Astatine, the last member of Group \(7 \mathrm{~A},\) can be prepared by bombarding bismuth- 209 with \(\alpha\) particles. (a) Write an equation for the reaction. (b) Represent the equation in the abbreviated form, as discussed in Section 19.4 .

Picture a tiny but incredibly energetic helium nucleus, known as an alpha particle, hurtling through space and smashing into the nucleus of another atom. This process, called alpha particle bombardment, is a type of nuclear reaction that can transform one element into another. In our specific textbook exercise, bismuth-209 is the target of such alpha particle bombardment. This interaction leads to the creation of a new element, astatine, through a dynamic and powerful exchange of particles.

Alpha particles are positively charged and consist of two protons and two neutrons, resembling a helium nucleus. When these particles collide with the nucleus of an atom like bismuth, they can be absorbed, resulting in an increase in both the atomic and mass numbers of the affected nucleus. This transformation is leveraged in nuclear chemistry to synthesize new elements and isotopes that are not readily available in nature. Understanding the mechanics of alpha particle bombardment is also critical in fields like radiotherapy, where it forms the underlying technology for certain types of cancer treatments.

In any nuclear reaction, including the one involving alpha particle bombardment, two fundamental principles are always observed: the conservation of mass and the conservation of charge. These principles indicate that the total mass and total charge must remain constant before and after a nuclear reaction has occurred. In other words, the sum of the mass numbers and the sum of the atomic numbers of the reactants must equal those of the products.

When an alpha particle ( isotopes and gaining insight into nuclear stability and radioactive decay patterns.

Navigating the world of nuclear chemistry requires familiarity with isotope notation, which provides a shorthand way to express the identity and characteristics of an atom. An isotope is defined by its atomic number (number of protons, often denoted as 'Z') and its mass number (combined number of protons and neutrons, denoted as 'A'). These are typically written as a subscript and superscript to the left of the element's symbol.

For instance, the notation isotopes.

At its core, nuclear chemistry delves into the reactions and changes that occur within the nucleus of an atom. Unlike traditional chemical reactions that involve the exchange or sharing of electrons, nuclear chemistry deals with transformations that can alter one element into another—such as in the alpha particle bombardment of bismuth-209 to form astatine.

Nuclear chemistry includes the study of radioactive decay, nuclear fission and fusion, and the behavior of elements at the nuclear level. It plays a vital role in energy generation through nuclear power plants, the development of medical technologies, such as radiopharmaceuticals for diagnosis and treatment, and even in our understanding of the origin of elements in the universe through stellar nucleosynthesis. As we've seen in our exercise, it also has practical applications in synthesizing new elements, significantly shaping the landscape of modern science and technology.