Biochem: Chemical principles
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78 terms
Terms | Definitions |
|---|---|
 aufbau principle | always feill lowest energy orbitals first |
| pauli exclusion principle | only two electrions in each orbital with opposite spin |
| hund's rule | if two or more empty orbitals of equal evergy are available, put one electron in each with spins parallel until all orbitals are half full |
| ionization energy | energy it takes to remove a valence electron from an atom in the gaseous state |
| metals ionization energy | low; eaisly give up electrons |
| non metals ionization energy | high; doesnt eaisly give up electrons |
| why do atoms bond together? | the resulting compound is more stable (has less energy) than separte atoms |
| energy in bond forming | energy is released from chemical bond in molecule |
| energy in bond breaking | energy is absorbed when chemical bond is broken |
| covalent bonds | bond formed when atoms share electrons |
| ionic bonds | bond formed when atoms completely transfer electrons |
| polar bond | covalent bond where electrons are unequally shared |
| nonpolar bond | covalent bond where electrons are equally shared |
| combination reaction | two or more reactants combind to yield a single product |
| decompostion reaction | a reactant splits into two for more products |
| single replacement | one element replaces another element |
| double replacement | two elements replace each other |
| redox reaction | an oxidation-reduction reaction transfers electrons from one reactant to another |
| OIL | oxidation is a loss of electrons |
| RIG | reduction is a gain of electrons |
| reducing agent | a substance that is oxidized gives up an election causing reduction |
| oxidizing agent | a substance that is reduced gains an electron causing oxidation |
| reaction conditions for a chemical reaction require: | -collisions between reacting molecules -collisions with sufficient energy to break the bonds in the reactants -the breaking of bonds between atoms of the reactants -the forming of new bonds to give products |
| what does the velocity of a reaction depend on? | the concentration of substrate |
| velocity | slope of the progress curve over an interval of time |
| increase in temperature causes.. | an increase in frequency of collisions and therefore an increase in reaction rate |
| increase in temperature causes.. | an increase in forcefulness of collisions and therefore an increase in reaction rate |
| increace in concentration causes.. | an increase in frequency of collisions and therefore an increase in reaction rate |
| catalyst | a substance that accelerates a chemical reaction but is itself unchanged in the process |
| what lowers the activation energy? | a catalyst |
| stoichiometry | simplest ration of the number of the reactant molecules to the number of product molecules |
| molecularity of a reaction | number of reactant molecules participating in a simple reaction consisting of a single elementary step |
| unimolecular | isomerizations and decompositions |
| biomolecular | associations and exchanges |
| termolecular | requires 3 molecules to simultaniously collide productively; dont see alot |
| the order of a reaction | an empirical quantity determined by inspection of experimentally determined rate law |
| zero order | rate of a reaction is independent of a particular reactant concentration |
| first order | rate of the reaction is directly proportional to a particular reaction concentration |
| second order | reaction is proportional to the square of a particular reactant |
| chemical equilibrium | a state in which the rates of forward and reverse reactions are the same -concentration is not equal, rate is equal |
| thermodynamics | study of the tranformations of energy |
| electrochemistry | movement of electrons |
| bioenergetics | thermochemistry in living systems |
| delta G | free energy change |
| delta H | enthalphy change |
| t | temperature |
| delta S | entropy change |
| state functions | properties that are only dependent on the current state of the system and are independent of the path taken to the current state of the system |
| enthalpy | heat of reaction; amount of evergy absorbed or released during a reaction |
| 1st law of thermodynamics | the internal energy of an isolated system is constant |
| open system | can exchange both energy and matter with its surroundings |
| closed system | can exchange energy but not matter with its surroundings |
| isolated system | can not exchange matter and energy with its surroundings |
| biological cell | open syste; nutrients and waste can exchange iwth surroundings |
| stoppered flask | closed system; can exchange energy but not matter |
| exothermic reactions | the energy of the products is less than the energy of the reactants; heat of reaction is released; heat is a product |
| endothermic reactions | heat is absorbed; the energy of the products is greater than the energy of the reactants; heat is a reactant |
| entropy | the measure of disorder; when matter and energy become disordered, the entropy increases |
| 2nd law of thermodynamics | the entropy of an isolated system tends to increase |
| spontaneous change | change that has a tendency to occur without needing work to be done to bring about the change -order --> disorder |
| nonspontaneous change | change that can be brought about by doing work; no natural tendency to occur -disorder --> order |
| thermodynamic spontaneity | change does or does not have a natural thendency occur |
| G is (-) always if | H (-) and S (+) |
| G is (+) always if | H (+) and S (-) |
| G is (-) | spontaneous |
| G is (+) | non spontaneous |
| H is (+) | unfavorable |
| H is (-) | favorable |
| S is (+) | favorable |
| S is (-) | unfavorable |
| G is (-) at low temp | H (-) and S (-) |
| G is (+) at high temp | H (-) and S (-) |
| G is (+) at low temp | H (+) and S (+) |
| G is (-) at high temp | H (+) and S (+) |
| standard conditions for temp | 25 degrees celcius; 298 K |
| standard conditions for pressure | 1 atm |
| standard conditions for molarity | 1.0 M |
| standard conditions for pH | 7.0 |
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