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the inherent tendency for the process to occur; implies nothing about speed |
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| : area of chemistry thath deals with reaction rates |
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| : series of steps by which a reaction takes place; understanding of the mechanics of a reaction – such as knowledge of catalysts and key concentrations – allows for efficient reactions |
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| change in concentration of a reactant or product per unit time n Rate = [concentration of A at time t(2) – concentration of A at time t (1)]/[t(1) – t(2)] n Delta [A] / Delta [t] |
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: a rate law that expresses how the rate depends on the concentration; considered when concentration changes |
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| : expresses how the concentrations depend on time; convenient for consideration when information of concentrations changing over time is present |
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| : a rate law in which the change in concentration over time remains constant; the equation [A] = -kt + [A0], where time “t1/2” for half-life orders is t1/2={[A]0/(2k)}; INCREASING THE CONCENTRATION does not speed up the reaction |
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| : depends on the concentration of only one reactant (a unimolecular reaction). Other reactants can be present, but each will be zero-order. The rate law for an elementary reaction that is first order with respect to a reactant A is [image] k is the first order rate constant, which has units of 1/time. |
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| cannot determine FUTURE concentratrions/conclusions |
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| proportionality constant called a rate constant, which must be determined experimentally |
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used to determine rate laws; different experiments are done for a short amount of time which change the concentrations |
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| factors that affect how rapidly a reaction will reach equilibrium |
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| what affects reaction rate? |
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| concentration; temperature; catalyst |
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| highest occupied Molecular orbital |
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| the lowest occupied molecular orbital |
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| vibrations in molecules can be treated as ideal springs and calculate force constant |
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| nuclear magnetic resonance |
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| applies a strong external magnetic field around a sample that contains nuclear protons with act as tiny magnets |
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| getting information about the structure of the molecule by shinging electromagnetic radiation ata sample and seeing what wavelengths of light are absorbed |
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| quantized electronic energy levels |
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vibrational energy levels (infra red) electronic energy levels ( VIS/ UV) Rotational energy levels ( microwave) magnetic dipole energy levels (radio) |
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| for this reaction, if the reactant (especially in dimerization) were multiplied by a constant ( such as in doubling or tripling), the products would be multiplied by that constant as well |
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| the time required for a reactant to reach half of its original concentration |
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| pseudo-first-order-rate law |
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| when the concentrations of some reactants remain approximately constant ove rthe course of the reaction; it is a rate law that is obtained by simplifying a more complicated one |
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| a proton split by "n" equivalent protons will give "n+1" peaks |
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| energy level of degenerate MO's on different atoms? |
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| to form bonding MO's they must be simialr in energy or order |
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| delocalized molecular electron orbital |
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| a pi-bond with electrond ensity spread between more than two nuclei |
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| when to use teh MO theory |
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| if you are asked to maek predictions about the bond length strength or look at bond order |
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| look at the HOMO or LUMO when... |
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| ...asked to predict about adding, subtracting electrons regarding bond length/strength; or EA/IA/size |
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long single/double bond alternating particle in a box treatment, energy level difference in vis. region |
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| Vibrational energy levels are quantized |
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| functional groups in different molecules absorb in ___ ____ spectroscopy. |
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| problem with predicting polarity in the LE model |
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| use EN to determine polarity by a fast prediction, but difficult to make quantitative |
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they bond because the bonded state has lower energy than the separated state. form using bonding orbitals |
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| high bond order = high strength= _____ ___? |
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| what is the proximity of electrons which have high stability? |
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| a delocalized Orbital model; the orbitals extend over the whole atom; unlike the LE model, it does not assume that the electrons are kept in one sole area, but that there is 100% probabilty of electron probabilty everywhere. |
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| orbitals on different atoms where the energy levels are similar, and thus can be utilized in Molecular Orbital bonding |
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| bonding in a homonuclear diatomic molecule |
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2 p orbitals have a head-on overlap and - through constructive interferenc - combine to make one big orbital this is a sigma orbital |
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nto described by th eLE model a form of magnetism which occurs only in the presence of an externally applied magnetic field |
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| is weak repulsion from a magnetic field. It is a form of magnetism that is only exhibited by a substance in the presence of an externally applied magnetic field. |
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| heteronuclear diatomic molecules |
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| adjacently placed atoms on the periodic table; therefore these are usually covalently bonded molecules |
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| a situation where the pi bonding can be distributed over a set of atoms, not just two |
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| study of the interaction of electromagnetic radiation with matter the relationship between electromagnetic radiation absorption/emission with state-jumping |
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| change from one electron arrangement to another |
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| are situated in lower enregy states, adn thus are the "preferred" orbitals for electrons because of their relative stability. THese are first to fill |
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nodes which result from electron repulsions between the nuclei, and thus high kinetic enregy adn instability. mismatched phases equate to high kinetic energy and instability and cancellation of charges
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higher electronegativity: for a half-filled bonding MO or for a half-filled anti-bonding orbital? whyyy? |
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bonding MO the bonding orbital is the one with the lower energy stet of the two, and ist he orbital which has the highest electron probability density. with this, it can be inferred that eh molecule which will have the greater attraction for an electron would be the one which needs to fill, or has left to fill, a bonding orbital. |
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| a MO's bonding character is based on .... |
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| .... the kind of native orbital (1s, 2s, etc.) it is situated next to. |
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| the splitting of the NMR signal produced by neighboring protons |
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| quantitative indicator of bond strength and length adn stability; the difference between the number of bonding electrons and the number of antibonding electrons, divided by two |
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