Identify the starting radioisotopes needed to balance each of these nuclear reactions:a.
b.

Verified step by step guidance

1. Identify the known particles in the reaction: \(^4_2He\) (alpha particle), \(^1_0n\) (neutron), and \(^244_{94}Pu\) (plutonium).
2. Apply the law of conservation of mass and atomic numbers: the sum of mass numbers and atomic numbers on the left must equal the sum on the right.
3. Calculate the total mass number on the right side: 244 (Pu) + 1 (n) = 245.
4. Calculate the total atomic number on the right side: 94 (Pu) + 0 (n) = 94.
5. Determine the missing isotope by subtracting the mass and atomic numbers of \(^4_2He\) from the totals on the right: Mass number: 245 - 4 = 241, Atomic number: 94 - 2 = 92.

Key Concepts

Nuclear Reactions

Nuclear reactions involve the transformation of atomic nuclei, resulting in the release or absorption of energy. They can include processes such as fusion, fission, and radioactive decay. Understanding the conservation of mass and charge is crucial, as the total number of nucleons (protons and neutrons) and the total charge must remain constant before and after the reaction.

Radioisotopes

Radioisotopes are unstable isotopes of elements that decay over time, emitting radiation in the form of alpha, beta, or gamma rays. They are characterized by their half-lives and decay modes. In nuclear reactions, identifying the correct radioisotopes is essential for balancing the equation, as they determine the reactants and products involved in the reaction.

Balancing Nuclear Equations

Balancing nuclear equations requires ensuring that both the mass number and atomic number are conserved. This involves adjusting the reactants to match the total mass and charge of the products. In the given reaction, one must identify the missing radioisotope that, when combined with helium, produces plutonium and a neutron, maintaining the balance of nucleons and charge.