We have discussed some of the molecules of living organisms (carbohydrates, lipids, proteins, etc.) in the context of the functions they perform in cells and tissues. We have also looked at the structure of cells, and the types of organelles found in typical cells. We know that some of our molecules are used to provide fuel, or energy for living organisms. We know too, that this form of energy cells use is chemical energy, the energy of the electrons of atoms.
Before discussing the metabolic reactions that occur in cells, we need to discuss a few things about energy flow in cells and how cells control their metabolic reactions. The purpose of this chapter is to look at the physical laws which govern energy flow, how energy flow relates to chemical reactions and how living organisms can control the chemical reactions that occur in their cells and tissues. Much of this is the stuff of chemistry and physics, but it applies to how our cells stay alive, so we are interested, too.
Some definitions first:
Energy
Energy is often defined as the capacity to do
work. The two fundamental types of energy are kinetic (energy at work, or
the movement of energy) and potential (stored energy waiting to do work,
such as the energy in the bonds of chemicals).
Both kinetic and potential energy can be found in many forms: electrical, light, chemical, heat, and mechanical. Under the right conditions, energy can be transformed from one type to another and from one form to another. This is a good thing, since different kinds of work require different kinds of energy, and as it applies to us, is often thought of as energy flow. Without this, we would have no life on earth. To make sense of this we have to understand both the quantity of energy available and the usefulness of that energy to do work.
Like everything else, energy transformations follow rules -- or laws, in this case the Laws of Thermodynamics (Thermodynamics is the field that studies energy transformations). There are two laws: one that addresses the quantity of available energy and the second which addresses the usefulness or availability of energy to do work.
The Two Laws of Thermodynamics The First Law of Thermodynamics states the amount of energy in any process is constant, meaning that energy can neither be created nor destroyed by ordinary processes. (But energy can be converted from one form to another and between potential and kinetic). The first law of thermodynamics is sometimes called the "law of conservation of energy".
When we apply this law to living organisms (or any system) we say that the total amount of energy of a system and its surroundings remains constant, because energy transformations occur constantly. With each transformation within any system (such as the cells of your body) some energy escapes to the surroundings as heat energy.
The Second Law of Thermodynamics says something like "the
amount of useful energy decreases when energy transformations occur", which
means there is a tendency for all systems to reach the lowest possible energy.
This is the famous entropy law. Entropy is the measure of the amount of
disorder (loss of higher level energy) in a system. Useful is the
critical term here. The amount of energy doesn't change, but the ability of that
energy to do the work we need accomplished diminishes.
To give an
example, Apple trees trap light waves of solar radiation in the process of
photosynthesis. They use the photosynthetic products to provide energy to
maintain their cells and tissues and to produce apple fruits. Apple trees are
maintaining their organized structure (and function) by obtaining "fresh" energy
through photosynthesis.
Plants, in this case the apples, then lose their energy to the organisms which feed on them - or - speaking plainly: An apple becomes seriously disordered as it passes through your digestive system as you process it for nutrients to maintain the organization of your cells.
This is a critical part of the second law of thermodynamics - order. Regions of concentrated energy, such as that found in the intact apple, tend to be more orderly than regions of more random energy, found in the individual molecules of the degraded apple in your intestine.
Laws of Thermodynamics, energy flow and chemical reactions
At
first, when we think of the Laws of Thermodynamics, we might think that life
canŐt exist if we must always put energy into a system to sustain it and if all
of the chemical reactions that occur in cells are increasing the amount of less
useful energy.
But life on earth relies on the sun. The sun constantly loses energy (the energy of sunlight) which is trapped by green plants on earth in the process of photosynthesis. Living organisms use the products of this to sustain their cells and tissues. We survive at the expense of the sunŐs increasing entropy. So we can see that while it might seem that we must violate some law of thermodynamics to have life on earth, we really donŐt.
Now that we've gotten the laws down, let's turn to energy flow and chemical reactions:
A chemical reaction takes one set of substances, called the reactants, (or sometimes, the substrate) and converts them to a different set of substances, called the products.
Some chemical reactions release energy -- the amount of energy in the products is less than that of the reactants. Such reactions are said to be exergonic.
One important exergonic reaction is the breaking of the bonds of the nucleotide, ATP (our "energy" molecule). ATP has three high-energy phosphate bonds. When ATP undergoes hydrolysis, the third phosphate bond is broken, releasing energy, which can then be used to do cell work. The chemical reactions of cellular respiration (from which we produce the ATP needed) are exergonic, as we shall see in a few days.
Some chemical reactions require or consume energy -- the amount of energy in the products is more than that of the reactants. Such reactions are said to be endergonic. The dehydration synthesis that forms the peptide bond between amino acids is an example of an endergonic chemical reaction.
Given enough time, an exergonic reaction can (and will) occur spontaneously. Endergonic reactions require energy from some other source in order to take place. In living organisms the source of this needed energy is usually ATP.
In addition, most chemical reactions are reversible; the direction they take depends on the concentration of the reactants versus the concentration of the products. Chemical equilibrium exists for many cell reactions, such as the binding of oxygen to hemoglobin for transport to cells and tissues, and release of the oxygen in cells.
How does energy flow apply to living organisms?
Keeping cells alive
takes work and requires energy. This energy comes from exergonic reactions
within the cells that provide the free energy to perform the endergonic
reactions needed to keep cells and tissues functioning. We refer to these paired
reactions as coupled reactions. ATP
For some reason, in order
for energy to be useful to do cell work, it must be in the form of ATP.
Cells do not directly use other forms of energy, so that the energy of chemical
fuel molecules must be transformed into ATP before cell work can be done. ATP is
then used to provide the energy to complete an endergonic chemical reaction.
