of its oxygen atoms to the carbon
skeleton (see TABLE 4.1). One function of phosphate groups is the transfer of energy between organic molecules.
In Chapter 6, you will learn how cells harness the transfer of phosphate groups to perform work, such as the
contraction of muscle cells.
ATP
DNA
The chemical elements of life: a review
Living matter, as you have learned, consists mainly of carbon, oxygen, hydrogen, and nitrogen, with smaller
amounts of sulfur and phosphorus. These elements share the characteristic of forming strong covalent bonds, a
quality that is essential in the architecture of complex organic molecules. Of all these elements, carbon is the
virtuoso of the covalent bond. The chemical behavior of carbon makes it exceptionally versatile as a building block
in molecular architecture: It can form four covalent bonds, link together into intricate molecular skeletons, and join
with several other elements. The versatility of carbon makes possible the great diversity of organic molecules,
each with special properties that emerge from the unique arrangement of its carbon skeleton and the functional
groups appended to that skeleton. At the foundation of all biological diversity lies this variation at the molecular
level.
Now that we have examined the basic architectural principles of organic compounds, we can move on to the next
chapter, where we will explore the specific structures and functions of the large and complex molecules made by
living cells: carbohydrates, lipids, proteins, and nucleic acids.