Organic compounds typically consist of groups of carbon atoms covalently bonded to hydrogen, oxygen, and often other elements as well. Created by living things, they are found throughout the world, in soils and seas, commercial products, and in every cell of the human body. The four types most important to human structure and function are carbohydrates, lipids, proteins, and nucleotides. Before exploring these compounds, it is essential to first understand the chemistry of carbon.

Part 1: The Chemistry of Carbon

What makes organic compounds ubiquitous is the chemistry of their carbon core. Recall that carbon atoms have four electrons in their valence shell and that the octet rule dictates that atoms tend to react in such a way as to complete their valence shell with eight electrons. Carbon atoms do not complete their valence shells by donating or accepting four electrons. Instead, they readily share electrons via covalent bonds.

Commonly, carbon atoms share with other carbon atoms, often forming a long carbon chain referred to as a carbon skeleton. It is also possible for carbon atoms to form more than one covalent bond with one another and can form double bonds and triple bonds.

In organic compounds, carbon atoms can be found to share electrons with hydrogen. Carbon and hydrogen groupings are called hydrocarbons. If you study the figures of organic compounds in the remainder of this chapter, you will see several with chains of hydrocarbons in one region of the compound.

Carbon may share electrons with oxygen or nitrogen or other atoms in a particular region of an organic compound. Moreover, the atoms to which carbon atoms bond may also be part of a functional group. A functional group is a group of atoms linked by strong covalent bonds and tending to function in chemical reactions as a single unit. You can think of functional groups as tightly knit “cliques” whose members are unlikely to be parted. Five functional groups are important in human physiology; these are the hydroxyl, carboxyl, amino, methyl, and phosphate groups (Table 5.1).

Table 5.1: Functional Groups Important in Human Physiology

Functional Group	Chemical Formula	Importance
Hydroxyl	-OH	Polar group. Components of all four major classes of organic compounds discussed in this chapter.  Involved in dehydration synthesis and hydrolysis reactions and hydrogen bonding.
Carboxyl	-COOH	A component of the organic acids discussed in this chapter.
Amino	-NH2	A component of all amino acids.
Methyl	-CH3	A component of all fatty acids.
Phosphate	-PO42-	A component of all phospholipids and nucleotides.

Carbon’s affinity for covalent bonding means that many distinct and relatively stable organic molecules nevertheless readily form larger, more complex molecules. Any large molecule is referred to as a  macromolecule (macro- = “large”), and the organic compounds in this section all fit this description. However, some macromolecules are made up of several “copies” of single units called monomers (mono- = “one”; -mer = “part”). Like beads in a long necklace, these monomers link by covalent bonds to form long polymers (poly- = “many”). There are many examples of monomers and polymers among the organic compounds.

Monomers form polymers by engaging in dehydration synthesis (Figure 5.1). As was noted earlier, this reaction results in the release of a molecule of water. Each monomer contributes. One monomer donates a hydrogen atom (H), and the other donates a hydroxyl group (OH). Polymers are split into monomers by hydrolysis (-lysis = “rupture”). The bonds between their monomers are broken via the donation of a molecule of water, which contributes a hydrogen atom to one monomer and a hydroxyl group to the other.

 

Part 2: Carbohydrates

A carbohydrate is a molecule composed of carbon, hydrogen, and oxygen. In most carbohydrates, hydrogen and oxygen are found in the same two-to-one relative proportions they have in water. In fact, the chemical formula for a “generic” molecule of carbohydrate is (CH₂O)_n. The structure also contains several hydroxyl groups, which makes carbohydrates polar in terms of chemical nature.

Carbohydrates are also referred to as saccharides, a word meaning “sugars.” Three forms are important in the body. Monosaccharides are the monomers of carbohydrates. Disaccharide (di- = “two”) are made up of two monomers. Polysaccharides are the polymers and can consist of hundreds to thousands of monomers.

Monosaccharides

A monosaccharide is a monomer of carbohydrates. Five monosaccharides are important in the body. Three of these are the hexose sugars, so called because they each contain six atoms of carbon. These are glucose, fructose, and galactose (Figure 5.1a). The remaining monosaccharides are the two pentose sugars, each of which contains five atoms of carbon: ribose and deoxyribose (Figure 5.1b).

Disaccharides

A disaccharide is a linked pair of monosaccharides. Disaccharides are formed via dehydration synthesis, and the bond linking them is referred to as a glycosidic bond (glyco- = “sugar”). Three disaccharides are important to humans. These are sucrose, commonly referred to as table sugar; lactose, or milk sugar; and maltose, or malt sugar (Figure 5.2). As you can tell from their common names, you often consume these in your diet; however, your body cannot use them in disaccharide form. Instead, in the digestive tract, they are split into their component monosaccharides via hydrolysis.

