Question

note: to answer some of the questions, it may help to reference a periodic table. how is the average mass of isotopes measured, and what unit is used to describe their average mass? the mass for each isotope of an element is divided by its percent abundance (in decimal form). then, the calculated values of all isotopes for that element are multiplied. angstroms (å) are used to describe average mass. the percent abundance for each isotope of an element (in decimal form) is multiplied by its mass. then, the calculated values of all isotopes for that element are summed. atomic mass units (amu) are used to describe average mass. the percent abundance for each isotope of an element (in decimal form) is divided by its mass. then, the calculated values of all isotopes for that element are multiplied. angstroms (å) are used to describe average mass. the mass for each isotope of an element is divided by its percent abundance (in decimal form). then, the calculated values of all isotopes for that element are summed. atomic mass units (amu) are used to describe average mass.

Explanation:

To find the average mass of isotopes of an element, we multiply the percent - abundance (in decimal form) of each isotope by its mass and sum these values. The unit for average mass of isotopes is atomic mass units (amu). Angstroms are used for length, not mass.

Answer:

The percent abundance for each isotope of an element (in decimal form) is multiplied by its mass. Then, the calculated values of all isotopes for that element are summed. Atomic mass units (amu) are used to describe average mass.