Write the nuclear equation for the fusion of two \(\mathrm{H}-2\) atoms to form He- 3 and one neutron. MISSED THIS?

Nuclear chemistry falls within the field of chemistry that deals with changes in the nucleus of atoms. Unlike traditional chemical reactions which involve electrons and their bonds, nuclear reactions involve changes in an atom's nucleus, leading to the transformation of one element into another.

Essential to understanding nuclear chemistry is the concept of the nuclear reaction, which is a process where a nucleus, bombarded by neutrons, protons, or other nuclei, undergoes a change that can result in a different element or isotope. The nuclear fusion equation we are considering is a brilliant example of nuclear reactions.

The fusion process, as mentioned in the exercise, leads to immense energy release and is the same process that powers the sun. One key factor in these reactions is the mass-energy equivalence principle, famously known by Einstein's equation, \( E=mc^2 \). This explains why nuclear reactions can release much larger amounts of energy compared to chemical reactions.

Isotopes are versions of a chemical element that have the same number of protons but a different number of neutrons in their nucleus. This variation in neutron number results in atoms with the same atomic number but different mass numbers.

For instance, in the textbook exercise, \( \mathrm{^2_1H} \) is an isotope of hydrogen known as deuterium. Its nucleus contains one proton and one neutron, distinguishing it from the common hydrogen isotope \( \mathrm{^1_1H} \), which has no neutrons.

Isotopes can be stable or radioactive. Stable isotopes do not change over time, while radioactive isotopes decay, releasing radiation. Deuterium is a stable isotope, which makes it crucial for studies in nuclear chemistry, including the exploration of nuclear fusion as a potential energy source.

Balancing chemical reactions is a fundamental skill in chemistry, ensuring that the same number of each type of atom is present on both sides of the equation. This principle stems from the law of conservation of mass, indicating that mass cannot be created or destroyed in a chemical reaction.

In nuclear chemistry, the process is similar but we focus on balancing both mass numbers and atomic numbers in nuclear equations. For our nuclear fusion equation, \( \mathrm{^2_1H} + ^2_1H \rightarrow ^3_2He + ^1_0n \), note that the mass numbers on the left total to 4 (2+2), which equals the sum of the mass numbers on the right (3+1). Similarly, the atomic numbers on the left total to 2 (1+1), which equals the atomic number of helium (2) plus the neutron (which does not contribute to the atomic number as its value is 0).

This balancing is crucial because it reflects the conservation of nucleons—protons and neutrons—in the reaction, and it follows the same principles whether the equation represents a simple chemical reaction or a complex nuclear transformation.