## Concept Question on Study Guide

H-Atom ($E_{n}=-\frac{hR}{n^{2}}$)

ariellasarkissian_3H
Posts: 46
Joined: Fri Sep 28, 2018 12:25 am

### Concept Question on Study Guide

Can someone explain how to use the Bohr frequency condition to explain the origin of lines in the spectrum of an element? Thank you!

Cody Do 2F
Posts: 62
Joined: Fri Sep 28, 2018 12:23 am

### Re: Concept Question on Study Guide

The Bohr Frequency Condition says that when the frequency matches the energy needed for the electron to jump to a higher energy level, then the light will be absorbed. If the frequency doesn't match the energy needed, then the light won't be absorbed. In essence, it simply states that light needs to have enough energy to kick an electron up a level.

In regards to the spectrum lines of an element, if light hits an element, the electrons of that element are excited and raised to a higher energy level. These electrons will then drop in energy level and hit a stable state. The energy level that these electrons drop from produce the lines on the atomic spectra (n=7 dropping to ground state, n=6 dropping to ground state, etc. will produce different lines).