Concepts of Biology (BIOL115) - Dr. S.G. Saupe (; Biology Department, College of St. Benedict/St. John's University, Collegeville, MN 56321

Introduction to General Chemistry

I.   Life is chemically unique. 
    This is one of the characteristics of life.  Recall that we can determine if something is, or was, alive simply by analyzing its elemental composition. 

    Imagine sampling atoms throughout the universe.  If you could do so, 91 out of 100 atoms (91%) sampled would be hydrogen, 9.1% helium, 0.6 % oxygen, 0.04% nitrogen.  A similar study of materials in the earth's crust would give yield an elemental composition of: 47% oxygen, 28% silicon, 7.9% aluminum, and 4.5% iron.  Values for seawater:  H 66%, O 33%, Cl 0.33%, Na 0.3%.

    Now, consider an organism like a cat.  Place it in a blender, set the selector to puree, and then sample the atoms.  The approximate elemental composition would be:  63% hydrogen, 25.5% oxygen, 9.6% carbon and 1.4% nitrogen.  These four elements make up 95-99% of the elements in any organism.  In addition, there are approximately 20 other elements are also required by living organisms, but in relatively small amounts.   What can we conclude from our experiment with the pureed cat?

II.  What's so special about C, H, N, O?

  1. These elements occur in gaseous form, alone (nitrogen, oxygen, hydrogen) or combined (water vapor, carbon dioxide).  This allows for rapid biogeochemical cycling through the environment;
  2. Other elements are unsuitable for various reasons (i.e., radioactive such as plutonium and uranium, inert like argon and neon, too rare, too toxic like the heavy metals);
  3. C, H, N, O forms stable covalent bonds. (see III below);
  4. Carbon is uniquely "fit" (properties) for biological systems (see below) enabling it to serve as the backbone for biological molecules
  5. Water has unique properties (click here for notes on water).  The abundance of H & O in living organisms reflects the importance of water.

III.  A look at bonding.

A chemical bond is an attraction that occurs between atoms to forms aggregates (molecules).  The bonding ability (and chemical properties) of an atom is largely determined by the number of subatomic particles.

IV.  Life fractionates isotopes
This is another characteristic of life.  We expect organisms, such as plants, to have the same concentration of isotopes that exists in nature.  As it turns out, they don't - usually they have a lower isotopic concentration.  Thus, plants are able to discriminate against (fractionate) radioactive isotopes and absorb non-radioactive ones.

V.  Chemical Properties

The arrangement of the electrons in the atom ultimately determines the bonding ability and hence, chemical properties, of the element.  Points to consider:

Table 1:  Electron composition of the elements of life
Element Atomic # Electrons in Inner Shell Electrons in Outer Shell

Electrons required to fill outer shell (valence)

H 1 1 - 1
O 8 2 6 2
N 7 2 5 3
C 6 2 4 4

VI.  Covalent Bonds
    This is a bond formed by a pair of shared electrons.  Each pair of shared electrons are symbolized with a dash "-".  Covalent bonds can be: 

VII.  Ionic bonds
    Transfer of electron from one atom to another with a mutual attraction of the ions (charged).  Cations are positively charged, anions are negatively charged (remember � anion = N for negative).  e.g., Sodium (11Na) + chlorine (17Cl) = salt

VIII.  Hydrogen bonds. 
    Weak electrostatic attraction between a hydrogen covalently bound to an electronegative atom and another electronegative atom.  More on this during the water lecture.

IX.  The importance of covalent bonds

A.  Proper strength.  Covalent bonds are not too strong nor too weak. 

Table 2:  Comparison of bond types
Bond Type Bond energy (kJ mol-1)
Covalent 158 � 828

582 � 1004


8 - 42

B.  Covalent bonds are not disrupted in water (aqueous solution).  Think what would happen every time we showered if we were made of, say, salt.

C.  Allow a great diversity of chemical structures (i.e., single, double and triple bonds; various shapes including long chains, rings, and branches)

D.  Strength of covalent bond inversely related to atomic weight.  C,N,H,O are the lightest elements capable of forming covalent bonds - and thus they form the strongest covalent bonds.

X.  Why is carbon so special (fitness)
More different types of molecules are based on a carbon skeleton than any other element (molecule with carbon � called organic compound; no carbon � inorganic.  At one time chemists thought that carbon containing molecules could only be made by living things.  Louis Pasteur helped to disprove this idea).

     Why carbon?  (especially considering that silicon is 146x more abundant in the earth�s crust and has 4 unshared electrons just like carbon): 

  1. Each C can form covalent bonds to as many as 4 others.  Thus, it can make chains, rings, branches, etc.  Silicon can only make short chains; polymers of silicon are not stable in water

  2. Carbon can readily form double and triple bonds, silicon does not
  3. C � C covalent bonds are stronger and more stable than S � S bonds (because silicon is a larger atom) 
  4. C can combine with oxygen to form countless water soluble compounds.  For example, the simplest form is carbon dioxide which readily dissolves in water.  In contrast, silicon is insoluble in water.  When silicon combines with oxygen it forms silicates or polymers of silicon dioxide (quartz).  One reason that this is important is because it provides an easy way for carbon to enter and dissolve in cells for use of organisms.  It also permits carbon dioxide utilization in aquatic systems. 
  5. Carbon combines with oxygen to form a variety of compounds, many like carbon dioxide, are soluble in water. 
  6. Carbon has a tetrahedral configuration of bonds � permits 3D structures. This also accounts for the handedness observed in many biological molecules (check out the biological chem notes for more details).

Some scientists claim that hydrogen, because it is so plentiful, is the basic building block of the universe.  I dispute that.  I say that there is plenty more stupidity than hydrogen, and that is the basic building block of the universe.

      Frank Zappa (quoted in Discover)


| Top | SGS Home | CSB/SJU Home | Biology Dept | Biol115  Section Home Page | Concepts Home Page | Disclaimer |

Last updated: September 08, 2004     Visitors to this site:  Hit Counter
� Copyright by SG Saupe / URL: