= 3. The emission spectrum of Hydrogen has a bright blue-green line at 486 nm. This electron ends in the nf 2 energy level. What is the initial energy of the electron that produced this photon? (Find the energy of the electron in its excited state, n₁). m.)

= 3. The emission spectrum of Hydrogen has a bright blue-green line at 486 nm. This electron ends in the nf 2 energy level. What is the initial energy of the electron that produced this photon? (Find the energy of the electron in its excited state, n₁). m.)

Inquiry into Physics

8th Edition

ISBN:9781337515863

Author:Ostdiek

Publisher:Ostdiek

Chapter10: Atomic Physics

Section: Chapter Questions

Problem 12P

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Concept explainers

The Bohr model

Students often get confused between Rutherford’s model and Bohr model of an atom. They interpret the postulates of both these models to be the same, which is incorrect. Rutherford’s model differs from Bohr’s model in the following ways:

Question

Work through the following problem to determine if the answer is correct or incorrect. Explain why.

3. The emission spectrum of Hydrogen has a bright blue-green line at 486 nm. This electron ends in the nf =
2 energy level. What is the initial energy of the electron that produced this photon? (Find the energy of
the electron in its excited state, nį).
с
Ephoton = h = (6.626 × 10-34 J. s)
Ephoton = 4.09 × 10-1⁹ J = 2.56 eV
Ephoton = -4Eelectron -(Eƒ – E₁)
-13.6 eV
n²
E₁ = Ephoton + Ef = 2.56 eV +
•
(3 × 108 m)
(486 × 10-⁹ m)
E = 2.56 eV +
(-13,6 eV)
E₁ =
= -0.84 eV

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