Nuclides symbol for

For each process, write the nuclide symbols for the reactant species and for the particle that is captured (as a reactant) or that is emitted (as a product). Then use mass balance and charge balance to write the super- and subscripts for the product nuclide. Determine the atomic symbol for the product nuclide from its atomic number (the subscript). 

A nuclide is an atom characterized by a definite atomic number and mass number. The shorthand notation for any nuclide consists of the symbol of the element with the atomic number written as a subscript on the left and the mass number as a supCT-script on the left. You write the nuclide symbol for the naturally occurring sodium nuclide as follows ... 

What is the nuclide symbol for a nucleus that contains 38 protons and 50 neutrons ... 

Use the list of elements on the inside back cover to obtain the atomic numbers of radium and radon, so you can write their nuclide symbols for the nuclear equation. The nuclide symbol of the alpha particle is He. 

Write the nuclear symbols for the following nuclides (a) the one that contains 92 protons and 143 neutrons and (b) the carbon isotope that has 8 neutrons. 

When determining symbols for nuclides, the key is to remember that the atomic number and number of protons are the same and that the mass number is the sum of the number of protons plus the number of neutrons. 

To summarize, the equation for a nuclear reaction is balanced when the total charge and total mass number of the products equals the total charge and total mass number of the reactants. This conservation requirement is one reason why the symbol for any nuclide includes its charge number (Z) as a subscript and its mass number as a superscript. These features provide a convenient way to keep track of charge and mass balances. Notice that in the equation for neutron decay, the sum of the subscripts for reactants equals the sum of the subscripts for products. Likewise, the sum of the superscripts for reactants equals the sum of the superscripts for products. We demonstrate how to balance equations for other reactions as they are introduced. 

Any nuclear species is referred to as a nuclide. Thus, H, 23uNa, 12SC, 23892U are different recognizable species or nuclides. A nuclide is denoted by the symbol for the atom with the mass number written to the upper left, the atomic number written to the lower left, and any charge on the species, q to the upper right. For example,... 

The atomic number, Z, is the number of protons in the nucleus. Both the proton and neutron have masses that are approximately 1 atomic mass unit, amu. The electron has a mass of only about 1/1837 of the proton or neutron, so almost all of the mass of the atoms is made up by the protons and neutrons. Therefore, adding the number of protons to the number of neutrons gives the approximate mass of the nuclide in amu. That number is called the mass number and is given the symbol A. The number of neutrons is found by subtracting the atomic number, Z, from the mass number, A. Frequently, the number of neutrons is designated as N and (A - Z) = N. In describing a nuclide, the atomic number and mass number are included with the symbol for the atom. This is shown for an isotope of X as AZX. 

Nuclide. Each nuclide is identified by its atomic number Z, equal to the number of protons in the nucleus the corresponding symbol for that element and the mass number A, equal to the sum of the numbers of protons Z and neutrons N in the nucleus. Thus, A = Z + N, or N = A — Z. The m following the mass number (e.g., 69mZn) indicates an isomer of that nuclide. 

A shorthand notation has been developed for nuclear reactions such as the reaction discovered by Curie and Joliot. The parent (or target) nuclide and the daughter nuclide are separated by parentheses that contain the symbols for the particle that hits the target and the particle or particles released in this reaction. 

A nuclide may be specified by attaching the mass number as a left superscript to the symbol for the element. The atomic number may also be attached as a left subscript, if desired, although this is rarely done. If no left superscript is attached, the symbol is read as including all isotopes in natural abundance. 

The symbols for particles, chemical elements and nuclides have been discussed in section 2.10. The recently recommended systematic nomenclature and symbolism for chemical elements of atomic number greater than 103 is briefly described in footnote U to table 6.2. 

There are two main methods used for naming isotopically labelled compounds. For specifically labelled compounds, lUPAC recommends forming the name by placing the nuclide symbols (plus locants if necessary) in square brackets before the name of the unlabelled compounds or that part of the name which is isotopically modified. 

For most purposes the nucleus can be regarded as a collection of nucleons (neutrons and protons), and the internal structures of these particles can be ignored. Recall that the number of protons in a particular nucleus is the atomic number (Z) and that the sum of the neutrons and protons is the mass number (A). Atoms that have identical atomic numbers but different mass number values are called isotopes. The general term nuclide is applied to each unique atom and is represented by where X represents the symbol for a particular element. 

