1 / 15

Three Types of Spectra

Three Types of Spectra. Hydrogen. Hydrogen and Helium. Hydrogen. Helium. Nitrogen and Krypton. Nitrogen. Krypton. Argon and Mercury. Argon. Mercury. Neon. What do you notice about the spectrum for each of the elements?. They are unique to each element. .

perrin
Download Presentation

Three Types of Spectra

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Three Types of Spectra

  2. Hydrogen

  3. Hydrogen and Helium Hydrogen Helium

  4. Nitrogen and Krypton Nitrogen Krypton

  5. Argon and Mercury Argon Mercury

  6. Neon

  7. What do you notice about the spectrum for each of the elements?

  8. They are unique to each element. Each element’s spectrum is a “fingerprint” for that element. It can be used to identify the element.

  9. Test Your Spectral Skills…. • Look at the different spectra below. • Look at the unknown spectrum. • Which two elements make up the unknown spectrum?

  10. By the way….. How does a bright line, or emission spectrum, form?

  11. Spectrum Excited State n=4 UV Excited State n=3 Excited State unstable and drops back down Vi s ible Excited State But only as far as n = 2 this time n=2 • Energy released as a photon • Frequency proportional to energy drop IR n=1 Ground State

  12. http://www.visionlearning.com/library/flash_viewer.php?oid=1347&mid=51http://www.visionlearning.com/library/flash_viewer.php?oid=1347&mid=51

  13. Summary • Electron normally in Ground State • Energy supplied [ as heat or electricity] • Electron jumps to higher energy level • Now in Excited State • Unstable • Drops back to a lower level

  14. Energy that was absorbed to make the jump up is now released as a photon • Frequency depends on difference in energy levels [ E2 - E1 = hf ] h is Plank’s Constant and f is frequency of light • When electron falls to n = 1 level gives UV Range n = 2 level gives Visible Range n = 3,4 or 5 levels gives IR Range

More Related