Introduction
Ecological Structures
Biodiversity
Life and the Earth's Environment
What is Life?
Materials for Life
Capturing Energy for Life
Evolution & the Environment
Disruptive Forces on Ecosystems
Measurement of Impact on Ecosystems
Sustainability & Ecological Integrity
Approaches to the Natural Environment
Global and Regional Scales
Global Agreements
Philosophies for Sustainability
Exercises
Internet Links
Other Resources
Ecological System PDF
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Ecological System
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Materials for Life

Carbon, hydrogen, oxygen, nitrogen, phosphorus, and calcium form the major chemical scaffolding of biological molecules. Hydrogen, nitrogen, oxygen, phosphorus, and sulfur combined with carbon generated the first group of compounds that eventually formed the chemical basis of life. Other elements, such as iron, magnesium, sodium, potassium, chlorine, and iodine also play specific and vital roles.

Hydrogen, oxygen, and carbon make up over 93% of the weight of the human body. Water is almost 80-90% by weight of all living organisms. Water has several physical and chemical properties that make it important in maintaining conditions fit for life on Earth.

Water
<student exercise on water?>
The large amount of water on the Earth's surface and the fact that at the average temperature over most of the Earth, water is in a liquid state, are both important to life. Water constitutes the largest fraction of most organisms.

If spread evenly over the Earth, the water present on Earth could form a layer about 2.5 km (1.6 miles) thick. Water has a high heat capacity. It can absorb quite a bit of heat (1 calorie for every gram for each degree rise in temperature) before its temperature rises significantly. This provides a moderating influence that prevents sudden rises in temperature, which could be damaging to live organisms. Water bodies on Earth work to moderate atmospheric temperature changes, and internal water helps organisms maintain temperature ranges.

Water also has a large latent heat of vaporization because a lot of energy is needed to break hydrogen bonds among water molecules. It takes a lot of heat to change liquid water to vapor--560 calories/gram. Thus organisms (plants and animals) can dissipate a lot of heat by having some of the water in them evaporate. For example, we are able to evaporate water from our body, as sweat, cooling the body because of the heat removed by the evaporating water.

Water has a high latent heat of fusion as well. Eighty calories are required to convert 1 gram of ice to water. In addition, because of the peculiarities of the hydrogen bond, ice is less dense than water. It rarely happens that a solid material is less dense than its liquid state. Ice also does not conduct heat well. The high latent heat, low heat conductivity, and low density of ice causes ice to float on water, keeping the warmer water sealed below the insulating ice layer on lakes and other bodies of water, and keeping the water habitable for aquatic life.

Water is a "universal" solvent. It is capable of dissolving a variety of materials. Salts dissolve in water to form ions because of the polar nature of the H2O molecule. As described in the Science Notes of the Energy System, water is a polar molecule. It has a positive and a negative end. The longer time spent by the covalent electrons near the oxygen atom makes the oxygen end negatively charged overall. Various ions play important roles especially in the conduction of nerve impulses. Balance of ionic flow across cell membranes (cell walls) are also an important mechanism of moving nutrients as well as in several other cell functions. <ornella animation?>

Finally, water vapor is one of the greenhouse gases that keeps the Earth's atmosphere at the temperatures suited to life.

Hydrogen
Many of the special properties of water come from hydrogen. The small size of the hydrogen atom makes it possible to fit into many more molecular configurations than a bigger atom can. Thus hydrogen can form numerous compounds. Hydrogen is light, so all hydrogen gas could have escaped the Earth's gravitational pull when the Earth was still very hot. However, its high chemical reactivity with nitrogen, oxygen, and carbon, and the abundance of these elements made it possible for the Earth to retain a large amount of hydrogen in combination with these elements as ammonia, water, and methane during the primitive days of the Earth.

