Iron
Common name
N/A
ID
HD0038
Scientific name of the plant
N/A
Anatomical part for use
N/A
Human use
Bodybuilding
Summary
Iron () is a chemical element with symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal that belongs to the first transition series and group 8 of the periodic table. It is, by mass, the most common element on Earth, right in front of oxygen (32.1% and 30.1%, respectively), forming much of Earth's outer and inner core. It is the fourth most common element in the Earth's crust.
In its metallic state, iron is rare in the Earth's crust, limited mainly to deposition by meteorites. Iron ores, by contrast, are among the most abundant in the Earth's crust, although extracting usable metal from them requires kilns or furnaces capable of reaching 1,500 °C (2,730 °F) or higher, about 500 °C (900 °F) higher than that required to smelt copper. Humans started to master that process in Eurasia by about 2000 BCE, and the use of iron tools and weapons began to displace copper alloys, in some regions, only around 1200 BCE. That event is considered the transition from the Bronze Age to the Iron Age. In the modern world, iron alloys, such as steel, stainless steel, cast iron and special steels are by far the most common industrial metals, because of their mechanical properties and low cost.
Pristine and smooth pure iron surfaces are mirror-like silvery-gray. However, iron reacts readily with oxygen and water to give brown to black hydrated iron oxides, commonly known as rust. Unlike the oxides of some other metals, that form passivating layers, rust occupies more volume than the metal and thus flakes off, exposing fresh surfaces for corrosion. Although iron readily reacts, high purity iron, called electrolytic iron, has better corrosion resistance.
The body of an adult human contains about 4 grams (0.005% body weight) of iron, mostly in hemoglobin and myoglobin. These two proteins play essential roles in vertebrate metabolism, respectively oxygen transport by blood and oxygen storage in muscles. To maintain the necessary levels, human iron metabolism requires a minimum of iron in the diet. Iron is also the metal at the active site of many important redox enzymes dealing with cellular respiration and oxidation and reduction in plants and animals.Chemically, the most common oxidation states of iron are iron(II) and iron(III). Iron shares many properties of other transition metals, including the other group 8 elements, ruthenium and osmium. Iron forms compounds in a wide range of oxidation states, −2 to +7. Iron also forms many coordination compounds; some of them, such as ferrocene, ferrioxalate, and Prussian blue, have substantial industrial, medical, or research applications.
Evidence Level
Level 4 (Individual reports repeated observed over 5 years among different countries)
Hepatotoxicity reports in literature
- Acute hepatitis in adult Still's disease apparently resulting from oral iron substitution--a case report : (Source)
- The liver in ferrous sulfate poisoning; a report of three fatal cases in children and an experimental study : (Source)
- Ferrous sulfate poisoning; report of a fatal case : (Source)
- Acute liver failure due to iron overdose in an adult : (Source)
- Hepatocellular damage following therapeutic intravenous iron sucrose infusion in a child : (Source)
- Acute iron poisoning in adult female : (Source)
- Fulminant hepatic failure in woman with iron and non-steroidal anti-inflammatory drug intoxication : (Source)
- Acute hepatic failure in severe iron poisoning : (Source)
- Severe iron poisoning treated with enteral and intravenous deferoxamine : (Source)
- Hepatic failure due to massive iron ingestion successfully treated with liver transplantation : (Source)
- Liver damage and hypoglycemia in acute iron poisoning : (Source)
- Fatal iron intoxication in an infant : (Source)
Hepatotoxicity Description
N/A
Common name
N/A
ID
HD0038
Scientific name of the plant
N/A
Anatomical part for use
N/A
Human use
Bodybuilding
Summary
Iron () is a chemical element with symbol Fe (from Latin: ferrum) and atomic number 26. It is a metal that belongs to the first transition series and group 8 of the periodic table. It is, by mass, the most common element on Earth, right in front of oxygen (32.1% and 30.1%, respectively), forming much of Earth's outer and inner core. It is the fourth most common element in the Earth's crust. In its metallic state, iron is rare in the Earth's crust, limited mainly to deposition by meteorites. Iron ores, by contrast, are among the most abundant in the Earth's crust, although extracting usable metal from them requires kilns or furnaces capable of reaching 1,500 °C (2,730 °F) or higher, about 500 °C (900 °F) higher than that required to smelt copper. Humans started to master that process in Eurasia by about 2000 BCE, and the use of iron tools and weapons began to displace copper alloys, in some regions, only around 1200 BCE. That event is considered the transition from the Bronze Age to the Iron Age. In the modern world, iron alloys, such as steel, stainless steel, cast iron and special steels are by far the most common industrial metals, because of their mechanical properties and low cost. Pristine and smooth pure iron surfaces are mirror-like silvery-gray. However, iron reacts readily with oxygen and water to give brown to black hydrated iron oxides, commonly known as rust. Unlike the oxides of some other metals, that form passivating layers, rust occupies more volume than the metal and thus flakes off, exposing fresh surfaces for corrosion. Although iron readily reacts, high purity iron, called electrolytic iron, has better corrosion resistance. The body of an adult human contains about 4 grams (0.005% body weight) of iron, mostly in hemoglobin and myoglobin. These two proteins play essential roles in vertebrate metabolism, respectively oxygen transport by blood and oxygen storage in muscles. To maintain the necessary levels, human iron metabolism requires a minimum of iron in the diet. Iron is also the metal at the active site of many important redox enzymes dealing with cellular respiration and oxidation and reduction in plants and animals.Chemically, the most common oxidation states of iron are iron(II) and iron(III). Iron shares many properties of other transition metals, including the other group 8 elements, ruthenium and osmium. Iron forms compounds in a wide range of oxidation states, −2 to +7. Iron also forms many coordination compounds; some of them, such as ferrocene, ferrioxalate, and Prussian blue, have substantial industrial, medical, or research applications.
Evidence Level
Level 4 (Individual reports repeated observed over 5 years among different countries)
Hepatotoxicity reports in literature
- Acute hepatitis in adult Still's disease apparently resulting from oral iron substitution--a case report : (Source)
- The liver in ferrous sulfate poisoning; a report of three fatal cases in children and an experimental study : (Source)
- Ferrous sulfate poisoning; report of a fatal case : (Source)
- Acute liver failure due to iron overdose in an adult : (Source)
- Hepatocellular damage following therapeutic intravenous iron sucrose infusion in a child : (Source)
- Acute iron poisoning in adult female : (Source)
- Fulminant hepatic failure in woman with iron and non-steroidal anti-inflammatory drug intoxication : (Source)
- Acute hepatic failure in severe iron poisoning : (Source)
- Severe iron poisoning treated with enteral and intravenous deferoxamine : (Source)
- Hepatic failure due to massive iron ingestion successfully treated with liver transplantation : (Source)
- Liver damage and hypoglycemia in acute iron poisoning : (Source)
- Fatal iron intoxication in an infant : (Source)
Hepatotoxicity Description
N/A