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Do Now 10/17

Do Now 10/17. WOD: DESPOT ( DES puht ) n. an absolute ruler My big brother thinks he is the DESPOT of the family; he is always bossing everyone around. 1.) How much water do you think you use in a day? Month? Year?. Chapter 6.1: The Water Planet. INB Pg 24. The Water Planet.

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Do Now 10/17

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  1. Do Now 10/17 • WOD: DESPOT (DES puht) n. • an absolute ruler • My big brother thinks he is the DESPOT of the family; he is always bossing everyone around. • 1.) How much water do you think you use in a day? Month? Year?

  2. Chapter 6.1: The Water Planet INB Pg 24

  3. The Water Planet • Water covers about ~71% of the Earth’s surface. • Considering the depth and volume, the world’s oceans provide more than 99% of the biosphere – the habitable space on Earth.

  4. Water Distribution • The vast majority of water on Earth can’t be used directly for drinking, irrigation, or industry because it’s salt water.

  5. Water Needs • As the population increases,so does the need for water. • Part of the solution to meeting this demand lies in understanding what water is, where it goes, and how it cycles through nature.

  6. The Water Cycle

  7. Water Wars • http://www.youtube.com/watch?v=eiv0PJzTiMc

  8. Chapter 6.2: Water’s Unique Properties Continue on INB Pg 24

  9. The Polar Molecule • Water is a simple molecule; the way it’s held togethergives it unique properties. • The hydrogen atoms bond to the oxygen atoms witha covalent bond. • A covalent bond is formed by atoms sharing electrons. This makes water a very stable molecule.

  10. The Polar Molecule • A molecule with positive and negative charged endshas polarity and is called a polar molecule. • The water molecule’s polarity allows it to bondwith adjacent water molecules.

  11. The Polar Molecule • The positively charged hydrogen end of one water molecule attracts the negatively charged oxygen end of another water molecule. • This bond between water molecules is called a hydrogen bond.

  12. The Effects of Hydrogen Bonds • Liquid Water. The most important characteristics of the hydrogen bonds is the ability to make water a liquid at room temperature. Without them, water would be a gas.

  13. The Effects of Hydrogen Bonds • Cohesion/Adhesion. Because hydrogen bonds attract water molecules to each other, they tend to stick together. This is cohesion. Water also sticks to other materials due to its polar nature. This is adhesion.

  14. The Effects of Hydrogen Bonds • Viscosity. This is the tendency for a fluid to resist flow.The colder water gets, the more viscous it becomes.It takes more energy for organisms to move through it,and drifting organisms use less energy to keepfrom sinking.

  15. The Effects of Hydrogen Bonds • Surface Tension. A skin-like surface formed due tothe polar nature of water. Surface tension is water’sresistance to objects attempting to penetrate its surface.

  16. The Effects of Hydrogen Bonds • Because of hydrogen bonding, water has a high specific heat • Takes a lot of energy to raise the temperature of water • Large bodies of water (lakes, oceans) are slow to change temperature as atmospheric temperature changes

  17. The Effects of Hydrogen Bonds • Ice Floats: as water cools enough to turn from a liquid into solid ice, the hydrogen bonds spread the molecules into a crystal structure that takes up more space than liquid water, so it floats. • If ice sank, the oceans would be entirely frozen – or at least substantially cooler – because water would not be able to retain as much heat. • The Earth’s climate would be colder – perhaps too cold for life.

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