Isoneutronic species are atoms (nuclides) that have the same number of neutrons.
To determine if two or more nuclides are isoneutronic, you need to calculate the number of neutrons in each. The number of neutrons is calculated by subtracting the number of protons (atomic number) from the mass number. According to the reference information, the iso neutronic species are those which have the same number of neutrons. The number of neutrons can be calculated from the mass number by subtracting the number of protons from it.
Understanding Isoneutronic Species
Here's a more detailed breakdown:
- Neutron Number: The defining characteristic of isoneutronic nuclides.
- Mass Number (A): The total number of protons and neutrons in the nucleus.
- Atomic Number (Z): The number of protons in the nucleus (determines the element).
How to Identify Isoneutronic Nuclides
The number of neutrons (N) is calculated as:
N = A - Z
Example
Consider the following nuclides:
- 14C (Carbon-14): A = 14, Z = 6, N = 14 - 6 = 8 neutrons
- 16O (Oxygen-16): A = 16, Z = 8, N = 16 - 8 = 8 neutrons
In this case, 14C and 16O are not isoneutronic because they do not have the same number of neutrons.
However, consider these:
- 37Cl (Chlorine-37): A = 37, Z = 17, N = 37 - 17 = 20 neutrons
- 39K (Potassium-39): A = 39, Z = 19, N = 39 - 19 = 20 neutrons
- 40Ca (Calcium-40): A = 40, Z = 20, N = 40 - 20 = 20 neutrons
37Cl, 39K, and 40Ca are isoneutronic because they all have 20 neutrons.