Nuclide the general term applied to each unique atom represented by zX, where X is the symbol for a particular element. (21)... 

Nuclear reactions are usually represented as eqs. (4.1) and (4.2), that is, on the left is the symbol for the target nuclides, the first symbol in the parenthesis indicates the bombarding particle (or projectile), the second the emitted particles, and the symbol of the product on the right. In the equation, the left side of the comma shows the system of the reactants, and the right the system of the products. Before and after the nuclear reaction, both the sum of mass number and the sum of atomic number remain unchanged. 

A nuclear species (nuclide) is characterized by its atomic number Z (that is, the nuclear charge in units of e, or the number of protons in the nucleus) and its mass number A (the sum of the number of protons plus the number of neutrons in the nucleus). We denote an atom that contains such a nuclide with the symbol zX, where X is the chemical symbol for the element. The atomic number Z is sometimes omitted because it is implied by the chemical symbol for the element. Thus, JH (or H) is a hydrogen atom and (or C) is a carbon atom with a nucleus that contains six protons and six neutrons. Isotopes are nuclides of the same chemical species (that is, they have the same Z), but with different mass numbers A, and therefore different numbers of neutrons in the nucleus. The nuclear species of hydrogen, deuterium, and tritium, represented by JH, jH, and jH, respectively, are all members of the family of isotopes that belong to the element hydrogen. 

As defined in Section 1.4, a nuclide is characterized by the number of protons, Z, and the number of neutrons, N, it contains. The atomic number Z determines the charge -l- Ze on the nucleus and therefore decides the identity of the element the sum Z + N = A s the mass number of the nuclide and is the integer closest to the relative atomic mass of the nuclide. Nuclides are designated by the symbol zX where X is the chemical symbol for the element. 

Nuclides are often denoted by E, where Z is the atomic number, A is the mass number (protons plus neutrons), and E is the symbol for the element. Note that A-Z equals the number of neutrons in the nuclide. 

The mass number for normal hydrogen atoms is 1 for deuterium, 2 and for tritium, 3. The composition of a nucleus is indicated by its nuclide symbol. This consists of the symbol for the element (E), with the atomic number (Z) written as a subscript at the lower left and the mass number (A) as a superscript at the upper left, By this system, the three isotopes of hydrogen are designated as H, H, and ]H. 

The identity of an element depends on the number of protons in the nucleus of the atom. This value is called the atomic number and it is sometimes written as a subscript before the symbol for the corresponding element. Atoms and ions of a given element that differ in number of neutrons have a different mass and are called isotopes. A nucleus with a specified number of protons and neutrons is called a nuclide, and a nuclear particle, either a proton or neutron, may be called a nucleon. The total number of nucleons is called the mass number and may be written as a superscript before the atomic symbol. 

One of the nuclides used in radiation therapy for the treatment of cancer has 39 protons and 51 neutrons. Write its nuclide symbol in the form of zX. Write two... 

To make the subscripts balance in our equation, the subscript for the missing nuclide must be 80, indicating that the symbol for the produa nuclide should be Hg, for mercury. The mass number stays the same in beta emission, so we write... 

To balance the subscripts, the atomic number for our missing nuclide must be 30, so the symbol for the product nuclide is Zn, for zinc. The mass number stays the same in electron capture, so we write 67. 

First, determine the subscript for the missing formula by asking what number would make the sum of the subscripts on the left of the arrow equal the sum of the subscripts on the right. That number is the atomic number of the missing nuclide and leads us to the element symbol for that nuclide. Next, determine the superscript for the missing formula by asking what number would make the sum of the superscripts on the left of the arrow equal to the sum of the superscripts on the right. 

Given a symbol for a nuclide, identify its atomic number and mass number (nucleon number). 

Given a symbol for a nuclide, identify the numbers of protons and neutrons that its nucleus contains, or given the numbers of protons and neutrons that its nucleus contains, write its symbol. 

Given the symbols for three nuclides of the same element—one that is stable and non-radioactive, one that is radioactive and has a lower mass number than the stable nuclide, and one that is radioactive and has a higher mass number than the stable nuclide—predict which of the radioactive nuclides would be more likely to undergo beta emission and which would be more likely to undergo positron emission (or electron capture). 

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