Isotopes

Isotopes are distinct forms of a chemical element that share the same number of protons (atomic number) but differ in the number of neutrons in their nuclei, leading to variations in mass numbers. Although isotopes exhibit similar chemical behaviours due to their identical electron and proton counts, they differ in physical attributes such as mass and stability. These differences make isotopes valuable for various applications, including medical imaging, archaeological carbon dating, and scientific research.

Key Features of Isotopes:

• Identical Proton Count, Varying Neutron Count: For instance, Carbon-12 has 6 protons and 6 neutrons, whereas Carbon-14 contains 6 protons and 8 neutrons.
• Uniform Chemical Properties: With identical electron arrangements and proton numbers, isotopes occupy the same position on the periodic table and exhibit similar chemical reactivity.
• Divergent Physical Attributes: Differing neutron counts result in variations in atomic mass, influencing their physical properties.
• Stability Variations: Isotopes may either be stable (unchanging over time) or unstable (radioactive). The latter, known as radioisotopes, undergo radioactive decay while releasing radiation.

Well-Known Examples:

• Hydrogen: Includes protium (no neutrons), deuterium (one neutron), and tritium (two neutrons).
• Carbon: Encompasses Carbon-12 and Carbon-13, both stable, and Carbon-14, a radioactive isotope commonly used for age determination through radiocarbon dating.

Sources:

[1] https://www.aakash.ac.in/blog/isotopes-definition-types-application-significance-in-physics/  

[2] https://www.cancer.gov/publications/dictionaries/cancer-terms/def/isotope  

[3] https://www.iaea.org/newscenter/news/what-are-isotopes  

[4] https://www.energy.gov/science/doe-explainsisotopes  

[5] https://byjus.com/chemistry/isotope-meaning/  

[6] https://en.wikipedia.org/wiki/Isotope  

[7] https://study.com/academy/lesson/what-are-isotopes-definition-types-examples.html