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Ch.2 - Atoms & Elements
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.2 - Atoms & ElementsProblema 131
Capitolo 2, Problema 131

Silver is composed of two naturally occurring isotopes: Ag-107 (51.839%) and Ag-109. The ratio of the masses of the two isotopes is 1.0187. What is the mass of Ag-107?

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First, let's denote the mass of Ag-107 as x. The mass of Ag-109 will then be 1.0187x, according to the given ratio.
Next, we need to use the formula for calculating the average atomic mass. The average atomic mass is the sum of the masses of the isotopes, each multiplied by its natural abundance. In this case, the average atomic mass of silver is the sum of the mass of Ag-107 times its abundance and the mass of Ag-109 times its abundance.
Set up the equation: 107.87 = 0.51839x + 0.48161(1.0187x), where 107.87 is the average atomic mass of silver, 0.51839 is the abundance of Ag-107, and 0.48161 is the abundance of Ag-109 (calculated as 1 - 0.51839).
Solve the equation for x, which represents the mass of Ag-107.
Finally, check your answer by substituting the value of x back into the equation to ensure that it balances.

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Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. For example, silver has two isotopes, Ag-107 and Ag-109, which differ in their neutron count and thus their mass, but both are chemically identical.
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Isotopes

Average Atomic Mass

The average atomic mass of an element is calculated by taking into account the masses of its isotopes and their relative abundances. This value reflects the weighted average of all isotopes present in nature, allowing for a more accurate representation of the element's mass as it occurs in nature.
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Atomic Mass

Mass Ratio

The mass ratio of isotopes refers to the relationship between the masses of two isotopes of the same element. In this case, the mass ratio of Ag-107 to Ag-109 is given as 1.0187, indicating that Ag-109 is slightly heavier than Ag-107. This ratio is crucial for calculating the mass of Ag-107 when combined with the known abundance of the isotopes.
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Neutron-Proton Ratio
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