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Chem 106 Assessment2
| Term | Definition |
|---|---|
| rate | amount of change in something per unit of time |
| factors affecting how fast reactions occur (4) | surface area/physical state concentration temperature catalysts |
| instantaneous rate of change | tangent line to the point of interest rate at one specific moment |
| average rate of change | rate over a time interval determined by comparing initial and final states |
| average rate of appearance | products |
| average rate of disappearance | reactants |
| rate of reaction ratio | -1/(stoichiometry coefficient)*rate of disappearance - REACTANTS 1/(stoichiometry coefficient)+rate of appearance - PRODUCTS |
| integrated rate law | change in reactant concentration with time |
| rate is proportional to | concentration |
| m n m+n | m and n are orders m+n --> overall reaction order |
| half-lives | interval in which the concentration of a reactant decreases by half |
| zero order | rate does not depend on concentration at all rate = k |
| first order | rate depends on the amount of one reactant |
| pseudo first order | A+B-->C make B so concentrated A doesn't even matter so it is more like B-->C |
| second order | rate depends on the square of one reactant, or two different reactants |
| first and zero order have ____ slope graphs | negative -k |
| second order has a _____ slope graph | positive k |
| collision theory: what conditions facilitate a rxn | collide oriented correctly enough energy/heat to react |
| Activation Energy (Ea) | minimum energy that reactant molecules need to collide and react |
| Activated Complex (or Transition Stat or intermediate) | temporary, unstable arrangement of atoms at the top of that hill |
| only a fraction of atoms have enough energy to react f= | e^-Ea/RT |
| arrhenius equation (both ways) | k=Ae^-Ea/RT lnk=-Ea/RT + lnA |
| as temp increases, k increases | which means the rate increases |
| low activation energy = | fastest reaction (because it's easier to get over that barrier) |
| elementary step | one single step written exactly as it happened, cannot be broken further rate law can be written directly from it |
| reaction mechanism | combo of two elementary steps |
| molecularity | number of reacting atoms/molecules in a step |
| catalyst | substance added to a reaction that increases the rate but is not consumed in the process |
| intermediate | produced in one step of the reaction but consumed in a later step |
| homogenous catalyst | exists in the same phase as reactants |
| heterogenous catalyst | different phase than reactants |
| unimolecular bimolecular termolecular | unimolecular - one reactant bimolecular - 2 reactants termolecular - 3 reactants (very rare, can assume multiple steps) |
| write rate law A--> D | rate = k [A] |
| write rate law A+A--> B | rate = k [A]^2 |
| write rate law A+B--> C | rate= k [A][B] |
| rate | amount of change in something per unit of time |
| factors affecting how fast reactions occur (4) | surface area/physical state concentration temperature catalysts |
| instantaneous rate of change | tangent line to the point of interest rate at one specific moment |
| average rate of change | rate over a time interval determined by comparing initial and final states |
| average rate of appearance | products |
| average rate of disappearance | reactants |
| rate of reaction ratio | -1/(stoichiometry coefficient)*rate of disappearance - REACTANTS 1/(stoichiometry coefficient)+rate of appearance - PRODUCTS |
| integrated rate law | change in reactant concentration with time |
| rate is proportional to | concentration |
| m n m+n | m and n are orders m+n --> overall reaction order |
| half-lives | interval in which the concentration of a reactant decreases by half |
| zero order | rate does not depend on concentration at all rate = k |
| first order | rate depends on the amount of one reactant |
| pseudo first order | A+B-->C make B so concentrated A doesn't even matter so it is more like B-->C |
| second order | rate depends on the square of one reactant, or two different reactants |
| first and zero order have ____ slope graphs | negative -k |
| second order has a _____ slope graph | positive k |
| collision theory: what conditions facilitate a rxn | collide oriented correctly enough energy/heat to react |
| Activation Energy (Ea) | minimum energy that reactant molecules need to collide and react |
| Activated Complex (or Transition Stat or intermediate) | temporary, unstable arrangement of atoms at the top of that hill |
| only a fraction of atoms have enough energy to react f= | e^-Ea/RT |
| arrhenius equation (both ways) | k=Ae^-Ea/RT lnk=-Ea/RT + lnA |
| as temp increases, k increases | which means the rate increases |
