Nuclear Reaction

Water (H2O)

• Represents the chemical formula for water.

Atomic Mass

Key Concepts

• Atomic mass is calculated using the formula: 2X A = Element Symbol x Atomic Number

• Example value represented is 4.

Atomic Number

• Defined as the number of protons in an atom.

• Equals the number of electrons in a neutral atom.

• Example: An atomic number of 2.

Identity of an Atom

• The atomic number serves as the identity of an atom.

• Each element has a unique atomic number.

Subatomic Particles and Stability

• Stable elements usually have the same number of subatomic particles: neutrons, protons, and electrons.

Isotopes

• Variants of a chemical element that differ in neutron number.

• Isotopes maintain the same atomic number but have different atomic masses.

Nuclear Reactions

Types

• Nuclear reactions involve changes to the nucleus and can occur in two main ways:

  • Nuclear Fusion: where two nuclei combine.

  • Nuclear Fission: where a nucleus splits into smaller parts.

Types of Nuclear Reactions

• Representations include alpha decay, beta decay, gamma radiation, and positron emissions:

  • Alpha particles (4𝛼)

  • Beta particles (0𝛽)

  • Gamma rays (0𝛾)

  • Electrons (−1 0𝑒)

Specific Nuclear Reactions

• Various nuclear equations displayed such as decay of Uranium-238 and conversion of Sodium-24, indicating transformations involving alpha and beta particles.

Beta Decay

• Example of a decay where a neutron changes into a proton and an electron is emitted (beta particle).

• Represented in reactions leading to the formation of nitrogen from carbon (14 6C -> 14 7N).

Positron Emission

• Involves the release of a positron, which is an anti-electron.

• Examples of positron emissions from different isotopes (e.g., 15 15N).

Bombardment of Alpha Particles

• The process of bombarding a nucleus with alpha particles, leading to a reaction with other elements, such as Boron and Uranium.

• Symbolically represented with equations indicating the resulting particles.