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| why is water chemically special? |
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Definition
it's polar hydrogen bonds |
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Definition
how hydrogen bonds hold water together the structure of water (and it's more structured than most liquids) |
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Term
| how can plants easily transport water against gravity |
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Definition
hydrogen bonds means that once water starts going up, attached molecules will also want ot come up also adhesion means water sticks to the sides of things, so it naturally creeps up or down any surface it is in contact with |
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Definition
water has a high surface tension (it won't break easily due to hydrogen bonds) fill a glass past full bugs that scuttle across water |
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Definition
a measurement of heat due to the kinetic energy of molecules |
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Term
| difference between heat and temperature |
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Definition
| a swimmer may have a higher temperature than the ocean he is swimming in, but the ocean has more heat. |
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Definition
a unit of heat amount of heat it takes to rasie the temerature of 1 gram of water 1 degree C |
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Definition
a measurement of heat like the calorie |
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Definition
| the amount of energy needed to be gained/lost for 1 gram of the substance to change 1 degree C |
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Term
| water has a _____ specific heat |
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Definition
high this means that water doesn't change temperature easily this is because it takes heat to disrupt and break hydrogen bonds, and water won't heat up until those hydrogen bonds are taken care of |
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Term
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Definition
the ammount of heat 1 gram of something must absorb for it to vaporize |
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Term
| water has a _____ heat of vaporization |
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Definition
high (again, due to hydrogen bonds) also leads to a more stable earth |
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Definition
| when water evaporates, it's only the hottest molecules on the surface that leave. Consequently, the average heat of the surface then declines (until it gets heated up again and the process continues) |
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Term
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Definition
hydrogen bonds.... again when water gets cold and starts to contract, it's too sluggish to break hydrogen bonds. It then takes the path of least resistence and keeps other water molecules at arms length, forming a lattice structure. The result is that ice is less dense than water and so it floats |
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Term
| why is ice floating so important to life? |
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Definition
| because instead of sinking to the bottom and letting the whole ocean freeze, it provides insulation for the depths below it. |
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Definition
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Definition
| the saluting sugar bowl (sugar) |
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Definition
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Definition
| when water is the solvent |
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Definition
| a sphere of water molecules that surrounds a solute |
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Term
| what can be dissolved in water? |
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Definition
anything that is polar or an ion even proteins! (so it can form hydrogen bonds with water) |
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Definition
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Definition
a stable suspension of fine particles in a liquid (it's too big to dissolve!) |
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Definition
relent of water from nonpolar bonds (no hydrogen bonds) |
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Term
| how do you calculate molecular mass? |
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Definition
| take the suscript of each atom and multiply it by the number of daltons in a single one of those atoms (but that's tedious... use mols!) |
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Definition
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Term
| dissassociation of water molecules |
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Definition
when hydrogen bonds are so stong that water molecules are pulled apart to form hydroxide and hydrogen ions. This RARELY ever occurs |
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Definition
a solution which increases te hydrogen ion concentration in a solution |
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Definition
a solution which decreases the number of loose hydrogen ions they can accept tem (NH3 to NH 4) or give off hydroxide ions which then pair up with hydrogen ions, so there are fewer free hydrogens around |
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Term
| strong acids and strong bases |
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Definition
acids and bases that completely dissassociate single arrows to show the reaction, as opposed to the double arrow of a weak acid or weak base |
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| culprit compounds of acid rain |
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Definition
| sulfur andnitrogen oxides |
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Term
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Definition
| acid rain increases the solubility of aluminum to a toxic level |
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