Cadmium (revised)

views updated May 14 2018


Note: This article, originally published in 1998, was updated in 2006 for the eBook edition.


Cadmium is a transition metal. The transition metals are the elements found in Rows 4 through 7 between Groups 2 and 13 in the periodic table, a chart that shows how elements are related. Cadmium was discovered by German chemist Friedrich Stromeyer (1776-1835) in 1817. It is found most commonly in ores of zinc.

Cadmium is a soft metal that is easily cut with a knife. It resembles zinc in many of its physical and chemical properties. However, it is much less abundant in the Earth's crust than zinc.

By far the most important use of cadmium in the United States is in the production of nicad (nickel -cadmium), or rechargeable, batteries. It is also used in pigments, coatings and plating, manufacture of plastic products, and alloys. An alloy is made by melting and mixing two or more metals. The mixture has properties different from those of the individual metals.




Group 12 (IIB)
Transition metal


Caution must be used when handling cadmium and its compounds, as they are toxic to humans and animals. They present a threat to the environment because of their many applications.

Discovery and naming

In addition to being a professor at Göttingen University, Stromeyer was a government official responsible for inspecting pharmacies in the state of Hanover, Germany. On one inspection trip, he found that many pharmacies were stocking a compound of zinc called zinc carbonate (ZnCO3) instead of the usual zinc oxide (ZnO). Zinc oxide is still readily available in pharmacies today.

Stromeyer was told that the supplier had problems making zinc oxide from zinc carbonate and had offered the substitution. The normal process was to heat zinc carbonate to produce zinc oxide:

The supplier explained that zinc carbonate turned yellow when heated. Normally, a yellow color meant that iron was present as an impurity. The supplier found no iron in his zinc carbonate, but it was still yellow. Pharmacies would not buy yellow zinc oxide, so the supplier sold white zinc carbonate instead.

Stromeyer analyzed the odd yellow zinc carbonate. What he discovered was a new elementcadmium. The cadmium caused the zinc carbonate to turn yellow when heated. The name comes from the ancient term for zinc oxide, cadmia. Zinc oxide is still available in pharmacies today. It is sold under the name of calamine lotion. Calamine lotion is a popular remedy for stopping the itch of sunburn or bug bites.

Physical properties

Cadmium is a shiny metal with a bluish cast (shade) to it. It is very soft and can almost be scratched with a fingernail. Its melting point is 321°C (610°F) and its boiling point is 765°C(1,410°F). The density of cadmium is 8.65 grams per cubic centimeter.

An interesting property of cadmium is its effect in alloys. In combination with certain metals, it lowers the melting point. Some common low-melting-point alloys are Lichtenberg's metal, Abel's metal, Lipowitz' metal, Newton's metal, and Wood's metal.

Chemical properties

Cadmium reacts slowly with oxygen in moist air at room temperatures, forming cadmium oxide:

Cadmium does not react with water, though it reacts with most acids.

Occurrence in nature

The abundance of cadmium in the Earth's crust is estimated to be about 0.1 to 0.2 parts per million. It ranks in the lower 25 percent of the elements in terms of abundance in the earth.

The only important ore of cadmium is greenockite, or cadmium sulfide (CdS). Most cadmium is obtained as a by-product of zinc refinement.

The largest producers of cadmium in 1996 were Canada, Japan, Belgium, the United States, China, Kazakhstan, and Germany.


Eight naturally occurring isotopes of cadmium exist. They are cadmium-106, cadmium-108, cadmium-110, cadmium-111, cadmium-112, cadmium-113, cadmium-114, and cadmium-116. Isotopes are two or more forms of an element. Isotopes differ from each other according to their mass number. The number written to the right of the element's name is the mass number. The mass number represents the number of protons plus neutrons in the nucleus of an atom of the element. The number of protons determines the element, but the number of neutrons in the atom of any one element can vary. Each variation is an isotope.

About 20 radioactive isotopes of cadmium are known also. A radioactive isotope is one that breaks apart and gives off some form of radiation. Radioactive isotopes are produced when very small particles are fired at atoms. These particles stick in the atoms and make them radioactive.

