Question

What are the naturally occurring isotopes of Magnesium along with their respective masses and percent abundances?

a) 23.98 amu (78.60%), 24.98 amu (10.10%), 25.98 amu (11.30%)
b) 23.98 amu (10.10%), 24.98 amu (11.30%), 25.98 amu (78.60%)
c) 24.98 amu (78.60%), 25.98 amu (10.10%), 23.98 amu (11.30%)
d) 25.98 amu (78.60%), 23.98 amu (10.10%), 24.98 amu (11.30%)

Answer 1

The naturally occurring isotopes of Magnesium include 24Mg, 25Mg, and 26Mg with masses of 23.98 amu, 24.99 amu, and 25.98 amu respectively. Their percent abundances are 78.70%, 10.13%, and 11.17%. To calculate the average mass of a Mg atom, multiply the mass of each isotope by its percent abundance and then sum the results.

Step-by-step explanation:

The naturally occurring isotopes of Magnesium include three different isotopes: 24Mg, 25Mg, and 26Mg. These isotopes have respective masses of 23.98 amu, 24.99 amu, and 25.98 amu. The percent abundances of these isotopes in a sample of magnesium are 78.70%, 10.13%, and 11.17% respectively. To calculate the average mass of a Mg atom, you would multiply the mass of each isotope by its percent abundance and then sum the results.