Carbon
The carbon compounds that make up essential molecules such as proteins are described in the notes on biological molecules. Carbon is second only to hydrogen in the number of compounds it can form, oxygen being the third in this capability. Carbon can form more than 2500 compounds with hydrogen alone. The next elements that form most hydrides are boron and nitrogen; each of which can form only seven! The C-C bonds make possible a great variety of molecules with different chains and rings. C, H, and O combine together to from even a richer variety of compounds. The same number of atoms can yield completely different compound depending on the arraignment of atoms. For example, C can form butyl alcohol (the prefix butyl refers to four carbons) in two alternate forms with slightly different but similar properties.

 
Butyl Alcohol 1
Butyl Alcohol 2

 

The -OH group is the hallmark group of an alcohol. These same number of atoms could also form an ether characterized by the -O- bond between carbon groups. Thus these atoms can form diethyl ether, two ethyl (C2H5) groups bridged by O, as in:

Diethyl Ether

For much larger molecules with many C atoms, the possible arrangements become very large. Recall that carbon is the middle element in the first period of the Periodic Table. It has four electrons (1s22s22p2) in the outer shell, needing four more to complete the outer shell. This capacity to form four covalent bonds makes for the capability of carbon to form compounds. The four bonding electrons and various spatial arrangements give carbon its enormous versatility.

This versatility and the fact that carbon dioxide is a gas at ordinary temperatures are two important aspects in carbon being the chemical basis of life. Photosynthesis occurs because CO2 is a gas and is soluble in H2O, so that this mixture, with energy from the violet part of sunlight, can form sugars.

The versatility of carbon comes from its central position in the periodic table. People have conjectured why silicon in an analogous position and, being one of the most plentiful elements in the Earth's crust, did not become that centerpiece. SiO2 is found in the solid form in plenty--as sand. But it becomes a gas at only 3000°, and it is not soluble in water. The chemical versatility of silicon is indeed the property we value for its use for computers.

Oxygen
With carbon and hydrogen, oxygen forms the third principal element in living systems. As we see later in this unit, our atmosphere was not always oxygen-rich. About 2000 million years ago, there was only about 0.0001% oxygen in the atmosphere. During the Archean and Proterozoic ages (when plants started to use photosynthesis), there was a radical increase of the O2 concentration to the almost 20% that it is today. This resulted in a major extinction of some bacteria as discussed in a later section.

As silicon is to carbon, so is sulfur to oxygen. So we could imagine a material and life configuration where H2S instead of H2O was the basic "liquid" of life. (H2S is actually a gas at Earth's average temperatures.) However the H-O bond is stronger than the H-S, and oxygen is 50 times more plentiful on Earth than sulfur. There are some organisms that use sulfur. This is discussed in the section on photosynthesis.

Other Elements
The other elements that play a vital role in living systems are N, Ca, P, Na, Fe, K, Cl, S, Zn, and Mg. Together these form about 1.72 atomic percent of the human body. Along with H, O, and C, these elements account for 99.96% of the human body. Lighter elements dominate this list and these elements have more specific roles in the function of biological molecules than the more general C, O, and H trio.

Nitrogen and sulfur are components of all proteins. Phosphorus is an essential component for the storage and use of energy in all cells. Cellular energy resides in phosphate bonds. Mg is a central component of chlorophyll, and iron is a component of hemoglobin and other respiratory enzymes. These elements serve very specialized but important functions.

Metals such as Fe and Na are rare in the body but play important roles either in very specific molecules as Fe in hemoglobin, Zn in gene transcription proteins, or Mg in chlorophyll; or with a specific function such as Na or K ions providing the flow of ions for conduction of information along nerves. Most metals, however, are toxic to most organisms. Examples of metal toxicity that have become significant environmental problems in the last half-century are cases of lead poisoning, mercury poisoning (Minamata disease), and poisoning by metals such as chromium (Cr), aluminum (Al), and cadmium (Cd). The amounts of chromium and cadmium in the environment have increased due to numerous technological uses ranging from steel production to household batteries.

 

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  ©Copyright 2003 Carnegie Mellon University
This material is based upon work supported by the National Science Foundation under Grant Number 9653194. Any opinions, findings, and conclusions or recommendations expressed in this material are those of the authors and do not necessarily reflect the views of the National Science Foundation.