Why don't we count the electrons when determining the mass of an element?

The center of an atom, known as the atomic nucleus, is the dense core where most of the atom's mass is concentrated. Despite being tiny compared to the overall size of the atom, the nucleus plays a crucial role in determining an atom's mass and, therefore, its atomic mass.

Within this core, two types of subatomic particles reside: protons and neutrons. Protons carry a positive electric charge, while neutrons are neutral, bearing no charge. However, what they have in common is their significant contribution to the mass of the atom. Each nucleon, be it a proton or neutron, has an approximate mass of 1 atomic mass unit (amu).

In the study of chemistry and physics, it's essential to note that the atomic mass of an element is almost entirely due to the nucleons within the nucleus. Although electrons are also part of the atom, their contribution to an atom's mass is minuscule and, as a result, often disregarded for practical purposes such as calculating the element's atomic weight.

Atoms are made up of tiny components called subatomic particles. These are predominantly protons, neutrons, and electrons. While protons and neutrons are located in the nucleus, electrons orbit the nucleus within a cloud referred to as the electron shell.

Understand the Mass Disparities

When considering mass, protons and neutrons are each roughly 1 amu, a considerable weight in atomic terms. Electrons, on the other hand, are significantly lighter, with a mass of about 0.00055 amu. This vast difference in mass is why when calculating atomic mass, the focus is on protons and neutrons, as electrons' contribution to the total mass of the atom is virtually negligible.

Importance of Electrons Despite Low Mass

It's worth noting that while their mass is minimal, electrons play a pivotal role in chemical reactions and bond formations. Although they don't impact the atomic mass much, they are integral to the chemical identity and behavior of the atom.

The term nucleon refers collectively to the two primary particles that reside in the nucleus: protons and neutrons. Nucleons are the heavyweight champions of the atom, as their combined mass gives an element its heft.

Their similar mass of approximately 1 amu makes their contribution to the atomic mass significant and equivalent in terms of mass units. Since atomic mass is a determining factor in the properties of elements and their behavior, understanding the role of nucleons is fundamental in chemistry.

An interesting point to consider is the slightly greater mass of a neutron compared to a proton. However, this slight difference is typically not enough to affect the general calculation of atomic mass in a way that includes consideration of electrons, whose mass is over 1800 times less than that of a proton or neutron.