Complete and balance the following nuclear equations. (b)

Verified step by step guidance

1. Identify the type of nuclear reaction involved (e.g., alpha decay, beta decay, positron emission, electron capture, etc.).
2. Write down the known parts of the nuclear equation, including the reactants and any given products.
3. Use the conservation of mass number and atomic number to determine the missing particles or nuclei. The sum of mass numbers (top numbers) and atomic numbers (bottom numbers) must be equal on both sides of the equation.
4. If the reaction involves a common particle (e.g., alpha particle \(^4_2\text{He}\), beta particle \(^0_{-1}\text{e}\), neutron \(^1_0\text{n}\), etc.), include it in the equation to balance it.
5. Double-check the balanced equation to ensure that both the mass numbers and atomic numbers are equal on both sides, confirming that the equation is balanced.

Key Concepts

Nuclear Reactions

Nuclear reactions involve changes in an atom's nucleus and can result in the transformation of one element into another. These reactions include processes such as alpha decay, beta decay, and nuclear fission. Understanding the type of nuclear reaction is crucial for balancing nuclear equations, as it dictates the particles involved and the resulting products.

Conservation of Mass and Charge

In nuclear equations, both mass and charge must be conserved. This means that the total mass number (sum of protons and neutrons) and the total charge (sum of positive and negative charges) before the reaction must equal those after the reaction. Balancing these quantities is essential for correctly completing nuclear equations.

Notation of Nuclear Particles

Nuclear particles are represented using specific notation, where the element symbol is accompanied by its mass number and atomic number. For example, an alpha particle is denoted as 4He2, indicating it has a mass number of 4 and an atomic number of 2. Familiarity with this notation is necessary for accurately writing and balancing nuclear equations.