Silver has two naturally occurring isotopes (Ag-107 and...

Silver has two naturally occurring isotopes (Ag-107 and Ag-109). (a) Use the periodic table to find the atomic mass of silver. (b) If the natural abundance of $\mathrm{Ag}-107$ is $51.84 \%,$ what is the natural abundance of Ag-109? (c) If the mass of $\mathrm{Ag}-107$ is 106.905 amu, what is the mass of Ag-109?

Silver has two naturally occurring isotopes (Ag-107 and Ag-109).
(a) Use the periodic table to find the atomic mass of silver.
(b) If the natural abundance of $\mathrm{Ag}-107$ is $51.84 \%,$ what is the natural abundance of Ag-109?
(c) If the mass of $\mathrm{Ag}-107$ is 106.905 amu, what is the mass of Ag-109?

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Key Concepts

Atomic Mass

Atomic mass is the weighted average mass of all the isotopes of an element, taking into account their respective natural abundances. It is generally listed on the periodic table and reflects the average mass of atoms of that element found in nature, rather than the mass of a single isotope.

Isotopes

Isotopes are forms of a given element that have the same number of protons but different numbers of neutrons. This difference in neutron number results in different mass numbers for the isotopes, although they generally exhibit similar chemical properties.

Natural Abundance

Natural abundance refers to the relative proportion of each isotope of an element as it occurs in nature. It is usually expressed as a percentage and directly affects the calculation of the atomic mass, since the atomic mass is the weighted sum of the masses of the isotopes based on their abundance.

Weighted Average Calculation

The weighted average calculation involves multiplying the mass of each isotope by its fractional natural abundance and then summing these products to obtain the atomic mass of the element. This method accounts for the contribution of each isotope to the overall atomic mass, making it a critical concept in understanding the measurement and significance of atomic mass as reported on the periodic table.

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