The Discovery of the Electron
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The Discovery of the Electron
At the end of the 19th century, there was no generally accepted model of the atom. Most physicists believed that the atom was indivisible, although the discovery of radioactivity cast doubt on that in the minds of some physicists. At the same time it was generally believed that electric charge, like mass, was infinitely divisible. To explain the connection between electricity and matter, some scientists in the late 19th century argued that there had to be a fundamental unit of electricity. In 1891 the Irish physicist, George Stoney, introduced the term “electron” to describe this smallest unit of negative charge. In 1897 J. J. Thomson, an English physicist, conducted a series of experiments on cathode rays and after observing that the beam of light in the cathode ray tube is attracted to a positive charge and repelled by a negative charge he concluded that the rays consist of a stream of small, electrically negatively charged particles which have a mass over a thousand times less than that of a hydrogen atom. Thomson has discovered the electron. From this point onward, it becomes increasingly clear that atoms are not fundamental particles, but in fact are made up of smaller particles. As a result of his experiments, Thomson was able to measure the charge to mass ratio of the electron; he could not however, measure accurately the charge or mass independently. The measurement of the electron's charge independently was achieved by Robert Andrews Millikan by his famous experiment from 1909 and with Thomson's results also a value for the electron mass was obtained. This experiment is called the "oil-drop experiment" and it was the first successful scientific attempt to detect and measure the effect of an individual subatomic particle. For this and his work on the photoelectric effect Robert Millikan won the 1923 Nobel Prize in physics.
The scheme of the experiment is as follows: An atomizer sprayed a fine mist of oil droplets into the upper chamber. Some of these tiny droplets fell through a hole in the upper floor into the lower chamber of the apparatus. Millikan first let them fall until they reached terminal velocity due to the air resistance within the container. Using the microscope, he measured their terminal velocity, and by use of a formula, calculated the mass of each oil drop. When the electric field is off at terminal velocity force is equal to zero
Where Fv is the upward force and Fg is the downward force
As the viscous force is not known we use stokes law
Where rd is the radius of the droplet is the viscosity of air and is the velocity of the droplet with the electric field off we do not know the volume or mass of the droplet
As m=v.ρ ⁄ Radius of oil droplet is √
Next, Millikan applied a charge to the falling drops by irradiating the bottom chamber with x-rays. This caused the air to become ionized, which basically means that the air particles lost electrons. A part of the oil droplets captured one or more of those extra electrons and became negatively charged. By attaching a battery to the plates of the lower chamber he created an electric field between the plates that would act on the charged oil drops; he adjusted the voltage till the electric field force would just balance the force of gravity on a drop, and the drop would hang suspended in mid-air. Some drops have captured more electrons than others, so they will require a higher electrical field to stop. Now the electric force is acting upwards and the viscous and gravitational forces are acting downwards. He measured the terminal velocity of the droplet. ∑
articles that did not capture any of the extra electrons were not affected by the electrical field and fell to the bottom plate due to gravity. When a drop is suspended, its weight m · g is exactly equal to the electric force applied, the product of the electric field and the charge q · E. The values of E (the applied electric field), m (the mass of a drop which was already calculated by Millikan), and g (the acceleration due to gravity), are all known values. So it is very easy to obtain the value of q, the charge on the drop, by using the simple formula:
m·g=q·E
Millikan repeated the experiment numerous times, each time varying the strength of the x-rays ionizing the air, so that differing numbers of electrons would jump onto the oil molecules each time. He obtained various values for q. The charge q on a drop was always a multiple of 1.59 x 10-19 Coulombs. This is less than 1% lower than the value accepted today: 1.602 x 10-19 C.
Source: http://www.juliantrubin.com/bigten/millikanoildrop.html
At the end of the 19th century, there was no generally accepted model of the atom. Most physicists believed that the atom was indivisible, although the discovery of radioactivity cast doubt on that in the minds of some physicists. At the same time it was generally believed that electric charge, like mass, was infinitely divisible. To explain the connection between electricity and matter, some scientists in the late 19th century argued that there had to be a fundamental unit of electricity. In 1891 the Irish physicist, George Stoney, introduced the term “electron” to describe this smallest unit of negative charge. In 1897 J. J. Thomson, an English physicist, conducted a series of experiments on cathode rays and after observing that the beam of light in the cathode ray tube is attracted to a positive charge and repelled by a negative charge he concluded that the rays consist of a stream of small, electrically negatively charged particles which have a mass over a thousand times less than that of a hydrogen atom. Thomson has discovered the electron. From this point onward, it becomes increasingly clear that atoms are not fundamental particles, but in fact are made up of smaller particles. As a result of his experiments, Thomson was able to measure the charge to mass ratio of the electron; he could not however, measure accurately the charge or mass independently. The measurement of the electron's charge independently was achieved by Robert Andrews Millikan by his famous experiment from 1909 and with Thomson's results also a value for the electron mass was obtained. This experiment is called the "oil-drop experiment" and it was the first successful scientific attempt to detect and measure the effect of an individual subatomic particle. For this and his work on the photoelectric effect Robert Millikan won the 1923 Nobel Prize in physics.
The scheme of the experiment is as follows: An atomizer sprayed a fine mist of oil droplets into the upper chamber. Some of these tiny droplets fell through a hole in the upper floor into the lower chamber of the apparatus. Millikan first let them fall until they reached terminal velocity due to the air resistance within the container. Using the microscope, he measured their terminal velocity, and by use of a formula, calculated the mass of each oil drop. When the electric field is off at terminal velocity force is equal to zero
Where Fv is the upward force and Fg is the downward force
As the viscous force is not known we use stokes law
Where rd is the radius of the droplet is the viscosity of air and is the velocity of the droplet with the electric field off we do not know the volume or mass of the droplet
As m=v.ρ ⁄ Radius of oil droplet is √
Next, Millikan applied a charge to the falling drops by irradiating the bottom chamber with x-rays. This caused the air to become ionized, which basically means that the air particles lost electrons. A part of the oil droplets captured one or more of those extra electrons and became negatively charged. By attaching a battery to the plates of the lower chamber he created an electric field between the plates that would act on the charged oil drops; he adjusted the voltage till the electric field force would just balance the force of gravity on a drop, and the drop would hang suspended in mid-air. Some drops have captured more electrons than others, so they will require a higher electrical field to stop. Now the electric force is acting upwards and the viscous and gravitational forces are acting downwards. He measured the terminal velocity of the droplet. ∑
articles that did not capture any of the extra electrons were not affected by the electrical field and fell to the bottom plate due to gravity. When a drop is suspended, its weight m · g is exactly equal to the electric force applied, the product of the electric field and the charge q · E. The values of E (the applied electric field), m (the mass of a drop which was already calculated by Millikan), and g (the acceleration due to gravity), are all known values. So it is very easy to obtain the value of q, the charge on the drop, by using the simple formula:
m·g=q·E
Millikan repeated the experiment numerous times, each time varying the strength of the x-rays ionizing the air, so that differing numbers of electrons would jump onto the oil molecules each time. He obtained various values for q. The charge q on a drop was always a multiple of 1.59 x 10-19 Coulombs. This is less than 1% lower than the value accepted today: 1.602 x 10-19 C.
Source: http://www.juliantrubin.com/bigten/millikanoildrop.html
