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Document Preview: Assignment Chapter 7Concept Explorations7.23. Light, Energy, and the Hydrogen Atoma. Which has the greater wavelength, blue light or red light?b. How do the frequencies of blue light and red light compare?c. How does the energy of blue light compare with that of red light?d. Does blue light have a greater speed than red light?e. How does the energy of three photons from a blue light source compare with the energy of one photon of blue light from the same source? How does the energy of two photons corresponding to a wavelength of 451 nm (blue light) compare with the energy of three photons corresponding to a wavelength of 704 nm (red light)?Energy of two Blue photons corresponds to the wavelength, ? = 451 x 10-9 mEnergy of three Red protons corresponds to the wavelength, ? = 704 x 10-9 mf. A hydrogen atom with an electron in its ground state interacts with a photon of light with a wavelength of 1.22 × 10-6m. Could the electron make a transition from the ground state to a higher energy level? If it does make a transition, indicate which one. If no transition can occur, explain.g. If you have one mole of hydrogen atoms with their electrons in the n = 1 level, what is the minimum number of photons you would need to interact with these atoms in order to have all of their electrons promoted to the n = 3 level? What wavelength of light would you need to perform this experiment?7.24. Investigating Energy LevelsConsider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equationE = - (RH / n3)where RHis the same as for hydrogen (2.179 ×10-18J). Answer the following questions, without calculating energy values.a. How would the ground-state energy levels of X and H compare?b. Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your...

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7.24. Investigating Energy Levels 
Consider the hypothetical atom X that has one electron like the H atom but has 
different energy levels. The energies of an electron in an X atom are described 
by the equation 
E = - (RH / n
3) 
where RHis the same as for hydrogen (2.179 ×10
−18J). Answer the following 
questions, without calculating energy values. 
• a. How would the ground-state energy levels of X and H compare? 
Answer- The Ground state energy levels will be same.
• b. Would the energy of an electron in the n = 2 level of H be higher or lower 
than that of an electron in the n = 2 level of X? Explain your answer. 
Answer- The energy of the electron in n=2  of X will be more than that of H, as X 
will be heavier (more atomic number) than H. E=-Z2(RH/n
2)
• c. How do the spacings of the energy levels of X and H compare? 
Answer- Spacing of energy will be higher for X than for H 
• d. Which would involve the emission of a higher frequency of light, the 
transition of an electron in an H atom from the n = 5 to the n = 3 level or a 
similar transition in an X atom? 
Answer- X involve higher energy, as energy levels of X will be higher than H, the 
energy required for the transitions will also be high. So for the same transition n-5 
to n=3, the heavier atom, X need more energy, hence high frequency.
• e. Which atom, X or H,

Need help completing this assignment Document Preview: Assignment Chapter 7 Concept Explorations 7.23. Light, Energy, and the Hydrogen Atom a. Which has the greater wavelength, blue light or red...

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