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Ch.2 - Atoms & Elements
Tro - Chemistry: A Molecular Approach 4th Edition
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Capitolo 2, Problema 51a

Write isotopic symbols in the form X-A (e.g., C-13) for each isotope. a. the silver isotope with 60 neutrons

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Identify the element: Silver is represented by the symbol 'Ag'.
Determine the atomic number of silver: Silver (Ag) has an atomic number of 47, which means it has 47 protons.
Calculate the mass number: The mass number is the sum of protons and neutrons. For this isotope, it has 47 protons and 60 neutrons, so the mass number is 47 + 60.
Write the isotopic symbol: Combine the element symbol with the mass number to write the isotopic symbol in the form X-A.
The isotopic symbol for the silver isotope with 60 neutrons is Ag-107.

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Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This difference in neutron count results in varying atomic masses. For example, carbon-12 and carbon-14 are isotopes of carbon, with 6 and 8 neutrons, respectively. Isotopes can be stable or radioactive, influencing their applications in fields like medicine and archaeology.
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Isotopic Notation

Isotopic notation is a way to represent isotopes using the format X-A, where 'X' is the chemical symbol of the element and 'A' is the mass number, which is the sum of protons and neutrons. For instance, in the notation C-14, 'C' represents carbon, and '14' indicates that the isotope has a total of 14 nucleons (6 protons and 8 neutrons). This notation helps in identifying specific isotopes and their properties.
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Isotope Notation Example

Mass Number

The mass number of an isotope is the total count of protons and neutrons in its nucleus. It is crucial for distinguishing between different isotopes of the same element. For example, if silver has 47 protons and 60 neutrons, its mass number would be 107 (47 protons + 60 neutrons), leading to the isotopic symbol Ag-107. Understanding mass numbers is essential for calculations involving atomic mass and nuclear stability.
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