The four lines observed in the visible emission spectrum of hydrogen e.docx

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The four lines observed in the visible emission spectrum of hydrogen ell us that a. Only certain energies are allowed for the electron in a hydrogen atom b. We could observe more lines if we had a stronger prism c. The hydrogen molecules they came from have th d. e formula H4 There are four electrons in an excited hydrogen atom According to the Bohr model, when a hydrogen electron makes a transition from n 4 to ne2, which of the following statements is true? l. Energy is emitted. Il. Energy is absorbed. IIl Electrons lose energy IV. Electrons gain energy a. I and IV b. Il and IV c. I only d. I and lIl Solution 1. the four lines observed in the visible emission spectrum of hydrogen tell us that only certain energies are allowed for the electron in a hydrogen atom because these are lines which allow only certain frequencies Hence option (a) is correct 2. When an electron jumps from higher orbital to lower orbital the energy is emitted and electrons loose energy. Hence option (d) is correct . .

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b. Does Rutherford\'s model predict the correct spectrum? Answer: According to Bohr, why did an atom not collapse in on itself while its electrons traveled around the nucleus? (1) 3. Answer: (1) 4. According to Bohr, what is happening in the atom when a photon of light is emitted? Answer: (1) 5. According to Bohr, what is happening in the atom when a photon of light is absorbed? Answer: 6. When you learned about the energy levels of hydrogen, an energy level diagram was introduced. On this diagram, the no energy level was represented. Go to the Hydrogen Atom simulation (Unit D), and complete the n 1 tono transition. Observe the energy state data. a. What is the energy of the n oo energy level? Answer b. If an electron is initially in the ground state, how much energy must be absorbed by the atom for its transition to the oo energy level? Answer: Solution 3) In Bhor\'s model electrons are moving around the neucleous. Neucleus attract the electrons but still they do not fall on neucleus or they do not collapse because due to movement of electron a centrifugal force is also acting on the electron. This centrifugal force and attractive force of neucleus acts as centripetal force and thus electrons do not collapse. 4) According to Bhor when a photon of light is emitting from an atom the electrons are coming to their higher energy state to lower energy state. 5) Similarly when photon of light absorbed by the atom electrons of lower energy states jumps to higher energy state. .

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Compare and contrast the ideas that led to the Bohr model of the atom to the ideas that led to the quantum mecchanical theory that gave rise to the hydrogen atom wave functions. Solution The difficulty with the planetary picture provided before the Bohr model is that it is inconsistent with a well established fact of classical electrodynamics which says that an accelerated electric charge must continually radiate energy. If electrons actually followed such a trajectory, all atoms would act as source of radiation. The radiated energy would come from the kinetic energy of the orbiting electron; as this energy gets radiated away, As a result the electron would quickly fall into the nucleus. According to classical physics, no atom based on this model could exist for more than a brief fraction of a second. In contrary The Bohr model is a mixture of classical physics and quantum physics. The main postulated of Bohr\'s orbit are as follows: 1.) The electron in the atom moves in a circular orbit centred on its nucleus. Its motion in the orbit is governed by the Coulomb electric force between the negatively charged electron and the positively charged proton.The radius of orbit can be given as [r = nh/(2*pi*m*v), where n is principal quantum number.Emission spectrum of hydrogen is nicely explained by Bohr model. However, one serious difficulty with the Bohr model was that it was unable to explain the spectrum of any atom more complicated than hydrogen. 2.) An electron in a Bohr orbit does not continuously radiate electromagnetic radiation. Its energy is therefore constant. The orbit is referred to as a stationary orbit. 3.) Electromagnetic radiation isonlyemitted when the electron changes from one orbit to another of a lower total energy. (The electron is said to undergo atransition.) In such a case, the energy lost, E, is emitted asonequantum of radiation of frequencyfas given by thePlanck–Einstein formula: E = hf Although the Bohr model hypothesis for the quantization of angular momentum can be justified in terms of electron wave ideas, the Bohr model remains profoundly unsatisfactory as a wave model for the atom and also was not able to answer that why it doesn\'t fall into the nucleus. The main failures of Bohr\'s model are: - a mixture of classical and quantum ideas (electrons move classically on orbits, but their possible energy states are quantified) - postulates that on the allowed orbits electrons do not radiate (conflict with Maxwell’s theory) - could not account for the maximal electron numbers on one shell - could not explain splitting of the spectral lines in magnetic fields - it is a non-relativistic theory although the speed of the electrons is close to c In the Quantum Mechanical Model, the electron is treated mathematically as a wave. The electron has properties of both particles and waves. The advantage of Quantum Mechanical model over Bohr model is that it was successful to give explaination of the fact that electron does not fall in.

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