Nuclide notation

Sub-atomic particle Symbol Relative mass Relative charge Nuclide notation... 

The subscript number in the nuclide notation is the atomic number. Hence an atom of phosphorus contains 15 protons and therefore 15 electrons. However, since the ion has a net charge of -3 the ion contains 18 (15 + 3) electrons. The difference between the subscript number (atomic number) and the superscript number (mass number) is equal to the number of neutrons, which in this example is 16 (31 - 15). 

The representation of elements In the periodic table of the IB Chemistry data booklet, 20.18 Is the relative atomic mass of neon. The nuclide notation for neon-20 Is Ne... 

Early studies of Mg isotope ratios in geological materials used the notation A Mg to mean per mil deviations from a standard as expressed in Equation (1) above, a convention that persists today (e.g., Elsu et al. 2000). The values assigned to A "Mg in those studies represent the level of mass-dependent isotopic fractionation relative to the standard. The same convention defined fi Mg as the per mil deviation from the standard after correction for the mass fractionation evidenced by A "Mg. In this system of nomenclature, A values refer to mass dependentfractionations while 5 values refer to deviations from mass-dependent fractionation (i.e., the S Mg defines excesses in Mg relative to mass fractionation attributable to decay of the extinct nuclide Al). In some cases A "Mg has been replaced by the symbol Fn,g (Kennedy et al. 1997) where the F refers to fractionation. ... 

Even though the above reactions are at the level of nuclei, in the notation adopted in this book, each nuclide is treated as a neutral atomic species including... 

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. 

Nuclide No. of protons (Z) No. of neutrons (N) N/Z (n/p) ratio Notation Nuclear stability... 

Experiments in which both the irradiated and the observed nuclei are protons are called homonuclear double-resonance experiments and are represented by the notation The irradiated nucleus is denoted by braces. When the observed and irradiated nuclei are different nuclides, as in proton-decoupled spectra, the experiment is a heteronuclear double-resonance experiment and is denoted, for example, C H. ... 

Our journey into the center of the atom begins with a brief review. You learned in Chapter 2 that the protons and neutrons in each atom are found in a tiny, central nucleus that measures about 1/100,000 the diameter of the atom itself You also learned that the atoms of each element are not necessarily identical they can differ with respect to the number of neutrons in their nuclei. When an element has two or more species of atoms, each with the same number of protons but a different number of neutrons, the different species are called isotopes. Different isotopes of the same element have the same atomic number, but they have a different mass number, which is the sum of the numbers of protons and neutrons in the nucleus. In the context of nuclear science, protons and neutrons are called nucleons, because they reside in the nucleus. The atom s mass number is often called the nucleon number, and a particular type of nucleus, characterized by a specific atomic number and nucleon number, is called a nuclide. Nuclides are represented in chemical notation by a subscript atomic number (Z) and superscript nucleon number (A) on the left side of the element s symbol (X) ... 

Nuclear equation The shorthand notation that describes nuclear reactions. It shows changes in the participating nuclides atomic numbers (the number of protons) and mass numbers (the sum of the numbers of protons and neutrons). 

The notation for nuclides is the same as that used in Chap. 3 and is defined under Nomenclature at the end of that chapter. 

This appendix lists some of the properties of nuclides and natural elements that are useful in nuclear engineering. Sources of data and explanations of notation are given below. 

Nuclear species are characterized in the first two columns of the table by the name of the element and the mass number of the nuclide. The complete symbol notation for a nuclide can be obtained from these two columns. For example, the symbol notation for the boron isotope of atomic number S and mass number 10 is 5B. 

The relative mass and charge of a particle—a nucleon, another kind of elementary particle, or a nuclide—is described by the notation X, where X is the symbol for the particle, A is the mass number, or the total number of nucleons, and Z is the charge of the particle for nuclides, A is the sum of protons and neutrons and Z is the number of protons (atomic number). In this notation, the three subatomic elementary particles are... 

