Submicroscopic Collisions Flashcards
Productive collisions
have enough kinetic energy, correct orientation
Is the presence of an amide favorable for a reaction?
Yes because an amide is stable and has resonance
Energy barrier to reaction
takes a certain amount of energy to go through a reaction
Why do reactions occur faster at higher temperatures?
There is increased kinetic energy, so more particles are able to overcome the energy barrier
Transition state
maximum on the reaction energy diagram
Transition-state structure (activated complex)
the structure that corresponds to the transition state
Why do activated complexes only occur for a short amount of time
they are unstable and have the highest energy that occurs in the reaction
Activation energy (Ea)
difference in energy between the transition state and the reactant(s)
Chemical kinetics
the study of rates and reactions
Steric factor
the fraction of collisions energetic enough to react that actually results in reaction
Rate of a chemical reaction
change in concentration of a reactant or a product per unit of time
Rate equation
rate = k[reactant A]^m[reactant B]^n
m and n are the reaction orders
Rate constant
proportionality constant independent of reactant concentrations that is specific to a particular reaction at a particular temperature
Factors that rate constant (k)
molecule collisions, sufficient energy (smaller Ea = larger rate constant), correct orientation (steric factor)
Arrhenius Equation
k = Ae^(-Ea/RT)
A = frequency factor; depends on the rate at which collisions occur and the fraction of collisions that have the correct orientation
