Term
| principle chemical elements & functions |
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Definition
O- component of water. need for cell respiration. in many organic molecules.
N- component of chlorophyll, nucleus acids & proteins.
C- backbone of organic molecules. bonds to 4 atoms
H- component of water. energy transfers |
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| electron configurations with concentric circles |
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Definition
| Bohr model. inaccurate; orbitals extremely large. |
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| amu/dalton. unit of subatomic particle. |
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| 1 hydrogen. 2 deuterium. 3 tritium |
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| unstable & breakdown into other elements. emit beta (B) particle. neutron becomes proton & electron. |
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| radiation causes dark silver grains in photographic film |
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| tracking stuff through body. dating. cancer- interfere with cell division |
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Definition
| all orbitals in same principle energy level make up the electron shell |
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Definition
| one principle energy level |
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Definition
| proportional to the probability an electron is present there at any given instant |
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| most energetic electrons lie where? least energetic? |
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Definition
| most- outer rings. least- inner rings. because it takes energy to move an electron farther away from charged nucleus. |
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| chemical behavior of an atom determined by? |
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Definition
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| isotopes have similar chemical properties bc |
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| valence shells are identical --> can be substituted in chemical reactions |
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| s orbitals shape? p orbitals shape? |
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Definition
| s- spherical. p- dumbbells. right angles. |
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Definition
| formula's arrangement. H-O-H |
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| rates of forward & reverse rxn's are equal |
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Definition
| electrons shared; fill valence shells |
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Definition
| orbitals become rearranged when bonds are formed; shape of molecule is changed |
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Definition
| "greediness" for shared electron in a covalent bond. |
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| electrons are shared equally |
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| electron closer to one atom. positive end & negative end |
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| oxygen forms polar covalent bonds with |
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Definition
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| oxygen, nitrogen, flourine. relatively weak, but strong collectively. |
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| as electrons move around, termpoarily positive & negative ends. operate over very short distances & very weak. |
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Definition
| can form hydrogen bonds with 4 other waters. cohesion (itself), adhesion (others), capillary action (cohesion & adhesion), surface tension (cohesion) |
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| water is an excellent solvent because |
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Definition
| it is polar; can pull ionic compounds apart |
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Definition
| nonpolar molecules interract with nonpolar molecules. are not disrupted. are insoluble in water, clump together. |
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Definition
| energy of motion of molecules |
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| difference between heat and temperature |
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Definition
| heat- total kinetic energy in a sample; temperature is average kinetic energy of particles |
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| heat of vaporization? units? |
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Definition
| amount of energy to change 1 g of liquid into vapor. units= calories |
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Definition
| amount of heat to raise 1 g of water 1 degree Celsius. 4.184 Joules. |
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| water has high specific heat because? what is water's specific heat? |
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Definition
| hydrogen bonding. 1 cal/g of water per degree Celsius. |
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| water expands when it is cooled because |
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Definition
| hydrogen bonding. bonds are formed- crystal lattice |
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Term
density of water is greatest at__.
above that, ___ |
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Definition
| 4 degrees C. above that, speed of molecules increases and water expands again. |
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Definition
| H+ and OH=. becomes H3O+. |
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Term
| ammonia acts as a base how? |
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Definition
| NH3 accepts a proton from water. NH3 + H2O --> NH4+ + OH- |
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| buffer definition. includes? |
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Definition
| resists changes in pH. includes weak acid or weak base. |
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| how buffers work? formula for carbonic acid? |
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Definition
| weak acids. some undissociated molecules are always present. CO2 + H2O --> H2CO3 --> H+ + HCO3-. carbonic acid; bicarbonate. if H+ ions added, combine with HCO3-. OH- ions are added, combine with H+, and more carbonic acid would dissociate. |
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| an acid and a base react to form a |
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| a compound in which the hydrogen ion of an acid is replaced by some other cation |
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