One isotope of cadmium, cadmium-109, is sometimes used to analyze metal alloys. It provides a way of keeping track of the alloys in stock and sorting different forms of scrap metal from each other.


Most cadmium is obtained as a by-product from zinc refinement. Cadmium and zinc melt at different temperatures, providing one way of separating the two metals. As a liquid mixture of zinc and cadmium is cooled, zinc becomes a solid first. It can be removed from the mixture, leaving liquid cadmium behind.

Cadmium and fire sprinklers

A common low-melting-point cadmium alloy is Wood's metal. This alloy melts at 70°C (158°F), and is used in fire sprinkler systems as a plug. When the temperature rises above 70°C (158°F), the plug melts and falls out. This opens up the water line and activates the sprinkler. Out sprays the water!

Today, about 70 percent of cadmium produced worldwide is used in nickel-cadmium (nicad) batteries. Nicad batteries are rechargeable.


At one time, the most important use of cadmium was in the electroplating of steel. Electroplating is a process by which a thin layer of one metal is deposited on the surface of a second metal. An electric current is passed through a solution containing the coating metal. The metal is electrically deposited on the second metal. A thin layer of cadmium protects steel from corrosion (rusting).

In the last 30 years, the use of cadmium for electroplating has dropped by about 70 percent due to environmental concerns. Discarded electroplated steel puts cadmium into the environment. Alternative coating methods are usually used now.

Today, about 70 percent of cadmium produced worldwide is used in nickel-cadmium (nicad) batteries. Nicad batteries can be used over and over. When a nicad battery has lost some or all of its power, it is inserted into a unit that plugs into an electrical outlet. Electricity from the outlet recharges the battery.

Nicad batteries are used in a large variety of appliances, including compact disc players, cellular telephones, pocket recorders, handheld power tools, cordless telephones, Laptop computers, camcorders, and scanner radios. Two French automobile manufacturers are exploring the possibility of using nicad batteries in electric cars.


A popular use of cadmium compounds is as coloring agents. The two compounds most commonly used are cadmium sulfide (CdS) and cadmium selenide (CdSe). The sulfide is yellow, orange, or brown, while the selenide is red. These compounds are used to color paints and plastics. There is concern about possible environmental effects of using cadmium for this purpose. However, no satisfactory substitutes have been found.

Health effects

The major sources of cadmium in humans are cigarette smoking, certain foods (such as shellfish, liver and kidney meats), coal burning, and contaminated water. Those most at risk for high intake of cadmium are people who work directly with the metal. Manufacturing plants where batteries are made use cadmium as a fine powder where it can easily be inhaled. Workers must be careful in handling cadmium.

There is growing concern about the dangers of cadmium in the environment. Rechargeable batteries are made with cadmium and nickel. Cadmium can escape from landfills (where trash is buried) and get into the ground and groundwater. From there, it can become part of the food and water that humans and animals ingest.

Low levels of cadmium cause nausea, vomiting, and diarrhea. Inhaled, cadmium dust causes dryness of the throat, choking, headache, and pneumonia-like symptoms.

Manufacturing plants where batteries are made use cadmium as a fine powder where it can easily be inhaled. Workers must be careful in handling cadmium.

The effects of extensive cadmium exposure is not known, but are thought to include heart and kidney disease, high blood pressure, and cancer. A cadmium poisoning disease called itai-itai, Japanese for "ouch-ouch," causes aches and pains in the bones and joints. In the 1970s, a number of cases of itai-itai were reported in Japan when waste from a zinc refinery got into the public water supply. Those wastes contained cadmium compounds.

Cadmium Poisoning

views updated May 18 2018

Cadmium poisoning


Cadmium is a metal with an atomic weight of 112.41. In the Periodic Table of the Elements, cadmium is located between zinc and mercury. It is used in a large number of industrial applications. In the United States, over 10 million pounds of cadmium are used industrially every year.

The uses for cadmium include:

  • component of several metal alloys
  • component of solder (metallic cement), particularly solder for aluminum
  • electroplating
  • nickel plating
  • engraving
  • cadmium vapor lamps
  • nickel-cadmium batteries
  • treatment of parasites in pigs and poultry

Cadmium can be very toxic, and is dangerous if it is swallowed or inhaled. While spontaneous recovery from mild cadmium exposure is common, doses as low as 10 milligrams can cause symptoms of poisoning. There is no accepted fatal dose amount.


