Loading presentation...

Present Remotely

Send the link below via email or IM

Copy

Present to your audience

Start remote presentation

  • Invited audience members will follow you as you navigate and present
  • People invited to a presentation do not need a Prezi account
  • This link expires 10 minutes after you close the presentation
  • A maximum of 30 users can follow your presentation
  • Learn more about this feature in our knowledge base article

Do you really want to delete this prezi?

Neither you, nor the coeditors you shared it with will be able to recover it again.

DeleteCancel

Make your likes visible on Facebook?

Connect your Facebook account to Prezi and let your likes appear on your timeline.
You can change this under Settings & Account at any time.

No, thanks

Atomic Emission Spectra of electrons

Learn about why elements emit different wavelength of light. This is exactly how fireworks get their color!
by

Renee Robinson

on 28 September 2015

Comments (0)

Please log in to add your comment.

Report abuse

Transcript of Atomic Emission Spectra of electrons

Atomic Emission Spectra of electrons
Electrons jump energy levels when they reach an excited state
As the electrons drop back down to their original energy level (or ground state),
they release energy in the form of light
We see different colors of light because of the different
wavelengths of light emitted
Each element has a unique color it emits
The unique color is derived from the different wavelengths of light emitted
Electromagnetic radiation
is a form of energy that exhibits wavelike behavior as it travels through space
The light being emitted by the colored fire is directly related to the behavior of

electrons
!

The accumulation of all forms of light is called the
electromagnetic spectrum.
... so basically elements have a unique color they emit which can consist of many wavelengths of light
When the light emitted by an element is passed through a prism or a spectrometer, the light is broken up spatially according to it's wavelength.
The wavelengths emitted by an element is known as it's emission spectrum
The wavelengths absorbed by an element is known as it's absorption spectrum
Red light
emits the highest wavelength of visible light
... but it has the lowest frequency and energy
Purple light
emits the lowest wavelength of visible light
... but it has the highest frequency and energy
-9
The
visible light spectrum
(what we can see) consists of wavelengths from 400 nm to 700 nm
(1 nm = 1 x 10 m)
Relationships between wavelength, frequency, and energy
Relating wavelength and frequency
Relating energy and frequency
The produce of wavelength ( ) and frequency (f) of a wave is equal tjo the speed of light (c)
The speed of light is equal to 3.00 x 10 m/s
Wavelength and frequency are inversely proportional to one another; meaning as one increases the other decreases!
The amount of radiant energy (E) emitted or absorbed by a body is proportional to thfrequency of radiation (f)
This relationship was discovered by Max Planck.
Planck's constant (h) is equal to 6.626 x 10 J/s
Energy and frequency are proportional to one another; meaning as one increases the other increases
Max Planck
8
c = f
E = h f
Mrs. Robinson
Full transcript