Learning Objectives

• What Is An Atomic Mass Unit
• Mass Of An Electron In Amu
• Mass Of Electron In Amu
• Mass Of One Electron In Amu

Thus, the bromine molecule may be composed of two 79 Br atoms (mass 158 amu), two 81 Br atoms (mass 162 amu) or the more probable combination of 79 Br-81 Br (mass 160 amu). Fragmentation of Br 2 to a bromine cation then gives rise to equal sized ion peaks at 79 and 81 amu. The invariant mass of an electron is approximately 9.109 × 10−31 kilograms, or 5.489 × 10−4 atomic mass units. On the basis of Einstein 's principle of mass–energy equivalence, this mass corresponds to a rest energy of 0.511 MeV. The ratio between the mass of a proton and that of an electron is about 1836. Boron has primarily two isotopes, one with an atomic mass of 11.0 amu and another with an atomic mass of 10.0 amu. If the abundance of the boron atom with a mass of 11.0 amu is 18.9 percent and the abundance of the other isotope is 81.1 percent, what would be the average mass of the boron atom? The mass of the atom 2311 Na is 22.9898 amu. (a) Calculate its binding energy per atom in millions of electron volts.

• Describe the locations, charges, and masses of the three main subatomic particles.
• Determine the number of protons and electrons in an atom.
• Define atomic mass unit (amu).

Dalton's Atomic Theory explained a lot about matter, chemicals, and chemical reactions. Nevertheless, it was not entirely accurate, because contrary to what Dalton believed, atoms can, in fact, be broken apart into smaller subunits or subatomic particles. We have been talking about the electron in great detail, but there are two other particles of interest to us: protons and neutrons. We already learned that J. J. Thomson discovered a negatively charged particle, called the electron. Rutherford proposed that these electrons orbit a positive nucleus. In subsequent experiments, he found that there is a smaller positively charged particle in the nucleus which is called a proton. There is also a third subatomic particle, known as a neutron.

Electrons

Electrons are one of three main types of particles that make up atoms. Unlike protons and neutrons, which consist of smaller, simpler particles, electrons are fundamental particles that do not consist of smaller particles. They are a type of fundamental particles called leptons. All leptons have an electric charge of (-1) or (0). Electrons are extremely small. The mass of an electron is only about 1/2000 the mass of a proton or neutron, so electrons contribute virtually nothing to the total mass of an atom. Electrons have an electric charge of (-1), which is equal but opposite to the charge of a proton, which is (+1). All atoms have the same number of electrons as protons, so the positive and negative charges 'cancel out', making atoms electrically neutral.

What Is An Atomic Mass Unit

Unlike protons and neutrons, which are located inside the nucleus at the center of the atom, electrons are found outside the nucleus. Because opposite electric charges attract each other, negative electrons are attracted to the positive nucleus. This force of attraction keeps electrons constantly moving through the otherwise empty space around the nucleus. The figure below is a common way to represent the structure of an atom. It shows the electron as a particle orbiting the nucleus, similar to the way that planets orbit the sun. This is however, an incorrect perspective, as quantum mechanics demonstrates that electrons are more complicated.

Protons

A proton is one of three main particles that make up the atom. Protons are found in the nucleus of the atom. This is a tiny, dense region at the center of the atom. Protons have a positive electrical charge of one (left( +1 right)) and a mass of 1 atomic mass unit (left( text{amu} right)), which is about (1.67 times 10^{-27}) kilograms. Together with neutrons, they make up virtually all of the mass of an atom.

Neutrons

Atoms of all elements—except for most atoms of hydrogen—have neutrons in their nucleus. Unlike protons and electrons, which are electrically charged, neutrons have no charge—they are electrically neutral. That's why the neutrons in the diagram above are labeled (n^0). The zero stands for 'zero charge'. The mass of a neutron is slightly greater than the mass of a proton, which is 1 atomic mass unit (left( text{amu} right)). (An atomic mass unit equals about (1.67 times 10^{-27}) kilograms.) A neutron also has about the same diameter as a proton, or (1.7 times 10^{-15}) meters.

As you might have already guessed from its name, the neutron is neutral. In other words, it has no charge whatsoever and is therefore neither attracted to nor repelled from other objects. Neutrons are in every atom (with one exception), and they are bound together with other neutrons and protons in the atomic nucleus.

Before we move on, we must discuss how the different types of subatomic particles interact with each other. When it comes to neutrons, the answer is obvious. Since neutrons are neither attracted to nor repelled from objects, they don't really interact with protons or electrons (beyond being bound into the nucleus with the protons).

Mass Of An Electron In Amu

Even though electrons, protons, and neutrons are all types of subatomic particles, they are not all the same size. When you compare the masses of electrons, protons, and neutrons, what you find is that electrons have an extremely small mass, compared to either protons or neutrons. On the other hand, the masses of protons and neutrons are fairly similar, although technically, the mass of a neutron is slightly larger than the mass of a proton. Because protons and neutrons are so much more massive than electrons, almost all of the mass of any atom comes from the nucleus, which contains all of the neutrons and protons.

Mass Of Electron In Amu

Mass Of One Electron In Amu

Table (PageIndex{1}) gives the properties and locations of electrons, protons, and neutrons. The third column shows the masses of the three subatomic particles in 'atomic mass units.' An atomic mass unit ((text{amu})) is defined as one-twelfth of the mass of a carbon-12 atom. Atomic mass units ((text{amu})) are useful, because, as you can see, the mass of a proton and the mass of a neutron are almost exactly (1) in this unit system.

Negative and positive charges of equal magnitude cancel each other out. This means that the negative charge on an electron perfectly balances the positive charge on the proton. In other words, a neutral atom must have exactly one electron for every proton. If a neutral atom has 1 proton, it must have 1 electron. If a neutral atom has 2 protons, it must have 2 electrons. If a neutral atom has 10 protons, it must have 10 electrons. You get the idea. In order to be neutral, an atom must have the same number of electrons and protons.

Summary

• Electrons are a type of subatomic particle with a negative charge.
• Protons are a type of subatomic particle with a positive charge. Protons are bound together in an atom's nucleus as a result of the strong nuclear force.
• Neutrons are a type of subatomic particle with no charge (they are neutral). Like protons, neutrons are bound into the atom's nucleus as a result of the strong nuclear force.
• Protons and neutrons have approximately the same mass, but they are both much more massive than electrons (approximately 2,000 times as massive as an electron).
• The positive charge on a proton is equal in magnitude to the negative charge on an electron. As a result, a neutral atom must have an equal number of protons and electrons.
• The atomic mass unit (amu) is a unit of mass equal to one-twelfth the mass of a carbon-12 atom

Contributions & Attributions

This page was constructed from content via the following contributor(s) and edited (topically or extensively) by the LibreTexts development team to meet platform style, presentation, and quality:

• CK-12 Foundation by Sharon Bewick, Richard Parsons, Therese Forsythe, Shonna Robinson, and Jean Dupon.

• Marisa Alviar-Agnew (Sacramento City College)

• Henry Agnew (UC Davis)