Isotopes

Definition

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 atomic masses for the isotopes of an element.

5 Must Know Facts For Your Next Test

1. Isotopes of an element have identical chemical properties but different physical properties due to their varying atomic masses.
2. Stable isotopes do not undergo radioactive decay, while unstable (radioactive) isotopes do.
3. Carbon-12, Carbon-13, and Carbon-14 are common isotopes of carbon, where Carbon-14 is radioactive and used in radiocarbon dating.
4. The presence of different isotopes is crucial for techniques like mass spectrometry and nuclear magnetic resonance (NMR).
5. Hydrogen has three major isotopes: protium (no neutrons), deuterium (one neutron), and tritium (two neutrons), with tritium being radioactive.

Review Questions

• What distinguishes one isotope from another within the same element?
• Why do isotopes have identical chemical properties but different physical properties?
• Give an example of how an isotope can be used in scientific research or practical applications.

Related terms

Atom: The smallest unit of matter that retains the identity of a chemical element, consisting of protons, neutrons, and electrons.

Ion: An atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

Molecule: A group of two or more atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction.