About Iron
Iron, labeled as "Fe," is the twenty-sixth element on the periodic table of elements, which means it has an atomic number of 26. It is a very common metallic element that is used in manufacturing processes and composes many different items. It is one of the most common metals found in meteorites as well as in the core of the Earth and similar planets.
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Geography
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Iron is found not only on the Earth, but also in most of the more dense, solid masses in the galaxy. This includes other planets as well as moons and meteors. On Earth, iron is the most abundant element, and it can be found mainly in the Earth's crust. Iron is abundant on the planet Mars, and is believed to give the planet its red color.
Identification
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As an element, the number of electrons in its valence shells, which are rings of electrons surrounding the nucleus, and the number of protons in its nucleus can identify iron. The nucleus of an iron atom contains 26 protons, which are positively charged particles. Electrons, which are negatively charged, are found in four different valence shells and total 26 as well. Found in nature, iron is a heavy metal with a smooth, silvery finish.
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History
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Iron was first extracted from various metal ores that contained the element through a process of smelting that was developed in India during the beginning of the second millennium. Cast iron, which is easier to melt and mold, was created first in China in 550 BCE, and then found its way into Europe during the medieval period. This is also when wrought iron, which is pure iron, was first mined and sold in abundance. Steel, which is a heavy, very tough iron alloy, was introduced in the seventeenth century and was a major factor in the industrial revolution. It is still widely used in modern times.
Types
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There are four different types, or isotopes, of iron that occur in nature: Fe-54, Fe-56, Fe-57 and Fe-58. Fe-54 is the radioactive isotope, while the remaining three are stable, meaning they are not as highly reactive. The most studied of these isotopes is Fe-56, which is used by nuclear scientists because it has one of the most stable nuclei in nature and is a byproduct of fusion reactions.
Warning
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The human body has no natural way of excreting iron. Since it is a necessary part of everyday nutrition, the human body has a very strict and regimented control of how iron is distributed throughout the body. An excess of iron can be toxic because of how it reacts with peroxides in the body. When too much iron reacts with these peroxides, free radicals are created, which damage cells by attacking them at the atomic level. This can damage various proteins in the body as well as strands of DNA.
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