We're asked to determine which of the following isotopes are expected to be stable.
Recall that Isotopes represent atoms of an element that contain the same atomic number (same number of protons), but different mass numbers (different number of neutrons) and can be written as:
In terms of stability of isotopes, we use the neutrons to protons (n/p) ratio:
For this problem, we need to do the following steps:
Step 1: Determine the # of protons, p based on the atomic number of each isotope using the Periodic Table
Recall that the atomic # = # of protons (p)
Step 2: Determine the # of neutrons, n for each isotope
Recall that the mass # = # of neutrons (n) + # of protons (p)
Step 3: Calculate the n/p ratio to determine its stability
Which of the following isotopes would you expect to be stable?
c. Uranium 235
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Band of Stability concept. You can view video lessons to learn Band of Stability. Or if you need more Band of Stability practice, you can also practice Band of Stability practice problems.
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Based on our data, we think this problem is relevant for Professor Wallace's class at LEHMAN-CUNY.