The symptoms of ingested cadmium poisoning are:

  • increased salivation
  • choking
  • vomiting
  • abdominal pain
  • anemia
  • painful spasms of the anal sphincter

When cadmium dust or powder is inhaled, the first symptoms are a sweet or metallic taste, followed by throat irritation. Other symptoms that may appear in three to five hours include:

  • dry throat
  • cough
  • headache
  • vomiting
  • chest pain
  • pulmonary edema , a congestive lung condition
  • bronchospasm, the abnormal tightening of airways that may be accompanied by wheezing and coughing
  • pneumonitis, inflammation of the lung
  • muscle weakness
  • leg pain

When a person has exposure to cadmium in low doses over a long period of time, symptoms may include loss of sense of smell, cough, shortness of breath, weight loss, and tooth staining. Chronic cadmium exposure may cause damage to the liver and kidneys.

Causes & symptoms

The most common cause of cadmium poisoning is a lack of proper precautions in places where cadmium is used. In such industries, air quality should be regularly monitored. Cadmium-plated containers should never be used to store acidic foods such as fruit juices or vinegar.

Fossil fuels, such as coal and oil, release cadmium fumes into the air. Chronic cadmium poisoning is also possible through soil or water contamination. This problem may occur with improper disposal of nickel-cadmium batteries used in items such as cameras. Cadmium poisoning has been associated with Itai-Itai disease in Japan.


Cadmium poisoning is usually diagnosed by its symptoms, particularly if there is reason to believe that the patient has been exposed to cadmium. Because patients may not request treatment for up to a day following cadmium exposure, diagnosticians should carefully question any patient who shows symptoms consistent with this condition.


Other than symptomatic treatment, there are no good options for dealing with cadmium poisoning. Hemodialysis may be used to remove circulating cadmium from the bloodstream, although the literature on the subject is scarce. Addition of a chelating agent, particularly ethylenediamine tetraacetic acid (EDTA), will increase the amount of cadmium removed by the dialysate (the fluid used in dialysis to carry substances to or remove from the kidney during hemodialysis).

These treatments are only effective for oral poisoning, and have no demonstrated benefit in cadmium fume inhalation.

Allopathic treatment

There are no generally accepted treatments for the acute effects of cadmium poisoning. Other than dialysis, dimercaptosuccinic acid (DMSA) (an oral chelating agent), has been recommended for removal of cadmium from the blood.

Expected results

The prognosis depends on the nature and severity of the cadmium load. Most cases of mild exposure resolve spontaneously after a few days. In other cases, cadmium can lead to permanent damage with shortened lifespan, or even death.

Cadmium may be carcinogenic.

Long-term exposure may also result in bone defects including osteoporosis .


All work done in areas where there may be cadmium fumes should be well ventilated. Ground water and soil should be checked for cadmium. Cadmium-coated containers should, in general, be avoided. They should never be used with acidic liquids such as fruit juices. Coal and oil-burning utilities should be monitored for cadmium discharge. Nickel-cadmium batteries should be recycled or disposed of as toxic waste.



Driesbach, R. M. Handbook of Poisoning. 7th ed. Lange, 1971.

Ford, M. D. Toxicology. 1st ed. Philadelphia, PA: W. B. Saunders, 2001.

Goldman, L., and J. C. Bennet. Cecil Textbook of Medicine. 21st ed. Philadelphia, PA: W. B. Saunders, 2000.

Murray J. F., and J.A. Nadel. Textbook of Respiratory Medicine. 3rd ed. Philadelphia, PA: W. B. Saunders Company, 2000.


Davis, R. D. "Cadmium - A Complex Environmental Problem. Part II. Cadmium in Sludges Used as Fertilizer." Experientia (February 15, 1984): 11726.


Canadian Centre for Occupational Health and Safety. 135 Hunter Street, East Hamilton, ON Canada L8N 1M5.