The second and third phosphate bonds of ATP are unstable. When this phosphate bond is broken by hydrolysis, energy is released (an exergonic reaction). This released energy is just perfect for the amount of energy needed for many cell reactions. This is why we call ATP an energy carrier. It "carries" the energy needed to do the cell work.
The product of the hydrolysis of ATP is a molecule of ADP and a free phosphate molecule (Pi ). The endergonic process called cell respiration makes more ATP using energy obtained by "burning" or oxidizing fuel molecules, like glucose, to bond a "new" Phosphate (Pi ) to ADP. This is a constant process in cells. About 88 pounds of ATP is made and broken in 24 hours just for basic cell maintenance. And a cell has only about a one-minute supply of ATP at any given time. The unstable ATP cannot be "stockpiled". Keep in mind, however, that not all of that 88 pounds is useful energy. Much of the energy released when ATP is broken is in the form of less useful heat energy.
When you are transferring phosphates (Pi ) from one thing to another it's called phosphorylation, a good term to know.
There are a number of additional energy carrier molecules, which we will learn when we look more closely at cell metabolic processes such as photosynthesis and cell respiration. A few of the more important ones are NAD+, NADP+, FAD and the Cytochromes.
Controlling Chemical Reactions in our Cells and Tissues
The laws of
Thermodynamics that indicate the "natural" direction of any specific chemical
reaction is not enough for our cells to function. Many of our metabolic
reactions take place along pathways in a series of chemical reactions that must
be tightly regulated for our cells to function. Fortunately, our cells have a
number of means to regulate metabolism. We have mentioned two ways - coupled
reactions and energy-carrier molecules. A third way cells regulate chemical
reactions is by using enzymes, protein catalysts.
To summarize:
Chemical Reactions, Enzymes and Enzyme Function
Activation
Energy
For any chemical reaction to get started, the reactants must come
together at the right bonding place at the right time. No matter how
"spontaneous" a chemical reaction is, some energy is needed to get the reaction
started. This energy is called the activation energy. The activation
energy is anything that increases the rate at which the reactants collide (or
come together).
Remember that all atoms and molecules are in motion, so at some time, it is possible that the reactants will come together randomly. Unfortunately, the rate of a chemical reaction at normal earth temperatures may be so slow that it is imperceptible.
Hence we use catalysts, substances which can speed the rate of chemical reactions, by lowering the activation energy. It is important to know that the catalyst is not part of the chemical reaction. It is neither a reactant nor a product. A catalyst facilitates the reaction. In living organisms, we use a special class of catalysts, called enzymes.
Note: Activation energy is separate from the energy input needed to sustain endergonic reactions. Any endergonic reaction needs energy added to it to keep it going, along with getting it started.
Characteristics of Catalysts
How do Enzymes Function as Catalysts?
Enzymes are almost always
globular proteins with a place on the surface where the enzyme can bind to the
reactant(s). This "notch" is the active site, comprised of just a few
amino acids. The remainder of the enzyme helps to maintain the integrity of the
active site. The active site has a precise size, shape, and electrical charge
that exactly complements the reactant(s) or substrate(s). Enzymes are
highly specific. Each chemical reaction that occurs in cells has its own enzyme.
Enzyme shape determines its function.
When a substrate binds to the enzyme, it "fits" into the active site, temporarily distorting the reacting molecules, which is called the induced fit. This distorted stage of the substrate is called the transition state and its bonds are more easily broken (lowered activation energy), promoting the reaction. Once the reaction occurs, the active site is altered, releasing the product. The enzyme is unaffected by the reaction.
In some cases, a substance can fit into the active site but does not have the chemical bonds that the enzyme acts on, so the substance just sits on the enzyme, blocking any further enzyme activity. Such substances are enzyme inhibitors. Some poisons work in such a manor.
Enzymes and Their Environment - Enzyme Regulation
Enzyme activity
is controlled by conditions of its environment. Each enzyme works at precise pH,
temperature and chemical conditions, such as the amount of sodium ions in the
cell. Some enzymes can only work when they have associate molecules, called
coenzymes or cofactors present. Many of our vitamins function as coenzymes, and
some of our minerals, notably zinc, copper and iron, function as cofactors.
Other metals may interfere with enzyme function. Mercury, for example, inhibits
the function of many enzymes, partly by blocking the attachment of the needed
cofactor.
Enzyme regulation is a natural part of how cells function.
Homeostasis in cells and organisms involves elaborate feedback mechanisms. They
are essential for control of metabolism and the orderly operation of cells. Many
of these metabolic controls work by activating or de-activating enzymes at
appropriate times. This is the subject of enzyme regulation.
Enzyme Regulation
Allosteric Regulation
Some enzymes have molecules that bind to the
enzyme at a specific receptor site changing its shape. Such molecules can either
inhibit the enzyme when they attach or activate the enzyme when they attach.
Such molecules are said to be allosteric regulators and the receptor site
is an allosteric site.
Competitive Inhibition
Some enzyme inhibitors compete with the
substrate for the enzyme's active site and wind up blocking the active site
since they do not undergo a chemical reaction and get released from the enzyme.
Substances that compete for the enzyme's active site are called
competitive inhibitors. Your textbook gives the example of the
competition of methanol and ethanol for the active site on the enzyme alcohol
dehydrogenase.
You might note that substances that bind to the enzyme at some other place changing its shape so it can no longer function effectively are called non-competitive inhibitors. A number of poisons block enzyme activity in this way. Many pesticides block essential nervous system enzymes. Mercury inhibits the function of many enzymes, partly by blocking the attachment of the needed cofactor.
Some Vocabulary Review
Endergonic