The breaking bond length changes over the course of the reaction.
Two-step reaction.
The reactant is split apart into two or more products, and a π bond is formed.
Two or more reactants combine to form one product.
One-step reaction.
The 'in-motion' state where the room transitions from being empty to full.
Three possible pathways from the initial state (only B) to the final state (only A).
Carbon.
They are dynamic, constantly changing as they progress.
Changes in energy and molecular shape over the course of a reaction.
The structure at its highest energy just as it breaks.
A large value indicates fast reactions, while a small value indicates slow reactions.
It is a dynamic process, constantly changing as it progresses.
Transition states are dynamic 'in-motion' processes with partial bonds, while mechanistic intermediates are stable enough to be isolated.
Favorable kinetics involves a fast process due to a small barrier, while unfavorable kinetics involves a slow process due to a big barrier.
Only the concentration of AB affects the rate.
The rate increases by 4 times.
The slow step, which is the first step (Ea[1]).
The slow step determines the reaction rate.
They represent structure/energy changes that occur over the course of a reaction.
One-step reaction.
Substitution, Elimination, Addition, and Rearrangement reactions.
As an addition, elimination, or substitution.
One atom or group is replaced or substituted for another.
2nd order.
Structure/energy changes that occur over the course of a reaction.
The reaction occurs in one step.
Favorable thermodynamics and kinetics.
Initial state: reactants (only person B in the room); Final state: products (only person A in the room).
Rate = k[X][NaOH].
Carbon.
The state where both A and B are present in the room.
A single reactant reorganizes its bonding arrangement, changing its atom connectivity.
Propose a mechanism based on the specific reactants and conditions.
The difference in energy between unbroken and broken bonds, indicating if the process is favorable.
ΔG° is less than 0.
When ΔG° is negative (-).
The reaction is favored.
It represents the transition from the intermediate state to the final state.
The structure of the bond at its highest energy just as it breaks.
The activation energy, which is the energy difference between reactants and the TS structure.
Transition state (TS) structure.
The rate of breaking the bond and how quickly the system comes to equilibrium.
It explains in stepwise fashion what bonds are made/broken, the order of bond formation/breakage, where and when charges or unpaired electrons develop, and the relative rates of each step.
The rate of reaction.
rate = k [reactants].
A reaction mechanism with no mechanistic intermediates, just a TS structure.
A very short-lived configuration of atoms at an energy maximum in the reaction sequence, which cannot be isolated as an individual molecule.
The energy barrier to B is high.
The reaction is exothermic and favors products.
Reactants: rubber band; Products: broken rubber band.
Equilibrium favors B, but the reaction will V. SLOWLY go to the right.
A reaction energy diagram showing the stability of products versus reactants and the barriers to reaction rates.
The reaction will rapidly come to equilibrium, converting A to B.
To show the reactants and products involved in the reaction.
Real objects that move in space toward each other.
Δ = heat; hν = light; RT = room temperature.
They are dynamic, involving the making and breaking of bonds.
96 kcal/mole.
By-products.
It involves a sequence of chemical reactions.
Kinetics.
Higher temperature results in a higher reaction rate.
The reaction rate slows down.
Thermodynamics, primarily through differences in bond energies between reactants and products.
(a) Equilibrium must favor products (thermodynamics) and (b) Reaction rate must be reasonably fast (kinetics).
Activation energy.
rate = k [A], where the sum of exponents equals 1.
A reaction energy diagram assuming favorable thermodynamics.
The reaction will NOT go completely to the right ever.
Carbocations, carbanions, and radicals.
The dynamic aspect of chemical reactions.
The energy barrier to B is low.
It takes energy and is the slow step.
It releases energy and is a fast step.
It involves sequential bond breaking and making.
Orbitals from one molecule can gradually overlap with orbitals on another molecule to make new bonds.
198 kcal/mole.
They can be written above or below the arrow in the equation.
In one step.
-1 kcal/mole.
It involves a simple calculation that determines the direction of equilibrium.
Reactants in the same physical state react faster.
Any factor that decreases activation energy will accelerate the reaction rate.
It can have one or several steps and records the fates of all atoms and electrons from all reactants to products.
Molecular species at an energy minimum in a reaction sequence that are theoretically isolable.
Equilibrium favors A.
Products are more stable than reactants.
rate = k [AB][C], where the sum of exponents equals 2.
It represents a reaction mechanism involving the transformation of reactants to products with the involvement of a leaving group.
High energy indicates less stability, while low energy indicates more stability.
They are high in energy and very reactive.
The rate increases by 9 times.
It can lower the activation energy (Ea), allowing the reaction to proceed rapidly to equilibrium.
It indicates that a molecule is formed as a by-product of the reaction.
79 kcal/mole.
Inorganic side products, such as H2O, can be omitted if their presence is clear from the products.
It explains in a stepwise fashion how a reaction occurs, including bond making and breaking.
Intermediate molecular species that form in one step and are quickly consumed in the next step.
199 kcal/mole.
An exothermic reaction.
Increased concentration increases reaction rate.
A catalyst can lower the activation energy (Ea), thus increasing the reaction rate without affecting thermodynamics.
The free energy change, which affects equilibrium.
They relate to the thermodynamics and kinetics of the reaction.
119 kcal/mole.
HBr acts as a reagent and is consumed in the reaction.
103 kcal/mole.
Reagents.
The product is lower in energy than the reactants, indicating stronger bonds and greater stability.
Bond breaking takes energy, while bond making releases energy.
The energy barrier that must be exceeded for reactants to be converted to products.
Activation energy (Ea) affects the rate (kinetics), while free energy change (ΔGo) affects equilibrium (thermodynamics).