 

Polysaccharides

Polysaccharides can contain a few to a thousand or more monosaccharides. Three are important to the body (Figure 5.3):

• Starches are polymers of glucose. They occur in long chains called amylose or branched chains called amylopectin, both of which are stored in plant-based foods and are relatively easy to digest.
• Glycogen is also a polymer of glucose, but it is stored in the tissues of animals, especially in the muscles and liver. It is not considered a dietary carbohydrate because very little glycogen remains in animal tissues after slaughter.
• Cellulose, a polysaccharide made of glucose that is the primary component of the cell wall of green plants, is commonly referred to as “dietary fiber.” In humans, cellulose/fiber is not digestible; however, dietary fiber has many health benefits. It helps you feel full so you eat less, it promotes a healthy digestive tract, and a diet high in fiber is thought to reduce the risk of heart disease and possibly some forms of cancer.

Functions of Carbohydrates

The human body obtains carbohydrates from plant-based foods. Grains, fruits, legumes, and vegetables provide most of the carbohydrates in the human diet, although lactose is found in dairy products. Polysaccharides such as starch and various monosaccharides and disaccharides play a role as a primary energy source, especially glucose, which is the main monosaccharide used in the body. Short chains of saccharides can also be used to form the glycocalyx (described in a later unit). The body is capable of storing glucose in the form of the polysaccharide glycogen.

Finally, pentose sugars are critical structural components of ATP and the nucleotides that make up RNA and DNA.

 

Part 3: Lipids

A lipid is one of a highly diverse group of compounds made up mostly of hydrocarbons. The few oxygen atoms they contain are often at the periphery of the molecule. Their nonpolar hydrocarbons make most lipids hydrophobic. In water, lipids do not form a true solution, but they may form an emulsion, which is the term for a combination of solutions that do not mix well.

Triglycerides

A triglyceride is one of the most common dietary lipid groups and the type found most abundantly in body tissues. This compound, which is commonly referred to as a fat, is formed by covalent bonding between two types of molecules (Figure 5.4):

• A glycerol backbone consists of three carbon atoms, each bonded to a hydroxyl group.
• Three fatty acids, long chains of hydrocarbons with a carboxyl group and a methyl group at opposite ends, extend from each of the carbons of the glycerol. These hydrocarbon chains are formed with nonpolar covalent bonds, making them hydrophobic by nature.

Triglycerides form via dehydration synthesis. Glycerol gives up hydrogen atoms from its hydroxyl groups at each bond, and the carboxyl group on each fatty acid chain gives up a hydroxyl group. A total of three water molecules are thereby produced.

Fatty acid chains that have no carbon double bonds and therefore contain the maximum number of hydrogen atoms are called saturated fatty acids. These straight, rigid chains pack tightly together and are solid or semi-solid at room temperature (Figure 5.5a). Butter and lard are examples, as is the fat found on a steak or in your own body. In contrast, fatty acids with one double carbon bond are kinked at that bond (Figure 5.5b). These monounsaturated fats are therefore unable to pack together tightly and are liquid at room temperature. Polyunsaturated fatty acids contain two or more double carbon bonds and are also liquid at room temperature. Plant oils such as olive oil typically contain both mono- and polyunsaturated fats.

 

As a group, triglycerides are a major fuel source for the body and are used when glucose storages are low or during extended fasting conditions. Triglycerides also fuel long, slow physical activity such as gardening or hiking and contribute a modest percentage of energy for vigorous physical activity. Dietary fat also assists the absorption and transport of the non-polar fat-soluble vitamins A, D, E, and K. Additionally, stored body fat protects and cushions the body’s bones and internal organs and acts as insulation to retain body heat.

Fatty acids are also components of glycolipids, which are sugar-fat compounds found in the cell membrane. Lipoproteins are compounds in which the hydrophobic triglycerides are packaged in protein envelopes for transport in body fluids.

Phospholipids

As its name suggests, a phospholipid is a molecule that contains a bond between the glycerol component of a lipid and a phosphate group. In fact, phospholipids are similar in structure to triglycerides. However, instead of having three fatty acids, a phospholipid is generated from a diglyceride, a glycerol with just two fatty acid chains (Figure 5.6). The third binding site on the glycerol is taken up by the phosphate group, which in turn is attached to a polar “head” region of the molecule. Recall that triglycerides are non-polar and hydrophobic. This still holds for the fatty acid portion of a phospholipid compound. However, the head of a phospholipid contains charges on the phosphate groups, as well as on the nitrogen atom. These charges make the phospholipid head hydrophilic. Therefore, phospholipids are said to have hydrophobic tails, containing the neutral fatty acids, and hydrophilic heads, containing the charged phosphate groups and nitrogen atom. Phospholipids form the phospholipid bilayer, which is the primary structural unit of cell membranes.

