HomeworkLib
Question

A) You are shining ultraviolet light on a gas of an unknown element. You know that...

A) You are shining ultraviolet light on a gas of an unknown element. You know that an electron starts in a ground state with an energy of -12.00 eV. The electron absorbs a 4.00-eV photon. The electron immediately drops to an intermediate energy state Einter of energy -10.80 eV (in this case we will assume it emits a photon when it drops to the intermediate state, though most often the energy is lost through other means). After several seconds the electron drops back down to the ground state. What is the energy of the state which the electron is in after absorbing the UV photon?

B) What is the energy of the first photon emitted?

C) What is the energy of the second photon emitted and is this process considered fluorescence or phosphorescence? (Both answers must be correct for the answer to be correct.)

science   physics   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
A) You are shining ultraviolet light on a gas of an unknown element. You know that...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Problem 2 An electron is confined to a quantum-well device whose potential is illustrated below. On...

    Problem 2 An electron is confined to a quantum-well device whose potential is illustrated below. On either side of the central region -a < x < a, there is a potential step of 5 eV. The walls of the device at x = £b are very rigid. - V(2) 1 -b -a a b х Here a = 1 nm and b= 2 nm. An initially stationary helium atom with mass m = 6.6 x 107 -27 kg absorbs a...

  • A hydrogen atom initially in the n = 3 level emits a photon and ends up...

    A hydrogen atom initially in the n = 3 level emits a photon and ends up in the ground state. (a) What is the energy of the emitted photon? eV (b) If this atom then absorbs a second photon and returns to the n = 3 state, what must the energy of this photon be? eV

  • 1. The energy of the electron in the lowest level of the hydrogen atom (n=1) is...

    1. The energy of the electron in the lowest level of the hydrogen atom (n=1) is -2.179×10-18 J. What is the energy of the electron in level n=5? -8.716×10-20 J (Answer is correct) 2. The electron in a hydrogen atom moves from level n=4 to level n=1. Is a photon emitted or absorbed? What is the wavelength of the photon? 3. An excited hydrogen atom emits a photon with a wavelength of 102.6 nm. In what region of the spectrum...

  • 11. (6 points) A He* ion in its ground state absorbs a photon of energy 51.0...

    11. (6 points) A He* ion in its ground state absorbs a photon of energy 51.0 eV. Which atomic orbital(s) may serve as the final state after the excitation? (i.e. after absorption of 51.0 eV, what excited orbital orbital(s) is the electron in?)

  • Calculate the energy of a photon required to excite a hydrogen atom from the n =...

    Calculate the energy of a photon required to excite a hydrogen atom from the n = 1 state to the n = 2 state. 10. [1pt] Calculate the energy of a photon required to excite a hydrogen atom from the - 1 state to the n - 2 state, Answer: Submit All Answers 11. [1pt] An electron in a hydrogen atom falls to an energy level n = 2. If the wavelength of the emitted electromagnetic radiation is 4.86x10m, what...

  • An electron in an excited state of a hydrogen atom emits two photons in succession, the...

    An electron in an excited state of a hydrogen atom emits two photons in succession, the first at 2624 nm and the second at 97.20 nm, to return to the ground state (n=1). For a given transition, the wavelength of the emitted photon corresponds to the difference in energy between the two energy levels. What were the principal quantum numbers of the initial and intermediate excited states involved?

  • 1. (a) Using the Rydberg formula, classify all of the spectral lines of atomic hydrogen as...

    1. (a) Using the Rydberg formula, classify all of the spectral lines of atomic hydrogen as ultra-violet, visible, orinfra-red. (b)Calculate the upper limit of the energy of photons that can be emitted by a hydrogen atom( Rydberg energy in eV). What is the lower limit? (c) Suppose that a hydrogen atom in its ground-state absorbs a photon whose wavelength is180nm. Will the electron be excited to another level, or will it be ejected from the atom?

  • 21. Suppose that we know that an electron emits a photon having a wavelength of 1.43...

    21. Suppose that we know that an electron emits a photon having a wavelength of 1.43 x 107 meters when it transitions from an unknown energy level to the second excited state ionization 0 eV . 4.9 eV -7.65 eV n=4 second excited state n 3 -13.6 eV first excited state n=2 30.6 ev ground state n# 1 - 122.4 ev On what level did it start? Second excited state a. b. Third excited state c. Fourth excited state d....

  • 27. The "seeing" ability or resolution of radiation is determined by its wavelength. If the size...

    27. The "seeing" ability or resolution of radiation is determined by its wavelength. If the size of an atom is approximately 10-10 m, how fast must an electron travel to have a wavelength smaller than that of an atom? (me 9.11x10- kg and h 6.63 x 10 J-s) a. 7.3 x 10% m/s b. 3.4 x 106 m/s c. 1.0 x 106 m/s d. 5.4 x 10 m/s 28. The ionization energy of the hydrogen atom is 13.6 eV. What...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT