What is the nuclear configuration of the daughter nucleus associated with the alpha decay of \(\mathrm{Hf}(A=157,\) \(Z=72\) )?

Understanding the nuclear configuration is crucial when discussing alpha decay. The nucleus of an atom consists of protons and neutrons, collectively known as nucleons. During alpha decay, a nucleus emits an alpha particle, which is essentially a helium-4 nucleus, composed of 2 protons and 2 neutrons. This emission causes the original nucleus to lose a total of 4 nucleons, altering both its atomic mass and atomic number, and resulting in a different nuclear configuration for the daughter nucleus. Therefore, the nuclear configuration refers to the specific arrangement and number of protons and neutrons in an atomic nucleus.

Nuclear configuration plays a pivotal role in the stability of an atom. Atoms aim for a balanced state, and alpha decay is one way a nucleus can move towards stability if it has an excess of protons or a high mass. By examining alpha decay, we get a glimpse into the natural processes helping to shape the elements around us.

The atomic mass number, denoted as 'A,' is a fundamental concept in understanding alpha decay. It represents the total number of nucleons (protons plus neutrons) in an atom's nucleus. An alpha particle has an atomic mass number of 4, which means that when an atom undergoes alpha decay, it will lose 4 from its atomic mass number. This reduction in 'A' is due to the ejection of an alpha particle.

For instance, in the provided exercise, the element Hafnium, which starts with an atomic mass number of 157, loses an alpha particle leading to a new atomic mass number of 153 for the daughter nucleus. It's important to note that, while the total mass of nucleons changes, the underlying mechanism doesn't alter the individual masses of the remaining protons and neutrons in the nucleus.

The atomic number, represented by 'Z,' indicates the number of protons in an atom's nucleus, which directly defines the chemical element. Unlike neutrons, protons are electrically charged, and their number determines the atom's identity within the periodic table. In alpha decay, the atomic number decreases by 2 because the alpha particle contains 2 protons that are emitted from the nucleus.

In our exercise, Hafnium with an original atomic number of 72 undergoes alpha decay resulting in a daughter nucleus with an atomic number of 70. This change is significant as it transforms the element into a completely different one as listed in the periodic table, from Hafnium to Ytterbium.

Nucleons are the building blocks of an atomic nucleus and include both protons and neutrons. The number of nucleons within a nucleus bears a direct effect on the atom's mass and stability. Alpha decay is a process that influences nucleons by reducing their count, specifically by releasing an alpha particle composed of 2 protons and 2 neutrons.

The concept of nucleons is central to the topic of alpha decay, as the loss of 4 nucleons during the decay alters the nuclear structure and stability of the original atom. After this emission, the resulting daughter nucleus has fewer nucleons, which often leads to a more stable nuclear configuration.

The periodic table is an organized chart of elements arranged by increasing atomic number. It is a fundamental tool in chemistry, that helps predict the properties of elements and their compounds. Each element on the periodic table is represented by its atomic number, which corresponds to the number of protons in its nucleus.

When studying alpha decay, the periodic table allows us to identify the new element formed after the process. Following the alpha decay of Hafnium in our exercise, we refer to the periodic table to find that the daughter nucleus with an atomic number of 70 is Ytterbium (Yb). Without the periodic table, understanding and identifying the outcomes of nuclear reactions like alpha decay would be much more complex.