In chapter seven we learned about the electron structure of an atom. We learned about the Bohr model, electromagnetic energy, and many other related topics. In this essay I will explain in further detail what light really is and how we describe it. I will describe the behavior of electrons in both a hydrogen atom and all atoms. I will explain the arrangement of the elements in the periodic table, state which electrons are chemically important in atoms, and lastly I will describe the properties of atoms and their relation to their electron arrangements. The information provided will be my interpretation of the chapter, and my outlook on what this chapter was about.
Light is the natural agent that stimulates sight and makes things visible. White light is a mix of colors that can be separated by a prism. Sources of white light would include the sun and light bulbs. In chemistry we consider light as electromagnetic radiation. This electromagnetic energy travels through space as waves, at the speed of light. In other words we believe light is a form of energy and that’s mainly what light is, it’s just energy.
Now the description of light is harder concept to grasp. We describe light by using wavelength and frequency. Wavelength would be the distance between two corresponding points on a wave. Frequency would be the number of waves that passes a point per second. For example the wavelengths of visible light such as red would be visible at seven hundred nanometers. Another example on how we describe light is to take the color green, for it to be visible it would have a wavelength of five hundred nanometers and a frequency of 6 x 10 14/s. Light can also be described on our scale as both waves and particles or packets of light called photons. The energy of a photon is proportional to the frequency. The last way we can describe light is to use the Atomic Spectra. The atomic spectra give only specific colors in a line spectrum, where each line is a specific wavelength of light. For example colored light, such as light from a neon sign would work perfectly with the atomic spectra.
The Bohr model of the hydrogen atom is the main tool in describing the behavior of the electron in a hydrogen atom. Niels Bohr studied the line spectra of the hydrogen atom to try and solve how electrons fit in the models of the hydrogen atoms.
In "Energy Story" uses an explanation of atoms and tells us the parts of an atom and its structure. In the text it
Primo Levi’s personal relationship to his profession as a chemist shows that philosophically and psychologically, he is deeply invested in it. His book THe PeriOdic TaBLe shows that his methodology cannot be classified as either purely objective or purely subjective. He fits into the definition of dynamic objectivity given by Evelyn Fox Keller in her book Reflections on Gender and Science.
J.J. Thompson didn’t really believe that the atom was the smallest piece to matter. So he did some experiments with running current through a glass tube with the air sucked out of it. That’s what a cathode ray tube is. It has a negative charge attached to the cathode (the metal piece farthest to the side of the tube) and the positive charge attached to the anode (the metal piece closer to the center of the tube). After running current through the cathode he realized that a stream of light was projected from the end that was being charged to the opposite and showing at the inside of the tube. He wasn’t very sure what it meant at first but then he figured it out.
Niels Bohr's model of the hydrogen atom, was the primary reason for the understanding of energy levels.Bohr was able to explain the bright line spectrum of hydrogen. Sparked by the recent discovery of the diffraction patterns, scientists believed electrons could be described as waves. Bohr hypothesized that energy is being added to the hydrogen gas in the electricity form, and then leaving the gas in the form of light. He figured the light rays to be quantized, meaning only certain frequencies of the light rays can be seen. In turn, he reasoned that the hydrogen atoms themselves were quantized and, that they only can exist in certain energy levels. When the atoms absorb specific amounts of energy, they exist for a small period of time in higher energy levels. But as soon as these atoms lose their energy, they move back down to the lower levels of energy. His theory went on to state how the hydrogen atom can move up and down the energy levels, one level at a time, and can never stop in between. Every hydrogen atom is made up of a single electron - proton system. Because the negative electron is attracted to the positive proton, potential energy is created inside the atom.He figured that the farther away the electron is from the proton, the greater the potential energy is inside. In conclusion, since hydrogen atoms emit light energy in specific frequencies, the hydrogen atom must be within a specific energy level and nothing else. The different wavelengths help to determine the different colors emitted from the atom. The greater the wavelength, the faster the atom can be filled and jump to a higher level.Bohr developed his theory after studying the work of Einstein's ideas on the photons of energy.
The author tells of how waves are effected by quantum mechanic. He also discusses the fact that electromagnetic radiation, or photons, are actually particles and waves. He continues to discuss how matter particles are also matter, but because of their h bar, is so small, the effects are not seen. Green concludes the quantum mechanics discussion by talking about the uncertainty principle.Chapter 5: The need for a New Theory: General Relativity vs.
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
Electromagnetic spectrum is a list of the most possible range of electromagnetic radiation around us. their many different electromagnetic radiation in the world. for example we got radio radiation, sun 's radiation , microwaves radiation, etc. many of ths radiation have different level of wavelength, energy, frequency, and also different classes. the way the electromagnetic spectrum works is by wavelength. the bigger the wave length the smaller power it have. the small wavelength is the most power it have. for example a radio tower, it haves a wavelength of the size of a football field. that wave meter is 105 and it frequency is 104. this is one of the longest wavelength in the electromagnetic. in the other hand Gamma Ray is one of the shortest wavelength in the electromagnetic but it hav...
Color is a product of many different things. We physically see color by the light hitting the retina and being absorbed by the rods and cones. Colors are distinguished by sorting them into categories. These could include tint, shade, tone, chroma, value, or hue. It could also be determined by whether a color is primary, secondary, intermediate, or complementary. The illusion of different colors can be created by the colors around a color or placing bits of color very close together as in a television. Afterimages create the opposite of colors. All color is a product of light. Without light, we would only be able to see in black and white (The World Book Encyclopedia p 818, 819, 822, 823).
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.
The Periodic Table of Elements is commonly used today when studying elements. This table’s history begins in ancient times when Greek scientists first started discovering different elements. Over the years, many different forms of the periodic table have been made which set the basis for the modern table we use today. This table includes over 100 elements and are arranged by groups and periods. Groups being vertical columns and periods being horizontal columns. With all of the research conducted over the years and the organization of this table, it is easy to use when needed.
A spectrum is an image or distribution of colour of any electromagnetic radiation arranged in a progressive series according to wavelength.
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
Light is what lets you experience colour. The pigment of the retina in your eyes is sensitive to different lengths of light waves which allows you to see different colours. The wavelengths of light that humans can see are called the visible colour spectrum.
From this simple observation, Rutherford concluded that the atom's mass must be concentrated in a small positively-charged nucleus while the electrons inhabit the farthest reaches of the atom. Although this planetary model of the atom has been greatly refined over the years, it remains as valid today as when it was originally formulated by Rutherford. In 1919, Rutherford returned to Cambridge to become director of the Cavendish laboratory where he had previously done his graduate work under J.
Light consists of electric and magnetic fields, commonly known as electromagnetic waves. These waves are generated by the movement back and forward of electric charges, or oscillation. The term light is commonly referred to just those electromagnetic waves that we are able to see. Light can only be visible when it has a wavelength within a narrow range of values called the visible spectrum, if the wavelength is too long or short, it is a different kind of wavelength in the electromagnetic spectrum. Visible light has a wavelength between about 300 nanometers and 700 nanometers. Violet light has the shortest wavelength in the visible spectrum, and red light has the longest wavelength; all the other colors in the spectrum have a wavelength between