7.4 Nuclear decay and conservation laws  (Page 2/25)

If you examine the periodic table of the elements, you will find that Th has $Z=\text{90}$ , two fewer than U, which has $Z=\text{92}$ . Similarly, in the second decay equation    , we see that U has two fewer protons than Pu, which has $Z=\text{94}$ . The general rule for $\alpha$ decay is best written in the format ${}_Z^A{\text{X}}_N$ . If a certain nuclide is known to $\alpha$ decay (generally this information must be looked up in a table of isotopes, such as in Appendix B ), its $\alpha$ decay equation    is

where Y is the nuclide that has two fewer protons than X, such as Th having two fewer than U. So if you were told that ${}^{\text{239}}\text{Pu}$ $\alpha$ decays and were asked to write the complete decay equation, you would first look up which element has two fewer protons (an atomic number two lower) and find that this is uranium. Then since four nucleons have broken away from the original 239, its atomic mass would be 235.

It is instructive to examine conservation laws related to $\alpha$ decay. You can see from the equation ${}_Z^A{\text{X}}_N\to {}_{Z-2}^{A-4}{\text{Y}}_{N-2}+{}_2^4{\text{He}}_2$ that total charge is conserved. Linear and angular momentum are conserved, too. Although conserved angular momentum is not of great consequence in this type of decay, conservation of linear momentum has interesting consequences. If the nucleus is at rest when it decays, its momentum is zero. In that case, the fragments must fly in opposite directions with equal-magnitude momenta so that total momentum remains zero. This results in the $\alpha$ particle carrying away most of the energy, as a bullet from a heavy rifle carries away most of the energy of the powder burned to shoot it. Total mass–energy is also conserved: the energy produced in the decay comes from conversion of a fraction of the original mass. As discussed in Atomic Physics , the general relationship is

Here, $E$ is the nuclear reaction energy    (the reaction can be nuclear decay or any other reaction), and $\mathrm{\Delta }m$ is the difference in mass between initial and final products. When the final products have less total mass, $\mathrm{\Delta }m$ is positive, and the reaction releases energy (is exothermic). When the products have greater total mass, the reaction is endothermic ( $\mathrm{\Delta }m$ is negative) and must be induced with an energy input. For $\alpha$ decay to be spontaneous, the decay products must have smaller mass than the parent.