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1) This question explores the energy associated with an electron transition from n = 5 to n = 2. a) Make a rough sketch of the electron energy level diagram for hydrogen. Make a horizontal line for each of the energy levels corresponding to n = 1 through n = 6. (Notice part b also has you add something else too!) Place a picture of your drawing here, by pasting it in as an image. It may help to email yourself a picture first (no need for camscanner, an image is acceptable). Delete these words when you do that! b) In your energy level sketch, make a vertical arrow between the levels that illustrates an electron transition from n = 5 to n = 2. Questions below, c, d, and e refer to the same transition. Answer above on your diagram above c) Find the energy change, in joules, for a single hydrogen electron undergoing this transition. Put your final answer here with units! d) Convert the energy change in part c to units of kilojoules per mole of electrons. Put your final answer here with units! e) Find the energy, frequency, and wavelength (in nm) of the photon emitted from a single hydrogen atom whose electron undergoes the relaxation. Label each result clearly.

1) This question explores the energy associated with an electron transition from n = 5 to n = 2. a) Make a rough sketch of the electron energy level diagram for hydrogen. Make a horizontal line for each of the energy levels corresponding to n = 1 through n = 6. (Notice part b also has you add something else too!) Place a picture of your drawing here, by pasting it in as an image. It may help to email yourself a picture first (no need for camscanner, an image is acceptable). Delete these words when you do that! b) In your energy level sketch, make a vertical arrow between the levels that illustrates an electron transition from n = 5 to n = 2. Questions below, c, d, and e refer to the same transition. Answer above on your diagram above c) Find the energy change, in joules, for a single hydrogen electron undergoing this transition. Put your final answer here with units! d) Convert the energy change in part c to units of kilojoules per mole of electrons. Put your final answer here with units! e) Find the energy, frequency, and wavelength (in nm) of the photon emitted from a single hydrogen atom whose electron undergoes the relaxation. Label each result clearly.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Educational Content Transcription** **2) Ionization Energy of Hydrogen Atom** Find the energy required to ionize a ground state hydrogen atom. This means finding the energy needed to transition from n = 1 to n = ∞. *Hint:* Notice the placement of the infinity symbol in the denominator of a fraction. To answer, you will need to approximate the fraction with the infinity symbol. [Box for student answer] "Put your final ENERGY answer here with units." --- **3) Photon Emission in Hydrogen Transitions** If an electron in a hydrogen atom relaxes to the second energy level, emitting a photon with a wavelength of 410.2 nm, from what higher energy level did it start? [Box for student answer] "Put your final answer for n here!" --- **4) Electron Transitions in Hydrogen Atom** Consider the electron transition in a hydrogen atom from n = 5 to n = 2, versus a transition from n = 3 to n = 2. Do not perform calculations to answer the following questions. a. Which transition emits a higher energy photon? How can you tell? [Box for student answer] "Put your typed answer here." b. One of these transitions corresponds to a red photon, the other to a blue photon. Which transition emits the red photon? [Box for student answer] "Put your typed answer here." --- **5) Visible and Non-Visible Photon Emissions** Consider an electron transition in a hydrogen atom from n = 3 to n = 2, versus a transition from n = 2 to n = 1. Do not perform calculations to answer the following questions. a. Which transition emits a higher energy photon? How can you tell? [Box for student answer] "Put your typed answer here." b. One transition corresponds to a photon in the visible spectrum, while the other is not visible due to higher energy. i. Which transition emits the photon out of the visible range? [Box for student answer] "Put your typed answer here." ii. Is it more likely in the UV-range or the IR-range? [Box for student answer] "Put your typed answer here."
