Argon has three naturally occurring isotopes, with mass numbers 36, 38, and 40.c. How are they different?

Verified step by step guidance

1. Identify that isotopes are atoms of the same element with different numbers of neutrons.
2. Recognize that all isotopes of argon have the same number of protons, which is 18, as this defines the element.
3. Calculate the number of neutrons in each isotope by subtracting the number of protons (18) from the mass number of each isotope: 36, 38, and 40.
4. Understand that the difference in the number of neutrons results in different mass numbers for the isotopes.
5. Conclude that the isotopes of argon differ in their mass numbers due to the varying number of neutrons, while having the same number of protons and electrons.

Key Concepts

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This difference in neutron count results in varying mass numbers for the isotopes. For example, argon has isotopes with mass numbers 36, 38, and 40, indicating that they contain 18 protons but differ in their neutron counts.

Mass Number

The mass number of an isotope is the total count of protons and neutrons in its nucleus. It is a crucial identifier for isotopes, as it helps distinguish between them. In the case of argon, the mass numbers 36, 38, and 40 reflect the different combinations of neutrons with the constant number of protons (18) in each isotope.

Stability of Isotopes

Isotopes can vary in stability, with some being stable and others radioactive. Stable isotopes do not undergo radioactive decay, while unstable isotopes may decay over time, emitting radiation. The isotopes of argon (36, 38, and 40) are all stable, which means they do not change into other elements or isotopes over time.