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Biology
Chapter 3
| Question | Answer |
|---|---|
| Why does water have the four emergent properties. | The water molecule has the ability to form hydrogen bonds |
| Name the four emergent properties of water. | 1. Cohesion 2. Water has high specific heat 3. Oceans and lakes don't freeze solid because ice floats 4. Water is the solvent of life. |
| Explain how water is a polar molecule. | ITs polar covalent bonds and asymmetrical V shape give water molecules polarity (partial units of opposite charge on opposite sides of the molecule). |
| Hydrogen bond | caused by the slightly positive region of one polar molecule being weakly attracted to the slightly negative region of another polar molecule. |
| Name the two factors that determine the length and duration of hydrogen bonds | 1. Molecular distance 2. Molecular energy (explain this: lower energy means lower speed, so H bonds can hold on longer and harder) |
| What is the structural shape of the water molecule | tetrahedral |
| Cohesion | Phenomenon of a substance being held together by hydrogen bonds. I.e. water clinging to itself in rain droplets. |
| Adhesion (definition and 3 examples) | Clinging of one substance to another substance because of hydrogen bonds between the two substances. Example: capillary action (combination of cohesion and adhesion) Example: Water transport up tree Example: Water on the shower doors. Geckos. |
| Surface tension | Measure of how difficult it is to stretch or break the surface of a liquid. |
| Explain difference between heat and temperature | Heat: Measure of all kinetic energy in a system Temperature: Measure of the average kinetic energy of molecules. |
| Calorie definition | amount of heat energy needed to raise 1g of water by 1 degree C |
| Specific heat | resistance to temperature change when absorbing or losing heat. |
| Why is it beneficial for organisms that water has a high specific heat? | So that organisms do not raise their body temperatures too high when doing reactions or using energy. |
| Why does water have a high specific heat? | Because of Hydrogen bonds. Water molecules connected by hydrogen bonds pass the heat through the H bonds onto other water molecules. The water molecules at the surface then take the heat energy off with them as they evaporate. |
| Heat of Vaporization | amount of heat that must be absorbed for 1g of a substance to be converted from liquid to gaseous state. |
| Solution | A homogenous mixture of two or more substances |
| Solvent | substance that dissolves another |
| Solute | substance that is dissolved |
| Acid | A substance that adds H+ (hydronium) |
| Base | A substance that adds OH- |
| What must the H+ and OH- concentrations add up to? | 1 x 10^(-14) M so it can be H+ = 1x10^(-8) and OH- = 1x10^(-16) |
| Buffer | any substance that minimizes pH change by adding or removing H+ example from blood: H2CO3 <=> H+ HCO3- Back and forth to either create H+ or take it away depending on the pH needs of the blood. |
| Alkalosis versus Acidosis | Alkalosis: blood moves toward basic on pH scale Acidosis: blood moves toward acidic on pH scale |
Created by:
hwirth19
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