* Isotopes have the same number of protons but different numbers of neutrons. This means the atomic mass can be a clue to the isotope's identity, but it's not enough.
* Abundance refers to the relative percentage of an isotope in a naturally occurring sample. To determine this, you need to know:
* The element: What element does this isotope belong to? (e.g., Copper, Zinc, etc.)
* Other isotopes of that element: Elements often have multiple isotopes. You need to know the atomic masses of these other isotopes and their relative abundances.
Example:
Let's say you're looking for the abundance of the isotope with mass 64.9278 in copper (Cu). Here's what you'd need to do:
1. Identify the isotopes of copper: Copper has two main isotopes: Cu-63 and Cu-65.
2. Find their atomic masses: Cu-63 has a mass of 62.9296 amu, and Cu-65 has a mass of 64.9278 amu.
3. Determine their relative abundances: The abundance of Cu-63 is approximately 69.17%, and the abundance of Cu-65 is approximately 30.83%.
Therefore, the abundance of the isotope with atomic mass 64.9278 (Cu-65) is approximately 30.83%.
Please provide the element or other information to determine the abundance of the isotope with atomic mass 64.9278.
