Electron Mass

Electrons are subatomic particles that make up the most fundamental part of atoms, along with protons and neutrons. For a long time, the atom was thought to be an element’s final structure. Because it derives from a Greek word that means “indivisible,” the term “atom” is a perfect representation of that idea. All of that changed in 1897, when English physicist J.J. Thomson discovered electrons as part of subatomic particles, or particles that make up the atom, through his now-famous cathode ray tube studies.

Atoms

Atoms are the smallest components of an element, and the study of atomic models became popular in the 18th and 19th centuries. Based on their research, many scientists developed theories on the structure of atoms. These hypotheses were presented in order to further our understanding of the structure of atoms and their constituents.

The atomic model’s most well-liked theories were proposed by Ernest Rutherford, John Dalton, J.J Thomson, Niels Bohr, and J.J Thomson.

All of these scientists’ ideas resulted in a new notion and better explanations. It also piqued the curiosity of other scientists in studying and researching the atom. Each hypothesis has its own brief explanation, strengths, and limitations, as well as exceptions.

An atom is made up of two parts: a nucleus in the centre that contains protons (positively charged particles) and neutrons (negatively charged particles), and an outer shell that contains electrons (negatively charged particles). In a spiral motion, the electrons in the outer shells constantly revolve around the nucleus.

Cathode ray tube

1. J. Thomson created a partially evacuated glass tube, meaning that a significant amount of air was driven out. He then applied a high electrical voltage to both ends of the tube using two electrodes. He noticed a stream of particles (ray) moving from the negatively charged cathode to the positively charged anode electrode (anode). A cathode ray is the name for the ray, while a cathode ray tube is the name for the overall structure.

Observations made from cathode ray tube

1. There were rays emerging from the cathode towards the anode when a high voltage power supply was turned on. The ‘Fluorescent dots’ on the ZnS screen utilised proved this. “Cathode Rays” were the name given to these rays.
2. The cathode rays are bent towards the positive electrode when an external electric field is introduced, but they move in a straight line when there is no electric field.
3. Rotor Blades appear to rotate when they are put in the path of the cathode rays. This demonstrates that cathode rays are composed of particles of a specific mass and so have energy.
4. Thompson determined that cathode rays are made up of negatively charged particles known as “electrons” based on all of the evidence.
5. Thomson discovered the charge to mass ratio (e/m) of electrons by applying an electric and magnetic field to cathode rays (electrons). 1.758820×1011 C/kg for electrons.

Proton:

The positively charged particles that make up an atom’s nucleus are known as protons. Goldstein discovered in 1886 that the charge and mass ratio of these positively charged particles is affected by the gas’s composition. As a result, the charge to mass ratio (e/m) varies depending on the gas.

Proton’s Charge: Protons have a positive charge. The number of charges in an electron equals the charge of a. (negative charge).

A proton’s charge is +1.602×10-19C

The mass of a proton is regarded to be the same as that of a hydrogen atom. Because a hydrogen atom is made up of one electron and one proton, and the mass of an electron is negligible, the mass of a proton is equal to that of a hydrogen atom.

A proton’s mass is1.676×10-27kg.

Electron:

The outer shells of an atom contain electrons, which are negatively charged particles. With his cathode ray tubes experiment in 1897, J.J Thomson discovered electrons. An electron’s charge is equal to and opposite that of a proton in an atom. Because their charges cancel each other out, atoms are naturally neutral.

Electron Charge: An electron is a negatively charged atom. It has a negative unit on it.

Charge of an electron is -1.602×10-19C

In an atom, the mass of an electron is insignificant. It has a mass of 1/1837 of that of a proton.

An electron’s mass is 9.1093×10-31kg.

Neutron

Neutrons are subatomic particles with the property of neutrality. They are exempt from any charges. Neutrons, along with protons, make up the nucleus’s primary ingredient. The mass of a neutron is somewhat larger than that of a proton. The chemical characteristics of an atom are determined by the protons and neutrons in the nucleus.

A neutron’s charge is: Neutrons have no charge because they are neutrally charged subatomic particles.

The mass of a neutron is derived by subtracting the mass of the proton from the mass of the deuterium nucleus. A neutron has a mass of 1.008 atomic mass units (amu).

A neutron’s mass is 1.676×10-27kg.

Conclusion

According to Dalton’s atomic theory, atoms are the tiniest particles of an element that have the same properties as the element and can never be generated or destroyed. However, as the atom is broken further, electrons, protons, and neutrons are produced. These three particles are the sole ones that make up an atom. Because every atom of any given element contains exactly the same subatomic particle as the other, it will have the same physical properties.