How many protons and neutrons are in this nuclide? 219 86Rn

Understanding the building blocks of an atom is crucial for grasping atomic structure.

Protons

Protons are the positively charged particles found in the nucleus of an atom. One of the fundamental characteristics of protons is that they define the element's identity. For example, the element with 86 protons will always be radon (Rn), and changing the number of protons means changing the element entirely.

Neutrons

Neutrons, on the other hand, are neutral particles, also located in the nucleus. They roughly have the same mass as protons but do not carry a charge. Neutrons play a key role in providing stability to the nucleus, and the number of neutrons can vary within atoms of the same element, forming different isotopes, or 'nuclides.'

In solving problems related to atomic structure, especially for identifying the atomic makeup of a nuclide, it's important to understand the delicate balance between these particles, which contributes to the properties of an atom.

The

atomic number

is a fundamental property that defines an element's identity on the periodic table. Represented by the symbol 'Z,' it is equal to the number of protons found in the nucleus of an atom. Since each element is unique, the atomic number will always be unique for every element. For example, the atomic number of radon (Rn) is 86, which implies that any atom with 86 protons will be recognized as radon.

In our example with radon, by looking at the symbol _86^219Rn, the atomic number is clearly indicated as 86, confirming the element and allowing us to conclude its proton count. This number is essential when determining the composition of a nuclide, as it provides the starting point to find out the other characteristics, like mass number and neutron count.

The

mass number

, represented by 'A,' is the sum of protons and neutrons in an atom's nucleus. It gives us a near approximation of an atom's total mass since electrons have a negligible mass compared to protons and neutrons. Mass number is crucial when one needs to distinguish between different isotopes of the same element.

For the nuclide _86^219Rn, 219 is the mass number indicating that the combined total of protons and neutrons in the nucleus is 219. With this information, coupled with the atomic number, one can easily deduce the neutron count. The subtle difference in mass number among isotopes can lead to varied properties, even though the element remains the same.

A

nuclide

is a term used to describe a specific type of an atom, identified by the number of protons and neutrons in its nucleus. While 'isotope' often refers to atoms with the same number of protons but a different number of neutrons, 'nuclide' is a more general term that includes all isotopes of all elements.

In our exercise, _86^219Rn is a nuclide of the element radon. By specifying the mass number (219) and the atomic number (86), the term pinpoints one particular kind of radon atom—one with 86 protons and 133 neutrons. Understanding nuclides is important not only in the context of chemistry and physics but also in fields like medicine and archaeology, where radioactive isotopes (radioisotopes) play a crucial role.