Science of Ozone

THE SCIENCE OF OZONE

Ozone, though similar to oxygen chemically, is composed of three molecules of oxygen and is usually blue in color with a very strong odor. The atmosphere contains less ozone than the common oxygen. While out of every ten million air molecules, there exist about two million molecules of normal oxygen and only three molecules of ozone. Most of these ozone molecules are typically concentrated in the Stratosphere, the atmospheric layer that runs roughly from ten kms to about fifty kms in altitude. Even though the amount of ozone in the atmosphere is small, it plays a vital role in the atmosphere. The ozone layer protects the Earth and everything on it by absorbing the sun’s UV radiation. When the ozone is not at an atmospheric level and is at ground level, ozone proves to have toxic effects.

‘Inhaling fairly low amounts of ozone can result in signs and symptoms such as coughing, congestion, wheezing, shortness of breath, and chest pain in otherwise healthy people. People with already existing asthma, bronchitis, heart disease, and emphysema may find their conditions worsen while inhaling ozone. Breathing ozone may also increase the risk of getting certain lung diseases. People can recover from short-term exposure to low levels of ozone. However, breathing high levels of ozone or breathing low levels of ozone over a long period of time may have more damaging and longer-lasting effects.’ Ozone has also been found to have positive effects on people. It has proven to be a very purifying substance. Doctors are now aware that it has three powerful properties:

1. It stimulates the immune systems through production of natural cancer-killing proteins called cytokines.

2. It improves oxygenation (delivery of oxygen to starved tissues) and metabolism.

3. It is a powerful antibiotic when applied locally.

Ozone is made naturally in the atmosphere or artificially by using high voltages or ultraviolet rays. Ozone and Oxygen work together efficiently to prevent the ultraviolet radiations reaching the earth’s surface. The ultraviolet radiations with shorter wavelengths, such as wavelengths less than 242 nm, have sufficient energy to break the O-O covalent bonds in the oxygen molecules and are thereby used up by the oxygen molecules.

< 242 nm

O2 (g) ® 2O (g)

Similarly, ultraviolet radiations with higher wavelengths, for example more than 242 nm to 320 nm, are used up in breaking the bonds between the oxygen atoms in an Ozone molecule.

242-320 nm

O3 (g) ®