Transcribed Image Text:**Educational Content Transcription** **2) Ionization Energy of Hydrogen Atom** Find the energy required to ionize a ground state hydrogen atom. This means finding the energy needed to transition from n = 1 to n = ∞. *Hint:* Notice the placement of the infinity symbol in the denominator of a fraction. To answer, you will need to approximate the fraction with the infinity symbol. [Box for student answer] "Put your final ENERGY answer here with units." --- **3) Photon Emission in Hydrogen Transitions** If an electron in a hydrogen atom relaxes to the second energy level, emitting a photon with a wavelength of 410.2 nm, from what higher energy level did it start? [Box for student answer] "Put your final answer for n here!" --- **4) Electron Transitions in Hydrogen Atom** Consider the electron transition in a hydrogen atom from n = 5 to n = 2, versus a transition from n = 3 to n = 2. Do not perform calculations to answer the following questions. a. Which transition emits a higher energy photon? How can you tell? [Box for student answer] "Put your typed answer here." b. One of these transitions corresponds to a red photon, the other to a blue photon. Which transition emits the red photon? [Box for student answer] "Put your typed answer here." --- **5) Visible and Non-Visible Photon Emissions** Consider an electron transition in a hydrogen atom from n = 3 to n = 2, versus a transition from n = 2 to n = 1. Do not perform calculations to answer the following questions. a. Which transition emits a higher energy photon? How can you tell? [Box for student answer] "Put your typed answer here." b. One transition corresponds to a photon in the visible spectrum, while the other is not visible due to higher energy. i. Which transition emits the photon out of the visible range? [Box for student answer] "Put your typed answer here." ii. Is it more likely in the UV-range or the IR-range? [Box for student answer] "Put your typed answer here."
1) This question explores the energy associated with an electron transition from \( n = 5 \) to \( n = 2 \). a) Make a rough sketch of the electron energy level diagram for hydrogen. Make a horizontal line for each of the energy levels corresponding to \( n = 1 \) through \( n = 6 \). (Notice part b also has you add something else too!) [Instructions: Place a picture of your drawing here, by pasting it in as an image. It may help to email yourself a picture first (no need for camscanner, an image is acceptable). Delete these words when you do that!] b) In your energy level sketch, make a vertical arrow between the levels that illustrates an electron transition from \( n = 5 \) to \( n = 2 \). Questions below, c, d, and e refer to the same transition. [Instructions: Answer above on your diagram above] c) Find the energy change, in joules, for a single hydrogen electron undergoing this transition. [Instructions: Put your final answer here with units!] d) Convert the energy change in part c to units of kilojoules per mole of electrons. [Instructions: Put your final answer here with units!] e) Find the energy, frequency, and wavelength (in nm) of the photon emitted from a single hydrogen atom whose electron undergoes the relaxation. Label each result clearly. [Instructions: Put your final answer for ENERGY here with units!] [Instructions: Put your final answer for frequency here with units!] [Instructions: Put your final answer for wavelength here with units!]
Transcribed Image Text:1) This question explores the energy associated with an electron transition from \( n = 5 \) to \( n = 2 \). a) Make a rough sketch of the electron energy level diagram for hydrogen. Make a horizontal line for each of the energy levels corresponding to \( n = 1 \) through \( n = 6 \). (Notice part b also has you add something else too!) [Instructions: Place a picture of your drawing here, by pasting it in as an image. It may help to email yourself a picture first (no need for camscanner, an image is acceptable). Delete these words when you do that!] b) In your energy level sketch, make a vertical arrow between the levels that illustrates an electron transition from \( n = 5 \) to \( n = 2 \). Questions below, c, d, and e refer to the same transition. [Instructions: Answer above on your diagram above] c) Find the energy change, in joules, for a single hydrogen electron undergoing this transition. [Instructions: Put your final answer here with units!] d) Convert the energy change in part c to units of kilojoules per mole of electrons. [Instructions: Put your final answer here with units!] e) Find the energy, frequency, and wavelength (in nm) of the photon emitted from a single hydrogen atom whose electron undergoes the relaxation. Label each result clearly. [Instructions: Put your final answer for ENERGY here with units!] [Instructions: Put your final answer for frequency here with units!] [Instructions: Put your final answer for wavelength here with units!]
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