Average Atomic Mass

The weighted average of the masses of an element's isotopes, taking into account their relative abundances.

Multiply the mass of each isotope by its relative abundance (as a decimal), then sum these values.

Atoms of the same element that have the same number of protons but different numbers of neutrons.

The number of protons in an atom's nucleus defines the element and its position on the periodic table.

33, as the atomic number is equal to the number of protons.

The total number of protons and neutrons in the nucleus of an atom.

Subtract the atomic number (number of protons) from the mass number.

To find the average atomic mass, calculate: (0.241 * 75.23) + (0.487 * 74.61) + (0.272 * 75.20).

It indicates the presence of multiple isotopes with different masses and their relative abundances.

28.09 amu.