Isotopes Summary

Isotopes Overview

• Isotopes are different versions of an element or atom.
• Defined by number of protons; same element, varying neutrons.

Analogies to Understand Isotopes

• Example: Car models (Lamona) demonstrate the concept of isotopes.
  • Different models have unique features (colors/options) but are fundamentally the same.

Carbon Isotopes

• Three common isotopes of carbon: Carbon-12, Carbon-13, Carbon-14.
  • Carbon-12: 6 protons, 6 neutrons.
  • Carbon-13: 6 protons, 7 neutrons.
  • Carbon-14: 6 protons, 8 neutrons.
• All share 6 protons; defines them as carbon.

Atomic and Mass Numbers

• Atomic number = number of protons.
• Mass number = protons + neutrons.
  • C-12: 6 + 6 = 12; C-13: 6 + 7 = 13; C-14: 6 + 8 = 14.

Isotope Notation

• Written as:
  • Mass number (top), Atomic number (bottom)
  • Example: Carbon-12 = \text{C}_{6}^{12}.

Other Elements and Isotopes

• Elements (like calcium and iron) also have multiple isotopes.
  • Calcium: Atomic number 20; Calcium isotopes vary in neutrons (e.g., 40, 42, 43).
  • Iron: Atomic number 26; known isotopes vary in neutrons.
• Isotope notation applied similarly for these elements.

Summary

• Atoms exist in different versions (isotopes) based on neutrons.
• Same number of protons = same element, different isotopes.