Ozone: General Information

Ozone is an allotropic form of oxygen in which three atoms of this element are combined to generate the ozone molecule. It is a blue-hued gas, heavier than the air, with a strong, penetrating scent. In its diluted natural state, it is present in the great masses of oxygen in the atmosphere.

Ozone is considered one of nature’s most energetic oxidants, since its electrochemical potential is 2.07 V as opposed to chlorine gas’s 1.36 V. Specifically, it oxidizes organic structures very quickly, meaning that for some time it has been the most widely used disinfectant for potable waters in the world’s most developed countries.

Other characteristics:

Ozone is very effective as a disinfectant, having approximately double the oxidation capacity of chlorine. Dosage and contact times are generally smaller for ozone than for chlorine, yielding the same results.

In spite of being recognized disinfectants, chlorine and other halogens like bromine and iodine require considerable contact time in order to eliminate viruses and are not always effective. In addition, chlorine becomes combined with organic matter and forms cloramines, which are proven carcinogens. Cloramines and chlorine gases are highly toxic for most organisms.

Water disinfectant properties

Ozone has very energetic oxidating characteristics that can be used to degrade or to eliminate certain organic substances or indisociable minerals.

The oxidating action of ozone in water can be presented in three different forms:

• As an oxidant, setting one of its oxygen atoms. This action, although energetic, is not particular to ozone; an analogical effect can be obtained with other oxidants.
• As an oxidant setting its three oxygen atoms to a double or triple connection; they form Ozonids characterized by the existence of a ‘oxygen bridge’. These unstable compounds can ‘be unfolded chemically’ by the action of an excess of ozone and by a sufficient contact time (ozonolisis reaction).
• As catalyst of oxygen, accelerating the speed of the oxidation reactions at a low temperature. In this use, however, a certain amount contact time is required.