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Molar Mass Of Energy Lab Report

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Claim: Electrons with higher energy will be positioned further away from the nucleus than electrons with lower energy. Evidence and Analysis: In this lab, eight solutions were tested to show how the energy of light given off by an atom describes the location of an electron in the atom. When certain solutions were placed in the flame from a bunsen burner, the flame turned different colours. Lithium made the flame change to a violet/teal colour, barium and copper made the flame become green, and strontium, calcium, sodium, sodium and potassium, and the unknown substance made the flame change to a red/orange colour. Reading and Reflection: Given the prior knowledge that purple light has the highest amount of energy and red light has the lowest amount of energy, it was inferred that solutions with purple/blue light have more energy and those with red/orange light have the smallest amount of energy. So lithium had the highest energy (in wavelengths), barium and copper had a moderate amount of energy, and the majority of the substances had low light energy. Other prior knowledge led to the fact that electrons further away from the nucleus have more energy. So lithium, which had the highest amount of energy, has to have electrons the furthest …show more content…

This was stated in the hypothesis of electrons further away from the nucleus having more energy. This remained the main belief of the experiment even after the experiment was conducted, because it was based on the prior knowledge that electrons are more “excited” when they have bounced to an orbital further away from their ground state. That is, it takes energy for an electron to leave its ground state, and when the electron returns to its ground state, the energy it gives off is emitted in the form of wavelengths of light, causing the observer to see the differing colours, depending on the amount of

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Protactinium currently has no uses due to its high levels of toxicity and radioactivity. Although it is used for scientific research. After this discovery Meisner continued her research which in 1923 lead to the radiationless transition known as the Auger effect. The Auger effect is when an electron in an outer shell of an atom makes a transition to a vacancy in an inner shell. The energy gained is shifted to an electron that leaves from the atom.

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Purpose The purpose of this experiment is to understand the different forms of energy as a ball is thrown into the air and falls back to the ground at rest. As well as comparing the potential energy, kinetic energy, and total energy to compare what happens when this ball is thrown and dropped. We will also measure the total energy to determine whether or not there is a change.

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That gives them a total of 10 electrons. Along with atomic number, protons, and electrons there is a atomic mass which is 20.1797. Neon was discovered by Sir William Ramsay, a Scottish chemist, and Morris M. Travers, an English chemist, shortly after their discovery of Krypton. Like krypton, neon was discovered through the study of liquefied air. Although neon is the fourth most abundant element in the universe, only 0.0018% of the earth’s atmosphere is made up of neon.

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Harold Urey - Experiment Harold Urey’s discovery of deuterium is perhaps his most revolutionary discovery. Not only did Urey receive a Nobel Prize for his work towards hydrogen-2, deuterium would go on to become invaluable both to chemists’ understanding of the elements, and the field of chemistry as a whole. Urey’s pursuit of deuterium began in 1931, after his interest was piqued by a scientific journal that discussed the supposed existence of the isotope. Using the Balmer series, which is the series of lines in the hydrogen atomic emission spectrum, Urey and a colleague by the name of George Murphy, calculated where hydrogen-2’s emission lines should be located. They determined that the isotope’s emission lines would be “redshifted” (shifted

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Bohr’s career began with his development of the Bohr model of the atom, a revolutionary model in that it was a relatively accurate depiction of the structure of an atom where electrons revolved around the dense nucleus in constant orbits. Bohr’s depiction of the Bohr model of the atom could not have been accomplished without the discoveries of Thomson, Rutherford, and Planck. In addition to creating an accurate depiction of the atom, Bohr also studied atomic radiation and how electrons jumped from different orbits in a process called the quantum leap. Bohr’s quantum leap idea was inspired by Planck’s quantum theory in that he believed that energy is transferred within atoms in constant quantities. Bohr’s discovery of the structure of the atom and his work to explain the transfer of energy within electrons led to him being awarded the Nobel Prize in Physics (“Neils Bohr - Biography” 2014).

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We call this today the “Bohr model” of the atom (Figure 4). In this model (based on a hydrogen atom) he theorised that electrons travelled in circular orbits at certain energy levels. These electrons could pick up energy and move to a higher energy level, a process we call excitation. The electrons would then release this energy in the form of a photon, and drop back down to a stable level. This model however breaks apart when we examine other elements with more electrons, as it does nothing to explain interaction between numerous negatively electromagnetically charged electrons and why they do not simply excite each

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It is well known that atoms are made up of protons which are the positive charges, electrons which are the negative charges, and neutrons which are the neutral charges, every scientist comes to a point where they make a mistake or were wrong about something. Dalton mistake was that he

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The noble gases group was then incorporated into the periodic table. In 1897 physicist J. J. Thomson first discovered electrons; small negatively charged particles in an atom. John Townsend and Robert Millikan later on were able to determine their exact charge and mass. In 1911 Rutherford and German physicist Hans Geiger found out that electrons orbit the nucleus of an atom. Radiation is emitted during movement from one orbital to another.

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Rutherford thought that the negative electrons orbited a positive center in a manner like the solar system where the planets orbit the sun. Rutherford knew that atoms consist of a compact positively charged nucleus, around which circulate negative electrons at a relatively large distance. The nucleus occupies less than one thousand million millionth of the atomic volume, but contains almost all of the atom's mass. If an atom had the size of the earth, the nucleus would have the size of a football stadium. Not until 1919 did Rutherford finally identify the particles of the nucleus as discrete positive charges of matter.

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The main idea of this experiment is also often highlighted in the theoretical discussion of the clarification of quantum

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When produced, colored pictures were extremely sensitive to light and when exposed to it would almost instantly disappear (Welch para 38). The Lumière brothers, Auguste and Louis, found a solution to the bothersome problem when they discovered that when dyed potato starch was used, that they could create colored images in a quality that no one had ever seen before (Andrews para 9). Co-founder of the famous company Polaroid, Edwin Land did not believe the theory of the RGB (Red Green Blue) color process, which was the main belief at the time, and thought instead that the human eye could sense red and green light as it passed through the structures of the eye, which he called the “two-color process” (Welch para 40). The two-color process became the idea from which Land and the Polaroid company would build their ideas and triumphs off of (Welch para

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He concluded that the atom not only had negatively charged particles, it also contained positive

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In 1913, he introduced “the trilogy”, three quantum papers describing the Bohr model of the atom which is currently used in many chemistry and physics texts. This brought him widespread recognition. His model presents atoms as small positively charged nuclei circularly orbited by negatively charged electrons. The electrons have separate orbits with the last orbit’s number of electrons significantly affecting the element’s chemical properties. He suggested that electrons are confined to particular orbits and can jump to other orbits by absorbing or emitting energy.

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Four color theorem is first proposed on October 23, 1852 by Francis Guthrie.

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