1 / 25

Cloze Reading

Warm-Up : W hat is weird about water? Watch video clip and complete the first column in the 3-column worksheet. Cloze Reading. Read Aloud: Textbook: Molecules at an Exhibition page 169- 170. By Emsley J. (1998)

hasad
Download Presentation

Cloze Reading

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. Warm-Up: What is weird about water?Watch video clip and complete the first column in the 3-column worksheet

  2. Cloze Reading • Read Aloud: • Textbook: Molecules at an Exhibition page 169- 170. By Emsley J. (1998) • Complete the second and third column of the 3-column worksheet as you listen to the article.

  3. Criss Cross Puzzle • Use the textbook read to complete this practice.

  4. Criss Cross Puzzle feedback • 1. Sonochemistry 10. Framework • 2. Boils 11. Cavendish • 3. honeycomb 12. Microbes • 4 Oxygen 13. Expand • 5. Down • 6. Pipes • 7. Supercritical • 8. Freezes • 9. Hydrogen

  5. Video Analysis • Re-watch the video clip and complete the structured video analysis worksheet #1-4

  6. Interactive Mini-LectureTake out a new note sheet and start taking note now

  7. Water is a Chemical!?

  8. H2O • Indeed! Water is one of our most plentiful chemicals. • Its chemical formula, H2O, is probably the most well known of all chemical formulas.

  9. What does the chemical formula tell us? • The formula H2Otells us that one molecule of water is comprised of 2 atoms of hydrogen and one atom of oxygen bonded together. • The bonds which hold the hydrogen and oxygen together are called covalent bonds - they are very strong.

  10. Let's look at a picture of a molecule of water: In this picture the two hydrogen atoms are represented by white spheres and the oxygen by a red sphere.

  11. Why does the water molecule look bent? • The water molecule maintains a bent shape because of two considerations. • First the tetrahedral arrangement around the oxygen and • Second the presence of lone pair electrons on the oxygen.

  12. Did I say "Tetrahedral" - What does that mean? • Tetrahedral means "four-sided". • This molecular shape is shown below. It has regular bond angles of 109.5 degrees

  13. However, there is one important difference - the bond angles for water are not 109.5. Because of the presence of the very negative lone pair electrons, the two hydrogen atoms are squeezed together as the two lone pairs try to get away from each other as far as possible. • The resulting angle gives water a 104.5 bond angleresulting to tetrahedron "looks" BENT!

  14. What are Lone Pair Electrons? • These are the electrons that are not involved in the covalent bonds. The pairs of electrons are left alone. In our picture they are represented by the double dots. • -

  15. These lone pairs are very negative- containing two negative electrons each - and want to stay away from each other as much as possible. • These repulsive forces act to push the hydrogen atoms closer together

  16. The lone pairs are negative - Are the Hydrogenspositive? • The hydrogensare slightly positive. They get this way because of the "electronegativity" of oxygen. • Electronegativityis a measure of how much one atom wants to have electrons, and oxygen wants to have electrons more than hydrogen does. • Oxygen has a higher electronegativity. Because of this difference in electronegativity, the electrons in the covalent bonds between oxygen and hydrogen get pulled slightly toward the oxygen.

  17. This leaves the hydrogen atoms a little bit electron-deficient and thus slightly positive. • We can draw this polarization like this:

  18. Or looking at it from a "net polarization" perspective, like this:

  19. What does the polarization have to do with the properties of water? • Everything! Because water has a slightly negative end and a slightly positive end, it can interact with itself and form a highly organized 'inter-molecular' network. • The positive hydrogen end of one molecule can interact favorably with the negative lone pair of another water molecule. • This interaction is call "Hydrogen Bonding". It is a type of weak electrostatic attraction (positive to negative). Because each and every one of the water molecules can form four Hydrogen Bonds, an elaborate network of molecules is formed.

  20. Ball-and-StickModel of a water molecule

  21. And to interact with other polar molecules - which is how substances become dissolved in water.

  22. Does this make water unusual? • YES! But it's not just that the molecule is bent that makes it special. Water is also highly polar - the two sides of water have very different charge. • Why Ice blocks float on water (Titanic) • Why insects can walk on water • Why water is called a “universal solvent”

  23. But if the Hydrogen Bonds are weak, how can they be important? • Think of how many there are! There is strength in numbers! • The polarity also allows water interact with an electric field:

  24. References • IMAGE SOURCE: "Chemistry in Context" Wm C Brown Publishers, Dubuque Iowa, 2nd edition, A project of the American Chemical Society, ed: A. Truman Schwartz et al., 1997, Chapter 5 "The Wonder of Water" • IMAGE SOURCE: "Chemistry and Life", 4th Edition, John W. Hill, Dorothy M. Feigl, and Stuart J. Baum, Macmillan Publishing Company, New York, 1993

More Related