Missing Figures
Characteristics of Light
There are a few fundamental characteristics of light that are useful to be aware of before proceeding with the discussion on how CCD's and Film can function to save a useful, meaningful image. One of these important fundamental qualities is the fact that visible light is electromagnetic radiation.
Electromagnetic Radiation, Photons, and Energy Levels
Electromagnetic radiation has many different classifications. Some such classifications include AM/FM Radio Waves, microwaves, visible light, x-rays, and gamma rays. A key factor in these classifications is that each different type or "level" of electromagnetic radiation contains different energy levels. These energy levels are determined by the speed or rate that charges from a given source move to create an electric field (for instance, moving charges through an antenna or lightbulb) (Serway 1090). Hence, this oscillating electric field has two very important characteristics: it has a frequency and a wavelength. Furthermore, light can also behave as a particle in some instances. This particle of light is called a photon, and is essentially the amount of energy that a light wave has at a certain frequency (the energy of a photon is not dependent on the intensity of the light, but rather only dependent upon its frequency) (Serway 1107). It is this "duality of light" that allows CCD's and film to function as they do, as energy is transferred to materials through light via. photons.
Since the energy of a photon is only related to its frequency, an equation (discovered by Einstein) relates photons to the electrons they produce by:
E = h * f
Where E is the energy of the produced electron, h is Planck's constant (6.63 * 10^-34 J...
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Once a value for e/m was obtained the mass of an electron can be calculated using this ratio and the charge of an electing (e=1.6 x 〖10〗^(-19) C). The result from this experiment was of an order of 〖10〗^6 times too large. Subsequent errors would of have lead to this but in principle the mass of an electron can be measured if the charge of an electron is known.
Wire time (or panghantar such as an antenna) conducts alternating current, electromagnetic radiation is propagated at the same frequency as the electric current. Depending on the situation, electromagnetic waves can be waves or like particles. As a wave, characterized by speed (speed of light), wavelength, and frequency. When considered as particles, they are known as photons, and each has an energy associated with the frequency of the waveform shown by the Planck relationship E = Hν, where E is the photon energy, h is the Planck constant - 6.626 × 10 -34 J · s - and ν is the frequency of the
The electromagnetic spectrum is a range of different types of radiations, this is energy that travels and spreads out as it goes. This range involves more than just visible light- small portion of the spectrum detected by the human eye- it goes beyond what the human eye cannot see. The two most important characteristics of the spectrum are wavelength and frequency. The electromagnetic spectrum can be divided into three different parts: the theory of visible light, the range of the electromagnetic spectrum, and how it benefits mankind.
Chemiluminescence is the production of light from a chemical reaction. This phenomenon is caused by the fall of an electron from a higher energy shell back to its ground state, its normal, lower energy shell. An electron is promoted to a higher energy level when it absorbs energy, causing the electron to be in an excited state. When the electron falls back down, the absorbed energy is released as a photon, a packet of energy in the form of electromagnetic energy. If the wavelength of this energy is within the visible spectrum, it is seen as light.
Kinetic Energy: 1/2mv2=eV, where m is the mass of an electron, v is the electron speed, e is the elementary charge of an electron, and V was the voltage used in the experimental calculation.
The idea that images formed by the Camera Obscura could be saved as permanent prints came to light in the 1790’s, when Thomas Wedgwood began experimenting with photo-sensitive silver salts. The discovery of light’s effect on certain chemicals was made b...
Light is both part particle and part wave. Light is “the electromagnetic radiation that may be perceived by the human eye”. It consists of photons, which are massless bundles of concentrated electromagnetic energy. Light’s lower frequency is red, and the higher frequency is blue. Like sound, light has frequencies humans can’t detect. Ultraviolet light is at a frequency higher than violet, and infrared is at the frequency lower than the red of visible light. We get UV (ultraviolet) rays from the sun, and infrared is used in night vision to see better.
In 1907, Einstein used Planck’s hypothesis of quantization to explain why the temperature of a solid changed by different amounts if you put the same amount of heat into the material. Since the early 1800’s, the science of spectroscopy had shown that different elements emit and absorb specific colors of light called “spectral lines.” In 1888, Johannes Rydberg derived an equation that described the spectral lines emitted by hydrogen, though nobody could explain why the equation worked. This changed in 1913 when Danish physicist Niel Bohr applied Planck’s hypothesis of quantization to Ernest Rutherford’s 1911 “planetary” model of the atom, which affirmed that electrons orbited the nucleus the same way that planets orbit the sun. Bohr offered an explanation for why electrical attraction does not make the electrons spiral into the nucleus. He said that electrons in atoms can change their energy only by absorbing or emitting quanta. When an electron absorbs a quantum it moves quickly to orbit farther from nucleus. When an electron emits a quantum the electron jumps to a closer
11C → 11B + e+ + ν Energy given off as a result e + 0.96 MeV
Spring, K. R., & Davidson, M. W. (2016, 05 17). Light: Particle or a Wave? Retrieved from Physics of Light and Color: http://micro.magnet.fsu.edu/primer/lightandcolor/particleorwave.html
Matter is energy (Fernflores 1). The fact that electron-positron interactions can either produce photons or...
...here the electrons move and go. The photons from the light transport energy and hit the electron, which transfers energy to the electron but slows down the photon. At last, in the 1920’s scientists came up with the wave-particle duality. The wave-particle duality stated that light had both properties of a wave and properties of a particle at the same time (Tavolacci).
According to the de Broglie relation and Bragg's law, a beam of 54 eV had a wavelength of 0.167 nm. The experimental outcome was 0.165 nm via the grating equation, which closely matched the predictions. Davisson and Germer's accidental discovery of the diffraction of electrons was the first direct evidence confirming de Broglie's hypothesis that particles can have wave properties as well.
Electromagnetic radiation is energy that flows through free space. Electromagnetic radiation comes in a list of energies known as the electromagnetic spectrum. Electromagnetic spectrum is the complete range of the different wavelength of electromagnetic radiation. It consists of light, radio waves, visible light, infrared waves, ultraviolet light, x-rays, microwaves and gamma rays.
Scientists from earlier times helped influence the discoveries that lead to the development of atomic energy. In the late 1800’s, Dalton created the Atomic Theory which explains atoms, elements and compounds (Henderson 1). This was important to the study of and understanding of atoms to future scientists. The Atomic Theory was a list of scientific laws regarding atoms and their potential abilities. Roentagen, used Dalton’s findings and discovered x-rays which could pass through solid objects (Henderson 1). Although he did not discover radiation from the x-rays, he did help lay the foundations for electromagnetic waves. Shortly after Roentagen’s findings, J.J. Thompson discovered the electron which was responsible for defining the atom’s characteristics (Henderson 2). The electron helped scientists uncover why an atom responds to reactions the way it does and how it received its “personality”. Dalton’s, Roentagen’s and Thompson’s findings helped guide other scientists to discovering the uses of atomic energy and reactions. Such applications were discovered in the early 1900’s by using Einstein’s equation, which stated that if a chain reaction occurred, cheap, reliable energy could b...