Taking into account the definition of isotopes, the atomic mass of 102 is not exactly match the atomic mass of 102.91 listed on the periodic table for this element because rhodium's atomic mass is a weighted average of all of the isotopes of that element.
Each chemical element is characterized by the number of protons in its nucleus, which is called the atomic number (Z).
The number of neutrons in the nucleus can vary. The atomic mass (A) is obtained by adding the number of protons and neutrons in a given nucleus.
The same chemical element can be made up of different atoms, that is, their atomic numbers are the same, but the number of neutrons is different. These atoms are called isotopes of the element.
In other words, atoms that have the same number of protons but different numbers of neutrons are called isotopes. Isotopes, by varying the number of protons, have different atomic masses.
The relative abundance of an isotope is the percentage of atoms with a specific atomic mass found in a naturally occurring sample of an element.
The atomic masses of chemical elements are usually calculated as the weighted average of the masses of the different isotopes of each element, taking into account the relative abundance of each of them. Therefore, the atomic mass of an element is not a whole number.
Finally, the atomic mass of 102 is not exactly match the atomic mass of 102.91 listed on the periodic table for this element because rhodium's atomic mass is a weighted average of all of the isotopes of that element.
Learn more:
- https://brainly.com/question/5527493?referrer=searchResults
- https://brainly.com/question/13596853
