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Okay, let's talk about **isotopes**. We touched on them before, but let's dive deeper! Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. This means they have the same atomic number (the number of protons) but different mass numbers (the sum of protons and neutrons). For example, carbon-12 has 6 protons and 6 neutrons, while carbon-14 has 6 protons and 8 neutrons. Both are carbon, but their different neutron counts give them different properties. Isotopes of the same element have the same chemical properties because their electron configurations are the same. However, they can have different physical properties, such as mass and stability. Some isotopes are stable, while others are unstable and undergo radioactive decay. **Radioactive isotopes** are widely used in medicine, archaeology, and other fields. For example, carbon-14 is used to date organic materials, uranium isotopes are used to generate nuclear power, and iodine-131 is used in treating thyroid disorders. Isotopes offer valuable insights into the behavior of atoms and their role in a wide range of applications. They show that even within the same element, there can be interesting variations that have significant impacts.