| low activation energy = | fastest reaction (because it's easier to get over that barrier) |
| elementary step | one single step written exactly as it happened, cannot be broken further rate law can be written directly from it |
| reaction mechanism | combo of two elementary steps |
| molecularity | number of reacting atoms/molecules in a step |
| catalyst | substance added to a reaction that increases the rate but is not consumed in the process |
| intermediate | produced in one step of the reaction but consumed in a later step |
| homogenous catalyst | exists in the same phase as reactants |
| heterogenous catalyst | different phase than reactants |
| unimolecular bimolecular termolecular | unimolecular - one reactant bimolecular - 2 reactants termolecular - 3 reactants (very rare, can assume multiple steps) |
| write rate law A--> D | rate = k [A] |
| write rate law A+A--> B | rate = k [A]^2 |
| write rate law A+B--> C | rate= k [A][B] |
| catalysis | catalyst lowers activation energy (kind of makes two smaller activation energies) to speed up reaction |
| the mechanism step with the slowest rate is called the | rate limiting or rate determining law |
| you can't use intermediates in rate laws so if you have a fast initial step you have to | assume equilibrium forward = reverse |
| "nuclear strong force" | holds pp np and nn together |
| unstable nuclei - radionuclides | are unstable and so spontaneously emit particles and EM to become stable |
| nuclear decay | unstable nucleus changes into a more stable one by releasing raditation |
| alpha decay | a releases 2 protons and 2 neutrons (He atom) travels 1 inch |
| beta emission | releases an electron (so a neutron turns into a proton) travels several feet |
| gamma radiation | releases electromagnetic energy travels 10-100 ft |
| electron capture | a proton absorbs an electron and turns into a neutron |
| positron emission | proton turns into neutron - so a positron is emitted |
| positron | an electron's mass, but a positive charge |
| a | 4He 2 |
| B | 0e -1 |
| EC | 0e -1 (on the side of reactants) |
| PE | 0e 1 |
| nuclei with 84 protons or above are | unstable, because they are so big and have so many nucleons |
| above belt of stability | too many neutrons beta emission to turn back into protons |
| below belt of stability | too many protons PE or EC to turn neutrons into protons |
| above 84 protons | alpha decay (2 neutrons and 2 protons) |
| carbon dating | n from sun bombard the earth and hit N and become C-14 live plants take the C-14 and slowly decays by beta decay back into N |
| mass defect calculation (static) | between sum of nucleon masses and a nucleus sum of individual nucleon masses - nucleus mass |
| binding energy | energy required to separate nucleons missing mass = energy holding them together |
| mass defect calculation (dynamic) | between parent cell and separate daughter cells final product masses (daughters) - initial reactant mass (parent) |
| fission | slow n enters nucleus making it unstable nucleus splits releasing neutrons and energy |
| fusion | small nuclei fusing into a larger one goes from very unstable to very stable - releases a ton of energy |
| radioactive decay is always | first order |
| activity | disentegrations/second |
| tritium decay | decay of the radioactive version of H -3H |
| geiger counter | used to detect radioactivity by clicking (ions in gas make an electric pulse) |
| alpha particles cant get through | paper/skin |
| beta particles can't get through | muscle/bone/lead |
| gamma rays can't get through | cement |
| not all radiation is dangerous and | radioactive isotopes are found in nature |
| ways to monitor a chemical change over time (4) | pressure concentration conductivity/ions absorption of color/light |
| TEST TIPS read the question how many times? | twice! one to get the story/general idea twice to really pay attention for what they give and why they are asking |
| TEST TIPS explain how to draw on the question | cross off anything distracting/unimportant box useful numbers and label what variable they are circle what they are asking and put in the correct units |
| TEST TIPS how far to round? how precise? | just round all the way! go to the end! |
| two different elements have different | molar masses take that into account when using two elements in a ratio |
| pay attention to units | ms is not the same as s |
| micro | -6 |
| nano | -9 |
| pico | -12 |
| femto | -15 |
| Mega | 6 |
| giga | 9 |
| tera | 12 |
| peta | 15 |
| NH3 | ammonia |
| NH4+ | ammonium ion |
| O2 2- | peroxide |
| OH- | hydroxide |
| H3O+ | hydronium |
| CN- | cyanide |
| SCN- | thiocyanate |
| S2O3 2- | thiosulfate |
| MnO4- | permaganate |
| CH3COO- | acetate |
| C2O4 2- | oxalate |
Created by:
anyasalmon