Fill in the missing particles in each nuclear equation.
a. ____ → ²¹⁷₈₅At + ⁴₂He
b. ²⁴¹₉₄Pu → ²⁴¹₉₅Am + ____
c. ¹⁹₁₁Ne → ¹⁹₁₀Ne + ____
d. ⁷⁵₃₄Se + _____ → ⁷⁵₃₃As

Verified step by step guidance

1. Identify the type of nuclear reaction occurring. In this case, the atomic number decreases by 1, indicating a beta-plus decay (positron emission).
2. In beta-plus decay, a proton is converted into a neutron, and a positron (\( \beta^+ \)) is emitted.
3. Write the nuclear equation for beta-plus decay: \( ^{19}_{11}\text{Ne} \rightarrow ^{19}_{10}\text{Ne} + \beta^+ \).
4. The missing particle is a positron, represented as \( \beta^+ \) or \( ^{0}_{+1}e \).
5. Verify that the mass number and atomic number are balanced on both sides of the 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 are characterized by the conservation of mass and charge, meaning that the total number of protons and neutrons must remain constant before and after the reaction.

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. In the context of nuclear equations, isotopes are crucial for understanding how elements can undergo decay or transformation while maintaining their elemental identity.

Particle Emission

In nuclear equations, particle emission refers to the release of particles such as alpha particles, beta particles, or gamma rays during a nuclear reaction. Identifying the missing particle in a nuclear equation often involves recognizing the type of decay or reaction occurring, which dictates what particle is emitted to balance the equation.