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Q: QUESTION 9 In the picture are two diagrams of the first five orbits in the Bohr model labeled A…
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The line absorption spectrum of a sample of hydrogen gas was observed in a laboratory at room temperature.
Answer the questions 1and 2 in relation to this spectrum.
1- Explain why the observed spectral lines would mainly correspond to the Lyman series.
2- Explain how a line absorption spectrum in the Balmer series could be produced.
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- The Lyman series in the hydrogen emission spectrum is formed by electron transitions from n;> 1 to nf= 1. What is the wavelength of the series limit (the lower bound of the wavelengths in the series)? nmA hypothetical atom has energy levels given in the figure below. Which figure most accurately depicts the absorption spectrum, assuming all transitions between energy levels is possible? The black vertical lines represent the absorbed wavelengths. Eo = -11.5 eV E₁ = -9.6 eV E₂ = -5.2 eV O E3 = -1.1 eV wavelength increases → wavelength increases → wavelength increases → wavelength increases → wavelength increases →A neutral atom of the element boron (B) has 5 electrons. Four of the electrons are removed, forming an ion with the one remaining electron. a) Sketch an energy level diagram for this ion, showing the ground state and the first two excited states. Label each state with the value of its energy. b) Calculate the two longest wavelengths at which this ion can absorb radiation. Assume all absorption occurs from the ground state. c) What is the minimum amount of energy needed to remove the electron from the ground state of this ion?
- The energy levels for a Bohr atom are shown below. Use this diagram to solve problems 7 and 8. 0 eV -2.5 eV -4.0 eV -7.0 eV -12.5 eV 7. What amount of energy is needed for an electron to jump from n = 1 to n = 4? 8. What is the wavelength of the photon needed to make this happen? Is it emission or absorption?Question 14 a) A narrow beam of white light is passed through a clear glass vessel containing cool hydrogen gas at a low pressure. A prism is used to disperse the light leaving the vessel. This results in a white light spectrum, crossed by a series of dark lines. Explain the origin of these dark lines and name the type of spectrum that is produced. b) Some of the atomic energy levels of hydrogen are shown in the diagram below. i. ii. iii. Energy/eV 0 -0.85 -1.51 -3.39 -13.58 n = 4 n = 3 n = 2 n = 1 Determine the ionization energy of hydrogen and express this in joules. Determine the wavelength of the light emitted when an electron falls from the n = 3 level to the n = 1 energy level. A photon of energy 10.19 eV is in collision with a hydrogen atom. What would happen to this photon?In the picture are two diagrams of the first five orbits in the Bohr model labeled A - E. The dot in an orbit is the electron. The nucleus is not shown. Shown is a BEFORE and AFTER state of the atom. An energy level diagram for the Bohr hydrogen atom is shown. Which of these events has occurred in going from the BEFORE to the AFTER state? a. a photon of energy 0.97 eV has been emitted b. a photon of energy 1.51 eV has been absorbed c. a photon of energy 1.51 eV has been emitted d. an electron of energy 1.51 eV has been emitted e. a photon of energy 0.97 eV has been absorbed
- QUESTION 1 IR radiation can. ionize atoms. cause valence e-1 transitions. induce rotations in molecules. cause inner-shell el transitions.The Balmer series in hydrogen includes the Paschen series. has four lines in the ultraviolet. O includes both the Paschen series and the Lyman series. O has four lines in the visible. O includes the Lyman series.Question in images