Calculate the atomic mass of silver if silver has 2 naturally occurring isotopes with the following masses and natural abundances: Ag-107 106.90509 amu 51.84% Ag-109 108.90476 amu 48.46% a 108.19 amu b 107.90 amu c 108.32 amu d 108.00 amu e 107.79 amu

a. 108.19 amu

Explanation:

Isotopes are atoms of the same element, which have the same number of protons and electrons, but a different number of neutrons, and, because of that, different masses.

The atomic mass (M) in the periodic table is a ponderation of the masses of all isotopes found in nature. Thus, it is the summation of the percent multiplied by the mass of each isotope, so:

M = 0.5184*106.90509 + 0.4846*108.90476

M = 108.19 amu

amu = atomic mass unit.