• NACE equips society to protect people, assets and
    the environment from the adverse effects of corrosion.

Corrosion Basics

Corrosion - A Natural but Controllable Process

By Gretchen A. Jacobson - Materials Performance Managing Editor

Corrosion is a naturally occurring phenomenon commonly defined as the deterioration of a material (usually a metal) that results from a chemical or electrochemical reaction with its environment.1 Like other natural hazards such as earthquakes or severe weather disturbances, corrosion can cause dangerous and expensive damage to everything from vehicles, home appliances, and water and wastewater systems to pipelines, bridges, and public buildings. Unlike weather-related disasters, however, there are time-proven methods to prevent and control corrosion that can reduce or eliminate its impact on public safety, the economy, and the environment.

The science of corrosion prevention and control is highly complex, exacerbated by the fact that corrosion takes many different forms and is affected by numerous outside factors. Corrosion professionals must understand the effects of environmental conditions such as soil resistivity, humidity, and exposure to salt water on various types of materials; the type of product to be processed, handled, or transported; required lifetime of the structure or component; proximity to corrosion-causing phenomena such as stray current from rail systems; appropriate mitigation methods; and other considerations before determining the specific corrosion problem and specifying an effective solution.

The first step in effective corrosion control, however, is to have a thorough knowledge of the various forms of corrosion, the mechanisms involved, how to detect them, and how and why they occur.2

Simply put, corrosion is the natural deterioration that results when a surface reacts with its environment. Different surfaces, environments and other factors add complexity to the equation.

corrosion 101

1. Corrosion Basics, An Introduction, L.S. Van Delinder, ed. (Houston, TX: NACE, 1984).
2. NACE International Basic Corrosion Course Handbook (Houston, TX: NACE, 2000).


Prevention and control requires consideration of many factors before determining specific problem and effective solution, including but not limited to:

  • Environmental conditions such as soil resistivity, humidity and exposure to salt water on various types of materials
  • type of product to be processed, handled or transported
  • required lifetime of structure or component
  • proximity to corrosion-causing phenomena such as stray current from rail systems
  • appropriate mitigation methods

Ten Basic Forms

There are 10 primary forms of corrosion, but it is rare that a corroding structure or component will suffer from only one. The combination of metals used in a system and the wide range of environments encountered often cause more than one type of attack. Even a single alloy can suffer corrosion from more than one form depending on its exposure to different environments at different points within a system.

All forms of corrosion, with the exception of some types of high-temperature corrosion, occur through the action of the electrochemical cell (Figure 1). The elements that are common to all corrosion cells are an anode where oxidation and metal loss occur, a cathode where reduction and protective effects occur, metallic and electrolytic paths between the anode and cathode through which electronic and ionic current flows, and a potential difference that drives the cell. The driving potential may be the result of differences between the characteristics of dissimilar metals, surface conditions, and the environment, including chemical concentrations. There are specific mechanisms that cause each type of attack, different ways of measuring and predicting them, and various methods that can be used to control corrosion in each of its forms.

CPFigure1 Figure 1: Electrochemical Cell
In a corrosion cell, electrons flow through a metallic path from sites where anodic reactions are occurring to sites where they allow cathodic reactions to occur. Ions (charged particles) flow through the electrolyte to balance the flow of electrons. Anions (negatively charged ions from cathodic reactions) flow toward the anode and cations (positively charged ions from the anode itself) flow toward the cathode. The anode corrodes and the cathode does not. There is also a voltage, or potential, difference between the anode and cathode. Source: NACE International Basic Corrosion Course Handbook, p. 2:9.   

General attack corrosion  


Group 1 - readily identifiable by ordinary visual examination

Group 2 - may require supplementary means of examination

Group 3 - verification is usually required by microscopy (optical, electron microscopy etc.)


Common Methods of Control