The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. ▼ Part A Submit Request Answer n=4 ? n=3 n=2 n=1 4.2 eV 2.4 eV Initially, electrons are in both the ground and first excited state (n=1 and n=2). A beam of light hits the gas. This beam is a continuous spectrum of yellow/green light (from 495 nm to 590 nm) How many absorption line/s will there be in the spectra? [5] ΑΣΦ 2.0 eV 0 eV BEG YO Color Wavelength Frequency violet 380-450 nm 668-789 THz blue 450-495 nm 606-668 THz green 495-570 nm 526-606 THz yellow 570-590 nm 508-526 THz orange 590-620 nm 484-508 THz red 620-750 nm 400-484 THz Photon energy 2.75-3.26 eV 2.50-2.75 eV 2.17-2.50 eV 2.10-2.17 eV 2.00-2.10 eV 1.65-2.00 eV

The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. ▼ Part A Submit Request Answer n=4 ? n=3 n=2 n=1 4.2 eV 2.4 eV Initially, electrons are in both the ground and first excited state (n=1 and n=2). A beam of light hits the gas. This beam is a continuous spectrum of yellow/green light (from 495 nm to 590 nm) How many absorption line/s will there be in the spectra? [5] ΑΣΦ 2.0 eV 0 eV BEG YO Color Wavelength Frequency violet 380-450 nm 668-789 THz blue 450-495 nm 606-668 THz green 495-570 nm 526-606 THz yellow 570-590 nm 508-526 THz orange 590-620 nm 484-508 THz red 620-750 nm 400-484 THz Photon energy 2.75-3.26 eV 2.50-2.75 eV 2.17-2.50 eV 2.10-2.17 eV 2.00-2.10 eV 1.65-2.00 eV

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter28: Quantum Physics

Section: Chapter Questions

Problem 25P

See similar textbooks

Similar questions

The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. n = 4 4.0 ev n = 3 1.8 eV n= 2 1.5 ev n= 1 O ev Part A Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nm to 750 nm) How many absorption line/s will there be in the spectra? nνα ΑΣφ ?
The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. n = 4 4.0 ev n = 3 1.8 eV n = 2 1.5 ev n=1 O ev Part A Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nm to 750 nm) How many absorption line/s will there be in the spectra? 1 Correct Part B Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nm to 750 nm) Calculate the wavelength of the absorption line ? da = nm Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining
The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. a) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) How many absorption line/s will there be in the spectra? 1 b) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) Calculate the wavelength of the absorption line λa = 690 nm c) After absorption of the red light, the electrons are now in the n = 3 energy level. How many possible line/s will there be in an emission spectra after absorption of the red light? 3 d) Calculate the wavelength of the emission lines. Enter from smallest wavelength to largest wavelength (or highest energy to lowest energy). Separate each answer by a comma. Please solve for D.
24. I FIGURE EX38.24 is an energy-level diagram for a simple atom. What wavelengths, in nm, appear in the atom's (a) emission spectrum and (b) absorption spectrum? - E, = 4.00 eV n=3 n=2 - Ez = 1.50 eV FIGURE EX38.24 n=1 E, = 0.00 eV
The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. a) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) How many absorption line/s will there be in the spectra? 1 b) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) Calculate the wavelength of the absorption line λa = 690 nm c) After absorption of the red light, the electrons are now in the n = 3 energy level. How many possible line/s will there be in an emission spectra after absorption of the red light? Please solve for C.
Current Time.03.31 1. A magnesium surface has a work function of 3.10 eV. Electromagnetic waves with a wavelength of 200 nm strike the surface and eject electrons. Find the maximum kinetic energy of the ejected electrons. Express your answer in electron volts. eV 16xet16
Calculate the wavelength radiated by the hot plate at 537 °C. A.5397 nm O B. 3580 nm OC.1556 nm OD.2347 nm O E. 3247 nm
When light of wavelength 310 nm is incident on a metal surface, electrons are ejected with a kinetic energy of 1.0 eV. a. What is the work function (binding energy) of this metal (in eV)? b. What is the cutoff wavelength of light (in nm) that can eject electrons? Will photons with wavelength 544 nm eject electrons? Explain your reasoning. c. Determine the wavelength of light (in nm) that should be used to double the kinetic energy of the electrons ejected from this surface.
Calculate the wavelength of a photon emitted when singly ionized helium (He+) transitions from the n = 3 to n = 2 state. The emitted photon has a wavelength of 0.164 nm. A photon is emitted when doubly ionized helium (He++) recombines with an electron to form He+ in the n = 2 state. How does the wavelength of the resulting photon compare to the answer from the previous problem? A. The wavelength is longer in this case because the change in energy (ΔE) is smaller. B. The wavelength is shorter in this case because the change in energy (ΔE) is smaller. C. The wavelength is longer in this case because the change in energy (ΔE) is greater. D. The wavelength is shorter in this case because the change in energy (ΔE) is greater. E. The wavelength is the same because both cases end with He+ in the n = 2 state.
values, and get the results.) 1. Figure on the right is an energy-level diagram for a simple atom. (a) What wavelengths, in nm, appear in the atom's emission spectrum? (b) What wavelengths, in nm, appear in the atom's absorption spectrum? n = 3 E, = 4.00 eV n = 2 E, = 1.50 eV n = 1 E, = 0.00 eV
I need some help with the following problem. 1a. What is the maximum number of electrons that can be emitted if a potassium surface of work function 2.40 eV absorbs 5.00 x 10-3 J of radiation at a wavelength of 325 nm? b. What is the kinetic energy and velocity of the electrons emitted?
Helium was first discovered when astronomers viewed the spectrum from the Sun and could not associate absorption lines associated with any terrestrial element. One wavelength that was strongly absorbed was 587.5 nm (1 nm = 1.0×10-9 m). What is the energy associated with this wavelength of light? a. 1.06 eV (or 1.70×10-19 J) b. 0.943 eV (or 1.51×10-19 J) c. 2.11 eV (or 3.38×10-19 J) d. 0.472 eV (or 7.57×10-20 J)