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, 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 an alpha particle is involved, remember it is represented as \(^4_2\text{He}\) or \(^4_2\alpha\). For a beta particle, use \(^0_{-1}\beta\) or \(^0_{-1}e\).
5. Balance the equation by ensuring that the sum of the mass numbers and atomic numbers are equal on both sides, and write the complete balanced nuclear equation.

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 (the sum of protons and neutrons) and the total charge (the sum of positive and negative charges) must be the same on both sides of the equation. Balancing these quantities is essential for accurately completing nuclear equations.

Notation of Nuclear Particles

Nuclear particles are represented using specific notation, where the mass number is written as a superscript and the atomic number as a subscript. For example, a helium nucleus is denoted as 4He, where 4 is the mass number and 2 is the atomic number. Familiarity with this notation is important for identifying and balancing the reactants and products in nuclear equations.