2.  How does the wavelength of a light beam and the size of a slit it is going through control the amount of diffraction? DO WORK STOP

4.  SLC  Expect more e-mails/phone calls if you’re not showing up  Physics Club  Missing Lens

5.  Learn what spectrometry is and how scientists use it to identify specific atoms.  Be able to calculate the photons released from different energy level drops.

6.  Let’s go over it.

7. What can electromagnetic waves tell us about stars, planets, and galaxies?

8.  Spectroscopy is the process of obtaining a spectrum and reading the information it contains.  Each element has its own unique spectra.  If we collect the spectra of distant objects in our universe we can figure out what elements they are made of.

9.  To perform spectroscopy you need a spectrometer  A spectrometer is an instrument used to measure properties of light over a specific portion of the electromagnetic spectrum  For visible light we will use a spectrometer that has a prism in it and we will use our eyes as the detector.  Different examples of spectrometers

10.  Two ways  1. Draw what you see  2. Plot an Intensity vs. Wavelength Graph

11.  Continuous Spectrum  Spectrum of an ordinary light bulb; rainbow because it has all the visible wavelengths in it  Emission Line Spectrum  A thin cloud of gas emits light only at specific wavelengths that depend on its composition and temperature  Absorption Line Spectrum  If a cloud of gas is between us and a white light source, we still see most of the continuous light emitted by the light. However, the cloud absorbs light of specific wavelength and leaves dark lines

14. 1. What can a spectrometer tell us about a very distant object? 2. What are the three types of spectra?

15.  In 1913 Niels Bohr proposed that an atom has a positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus – similar to the structure of a solar system, but with the attraction provided by electrostatic forces rather than gravity.

17.  Bohr said that when energy is added to an atom it becomes excited and the electrons can temporarily move up to higher orbits.

18.  The Bohr Model says that as an electron returns to its normal orbit it releases the energy it previously absorbed in the form of a photon.

20.  When incoming energy excites a hydrogen atom, its electron is moved into a higher energy level.  Atoms do not want to stay in higher energy levels  So as the electron returns to its original energy level it releases the energy that originally excited it as a photon (light particle)

21.  The Bohr model has been superseded by quantum mechanics.  Electrons do not stay in perfect little orbits, nor are they held there by the electrostatic force.  Quantum mechanics says that electrons are in “electron clouds” that show the probability of an electron being there.

24. 1. What does an electron do as it absorbs energy? 2. What happens when an electron drops an energy level?

26.  SLC  Expect more e-mails/phone calls if you’re not showing up  Physics Club  Missing Lens

27.  Learn what spectrometry is and how scientists use it to identify specific atoms.  Be able to calculate the photons released from different energy level drops.

28.  A specific photon is emitted during any energy level transition as long as the electron is dropping down at least one energy level.  To figure out the energy between any transition use:

29.  This photon has a specific frequency that corresponds to the energy released from the atom  Remember:  We organize energy levels on “Energy Level Diagrams”

31.  Emission and absorption lines form as a direct consequence of the fact that each type of atom, ion, or molecule possesses a unique set of energy levels.  We know the energy levels of atoms, ions, and molecules so we just need to match our experimental observations with what we already know.

32. 1electronvolt (eV) = 1.60x10^-19 J (Reference Table) When an atom ionizes it loses all of its electrons

33.  The negative eV value describes the difference in energy between an electron in an energy level and an electron infinitely far from the nucleus  Where  Z is the atomic number  n is the energy level (1, 2, 3,….)  This only works as an approximation for a single electron (need quantum mechanics)

34.  What is the energy of the photon emitted from a hydrogen atom when the electron falls from level 3 to 1?  Is this different than if it fell from level 3 to 2 and then 2 to 1?

35.  n=3 to n=1;  n=3:-1.51eV  n=1:-13.60eV

36.  n=3 to n=2  n=3:-1.51eV  n=2:-3.40eV  n=2 to n=1  n=2:-3.40eV  n=1:-13.60eV

39.  Page 772 answer questions 29, 30, 32, 33 29. 3.91eV; this energy corresponds to level E6 30. 1.91eV 31. Skip it. 32. A) 2.72eV B) 3.06eV 33. 1.24eV; 2.99x10^14Hz

40.  Regents Part 2  June 2014  Due Friday: Even if you miss class

41.  Using a spectrometer with LEDs demo  Why aren’t the colors in very thin circles?  What can a spectrometer tell you about how a fluorescent light works?

43.  Missing Lens  Homework due Friday  No Physics Club today  Tomorrow  SLC Thursday

44.  We will use 5 samples  Draw what you see  Compare it to a known spectrum

45.  Record spectra on a separate sheet of graph paper. Your scale should range from 400nm to 700nm.  Use the whole width of the paper. 400nm 450nm 500nm 550nm 600nm 650nm 700nm