chapter 4 Flashcards
thermodynamics
deals with energy changes accompanying chemical and physical transformations
- describes properties of systems at equilibrium
kinetics
variation of reaction rates with different condition and concentrations of reagents
- rates: how fast something happens
3 steps of chain reaction mechanism
- initiation
- propagation
- termination
initiation
generates reactive intermediate
propagation
reactive intermediate reacts with stable molecule to form product and another reactive intermediate
termination
reactive intermediates destroyed
what kind of light is used to split Cl2
blue light (hv)
reactive intermediate
short-lived series never present in high concentration because it reacts as quickly as it is formed
free radicals
species with unpaired electrons
stability of free radicals
methyl < primary < secondary < tertiary < allylic/benzylic
stability of free radicals according to hybridization
sp < sp2 < sp3
if Keq is larger than 1…
then reaction is favored from left to right
if Keq is less than 1
reaction is favored from right to left
Gibbs free energy (delta G)
change in free energy:
(free energy of products) - (free energy of reactants)
delta H (enthalpy)
(enthalpy of products) - (enthalpy of reactants)
delta G in relation to H,T,S
delta G = delta H - T(delta S)
delta S (entropy)
(entropy of products) - (entropy of reactants)
reactions tend to favor products with the ________ enthalpy
lowest
change in enthalpy (heat of reaction)
amount of heat evolved or consumed in the course of a reaction
do exergonic reactions have a negative or positive g
negative
do endergonic reactions have a negative or positive g
positive
if weaker bonds are broken and stronger bonds are formed, it is an ____________ reaction
exothermic
if stronger bonds are broken and weaker bonds are formed, it is an ____________ reaction
endothermic
entropy
measure of randomness, disorder, or freedom of motion
reactions favor products with the _________ entropy
greatest
bond-dissociation enthalpy (BDE)
amount of enthalpy required to break a particular bond homolytically
homolytic cleavage
each bonded atom retains one of bond’s two electrons - free radicals result
heterolytic cleavage
one of the atoms retains both electrons - ions results
is energy consumed or released when bonds are formed
released
is energy consumed or released when bonds are broken
consumed
are bond-dissociation enthalpies positive or negative
positive (endothermic)
what is the rate of reaction a measure of
how fast the products appear and the reactants disappear
reaction rates depend on the concentration of the __________
reactants
the values of the powers in a rate equation are determined _____________
experimentally
activation energy
energy difference between the reactants and the transition state
transition state
highest-energy state in a molecular collision that leads to reaction
is a transition state stable or unstable
unstable
is a transition state an intermediate
no
is the Ea value always positive or negative
positive
catalysts
lower the activation energy and increase the reaction rate, but don’t affect energies of reactants/products
enzymes
biological catalysts
which step determines the rate of a reaction
the highest-energy step (transition state)
does temperature usually increase or decrease reaction rate
increase - within limits
is the transition state of an endothermic reaction closer to the reactants or products
produc ts
is the transition state of an exothermic reaction closer to the reactants or products
reactants
is chlorination more or less selective
less
is bromination more or less selective
more
is chlorination exothermic or endothermic
exothermic
is bromination exothermic or endothermic
endothermic
rate-limiting step of bromination and chlorination
first propagation step
Hammond’s postulate
related species that are closer in energy are closer in structure
is there a large or small difference in Ea of bromination
large
is there a large or small difference of Ea in chlorination
small
radical inhibitors
slow down or prevent free-radical reactions
carbocation
species that contains a C atom bearing a positive charge
2 ways an alkyl group stabilizes a carbocation
- inductive effect
- partial overlap of filled orbitals with empty ones
4 types of reactive intermediates
- carbocation
- radical
- carbanion
- carbene
stability of carbocations
resonance > 3 > 2 > 1 > methyl
hybridization of carbocations
sp2
hybridization of free radicals
sp2
stability of radicals
resonance > 3 > 2 > 1 > methyl
carbanion
has trivalent carbon atom that bears a negative charge
- Lewis base)
hybridization of carbanion
sp3
stability of carbanions
resonance > methyl > 1 > 2 > 3
carbenes
uncharged reactive intermediates containing a divalent carbon atom
hybridization of carbene
sp2
what happens when 2 carbenes collide
make alkene (double bond)
properties of carbocations
electrophilic, strong acids
properties of radicals
electron-deficient
properties of carbanions
nucleophilic, strong bases
properties of carbenes
both nucleophilic and electrophilic