corrosion

Most metals in their refined form (except for a few noble metals such as gold) are inherently unstable. The tendency of refined metals to revert to their natural mineral states is a driving force behind corrosion processes.

There are a number of different types of corrosion, including:

• General or overall corrosion: a uniform attack over the entire exposed area of a surface across a wide range of temperatures.
• Pitting corrosion: high localized corrosion rates with little or no general corrosion to the areas surrounding the pits.
• Galvanic corrosion: when two dissimilar metals are electrically connected in the presence of an electrolyte, the more electrochemically active metal corrodes by giving up electrons and corrodes an increased rate.
• Microbiologically-induced corrosion (MIC): Microorganisms form colonies on surfaces, leading to corrosive conditions.
• Stress-corrosion cracking (SCC): when a stressed metal is exposed to certain types of environments it may become susceptible to stress-corrosion cracking at stress levels that may be significantly below the yield strength of the material.

galvanic corrosion

Galvanic corrosion is a form of electrochemical corrosion that occurs when two dissimilar metals in the presence of an electrolyte form an electrical circuit, known as a galvanic cell.

In a galvanic cell, an exchange of electrons takes place, that causes one of the metals to corrode at an accelerated rate (compared to its corrosion rate without the presence of the other metal). The active, corroding metal, called the "anode" gives up electrons to the less active, non-corroding metal called the "cathode". After the anode corrodes completely away, the cathode will again begin to corrode as reflected by its position in the Galvanic Series.

By preventing the attachment and proliferation of microbes, and stabilizing the dispersion of colloidal particles, the Zeta Rod eliminates two major sources of corrosion in water systems.