As indicated in our course introduction, much of Biology 101 emphasizes the
study of cells, which structurally and functionally are an aggregate of atoms
and molecules (chemicals) working together, and which require the energy
of these chemicals to stay alive and to function.
Atoms and molecules combine in various ways (to be discussed) to form the structures of the cells and tissues of which living organisms are composed, and provide the energy to sustain these cells and tissues.
In our first unit of lectures we will discuss the basic structure of atoms and molecules to help us understand the biological concepts that will follow in this course.
AtomsThere are 92 naturally occurring atoms on earth. We have about 108 total different kinds of atoms, because humans have been able to make atoms through nuclear reactions.
Each type of atom is composed of hundreds of smaller, subatomic particles, three of which we shall discuss. The proportion of these subatomic particles in any given atom identifies the kind of atom.
An element is a substance composed exclusively of one kind of atom. An element is a pure chemical that cannot be separated into or converted into a simpler substance. An atom is the smallest portion of an element that retains the properties of the element.
Each element (atom) has a name and a one- or two-letter abbreviation. The Periodic Table of Elements shows these, along with other useful information about each element. (See Appendix D of your Biology 101 Handbook.)
Although we have 92 different elements (formed from the 92 different kinds of atoms, there are just a few elements from which we are organized, and even fewer that are abundant in living organisms. We shall get acquainted with some of these.
The Arrangement and Properties of Atoms
Atoms are
composed of hundreds of smaller subatomic particles. Fortunately, to
understand Biology 101, we need only look at three of these basic particles,
which are located in two regions of the atom: the nucleus and the
surrounding electron orbitals. The "force" that holds these particles
"together" forming the atom is an electrical charge (positive and negative)
between subatomic particles.
The nucleus of an atom contains two sub-atomic particles: protons and neutrons. A third type of particle, electrons, are found in orbitals in motion surrounding the nucleus of the atom.
Let's look a little at the structure of the atom.
The Nucleus
Energy and Electrons
With reference to the energy of electrons, one
might think of electron orbitals and shells like stairs. Electrons can be raised
to a higher energy level with additional energy (climbing upstairs), and can
release energy when (if) they fall to a lower energy level (going down the
steps).
Electron Orbitals and the Stability of
Atoms
Generally there are two rules for finding electrons in orbitals
Again, there are a variety of possible energy levels (shells) for the electrons of an atom to occur in, and within each energy level, a set number of electron orbitals. The energy levels and orbital patterns are specific characteristics of each type of atom, and are best left to chemistry classes for detailed discussion. But we can have a little lesson.
Electrons fill lower energy level shells first, and then progress to higher shells.
As we look at a hypothetical atom, the electron fill pattern would be:
Shell | Orbital(s) | #Electrons |
1st | (1)2 one | 2 |
2nd | (2)2 four | 8 |
3rd | (3)2 nine | 18 |
Interactions Between Atoms
The nucleus of the atom tends to provide
stability, while electron shells permit interactions between atoms, called
bonds. Nuclei of atoms are not affected by normal energy sources, whereas
electrons are dynamic; bonds form when electrons from one atom are gained, lost
or shared with other atoms. Such interactions are called chemical bonds.
When two or more atoms join together in a chemical bond they form a molecule. Chemical bonds are interactions that occur between the outermost energy level electrons of different atoms, details to follow. When molecules are formed from different atoms, they form a compound.
As mentioned, different electron orbitals have patterns which are unique and identified by shape. Further, an atom is most stable when its electron shells have pairs of electrons in each of the orbitals, and when the orbitals of its outermost energy level are filled.
Atoms that naturally have filled outer energy level orbitals are non-reactive and are found in nature as pure elements. (The noble gases were named that way because they were always found in the pure element state. It is not coincidence that the noble gases have filled outer energy levels.) Most of the atoms naturally have numbers of electrons that do not result in filled outer energy level orbitals. These atoms are not stable and tend to undergo chemical reactions, or bonding, with other atoms to form molecules or compounds, which are more stable. Atoms that have similar electron configurations have similar properties and undergo similar chemical bonding. (The periodic table is organized according to these similar properties.)
By the way, there are some nice "rules" which help determine how an atom will bond. One of these is the octet rule. When the outer energy level of an atom has a total of 8 electrons it is especially stable, so most bonds take place to obtain eight electrons in the outer energy level.
Chemical Bonding
When an atom lacks a stable number of
electrons In its outer energy level, it will share or transfer electrons to or
from other atoms in very precise ways to achieve a stable number of electrons
(again, generally 8) in its outer shell. This is the subject of chemical
bonding. Note that a chemical bond is an energy relationship, involving
electrons, and the energy that each electron has
The energy all living organisms need to sustain life comes from making and breaking chemical bonds. ItŐs vital that we understand how this works!
