Consider the electron transition in the Bohr model of the H atom from the n=2 orbit to the n=6 state? a. Is light absorbed or emitted? b. Calculate the energy, frequency and wavelength in nm of the photon involved.

answer

watching

147

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Jamar FerryLv2

31 Dec 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

1] write the complete and abbreviated electron configuration for each of the following ions, for each ion, identify another ions that is isoelectronic with it. a) Na+ b) P3- c) H-

2] consider the electron cofigurations of the noble gases. which valence sublevels are completely filled for each noble gas?

3] In the Bohr model, is light emitted or absorbed when an electron moves from a higher energy orbit to a lower-energy orbit?

4] in the bohr model, which of the following electron transitions in a hydrogen atom results in emission of the highest -energy photon? n= 3 to n= 2 , n=4 to n = 3

When an electron makes a transition from the n=4 to the n=2hydrogen atom Bohr orbit, the energy difference between these twoorbits (4.1x10^-19J) is emitted as a photon of light. Therelationship between the energy of a photon and its wavelenght isgiven by E=hc/, where E is the energy of thephoton in J, h is Planck's constant (6.626x10^-34J s), and c is thespeed of light (3.00x10⁸m/s). Find the wavelenght oflight emitted by hydrogen atoms when an electron makes thistransition.