Samuel Uretsky, Pharm.D.


views updated May 11 2018


melting point: 320.9°C
boiling point: 767°C
density: 8.642 g/cm3
most common ions: Cd2+

Cadmium is a silver-white, malleable metal that exists as crystals having the hexagonal close-packed arrangement, and is usually found combined with other elements in mineral compounds (e.g., cadmium oxide, cadmium chloride, cadmium sulfate, and cadmium sulfide). Cadmium dust can ignite spontaneously in air and is both flammable and explosive when exposed to heat, flame, or oxidizing agents. Toxic fumes are emitted when cadmium metal is heated to high temperatures. Cadmium lacks a definite taste or odor. It was discovered as an impurity in zinc carbonate by Friedrich Strohmeyer in Germany in 1817. Most cadmium is obtained as a byproduct of the chemical treatment of copper, lead, and zinc ores, although it is a naturally occurring element in Earth's crust.

Industrial uses of cadmium include electroplating and the manufacture of batteries, metal coatings, and alloys . Cadmium is also used as a pigment in paints and plastics. Some fertilizers also contain cadmium.

Food and cigarette smoke are the most likely sources of cadmium exposure for the general population. The total daily intake of cadmium from food, water, and air for an adult living in North America or Europe is estimated to be between 10 and 40 micrograms (3.53 × 107 and 1.41 × 106 ounces). The U.S. Environmental Protection Agency has established oral reference doses for cadmium: 0.0005 mg/kg/day (from water) and 0.001mg/kg/day (from food). The reference dose is the level that may be consumed over a lifetime with minimal risk of adverse effects. Occupational exposure may occur in individuals who work with cadmium or in industries that produce cadmium. About 15 percent of inhaled cadmium is absorbed by the body, whereas 5 to 8 percent is absorbed from the gastrointestinal tract following cadmium ingestion. Cadmium is transported in the blood by hemoglobin, as well as by albumin and other large molecular weight proteins. The half-life for cadmium in the body is about thirty days, with most of the excess cadmium accumulating in the liver and kidneys. Cadmium is excreted primarily in the urine.

Acute toxicity may result from the ingestion of cadmium. Symptoms that follow cadmium ingestion may include abdominal pain, nausea, and vomiting; symptoms that follow inhalation include acute respiratory irritation and/or inflammation. Epidemiologic studies in humans have found associations between cadmium exposure and lung cancer, and between cadmium exposure and prostate cancer. Other evidence of the carcinogenic potential of cadmium has been found in the results of animal studies.

see also Toxicity.

Ronald Brecher


Agency for Toxic Substances and Disease Registry (ATSDR) (1999). Toxicological Profiles. Boca Raton, FL: CRC Press.

Klaassen, C. D., ed. (1996). Casarett and Doull's Toxicology: The Basic Science of Poisons, 5th edition. New York: McGraw-Hill.

Lide, D. R., ed. (2001). CRC Handbook of Chemistry and Physics, 82nd edition. Boca Raton, FL: CRC Press.

Lewis, R. J., ed. (1992). Sax's Dangerous Properties of Industrial Materials, 8th edition. New York: Van Nostrand Reinhold York.

Internet Resources

Integrated Risk Information System (IRIS), U.S. Environmental Protection Agency (USEPA). Available from <>.

Toxicology Data Network, National Library of Medicine. Hazardous Substances Data Bank (HSDB). Available from <>.

Web ElementsThe Periodic Table on the WWW:Professional Edition. Cadmium. Available from<>.


views updated May 17 2018

cadmium (symbol Cd) Silvery-white metallic element in group II of the periodic table, first isolated in 1817 by the German chemist Friedrich Stromeyer. Cadmium is mainly obtained as a by-product in the extraction of zinc and lead. Malleable and ductile, it is used in electroplating, as an absorber of neutrons in nuclear reactors, and in nickel-cadium batteries. Properties: 48; r.a.m. 112.4; r.d. 8.65; m.p. 320.9°C (609.6°F); b.p. 765°C (1409°F); most common isotope Cd114 (28.86%).


views updated May 21 2018

cad·mi·um / ˈkadmēəm/ • n. the chemical element of atomic number 48, a silvery-white metal. (Symbol: Cd)

About this article

Periodic Table of the Elements Cadmium

All Sources -
Updated Aug 24 2016 About content Print Topic


Periodic Table of the Elements Cadmium