 

Steroids

A steroid compound (referred to as a sterol) has as its foundation a set of four hydrocarbon rings bonded to a variety of other atoms and molecules (see Figure 5.6b). Although both plants and animals synthesize sterols, the type that makes the most important contribution to human structure and function is cholesterol, which is synthesized by the liver in humans and animals and is also present in most animal-based foods. Like other lipids, cholesterol’s hydrocarbons make it hydrophobic; however, it has a polar hydroxyl head that is hydrophilic. Cholesterol is an important component of bile, a compound that helps emulsify dietary fats. Cholesterol is also a building block of many hormones, signaling molecules that the body releases to regulate processes at distant sites.

 

 

Part 4: Proteins

You might associate proteins with muscle tissue, but in fact, proteins are critical components of all tissues and organs. A protein is an organic molecule composed of amino acids linked by peptide bonds. Proteins include keratin in the epidermis of skin that protects underlying tissues and collagen found in the dermis of skin, in bones, and in the meninges that cover the brain and spinal cord. Proteins are also components of many of the body’s functional chemicals, including digestive enzymes in the digestive tract, antibodies, the neurotransmitters that neurons use to communicate with other cells, and the peptide-based hormones such as growth hormone that regulate certain body functions.

Microstructure of Proteins

Proteins are polymers made up of nitrogen-containing monomers called amino acids. An amino acid is a molecule composed of an amino group and a carboxyl group, together with a variable side chain. Just 20 different standard amino acids contribute to nearly all of the thousands of different proteins important in human structure and function. Body proteins contain a unique combination of a few dozen to a few hundred of these 20 amino acid monomers. All 20 of these amino acids share a similar structure (Figure 5.7). All consist of a central carbon atom to which the following are bonded:

• a hydrogen atom
• an alkaline (basic) amino group NH₂ (see Table 5.1)
• an acidic carboxyl group COOH (see Table 5.1)
• a variable group

Notice that all amino acids contain both an acid (the carboxyl group) and a base (the amino group; amine = “nitrogen-containing”). What distinguishes the 20 amino acids from one another is their variable group, which is referred to as a side chain or an R-group. This group can vary in size and can be polar or nonpolar, giving each amino acid its unique characteristics.

Amino acids join via dehydration synthesis reactions to form protein polymers (Figure 5.8). The unique bond holding amino acids together is called a peptide bond. A peptide bond is a covalent bond between two amino acids that forms by dehydration synthesis. A peptide, in fact, is a very short chain of amino acids. Strands containing fewer than about 100 amino acids are generally referred to as polypeptides rather than proteins.

The body is able to synthesize most of the amino acids from components of other molecules; however, some cannot be synthesized and have to be consumed in the diet. These are known as the essential amino acids.

 

Shape of Proteins

A protein’s shape is essential to its function, which is fundamentally determined by the sequence of amino acids of which it is made (Figure 5.9a). The sequence is called the primary structure of the protein.

Although some polypeptides exist as linear chains, most are twisted or folded into more complex secondary structures that form when bonding occurs between amino acids with different properties at different regions of the polypeptide.

The secondary structure of proteins further folds into a compact three-dimensional shape, referred to as the protein’s tertiary structure (Figure 5.9c). Often, two or more separate polypeptides bond to form an even larger protein with a quaternary structure (Figure 9d). The polypeptide subunits forming a quaternary structure can be identical or different. For instance, hemoglobin, the protein found in red blood cells is composed of four tertiary polypeptides, two of which are called alpha chains and two of which are called beta chains.

 

Functions of Proteins

Proteins in the body have a variety of functions. Some proteins, such as actin and myosin, are used for movement, such as muscle cell contraction and intracellular transport. Some proteins are also used to provide a structural framework or mechanical support of connective tissues (e.g., collagen, keratin, elastin), individual cells (e.g., titin), and plasma membranes (e.g., spectrin, dystrophin). Some proteins called enzymes play a role in catalytic action (e.g., salivary amylase, etc.) to speed up chemical reactions in the body.

