Chapter Terms/Concepts for MI/LfU
Chapter 13. Chemical Kinetics
rate of reaction
average rate
instantaneous rate
factors that affect rate of reaction
rate law
reaction order
method of initial rates
integrated rate laws
graphical determination of reaction order
0, 1st, and 2nd order plots
half life
rate constant (k)
collision theory
kinetic energy of molecules
orientation of molecules
Arrhenius Equation
activation energy (Ea)
exothermic potential energy diagram vs. endothermic potential energy diagram
activated complex (transition state)
overall heat of reaction (∆H)
reactant and product energy levels
reaction mechanism
molecularity
elementary step
rate determining step
fast vs. slow steps
intermediate
catalyst
homogeneous vs. heterogeneous catalyst
Chapter 14. Chemical Equilibrium
equilibrium
equilibrium constant, Kc
equilibrium reactant and product concentrations
law of mass action
relationship between the extent of reaction and the size of Kc
homogeneous equilibrium reaction
Kp for gas phase reactions
heterogeneous equilibrium reaction
relationship between Kc and Kp
relationship between equilibrium constants (K) and rate constants (k)
reaction quotient (Q)
From comparing Q to K, predict the direction in which a reaction will proceed to reach equilibrium.
ICE table
LeChatelier’s principle
Effect of concentration changes on the equilibrium position.
Effect of pressure (volume) change on the equilibrium position
Effect of temperature change on the equilibrium position.
Effect of temperature change on the size of Kc.
Effect of catalyst on the equilibrium position.
How to select optimum conditions to form a substance
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Chapter 15. Acids and Bases
Bronsted Lowry acid & base
conjugate acid
conjugate base
conjugate acid-base pairs
amphoteric substance
water ionization
relationship between [H+], pH & acidity of a solution.
conversions between pH, [H+], [OH-], and pOH
strong acids
strong bases
weak acids
weak bases
difference between strong acids & bases vs. weak acids & bases
pH of strong acid
pH of strong base
weak acid hydrolysis reaction
Ka expression
relative strengths of acids from Ka values
pH of weak acid
% ionization
weak base hydrolysis reaction
Kb expression
relative strengths of bases from Kb values
pH of weak base
relationship between Ka and Kb values for conjugate acid-base pairs
acidity of salt solutions
neutral, basic and acidic ions
Lewis acids and bases
Chapter 16. Acid-Base Equilibria and Solubility Equilibria
common ion effect
Predict the effect on the pH if a common ion is added to a weak acid or weak base solution.
buffer solution
What types of compounds can form a buffer solution?
buffer capacity
What happens when a strong acid is added to a buffer?
What happens when a strong base is added to a buffer?
Henderson-Hasselbalch equation
indicator
equivalence point
endpoint
strong acid-strong base titration curve
weak acid-strong base titration curve
strong base-strong acid titration curve
weak base-strong acid titration curve
pH at the equivalence point for each of the titration curves
half neutralization point of weak acid-strong base curve
How to select appropriate indicator
salt dissolution reaction
Ksp expression
molar solubility for a salt
effect of adding a common ion on the solubility of a salt.
effect of pH on the solubility of a salt
Predict whether a precipitate will form after mixing 2 solutions.
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Chapter 18. Thermodynamics and Equilibrium
First Law of Thermodynamics
enthalpy (∆H)
state function
standard enthalpy of formation for a compound
nonspontaneous vs. spontaneous processes
Second Law of Thermodynamics
entropy (∆S)
Predict whether ∆S < 0 or > 0 for a given process.
standard entropy of reaction
Third Law of Thermodynamics
entropy vs. temperature plot
Gibbs free energy equation
standard state for elements
standard free energy of formation for a compound
standard free energy of reaction
relationship between ∆G and spontaneity
spontaneous free energy curve
nonspontaneous free energy curve
factors affecting the sign of ∆G
temperature at which a process becomes spontaneous
∆G under nonstandard conditions
relate the ∆G° value (+, - or 0) to the size of K (< 1, > 1, = 1)
Chapter 19. Electrochemistry
oxidation
reduction
oxidizing agent
reducing agent
oxidation-reduction reactions
oxidation number for an atom
voltaic cells (galvanic cells)
battery
standard reduction potential
Standard Hydrogen Electrode (SHE)
relative strength of oxidizing vs. reducing agent from a list of reduction potentials
anode
cathode
salt bridge
half reaction
standard emf of a cell (E°)
relationship between the cell emf (E°) and spontaneity
relationship between E°, ∆G° and K
Nernst Equation
cell potential under nonstandard conditions
electrolytic cells
current (amperes)
coulomb
Faraday
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Chapter 19. Nuclear Chemistry
radioactivity
nuclide
nuclear reactions
alpha decay
beta decay
alpha decay
positron emission
electron capture
nuclear stability
transmutation
radioactive decay series
half life
fission
fusion
critical mass
control rods
fuel rods
moderator
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