Iron has several isotopes, which are variants of the element that have the same number of protons but different numbers of neutrons. The most stable and commonly occurring isotopes of iron are: 1. **Iron-54 (\(^{54}Fe\))**: This is the most abundant stable isotope, making up about 5.8% of natural iron.
Iron-55 (Fe-55) is a radioactive isotope of iron. It has a nuclear mass number of 55, meaning it has 26 protons and 29 neutrons in its nucleus. Iron-55 is produced as a decay product of manganese-55 and can also be formed in nuclear reactions. The half-life of Iron-55 is about 2.
Iron-56 (Fe-56) is a stable isotope of iron, which is one of the most abundant elements in the universe and a key component of many materials found on Earth. Isotopes of an element have the same number of protons but different numbers of neutrons. For Iron-56, it has 26 protons and 30 neutrons, giving it a total atomic mass of approximately 56 atomic mass units (amu).
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