Here's a breakdown:
* Atomic Number: All isotopes of a given element have the same atomic number, which represents the number of protons in the nucleus. This is what defines the element itself.
* Mass Number: Isotopes differ in their mass number, which is the total number of protons and neutrons in the nucleus.
* Neutrons: Since isotopes of the same element have the same number of protons, the difference in their mass number comes from the varying number of neutrons.
Example:
* Carbon-12 has 6 protons and 6 neutrons (mass number = 12).
* Carbon-14 has 6 protons and 8 neutrons (mass number = 14).
Both are carbon because they have 6 protons, but they have different numbers of neutrons, leading to different mass numbers.
Key Points:
* Isotopes have the same chemical properties due to having the same number of electrons.
* Isotopes can be stable or radioactive, depending on the neutron-to-proton ratio.
* Some isotopes are used in various applications, including medicine, dating techniques, and nuclear energy.