Some proteins are used to transport specific molecules such as non-polar steroid hormones or gases in the blood. Hemoglobin contained in erythrocytes is used to transport both oxygen and carbon dioxide between the lungs and tissue cells. Others (e.g., albumin, hemoglobin) can help regulate body fluid pH by reversibly functioning as acids or bases, thus serving as buffers. Some protein hormones help to regulate cellular metabolism (e.g., insulin, growth hormone, oxytocin). Others are used to defend the body against foreign substances including invading pathogens and toxins (e.g., antibodies, complement proteins). Finally, some proteins known as molecular chaperones (e.g., heat-shock proteins) are essential to the production of other proteins and the appropriate breakdown of damaged proteins.

As was noted earlier, the basic and acidic components enable proteins to function as buffers in maintaining acid–base balance, but they also help regulate fluid–electrolyte balance. Proteins attract fluid, and a healthy concentration of proteins in the blood, the cells, and the spaces between cells helps ensure a balance of fluids in these various “compartments.” Moreover, proteins in the cell membrane help transport electrolytes in and out of the cell, keeping these ions in a healthy balance. Like lipids, proteins can bind with carbohydrates. They can thereby produce glycoproteins or proteoglycans, which have numerous functions, including cell membrane integrity and the immune response.

The body can use proteins for energy when carbohydrate and fat intake is inadequate and stores of glycogen and adipose tissue become depleted. However, since there is no storage site for protein except functional tissues, using protein for energy causes tissue breakdown and results in body wasting.

 

 

Part 5: Nucleotides and Nucleic Acids

The fourth type of organic compound important to human structure and function are the nucleotides (Figure 5.12). A nucleotide is one of a class of organic compounds composed of three subunits:

• one or more phosphate groups
• a pentose sugar: either deoxyribose or ribose
• a nitrogen-containing base: adenine, cytosine, guanine, thymine, or uracil

Nucleotides can be assembled into nucleic acids (DNA or RNA) or the energy compound adenosine triphosphate.

Adenosine Triphosphate

The nucleotide ATP is composed of a ribose sugar, an adenine base, and three phosphate groups (Figure 5.10). ATP is classified as a high-energy compound because the covalent bonds linking its three phosphates store a significant amount of potential energy. In the body, the energy released from these high-energy bonds helps fuel the body’s activities, from muscle contraction to active transport and to anabolic chemical reactions.

When a phosphate group is cleaved from ATP, the products are adenosine diphosphate (ADP) and an inorganic phosphate (P_i). This hydrolysis reaction can be written:

ATP + H₂O → ADP + P_i + energy

Removal of a second phosphate leaves adenosine monophosphate (AMP) and two phosphate groups. Again, these reactions also liberate the energy that had been stored in the phosphate-phosphate bonds. They are reversible, too, as when ADP undergoes phosphorylation, which is the addition of a phosphate group to an organic compound, in this case, resulting in the formation of ATP.

 

Cells can also transfer a phosphate group from ATP to another organic compound. For example, when glucose first enters a cell, a phosphate group is transferred from ATP, forming glucose phosphate (C₆H₁₂O₆—P) and ADP. Once glucose is phosphorylated in this way, it can be stored as glycogen or metabolized for immediate energy.

Nucleic Acids

The nucleic acids differ in their type of pentose sugar. Deoxyribonucleic acid (DNA) is a nucleotide that stores genetic information. DNA contains deoxyribose plus one phosphate group and one nitrogen-containing base. The bases for DNA are adenine, cytosine, guanine, and thymine. Ribonucleic acid (RNA) is a ribose-containing nucleotide that helps express the genetic code as protein. RNA contains ribose, one phosphate group, and one nitrogen-containing base, but the bases for RNA are adenine, cytosine, guanine, and uracil (Figure 5.11).

Bonds formed by dehydration synthesis between the pentose sugar of one nucleic acid monomer and the phosphate group of another form a “backbone,” from which the components’ nitrogen-containing bases protrude. In DNA, two such backbones attach at their protruding bases via hydrogen bonds. These twist to form a shape known as a double helix (Figure 5.12). The sequence of nitrogen-containing bases within a strand of DNA form the genes that act as a molecular code, instructing cells in the assembly of amino acids into proteins. Humans have almost 22,000 genes in their DNA, stored within the 46 chromosomes inside the nucleus of each somatic cell (except red blood cells, which lose their nuclei during development). These genes contain the genetic code to build one’s body and are unique for each individual, with the exception of identical twins.

 

In contrast, RNA consists of a single strand of a sugar-phosphate backbone studded with nitrogenous bases. Messenger RNA (mRNA) is created during transcription to carry the genetic instructions from the DNA housed within the nucleus to the protein manufacturing organelles called ribosomes, located in the cell’s cytoplasm.

Watch this Amoeba Sisters video to learn more about biomolecules! Direct link: https://youtu.be/YO244P1e9QM