Select the correct option for the periodic table’s structure.

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Chapter 29, Problem 4OQ

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Select the correct option for the periodic table’s structure.

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Question 2. Let us consider a hypothetical Atom with the following list of energy levels: E1 = 1.5 eV E2 = 3.5 eV E3 = 4.8 eV E4 = 5.6 eV a) Compute the energy of ALL the spectral lines in the ABSORPTION SPECTRUM and list the corresponding "colors" b) Compute the energy of ALL the spectral lines in the EMISSION SPECTRUM and list the corresponding "colors" Wavelength Frequency Photon energy (nm) (THz) 380-450 670-790 450-485 620-670 cyan 485-500 600-620 green 500-565 530-600 yellow 565-590 510-530 orange 590-625 480-510 red 625-750 400-480 Color violet blue (eV) 2.75-3.26 2.56-2.75 2.48-2.56 2.19-2.48 2.10-2.19 1.98-2.10 1.65-1.98

Which of the following is not true of Bohrs atomic model? The angular momentum of an electron in the allowed orbit is equal to an integral multiple of h 2? The Coulomb force between the nucleus and the electron maintains the electron in orbit. Radiation is emitted when an electron orbits in the allowed orbit. The electron in the orbit nearest to the nucleus has the lowest energy.

The electron volt (eV) is a convenient unit of energy for expressing atomic-scale energies. It is the amount of energy that an electron gains when subjected to a potential of 1 volt; 1 eV = 1.602 × 10–19 J. Using the Bohr model, determine the energy, in electron volts, of the photon produced when an electron in a hydrogen atom moves from the orbit with n = 5 to the orbit with n = 2.