I’m asking for curriculum planning. Give me a list of topics that I need to teach to meet the questions you need to be able to explain and the additional info you can be required to know. Please only refer to what is explicitly stated and don’t infer any other info.
Questions you need to be able to explain:
Explain the relationship
between the rate of a
chemical reaction and
experimental parameters.
Represent experimental
data with a consistent rate
law expression.
Identify the rate law
expression of a chemical
reaction using data that show
how the concentrations of
reaction species change
over time.
Represent an elementary
reaction as a rate
law expression using
stoichiometry
Explain the relationship
between the rate of an
elementary reaction and
the frequency, energy,
and orientation of
molecular collisions.
Represent the activation
energy and overall energy
change in an elementary
reaction using a reaction
energy profile.
Identify the components of a
reaction mechanism.
Identify the rate law for a
reaction from a mechanism
in which the first step is
rate limiting.
Represent the activation
energy and overall energy
change in a multistep
reaction with a reaction
energy profile.
Explain the relationship
between the effect of
a catalyst on a reaction
and changes in the
reaction mechanism.
Additional info you will be required to know:
TRA-3.A.1
The kinetics of a chemical reaction is defined
as the rate at which an amount of reactants is
converted to products per unit of time.
TRA-3.A.2
The rates of change of reactant and
product concentrations are determined
by the stoichiometry in the balanced
chemical equation.
TRA-3.A.3
The rate of a reaction is influenced by reactant
concentrations, temperature, surface area,
catalysts, and other environmental factors.
TRA-3.B.1
Experimental methods can be used to monitor
the amounts of reactants and/or products
of a reaction and to determine the rate of
the reaction.
TRA-3.B.2
The rate law expresses the rate of a reaction
as proportional to the concentration of each
reactant raised to a power.
TRA-3.B.3
The power of each reactant in the rate law
is the order of the reaction with respect to
that reactant. The sum of the powers of the
reactant concentrations in the rate law is the
overall order of the reaction.
TRA-3.B.4
The proportionality constant in the rate law
is called the rate constant. The value of this
constant is temperature dependent and the
units reflect the overall reaction order.
TRA-3.B.5
Comparing initial rates of a reaction is a
method to determine the order with respect to
each reactant.
TRA-3.C.1
The order of a reaction can be inferred from a
graph of concentration of reactant versus time.
TRA-3.C.2
If a reaction is first order with respect to a
reactant being monitored, a plot of the natural
log (ln) of the reactant concentration as a
function of time will be linear.
TRA-3.C.3
If a reaction is second order with respect
to a reactant being monitored, a plot of the
reciprocal of the concentration of that reactant
versus time will be linear.
TRA-3.C.4
The slopes of the concentration versus
time data for zeroth, first, and second order
reactions can be used to determine the rate
constant for the reaction.
Zeroth order:
EQN: [A]t − [A]0 = −kt
First order:
EQN: ln[A]t − ln[A]0 = −kt
Second order:
EQN: 1/[A]t − 1/[A]0 = kt
TRA-3.C.5
Half-life is a critical parameter for first order
reactions because the half-life is constant and
related to the rate constant for the reaction by
the equation:
EQN: t
1/2 = 0.693/k.
TRA-3.C.6
Radioactive decay processes provide an
important illustration of first order kinetics.
TRA-4.A.1
The rate law of an elementary reaction can
be inferred from the stoichiometry of the
molecules participating in a collision.
TRA-4.A.2
Elementary reactions involving the
simultaneous collision of three or more
particles are rare.
TRA-4.B.1
For an elementary reaction to successfully
produce products, reactants must successfully
collide to initiate bond-breaking and bondmaking events.
TRA-4.B.2
In most reactions, only a small fraction of
the collisions leads to a reaction. Successful
collisions have both sufficient energy to
overcome energy barriers and orientations
that allow the bonds to rearrange in the
required manner.
TRA-4.B.3
The Maxwell-Boltzmann distribution curve
describes the distribution of particle energies;
this distribution can be used to gain a
qualitative estimate of the fraction of collisions
with sufficient energy to lead to a reaction, and
also how that fraction depends on temperature.
TRA-4.C.1
Elementary reactions typically involve the
breaking of some bonds and the forming of
new ones.
TRA-4.C.2
The reaction coordinate is the axis along
which the complex set of motions involved
in rearranging reactants to form products can
be plotted.
TRA-4.C.3
The energy profile gives the energy along the
reaction coordinate, which typically proceeds
from reactants, through a transition state, to
products. The energy difference between
the reactants and the transition state is the
activation energy for the forward reaction.
TRA-4.C.4
The Arrhenius equation relates the
temperature dependence of the rate of an
elementary reaction to the activation energy
needed by molecular collisions to reach the
transition state. 
TRA-5.A.1
A reaction mechanism consists of a series
of elementary reactions, or steps, that occur
in sequence. The components may include
reactants, intermediates, products, and catalysts.
TRA-5.A.2
The elementary steps when combined should
align with the overall balanced equation of a
chemical reaction.
TRA-5.A.3
A reaction intermediate is produced by some
elementary steps and consumed by others, such
that it is present only while a reaction is occurring.
TRA-5.A.4
Experimental detection of a reaction
intermediate is a common way to build
evidence in support of one reaction
mechanism over an alternative mechanism.
TRA-5.B.1
For reaction mechanisms in which each
elementary step is irreversible, or in which the
first step is rate limiting, the rate law of the
reaction is set by the molecularity of the slowest
elementary step (i.e., the rate-limiting step).
If the first elementary reaction is not rate limiting,
approximations (such as steady state) must be
made to determine a rate law expression.
Knowledge of the energetics of each
elementary reaction in a mechanism allows
for the construction of an energy profile for a
multistep reaction.
ENE-1.A.1
In order for a catalyst to increase the rate of
a reaction, the addition of the catalyst must
increase the number of effective collisions and/
or provide a reaction path with a lower activation
energy relative to the original reaction coordinate.
ENE-1.A.2
In a reaction mechanism containing a catalyst,
the net concentration of the catalyst is constant.
However, the catalyst will frequently be
consumed in the rate-determining step of the
reaction, only to be regenerated in a subsequent
step in the mechanism.
ENE-1.A.3
Some catalysts accelerate a reaction by binding to
the reactant(s). The reactants are either oriented
more favorably or react with lower activation
energy. There is often a new reaction intermediate
in which the catalyst is bound to the reactant(s).
Many enzymes function in this manner.
ENE-1.A.4
Some catalysts involve covalent bonding
between the catalyst and the reactant(s). An
example is acid-base catalysis, in which a
reactant or intermediate either gains or loses
a proton. This introduces a new reaction
intermediate and new elementary reactions
involving that intermediate.
ENE-1.A.5
In surface catalysis, a reactant or intermediate
binds to, or forms a covalent bond with,
the surface. This introduces elementary
reactions involving these new bound
reaction intermediate(s).