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Polarity of H2O
| Term | Definition |
|---|---|
| Polar Covalent | Electrons not shared equally: H2O, are attracted to other polar molecules, like for like. This result in partial charged on Oxygen and Hydrogen |
| Hydrogen bonds | Partially positive hydrogen attracted to an electronegative atom in another polar covalent molecule |
| Intermolecular bond | Between molecules |
| Hydrogen bond | Water molecules move a lot. Hydrogen bonds form, break, and re-form with great frequency. The hydrogen bonds between water make it more structured than most liquids. |
| Weak bonds | Weak bonds are found in many large biomolecules. Hydrogen bounds are in DNA and Water. Van der Waals Forces - instantaneous dipole interactions ex: in gecko feet. Reversibility can be an advantage |
| Emergence | Increasing levels of complexity in a system can demonstrated novel properties not seen in levels below them |
| Water’s unique properties | Due to polarity of water and its resulting hydrogen bonds |
| Cohesion and Adhesion | Cohesion : sticking to other water molecules and Adhesion: sticking to other things - water does both. |
| Transpiration | Moves water upwards in trees; utilizes cohesion and adhesion |
| Capillary Action | The spontaneous upward movement of water to the forces of adhesion cohesion and surface tension; occurs when adhesion is greater than cohesion due to tubes in plants/trees (xylem) |
| Specific Heat | How much heat is absorbed/released before an increase/decrease in temp; Water specific heat capacity is high (4.18) -> heat must be absorbed to break hydrogen bonds, but heat is released when hydrogen bonds form |
| Specific Heat: in nature/environment | Moderates air temperature in large bodies of water can absorb hear in the daytime and release heat at nigh, stabilizes ocean temperature, benefits marine life, organisms can resist changes in their own internal temperature. |
| Evaporative Cooling | Water has a high heat of vaporization and the molecules with the highest kinetic energy leave as gas : moderate earth’s climate, stabilizes temperature in lakes and ponds, prevents terrestrial organisms from overheating, prevents leaves from becoming hot |
| Expansion of solid form | Ice floats, solid water is less dense than liquid water which is why aquatic life can live under ice |
| Water is an excellent solvent | Water comes close to universal solvent because of the polarity and hydrogen bonds. |
| Water dissociation | Because water is so polar, it can easily break apart, which produced hydronium (H+)and a hydroxide (OH-) ion; in pure water the concentration is even. |
| Acids and Bases | Donate protons (H+) to water and in acidic solutions: H3O is greater than OH and opposite in basic solutions |
| pH | Measure of acidity, potential of hydrogen |
| Acids | Materials that can release H+. HCl -> H+ + Cl- |
| Bases | Materials that can absorb H+ and produce OH NaOH -> Na+ and OH- |
| Buffers | Materials that have both acid and base properties, which resist pH shifts, cells and other biological solutions often contain buffers to prevent damage. |
Created by:
nuhaSalim