Nuclide · Lablypedia

The word nuclide was coined by the American nuclear physicist Truman P. Kohman in 1947. Kohman defined nuclide as a "species of atom characterized by the constitution of its nucleus" containing a certain number of neutrons and protons. The term thus originally focused on the nucleus.

Nuclide vs. isotope

A nuclide is an atom with a specific number of protons and neutrons in its nucleus, for example carbon-13 (¹³
₆C) with 6 protons and 7 neutrons. The term was coined deliberately in distinction from isotope in order to consider the nuclear properties independently of the chemical properties, though isotope is still used for that purpose especially where nuclide might be unfamiliar as in nuclear technology and nuclear medicine. For nuclear properties, the number of neutrons can be practically as important as that of protons, as is never the case for chemical properties: even in the case of the very lightest elements, where the ratio of neutron number to atomic number varies the most between isotopes, it is a relatively small effect, and only substantial for hydrogen and helium (the latter of which has no chemistry proper). For hydrogen the isotope effect is large enough to affect biological systems strongly. In helium, ⁴
₂He obeys Bose–Einstein statistics, while ³
₂He obeys Fermi–Dirac statistics, which is responsible for sharp differences in physical properties at low temperature.

4 more chapters are free with a Lably account.

Types of nuclides

Although the words nuclide and isotope are often used interchangeably, being isotopes is actually only one relation between nuclides. The following table names some other relations.

A set of nuclides with equal proton number (atomic number), i.e., of the same chemical element but different neutron numbers, are called isotopes of the element. Particular nuclides are still often loosely called "isotopes", but the term "nuclide" is now considered the correct one in the general case when no specific element (Z value) encompasses them. In similar manner, a set of nuclides with equal mass number A, but different atomic number, are called isobars (isobar = equal in weight), and isotones are nuclides of equal neutron number but different proton numbers. Likewise, nuclides with the same neutron excess (N − Z) are called isodiaphers. The name isotone was derived from the name isotope to emphasize that in the first group of nuclides it is the number of neutrons (n) that is constant, whereas in the second the number of protons (p).

See Isotope#Notation for an explanation of the notation used for different nuclide or isotope types.

Nuclear isomers are members of a set of nuclides with equal proton number and equal mass number (thus making them by definition the same isotope), but different states of excitation. An example is the two states of the single isotope ⁹⁹
₄₃Tc shown among the decay schemes. Each of these two states (technetium-99m and technetium-99) qualifies as a different nuclide, illustrating one way that nuclides may differ from isotopes (an isotope may consist of several different nuclides of different excitation states).

The longest-lived non-ground state nuclear isomer is the nuclide tantalum-180m (^180m
₇₃Ta), which has a half-life in excess of 10¹⁷ years. This nuclide occurs primordially, and has never been observed to decay to the ground state. (In contrast, the ground state nuclide tantalum-180 does not occur primordially, since it decays with a half-life of only 8 hours to ¹⁸⁰
₇₂Hf (86%) or ¹⁸⁰
₇₄W (14%).)

There are 251 nuclides in nature that have never been observed to decay. They occur among the 80 different elements that have one or more stable isotopes. See stable nuclide and primordial nuclide. Unstable nuclides are radioactive and are called radionuclides. Their decay products ('daughter' products) are called radiogenic nuclides.

Origins of naturally occurring radionuclides

Natural radionuclides may be conveniently subdivided into three types.

Those whose half-lives exceed a few percent of the age of the Earth (about 4.6×10⁹ years) survive from its formation and are remnants of nucleosynthesis that occurred in stars before the formation of the Solar System. For example, the isotope ²³⁸
₉₂U (t_1/2 = 4.463×10⁹ years) of uranium is still fairly abundant in nature, but the shorter-lived isotope ²³⁵
₉₂U (t_1/2 = 0.704×10⁹ years) is now 138 times rarer. 35 of these primordial radionuclides have been identified (see List of nuclides and Primordial nuclide for details).
Radiogenic nuclides (such as ²²⁶
₈₈Ra (t_1/2 = 1600 years), an isotope of radium) that are formed by radioactive decay. They occur in the decay chains of primordial isotopes of uranium or thorium. Some of these nuclides are very short-lived, such as isotopes of francium. There exist about 50 of these daughter nuclides that have half-lives too short to be primordial, and which exist in nature solely due to decay from longer lived radioactive primordial nuclides.
Nuclides that are continuously being made in another fashion that is not simple spontaneous radioactive decay (i.e., only one atom involved with no incoming particle) but instead involves a natural nuclear reaction. These occur when atoms react with natural neutrons (from cosmic rays, spontaneous fission, or other sources), or are bombarded directly with cosmic rays. The latter, if non-primordial, are called cosmogenic nuclides.

Other types of natural nuclear reactions produce nuclides that are said to be nucleogenic nuclides. Nuclides produced as direct products of spontaneous fission span a wide range, but every one will quickly (in geologic time) decay either to a primordial nuclide or one of the seven long-lived fission products, which are thus present in nature, but might be considered either radiogenic or nucleogenic.

Examples of nuclides made by nuclear reactions are cosmogenic ¹⁴
₆C (radiocarbon) that is made by cosmic ray bombardment of other elements and nucleogenic ²³⁹
₉₄Pu still being created by neutron bombardment of natural ²³⁸
₉₂U as a result of natural fission in uranium ores.

Summary table for each class of nuclides

This is a summary table for the 987 nuclides with half-lives longer than one hour, given in List of nuclides. Note that that number, while exact to present knowledge, will likely change slightly in the future, as some "stable" nuclides are observed to be radioactive with very long half-lives, and some half-lives or known radioactive ones are revised.

Nuclear properties and stability

The main discussion of this topic is at Isotope#Nuclear properties and stability.

Atomic nuclei other than ¹
₁H, a lone proton, consist of protons and neutrons bound together by the residual strong force, overcoming electrical repulsion between protons, and for that reason neutrons are required by bind protons together; as the number of protons increases, so does the ratio of neutrons to protons necessary for stability, as the graph illustrates. For example, although light elements up through calcium have stable nuclides with the same number of neutrons as protons, lead requires about 3 neutrons for 2 protons.