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» View Examples of Stable Isotope Compounds Many of the chemical elements have a number of isotopes.The isotopes of an element have the same number of protons in their atoms (atomic number) but different masses due to different numbers of neutrons.In an atom in the neutral state, the number of external electrons also equals the atomic number.
An "isotopically labeled compound" has one or more of its atoms enriched in an isotope.
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Isotopes | Stable & Unstable | Applications | Definitions | Diagnosis | Radiotherapy | Biochemical Analysis Diagnostic/Therapeutic Radiopharmaceuticals | Discovery | Isotopes in Medicine | Terms & Concepts An isotope is one of two or more species of atoms of a chemical element with the same atomic number (same number or protons in the nucleus) and position in the periodic table and nearly identical chemical behavior but with different atomic masses and physical properties. An atom is first identified and labeled according to the number of protons in its nucleus.
The specification of Z, A, and the chemical symbol (a one- or two-letter abbreviation of the element's name, say Sy) in the form A/ZSy identifies an isotope adequately for most purposes.
Thus in the standard notation, 1/1H refers to the simplest isotope of hydrogen and 235/92U to an isotope of uranium widely used for nuclear power generation and nuclear weapons fabrication. A "stable isotope" is any of two or more forms of an element whos nuclei contains the same number of protons and electrons, but a different number of neutrons.
The total number of neutrons and protons (symbol A), or mass number, of the nucleus gives approximately the mass measured on the so-called atomic- mass-unit (amu) scale.