In nuclear notation, the element symbol refers to the nucleus only, so a proton is also sometimes represented as jH.) The number of neutrons N) in a nucleus is the mass number (/ ) minus the atomic number (Z) N = A — Z. The two naturally occurring isotopes of chlorine, for example, have 17 protons (Z = 17), but one has 18 neutrons (nCl, also written Cl) and the other has 20 ( Cl, or Cl). Nuclides can also be designated with the element name followed by the mass number, for example, chlorine-35 and chlorine-37. Despite some small variations, in naturally occurring samples of an element or its compounds, the isotopes of the element are present in particular, fixed proportions. Thus, in a sample of sodium chloride (or any Cl-containing substance), 75.77% of the Cl atoms are chlorine-35 and the remaining 24.23% are chlorine-37. 

The nucleus is composed of protons (charge = +1 mass = 1.007 atomic mass units ([p.]) and neutrons. The number of protons in the nucleus is called the atomic number Z and defines which chemical element the nucleus represents. The number of neutrons in the nucleus is called the neutron number N, whereas the total number of neutrons and protons in the nucleus is referred to as the mass number A, where A = N -I- Z. The neutrons and protons are referred to collectively as nucleons. A nucleus with a given N and Z is referred to as a nuclide. Nuclides with the same atomic number are isotopes, such as and whereas nuclides with the same N, such as and are called isotones. Nuclei such as " N and which have the same mass number, are isobars. Nuclides are designated by a shorthand notation in which one writes Chemical Symbol, that is, for a nucleus with 6 protons and 8 neutrons, one writes gCs, or, g C, or just The size of a nucleus is approximately 1 to 10 x 10 m, with the nuclear radius being represented more precisely as 1.2 x A x 10 m. We can roughly approximate the nucleus as a sphere and thus we can calculate its density... 

Half-life in decimal notation, ps = microseconds ms = milliseconds s = seconds m = minutes h = hours d = days and y = years. For quasi-stable nuclides, the measured width at half maximum of the energy resonance is given... 

Figure 2-1 shows the nuclear notation (a way of writing elements that gives information about the nucleus of element) for the 82 polyatomic ion with 16 neutrons on each sulfur atom, or nuclide. 

Atomic number 0ower left, IQ This is the number of protons within the nuclide. As the atomic number tells you the element, which is also represented by the element s symbol at the center of the nuclear notation (in this case, S for sulfur), it s commonly not included. All atoms that have 16 protons are sulfur atoms. 

In this chapter, the following shorthand notation is used. [" X] denotes the number of atoms/concentration of nuclide where X stands for the chemical symbol of some element... 

We will generally use the notation with subscripts and superscripts only when referring to a particular isotope of an element. An atom of a specific isotope is called a nuclide. Thus, an atom of is referred to as a nuclide. 

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 ... 

Nuclides of a chemical element are described by the notation 2X, where X represents the symbol of the chemical element, Z represents the atomic number and A represents the mass number. For example ... 

The notation for a specific nuclide can be written if the mass number and atomic number are given. For example, the notation for a sodium atom with a mass number of 23 is written in the following way ... 

With this nomenclature, the notation 13-A1-27 represents stable aluminum as found in nature. If you look at a Chart of the Nuclides, you will find there are 11 different aluminum isotopes (all are aluminum because they have 13 protons, but they have masses from 23-33 They are all isotopes of aluminum, and all but 13-A1-27 are radioactive isotopes --radioisotopes). Since only aluminum has 13 protons in the nucleus, we often leave the Z value off the notation, such as Al-27. Some of our information sheets have the entries arranged in order of increasing Z, so it is helpful to remember about what the atomic numbers of different elements are to make it easier to find entries in tables. 

Stainless steel is composed of iron (Fe), chromium (Cr), and nickel (Ni). What reactions would produce the following radioactive isotopes if stainless steel is irradiated in the reactor You may refer to a chart of the nuclides, and the short version of notation is acceptable (e g. Al-27(n,a)Na-24). 

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