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13. Does a gas discharge tube filled with boron emit the same wavelengths of light as a tube filled with hydrogen? Use evidence from Model 2 to support your answer. 14. "The spectral lines for atoms are like fingerprints for humans." How do the spectral lines for hydrogen and boron support this statement? Circle the appropriate word to complete each statement in Questions 14-17 15. Electrons and protons (attract/repel) each other. 16. As an electron gets closer to the nucleus the (attraction/repulsion)to the nucleus gets (stronger/ weaker). 17. For an electron to move from an energy level close to the nucleus to an energy level far from the nucleus it would need to (gain/lose energy. 18. For an electron to move from an energy level far from the nucleus to an energy level close to the nucleus it would need to (gain/lose)energy. Niels Bohr modified Rutherford'Nuclear Atom model to explain how light interacted with the electrons in an atom to produce spectral lines. His model included electrons orbiting the nucleus at specific energy levels. Electrons absorb energy from various sources (electricity) when they move from lower energy levels (ground state) to higher energy levels (excited states). Energy is released as electrons return to their lower energy levels. Is energy absorbed or released for the electron transition shown in the diagram to the right? Explain.

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13. Does a gas discharge tube filled with boron emit the same wavelengths of light as a tube filled with hydrogen? Use evidence from Model 2 to support your answer. 14. "The spectral lines for atoms are like fingerprints for humans." How do the spectral lines for hydrogen and boron support this statement? Circle the appropriate word to complete each statement in Questions 14-17 15. Electrons and protons (attract/repel) each other. 16. As an electron gets closer to the nucleus the (attraction/repulsion)to the nucleus gets (stronger/ weaker). 17. For an electron to move from an energy level close to the nucleus to an energy level far from the nucleus it would need to (gain/lose energy. 18. For an electron to move from an energy level far from the nucleus to an energy level close to the nucleus it would need to (gain/lose)energy. Niels Bohr modified Rutherford'Nuclear Atom model to explain how light interacted with the electrons in an atom to produce spectral lines. His model included electrons orbiting the nucleus at specific energy levels. Electrons absorb energy from various sources (electricity) when they move from lower energy levels (ground state) to higher energy levels (excited states). Energy is released as electrons return to their lower energy levels. Is energy absorbed or released for the electron transition shown in the diagram to the right? Explain.

13. Does a gas discharge tube filled with boron emit the same wavelengths of light as a tube filled with hydrogen? Use evidence from Model 2 to support your answer. 14. "The spectral lines for atoms are like fingerprints for humans." How do the spectral lines for hydrogen and boron support this statement? Circle the appropriate word to complete each statement in Questions 14-17 15. Electrons and protons (attract/repel) each other. 16. As an electron gets closer to the nucleus the (attraction/repulsion)to the nucleus gets (stronger/ weaker). 17. For an electron to move from an energy level close to the nucleus to an energy level far from the nucleus it would need to (gain/lose energy. 18. For an electron to move from an energy level far from the nucleus to an energy level close to the nucleus it would need to (gain/lose)energy. Niels Bohr modified Rutherford'Nuclear Atom model to explain how light interacted with the electrons in an atom to produce spectral lines. His model included electrons orbiting the nucleus at specific energy levels. Electrons absorb energy from various sources (electricity) when they move from lower energy levels (ground state) to higher energy levels (excited states). Energy is released as electrons return to their lower energy levels. Is energy absorbed or released for the electron transition shown in the diagram to the right? Explain.

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13. Based on the information provided and the understanding of atomic emission spectra, a gas discharge tube filled with boron will not emit the same wavelengths of light as a tube filled with hydrogen. This is because each element has a unique electronic structure, and the energy levels of the electrons in boron atoms are different from those in hydrogen atoms. When electrons transition between energy levels, they emit or absorb photons with specific energies, corresponding to specific wavelengths of light. Since boron and hydrogen have different energy levels, the wavelengths of light emitted during these transitions will be different.Answer: No, a gas discharge tube filled with boron does not emit the same wavelengths of light as a tube filled with hydrogen.14. The spectral lines for atoms are indeed like fingerprints for humans because each element has a unique set of spectral lines that can be used to identify it. This uniqueness arises from the specific energy levels of electrons in each type of atom. When electrons transition between these levels, they emit or absorb light at specific wavelengths, creating a pattern of spectral lines that is characteristic of that element. The spectral lines for hydrogen and boron support this statement because they are different for each element, just like fingerprints are different for each person.Answer: The spectral lines for hydrogen and boron are unique to each element, supporting the statement that spectral lines are like fingerprints for atoms.15. Electrons and protons attract each other due to their opposite charges.Answer: attract16. As an electron gets closer to the nucleus, the attraction to the nucleus gets stronger because the force of attraction between opposite charges increases as the distance between them decreases.Answer: attraction, stronger17. For an electron to move from an energy level close to the nucleus to an energy level far from the nucleus, it would need to gain energy. This is because moving to a higher energy level requires an input of energy.Answer: gain18. For an electron to move from an energy level far from the nucleus to an energy level close to the nucleus, it would need to lose energy. This is because dropping to a lower energy level releases energy.Answer: loseRegarding the electron transition shown in the diagram (with the arrow pointing from the outermost circle to the innermost circle), energy is released. This is because when an electron transitions from a higher energy level to a lower one, it emits a photon, which carries away the energy difference between the two levels.Answer: Energy is released for the electron transition shown in the diagram. The arrow pointing inward indicates a transition to a lower energy level, which results in the emission of a photon and the release of energy.
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