Fill in the missing particles in each nuclear equation. c. ²³⁷₉₃Np → _____ + ⁴₂He

Verified step by step guidance

1. Identify the type of nuclear reaction. In this case, the presence of a helium nucleus (\( ^4_2\text{He} \)) indicates an alpha decay.
2. In alpha decay, the parent nucleus loses 2 protons and 2 neutrons, which means the atomic number decreases by 2 and the mass number decreases by 4.
3. Write the general equation for alpha decay: \( ^A_Z\text{X} \rightarrow ^{A-4}_{Z-2}\text{Y} + ^4_2\text{He} \).
4. Apply the changes to the given nucleus \( ^{237}_{93}\text{Np} \): the new mass number is \( 237 - 4 = 233 \) and the new atomic number is \( 93 - 2 = 91 \).
5. Determine the element with atomic number 91, which is Protactinium (Pa), so the missing particle is \( ^{233}_{91}\text{Pa} \).

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 often include the emission or absorption of particles, such as alpha particles (helium nuclei), beta particles, or gamma rays. Understanding the type of nuclear reaction is crucial for predicting the products formed during the process.

Alpha Decay

Alpha decay is a type of radioactive decay in which an unstable nucleus emits an alpha particle, consisting of two protons and two neutrons. This process decreases the atomic number by two and the mass number by four, resulting in the formation of a new element. Recognizing the characteristics of alpha decay is essential for completing nuclear equations accurately.

Balancing Nuclear Equations

Balancing nuclear equations requires ensuring that both the mass number and atomic number are conserved during the reaction. This means that the sum of the mass numbers and the sum of the atomic numbers on both sides of the equation must be equal. Mastery of this principle is vital for identifying missing particles in nuclear equations.