Your SlideShare is downloading. ×
CP5.3--electrons
Upcoming SlideShare
Loading in...5
×

Thanks for flagging this SlideShare!

Oops! An error has occurred.

×
Saving this for later? Get the SlideShare app to save on your phone or tablet. Read anywhere, anytime – even offline.
Text the download link to your phone
Standard text messaging rates apply

CP5.3--electrons

624
views

Published on

Published in: Technology, Education

0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total Views
624
On Slideshare
0
From Embeds
0
Number of Embeds
0
Actions
Shares
0
Downloads
9
Comments
0
Likes
0
Embeds 0
No embeds

Report content
Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
No notes for slide

Transcript

  • 1. Section 3:Physics and the Quantum Mechanical Model
  • 2.  Draw and identify the features of a wave;  Describe the relationship among the frequency, wavelength, and energy of light;  Identify the general ranges of electromagnetic radiation and their relative wavelengths and frequencies;  Explain the source of atomic emission spectra;  Explain how the frequencies of emitted light are related to changes in electron energy
  • 3.  Light made of electromagnetic waves ◦ Considered to be quanta of energy called photons ◦ Has properties of particles and waves Wavelength (λ) :distance between crests Amplitude
  • 4.  Frequency (ν): number of wave cycles to pass a given point per unit of time ◦ SI unit is Hertz (Hz), or s-1  Two are related by the formula:  Since c is constant, λ and ν are inversely proportional  If one is big, the other is small speed of light 3 x 108m/s
  • 5.  If you know either λ or ν, can solve for other  Example: What is the wavelength of a wave with frequency equal to 5.10 x 1014 Hz? c   c Rearrange
  • 6.  Energy of light is related to frequency ◦ Higher the frequency, more energy  Visible light is small slice in the middle of spectrum ◦ Red is lowest ν(longest λ) that the human eye “sees”
  • 7.  Ground state: electrons in lowest possible energy level  Excited state: atoms absorb energy and electrons move to higher energy levels ◦ Once energy source is removed, electrons drop back down to ground state ◦ Emit quanta of energy in the form of… light (sometimes visible)
  • 8.  Atomic emission spectrum: pattern of discreet lines given off by electrons dropping to ground state ◦ Energy levels are quantized ◦ Each line represents a frequency (energy) that is directly proportional to the energy lost by the electron ◦ No two elements have exactly the same spectrum
  • 9.  Each drop an electron makes relates to a specific frequency of energy  Not all is in visible range, but always at discreet frequencies (not continuous)
  • 10.  Draw and identify the features of a wave?  Describe the relationship among the frequency, wavelength, and energy of light?  Identify the general ranges of electromagnetic radiation and their relative wavelengths and frequencies?  Explain the source of atomic emission spectra?  Explain how the frequencies of emitted light are related to changes in electron energy?
  • 11.  Page 140 #14, 15  Page 146 #16, 17, 21

×