1 / 29

Understanding Water Molecules: Protons, Electrons, Polarity, and Hydrogen Bonds

This resource provides a comprehensive look at the water molecule, including the number of protons and electrons it contains, its overall charge, and its unique properties such as polarity and hydrogen bonding. Discover how the uneven charge distribution causes water's cohesiveness and adhesion, which play crucial roles in phenomena like capillary action in plants. Additionally, explore solutions, suspensions, and the importance of buffers in maintaining pH balance in biological systems. Ideal for students studying chemistry or environmental science.

delora
Télécharger la présentation

Understanding Water Molecules: Protons, Electrons, Polarity, and Hydrogen Bonds

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. Solutions, Acids & Bases

  2. The Water Molecule • How many protons does a water molecule have? • How many electrons? • What is the overall charge of a water molecule? 1 H Hydrogen 1.0079 8 O Oxygen 15.9999

  3. The Water Molecule • How many protons does a water molecule have? 10 • How many electrons? • What is the overall charge of a water molecule? 1 H Hydrogen 1.0079 8 O Oxygen 15.9999

  4. The Water Molecule • How many protons does a water molecule have? 10 • How many electrons? 10 • What is the overall charge of a water molecule? 1 H Hydrogen 1.0079 8 O Oxygen 15.9999

  5. The Water Molecule • How many protons does a water molecule have? 10 • How many electrons? 10 • What is the overall charge of a water molecule? 0 + 10 – 10 = 0 1 H Hydrogen 1.0079 8 O Oxygen 15.9999

  6. Polarity • Draw a water molecule e- e- e- e- e- e- e- e- e- e-

  7. Polarity • Draw Hydrogen bonds between one water molecule and another.

  8. Polarity • Oxygen has _____ protons, while Hydrogen only has _____ proton. Oxygen’s greater attraction for electrons causes the Oxygen to have a slightly ______________ charge, while Hydrogen maintains a slightly _____________ charge. 1 H Hydrogen 1.0079 8 O Oxygen 15.9999

  9. Polarity 1 8 • Oxygen has _____ protons, while Hydrogen only has _____ proton. Oxygen’s greater attraction for electrons causes the Oxygen to have a slightly ______________ charge, while Hydrogen maintains a slightly _____________ charge. negative positive 1 H Hydrogen 1.0079 8 O Oxygen 15.9999

  10. Polarity • Key: Why is a water molecule polar? There is an uneven charge between the positive hydrogen and negative oxygen.

  11. Hydrogen Bonds • In terms of a water molecule explain what a hydrogen bond is: The attraction of the positively charged hydrogenatom of one water molecule to the negatively charged oxygenof another water molecule.

  12. Hydrogen Bonds • Cohesion: The ability for water molecules to stick to themselves.

  13. Hydrogen Bonds • How does cohesion explain why some insects can walk on water?

  14. Hydrogen Bonds • Adhesion: The ability for water molecules to stick to other materials.

  15. Hydrogen Bonds • How does adhesion change the way you read this graduated cylinder? Why?

  16. Hydrogen Bonds • What is capillary action in plants? Water clings to the inside of plant roots and climbs, just like water will climb up a paper towel if you put half of it in water.

  17. Solutions and Suspensions • Mixture: A combination of two or more substances that are physically mixed, not chemically combined. • Example: Soil, salsa, trail mix, milk, cereal, sugar water

  18. Solutions and Suspensions • Solutions: A mixture formed when one substance dissolves in another EVENLY. • Example: Salt water

  19. Solutions and Suspensions • Solutions: A mixture formed when one substance dissolves in another EVENLY. • Example: Salt water • A. Solute: Substance dissolved in a solution Salt = Solute

  20. Solutions and Suspensions • Solutions: A mixture formed when one substance dissolves in another EVENLY. • Example: Salt water • A. Solute: Substance dissolved in a solution • B. Solvent: Substance that does the dissolving Salt = Solute Water = Solvent

  21. Solutions and Suspensions • Suspensions: A mixture of water and non-dissolved materials. Example: Blood, aerosol sprays, milk

  22. Apply What You Know Solution or Suspension? Salt and Water Sand and Water Milk Kool-Aid Chicken Noodle Soup

  23. Acids, Bases, and pH pH • The ______ scale is used to measure the strength of acids and bases. • Complete the table: Lemon, vinegar, soda, aspirin Sour, burns, dissolves things 1-7 H+ 7 H2O Pure Water Not acidic, not basic! Soap, baking soda, ammonia 7-14 OH- Bitter, slippery

  24. Acids, Bases, and pH C. Buffer: Weak acids or bases that neutralize strong acids or bases. Why are buffers important? When acids and bases are added to the body, the blood “buffers” preventing a pH change.

  25. Buffers in the Body • pH of blood MUST be between 7.35 and 7.45 • Removing CO2 from the blood helps increase the pH • Removing HCO3- from the blood helps lower the pH • Buffers (Bicarbonate) maintain this acid-base balance in the blood.

  26. pH Lab 3 1 2 4 Each lab station is doing 2 experiments! (3 people per tray) Check assignment on back wall 7 5 6 8

  27. pH Lab 3 1 2 4 Overview • 4 drops of each sample • Put on white scratch paper • Dip a small strip of pH paper in each sample • Compare the color to the chart • Add 4 drops cabbage juice • Color the box & record • Answer questions 7 5 6 8

  28. General Lab Rules • Stay at your lab table unless you are the designated person to get supplies. • Read ALL DIRECTIONS CAREFULLY!!!! • Wash your trays with hot, soapy water. • Clean your lab station & push in stools. • Your lab should look cleaner than when you started! • Have fun!

More Related