Here's a breakdown:
* Element: Defined by the number of protons in its nucleus. All atoms of a specific element have the same number of protons.
* Isotopes: Atoms of the same element that have different numbers of neutrons. This means they have the same atomic number (number of protons) but different atomic mass (number of protons + neutrons).
Here's an example:
* Carbon-12 has 6 protons and 6 neutrons.
* Carbon-14 has 6 protons and 8 neutrons.
Both are carbon atoms (because they have 6 protons), but they have different numbers of neutrons. This difference in neutron count makes them isotopes.
Key takeaways:
* Isotopes of the same element have the same chemical properties because they have the same number of electrons, which determine how an atom interacts with other atoms.
* Isotopes can have different physical properties, such as density and radioactive decay rates, due to the different number of neutrons.