Types of Bonds
There are two types of common or strong
bonds that occur between atoms:
Ionic bonds
One or more electrons are transferred from one atom to
a second atom.
When an atom gains or loses one or more electrons, it becomes a charged atom, or an ion, because its number of electrons relative to the number of protons has changed.
Covalent bonds
Electron(s) of one atom are shared with
electron(s) of a second atom.
Atoms that form covalent bonds do not carry a charge.
Ionic Bonds
An atom which has 1 or maybe 2 electrons in its
outermost energy level (shell) may donate (give up) these electrons, which
results in an outer energy layer with full orbitals.
This action results in an atom with more protons than electrons, which
results in a charged atom, an ion.
Example: Na11p 11e
---> Na11p 10e = Na (+11) ion
A second atom may
have 7 electrons in its outer shell, and may take on a donated electron to
complete its orbitals.
This too, produces a charged atom, or ion, but now one
which is negatively charged.
Example: Cl17p 17e --->
Cl17p 18e = Cl (-1) ion
The bond which forms then
occurs between the charges of the respective ions. This bond is
called the ionic bond .
Ions can be formed from atoms:
Na+, Cl-, or from molecules: CO33=,
NH4+
Covalent Bonds
The major elements found in living organisms,
carbon, hydrogen, oxygen, and nitrogen, tend to form covalent
bonds. Our carbohydrates, proteins, lipids and genetic molecules are formed from
these elements, as are the vitamins needed for living organisms. The exception
to covalent bonding in the compounds found in living organisms are the minerals,
or salts, which form ionic bonds.
Covalent Bond Characteristics
Electronegativity and Polar and Non-Polar Bonds
As stated, in a
covalent bond, the electrons of the bonding atoms are shared rather than
transferred, so that no charged atoms or ions are formed. We also mentioned that
atoms tend to form covalent bonds when a transfer of electrons would result in
too great of a charge imbalance between the atom's positively charged nucleus
and it's negatively charged electron field. All atoms, however, have a property,
called electronegativity, which is a measure of how strongly the protons
of the atom's nucleus attract and hold electrons. The electronegativity of all
atoms is not the same.
Atoms that form ionic bonds typically have a reasonably high electronegativity. When covalent bonds are formed between atoms which have similar electronegativity, the electrons of the atoms are equally shared and the bond is said to be nonpolar (with no charge attraction).
When covalent compounds are formed between atoms which have very different electronegativities, the electrons of the two atoms are not shared equally. The electrons that are spinning around both atoms will be attracted to the atom which has the stronger electronegativity, so that the electrons spend more time closer to the nucleus of that atom than in the field of the atom with a weaker electronegativity.
A compound (or molecule) formed by the unequal sharing will have one end functionally slightly negative (the end with the atom having a strong attraction for electrons) and the other end of the molecule slightly positive, resulting in a polar covalent bond and molecule.
These slightly charged polar covalent molecules are attracted to other polar
molecules (+ attracts -) and form very weak polar bonds. These bonds are weak
because the charges are weak and because the electrons are always in motion.
(Some of the time anyway, the end which is primarily positive will have the
electrons spinning there and lose its polarity for that instant.) The bond that
forms between adjacent polar covalent molecules is called a Hydrogen
bond.
Hydrogen Bonding
Other Weak Bonds
Hydrophilic (polar) and Hydrophobic (non-polar)
molecules separate from each other in aqueous solutions because water is a polar
molecule, and water molecules are attracted to other polar substances and
repelled by non-polar molecules. Likewise, non-polar molecules are attracted to
other non-polar substances and repelled by polar molecules. (Oil and water truly
do not mix.)
The hydrophobic interactions of non-polar molecules in solution are reinforced by very weak interactions called van der Waals forces. These interactions are the result of electron motions and the brief attraction a polar molecule will have for another atom's electrons when adjacent to it. This attraction causes a brief charge reaction between the two molecules
Water and Life on Earth
As we know, life on earth is
based on the substance, water. Water is the most abundant compound found
in living organisms (about 80%).
We have just seen that polar and non-polar molecules act differently in water. We have seen too, that water is one of the polar covalent molecules, and hydrogen bonds form between adjacent water molecules.
Lets look now at some properties of water, especially as these properties relate to water's polar nature and the phenomenon of hydrogen bonding.
Properties of Water
Solvent
Properties
Water in Biochemical Reactions
Base or alkaline substance
A substance which combines
with H+ in solution
A substance which donates OH- to
solution
Salt