Radioactive Decay in Nuclear Chemistry

Types of Particles

1. Alpha Particle

   • Mass: 4
   • Charge: 2
   • Equivalent to the nucleus of a helium atom.

2. Beta Particle

   • Mass: 0
   • Charge: -1
   • Equivalent to an electron.

3. Positron

   • Mass: 0
   • Charge: +1
   • Antiparticle of an electron.

4. Proton

   • Mass: 1
   • Charge: 1

5. Neutron

   • Mass: 1
   • Charge: 0

6. Gamma Particle

   • Mass: 0
   • Charge: 0
   • High energy photon.

Example: Beta Decay

• Equation Setup: Nitrogen-13 decays into a beta particle and another element.
  • Mass: 0 + 13 = 13
  • Charge: -1 + 8 = 7
  • Resulting Element: Oxygen-13
• Effects of Beta Decay:
  • Mass remains constant.
  • Atomic number increases (number of protons increases).
  • Number of neutrons decreases (neutron converted to a proton).

Example: Positron Production

• Equation Setup: Nitrogen-13 decays into a positron and another element.
  • Atomic Number: 7 - 1 = 6
  • Resulting Element: Carbon
• Effects of Positron Production:
  • Atomic number decreases (proton converted to a neutron).
  • Neutron number increases.
  • Positron meets an electron, annihilating to form gamma radiation.

Electron Capture

• Explanation: The nucleus captures an electron, forming a neutron.
• Example: Arsenic-73 captures an electron.
  • Atomic Number: 33 + 1 = 32, resulting in Germanium.
  • Effects:
    • Proton number decreases.
    • Neutron number increases (proton + electron = neutron).

Alpha Particle Production

• Explanation: Production of an alpha particle by an element.
• Example: Element with atomic number 84 produces an alpha particle.
  • Mass Loss: 4
  • Atomic Number Loss: 2
  • Resulting Element: Lead (Pb)
• Balancing Reactions: Ensure masses and charges are balanced on both sides of the equation.

Conclusion

• Introduction to nuclear chemistry focusing on radioactive decay.
• Importance of balancing nuclear equations using mass and atomic number conservation.