1 / 20

Chapter 2: Protecting the Ozone Layer

Chapter 2: Protecting the Ozone Layer. Ozone Formation. 3 O 2 2 O 3. Energy must be absorbed for this reaction. Ozone is an allotropic form of oxygen. Element Allotropes oxygen O 2 , O 3 carbon graphite, diamond, buckminister fullerenes. 2.1. Atomic number (A).

addison
Download Presentation

Chapter 2: Protecting the Ozone Layer

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. Chapter 2: Protecting the Ozone Layer

  2. Ozone Formation 3 O2 2 O3 Energy must be absorbed for this reaction Ozone is an allotropic form of oxygen. ElementAllotropes oxygen O2, O3 carbon graphite, diamond, buckminister fullerenes 2.1

  3. Atomic number (A) -The number of protons 8 O 16.00 Mass number (Z) -The sum of the protons and neutrons 2.2

  4. The electrons in the outermostenergy levels are called valence electrons. The group number (of the representative elements) on the periodic table tells you the number of valence electrons. Group 1A: 1 valence electron 1A 8A Group 3A: 3 valence electrons 3A 6A 7A 4A 5A 2A 2.2

  5. Isotopes are two or more forms of the same element (same number of protons) whose atoms differ in number of neutrons, and hence in mass. Isotopes of carbon: C-12, C-13, C-14 also written as: 12C 13C 14C 2.2

  6. Representing molecules with Lewis structures: Consider water, H2O: • 1. Find sum of valence electrons: • 1 O atom x 6 valence electrons per atom = 6 • + 2 H atoms x 1 valence electron per atom = 2 • 8 valence electrons 2. Arrange the electrons in pairs; distribute them so that the octet rule is satisfied: 2.3

  7. Representing molecules with Lewis structures: Typical valence for selected atoms 2.3

  8. Representing molecules with Lewis structures: Multiple bonds Triple bond Double bond Occasionally a single Lewis structure does not adequately represent the true structure of a molecule; so we use resonance forms: 2.3

  9. The Nature of Light Low E High E Wavelength (l) = distance traveled between successive peaks (nm) Frequency (n) = number of waves passing a fixed point in one second (waves/s or 1/s or s-1 or Hz) 2.4

  10. The Electromagnetic Spectrum The various types seem different to our senses, yet they differ only in their respective l and n. 2.4

  11. Visible: l = 700- 400 nm ROY GBIV Decreasingwavelength Infrared (IR) : longest of the visible spectrum, heat ray absorptions cause molecules to bend and stretch Microwaves: cause molecules to rotate At short l range: UV (ultraviolet), X-rays, gamma rays 2.4

  12. The wavelength and frequency of electromagnetic radiation are related by: C = ln where C = 3 x108 m/s (the speed of light). The energy of a photon of electromagnetic radiation is calculated by: E = hn where h = 6.63 x 10-34 J.s (Plank’s constant). Energy and frequency are directly related-higher frequency means higher energy. 2.5

  13. UV radiation is of sufficient energy to cause molecular bonds to break. 2.5

  14. 2.6

  15. The Chapman Cycle A steady state condition 2.6

  16. Biological Effects of Ultraviolet Radiation • The consequences depend primarily on: • The energy associated with the radiation, and • The sensitivity of the organism to that radiation. 2.7

  17. How CFCs Interact with Ozone First, UV radiation breaks a carbon-halogen bond: Photon (l < 220 nm) + CCl2F2 .CClF2 + Cl. (free radicals) 2.9

  18. The chlorine radical attacks an O3 molecule: 2Cl. + 2O3 2ClO. + 2O2 Then two chlorine monoxide radicals combine: 2 ClO. ClOOCl The ClOOCl molecule then decomposes: UV photon + ClOOCl ClOO. + Cl. ClOO. Cl. + O2 The Cl. Radicals are free to attack more O3. The net reaction is: 2 O3 3O2 2.9

  19. As ClO. concentrations increase, ozone concentration decreases. 2.9

  20. HCFCs are alternatives to CFCs: they decompose more readily in troposphere so they will not accumulate to the same extent in stratosphere. 2.9

More Related