This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10any SI prefix in the ALEKS Data tab.)energy (ZJ)140012001000800600A4002000Use this diagram to complete the table below.What is the energy of the electron in the ground state?ZJ☐ x10☑What is the energy of the electron in the first excitedstate?If the electron makes the transition shown by the redarrow, from C to B, will a photon be absorbed oremitted?Calculate the wavelength of the photon that would beabsorbed or emitted. Round your answer to 3significant digits.☐ ZJabsorbedemitted☐um21. You can find the meaning of

Final answer = 3.755Explanation:

Answered: This energy diagram shows the allowed…

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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of 33 > % A In scenario C, visible light is in the middle of the yellow region of the visible spectrum. Estimate its wavelength, frequency, and energy per photon. frequency: In scenario D, visible light has a photon energy of 4.151 x 10-19 J. Determine its wavelength, frequency, and color. frequency: O a R LE 5 25 6 00 G H 8 ST1 $1 9 K wavelength: energy per photon: wavelength: The visible light in scenario D is RA L P 90°F nm nm J 3:36 PM 7/28/2022
> Question Completion Status: QUESTION 4 Roaches for sale | C... For Sale/Trade/Wan... * Tarantulas CSL Behring Hell Let Loose TR St... Indicate which three of the following statements about the electron in a hydrogen atom are true by checking the box in front of each true statement. The atom is in the ground state when the electron is in the n=1 level. Energy is released when the electron is excited from the n=1 level to the n=3 level. A shorter wavelength of light is emitted when the electron moves from the n=3 level to the n=2 level than when the electron moves from the n=4 level to the n=2 level. Energy is always released when an electron relaxes. A lower frequency of light is emitted when the electron moves from the n=3 level to the n=2 level than when the electron moves from the n=4 level to the n=2 level. The atom is stable when the electron relaxes to the n=2 level.
need it fast! In a hydrogen atom, an electron loses energy from n = 5 to n = 2, a process that leads to some kind of “interaction” with electromagnetic radiation. What is the energy of this electromagnetic radiation in Joules? Do NOT include a sign with this answer. Rydberg's constant is equal to -2.179 x 10-18 J. Express exponents as number followed by E followed by the power (e.g., 7.34E-12).
A hydrogen atom absorbs a photon of ultraviolet light, exciting an electron from energy level 1 to energy electron drops back down in three steps, as shown. Using the table, identify the energy released in each tr visible, or infrared. 7 Transition from 7→5: 6. E = 4.23 x 10-20 J 2 = 4,668 nm 4 Transition from 5→ 2: E = 4.58 × 10-19 J 1 = 434 nm 2 Transition from 2→ 1: E = 1.63 x 10-18 J 1 = 122 nm Transition Wavelength Region 7 → 5 4,668 nm 5 → 2 434 nm 2 → 1 122 nm Answer Bank ultraviolet infrared visible Energy
Consider the four scenarios involving visible light. In scenario A, visible light has a wavelength of 729.9 nm.729.9 nm. Determine its frequency, energy per photon, and color. frequency: s−1−1 energy per photon: J The visible light in scenario A is In scenario B, visible light has a frequency of 5.490×1014 s−1.5.490×1014 s−1. Determine its wavelength, energy per photon, and color. wavelength: nm energy per photon: J The visible light in scenario B is In scenario C, visible light is yellow. Determine its wavelength, frequency, and energy per photon. wavelength: nm frequency: s−1−1 energy per photon: J In scenario D, visible light has a photon energy of 4.202×10−19 J.4.202×10−19 J. Determine its wavelength, frequency, and color. wavelength: nm frequency: s−1−1 The visible light in…
What is the formal charge of carbon in the following resonance structure of CH-2N2? (Can you draw the other resonance forms?)
Consider a hydrogen atom in the ground state. What is the energy of its electron? E = Now consider an excited-state hydrogen atom. What is the energy of the electron in the n = 3 level? E3 = PAGES · O J J
ledu.co Question 16 of 16 In Einstein's photoelectric experiment, the kinetic energy (K.E.) of an electron displaced from a metal by a photon was the difference between the energy of a photon and a threshold energy value for the metal. If you were to perform a similar experiment with lead, which has a threshold energy of 6.81 x 10 19 J, and ultraviolet light of wavelength 38.5 nm, what would be the speed (v) of the dislodged electron? (K.E. = 1/2mv2. The mass of the electron = 9.109 x 10 1 kg.) | m/s 9. 4 8. x 100 +/- A ENG to search 60
An unidentified element is known to have an electron configuration, [X] ns2, in its ground state. This element must be in the same family as radon (Rn) O rubidium (Rb) arsenic O radium (Ra) O lead
4. Electrons must gain energy in order to move from lower energy levels to higher energy levels. When the electron moves back down from a higher energy level to a lower one, how does it "lose" this energy? Where does the energy go? Edit View Insert Format Tools Table 12pt v Paragraph v BIU T?v:
An atom emits light at various wavelengths, two of which are 434 nm and 472 nm. Both of these transitions are to the same final state. What is the energy difference between the two states for each transition ? 3.7 x 10 - 20 J O 1.2 x 10 - 19 O 4.2 x 10- 20J O 3.4 x 10 - 19
any SI prefix in the ALEKS Data tab.) 1400 - 1200- 1000 800 energy (z) 600 400 200 Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from C to A, will a photon be absorbed or absorbed emitted emitted? Calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. nm I Don't Know Submit © 2022 McGraw Hill LLC. All Righ

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