An electron in a hydrogen atom changes from the n = 7 to the n= 2 state. Determine the wavelength of the emitted photon. Express your answer to three significant figures and include the appropriate Templetes Symbo undo' regto Peskt keyboard shortouts Hletp Value Units

An electron in a hydrogen atom changes from the n = 7 to the n= 2 state. Determine the wavelength of the emitted photon. Express your answer to three significant figures and include the appropriate Templetes Symbo undo' regto Peskt keyboard shortouts Hletp Value Units

College Physics

1st Edition

ISBN:9781938168000

Author:Paul Peter Urone, Roger Hinrichs

Publisher:Paul Peter Urone, Roger Hinrichs

Chapter30: Atomic Physics

Section: Chapter Questions

Problem 16CQ: Atomic and molecular spectra are discrete. What does discrete mean, and how are discrete spectra...

See similar textbooks

Similar questions

AK éléctron in a hydrogen atom makes a transition from the state n= 12 to the state n= 2. Give the wavelength of the photon emitted during this transition in units of nm. Round your answer to 2 significant figures. Add your answer
An atomic emission spectrum of hydrogen shows three wavelengths: 656.5 nm, 486.3 nm, and 434.2 nm. Assign these wavelengths to transitions in the hydrogen atom. Match the items in the left column to the appropriate blanks in the sentences on the right. Reset Help 1 1 AE 1.1 x 107 2 nimal nitial the wavelengths of the visual The wavelengths of the three transitions are region. Therefore, it can be assumed that the electrons return to the level. shorter than longer than n = 7 The difference in energy between the two levels initial and nfinal is given by the 1 1 equation AE-2.18 x 10-18 2 ninal After calculating the energy difference using the given wavelengths, solving the equation for initial, and subtituting the proper values the following initial energy levels can be 1 1 AE -2.18 x 10-18 2 ninal ninitial obtained: n = 1 for 434.2nm. 1 AE -2.18 x 10-18 initial ninal n = 8 equal to n=6 n = 2 n = 3 n = 4 n = 5 Submit Request Answer for 656.5nm, for 486.3nm, and
The figure below shows some energy levels of the lithium atom. I) Considering the conditions for atomic transitions, what should be the shortest wavelength in the lithium state emission spectrum starting from the 4s excited state? Justify the calculations. II) What must be the longest wavelength that must be absorbed by the atom in the ground state so that the emission at 816 nm is possible to be observed? Justify your answer. III) What must be the slowest speed of an electron such that, after colliding with the atom in the ground state, the wavelength 816 nm can be observed in the emission spectrum? Justify the calculations.
What is the wavelength of light (in nm) emitted when an electron in a hydrogen atom undergoes a transition from the n = 4 energy state to the n = 2 energy state? Express your answer to the nearest nm. Answer:
Solve using GUESS method. Atomic and Nuclear Phenomena 2. The work function of a metal is 2.6 eV. What is the longest wavelength of radiation that can eject a photoelectron from this metal?
The electron in a hydrogen atom makes a transition from the n = 4 state to the n = 2 state, as indicated in the image. (Figure 1) Determine the linear momentum of the photon emitted as a result of this transition. Figure Momentum of atom Electron jump > p = ΜΕ ΑΣΦ Submit Request Answer Part B ? kg. m/s Using your result to part A, find the recoil speed of the hydrogen atom, assuming it was at rest before the photon was emitted. v = ΜΕ ΑΣΦ Submit Request Answer Provide Feedback 1 of 1 Momentum of photon ? cm/s Next >
https://en.wikipedia.or g/wiki/George_Paget Thomson#/media/File: George Paget_Thomso n.jpg LESSON 1: WAVE BEHAVIOR OF ELECTRONS ACTIVITY 1 Directions: To help you fully understand the wave behavior of electrons, you must first understand the dual nature of light. Test your ability and apply the principles you have learned in the previous lesson by completing the sentences below. Choose your answer from the parentheses. Light has a (single, dual) nature. Sometimes, it behaves like a particle (proton, photon). Light's particle-like traits are best explained by the theory (Thomas Young, Albert Einstein) won his Nobel Prize for. called (photoelectric effect, scattering of light), the that Light also behaves like a wave, which explains how it (reflects, refracts) or (image, how it bounces off in an obstacle. This results in the formation of an object) in a mirrored surface. Light, like any wave, is known to undergo (reflection, refraction) when it passes from one medium to another medium…
Question 3: show your working A hydrogen atom transitions from a state with n = 4 to a state with n = 2. (c) A photon is then emitted: calculate its i. energy ii. wavelength iii. magnitude of the momentum
4.5 Telkom-Monat. 9% - 14:12 K/s Document View Spectral Classification-- Procedure and Worksheet Note: In this lab al wavelengths are given in units of Angstroms. 1 Angstrom = 10" meters; Inm = 10 Angstroms. Write all answers in the space below each question. 1. Look at the energy level diaggram below. The open circles on the figure represent electrons. The electron transitions that correspond to the first four absorption lines of the Lyman series are drawn for you as well as their identifying wavelengths (i.e. the wavelength of the photons the atom must absorb to allow the electron to make each transition.) Also shown are the first 2 transitions of the Paschen series. a) Draw the first 3 transitions of the Balmer series on the energy level diagram below. b) Each Balmer series transition is associated with one of the following wavelengths: 4340, 6563 and 4861 Angstroms. On the diagram, label which wavelength corresponds to each transition. Energy Levels for Hydrogen n5 n=4 n3 A- 18756…
TOPIC: LIGHT ABSORBED AS PHOTONS: PHOTO ELECTRIC EFFECT. INSTRUCTIONS: ANSWER THE PROBLEM. CHOOSE THE ANSWER FROM [(i),(ii),(iii)...] AND PROVIDE EXPLANATION/SOLUTIONS. *please provide simple and clearer explanation. (in the previous answer some elements seems to be missing) View Image
Iron has a magnetic moment of 2.22 Bohr magnetons per atom and a density of 7.87-103 kg.m-3. Calculate the expected magnetization of iron at 0 K and describe any assumptions that you have made. How would you expect this magnetization of iron to vary as temperature is increased. How does the number of Bohr magnetons per atom change from 0 K to 300 K. Why does a piece of iron typically not exhibit high magnetization at room temperature (unless it has been "magnetized")?
Solve correctly please. How much energy, in eV, is needed to move an electron in a hydrogen atom from n1 = 2 to n2 = 6. Please round your answer to two decimal places. (Gpt/ai wrong answer not allowed)