What exactly are isotopes?

Isotopes are variants of a particular chemical element which have different numbers of neutrons in their nucleus.

Isotopes are a fundamental concept in chemistry. They are versions of a particular chemical element that share the same number of protons but have different numbers of neutrons in their nucleus. This means that while they are the same element, they have different atomic masses. For example, carbon-12 and carbon-14 are both isotopes of carbon, but carbon-12 has 6 neutrons while carbon-14 has 8.

The term 'isotope' comes from the Greek words 'isos' meaning 'same' and 'topos' meaning 'place', referring to the fact that different isotopes of an element occupy the same position on the periodic table. Despite their differences in atomic mass, isotopes of an element exhibit almost identical chemical behaviour. This is because the number of protons in an atom (its atomic number) determines its chemical properties, and this number is the same for all isotopes of a given element.

However, isotopes can have different physical properties. For instance, some isotopes are stable, meaning they remain unchanged indefinitely. Others are unstable or radioactive, meaning they decay over time into other elements and emit radiation. This radioactive decay is a key tool in many scientific fields, including archaeology (for carbon dating), medicine (for radiation therapy), and nuclear power.

In summary, isotopes are versions of a particular chemical element that have the same number of protons but different numbers of neutrons. They have the same chemical properties as the parent element, but can have different physical properties, including atomic mass and stability. Understanding isotopes is crucial for many areas of science and technology.