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CHM135 > Key terms test 2 > Flashcards

Key terms test 2 Flashcards

(72 cards)

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1
Q

activation energy

A

the minimum energy with which molecules must collide to react

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2
Q

active site

A

the region of an enzyme formed by specific amino-acid side chains at which catalysis occurs

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3
Q

arhenius equation

A

an equation that expresses the exponential relationship between temperature and the rate constant

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4
Q

average rate

A

the change in concentration of reactants/products divided by a finite time period

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5
Q

biomolecular reaction

A

an elementary reaction involving the collision of two reactant species

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6
Q

catalyst

A

a substance or mixture that increases the rate of reaction without being used up in the process

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7
Q

chemical kinetics

A

the study of the rates of reactions and the factors that affect them

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8
Q

collision theory

A

a model that explains reaction rate based on the number, energy, and orientation of colliding particles

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9
Q

effective collision

A

a collision in which the particles meet with sufficient energy and an orientation that allows them to react

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10
Q

elementary reaction/step

A

a simple reaction that describes a singular molecular event in a proposed reaction mechanism

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11
Q

enzyme

A

a biological macromolecule that acts as a catalyst

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12
Q

enzyme-substrate complex

A

the intermediate in an enzyme-catalyzed reaction, which consists of enzyme and substrates and whose concentration determines the rate of a product formation

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13
Q

frequency factor

A

the product of the colision frequency Z and an orientation probability factor p that is specific for a reaction

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14
Q

half life

A

in chemical porcesses, the time required for the reactant concentration to reach hald of its initial value. in nuclear processes, the time required for half the initial number of nuclei in a sample to decay

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14
Q

heterogeneous catalyst

A

a catalyst that occurs in a different phase from the reactants, usually a solid interacting with gaseous or liquid reactants

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15
Q

homogenous catalyst

A

a catalyst that exists in the same phase as the reactants

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16
Q

hydrogenation

A

the addition of hydrogen to a carbon-carbon multiple bond to form a carbon-carbon single bond

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17
Q

induced-fit model

A

a model of enzyme action that pictures the binding of the substrate as inducing the active site to change its shape and become catalytically active

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18
Q

initial rate

A

the instantaneous rate at the moment the reactants are mixed, that is, at t=0

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19
Q

instantaneous rate

A

the reaction rate at a particular time, given by the slope of a tangent to a plot of reactant concentration vs. time

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20
Q

integrated rate laws

A

a mathematical expression for reactant concentration as a function of time

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21
Q

lock and key model

A

a model of enzyme function that pictures the enzyme active site and the substrate as rigid shapes that fit together as a lock and key, respectively

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22
Q

molecularity

A

the number of reactant particles involved in an elementary step

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22
Q

rate constant (k)

A

the proportionality constant that related reaction rate to reactant (and product) concentrations

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23
rate-determining/limiting step
the slowest step in a reaction mechanism and therefore the step that limits the overall rate
24
rate law/equation
an equation that expresses the rate of a reactin as a function of reactant/product concentrations and temperature
25
reaction energy diagram
a graph that shows the potential energy of a reacting system as it progresses from reactants to products
26
reaction intermediate
a substance that is formed and used up during the overall reaction and therefore does not appear in the overall equation
27
reaction mechanism
a series of elementary steps that sum to the overall reaction and is consistent with the rate law
28
reaction order
the exponent of a reactant concentration in a rate law that shows how the rate is affected by changes in that concentration
29
reaction rate
the change in the concentrations of reactants/products with time
30
substrate
a reactant that binds to the active site in an enzyme-catalyzed reaction
31
transition state / activated complex
an unstable species formed in an effective collision of reactants that exist momentarily when the system is highest in energy and that can either form products or re-form reactants
32
transition state theory
a model that explains how the energy of reactant collisions is used to form a high-energy transitional species that can change to reactant or product
33
unimolecular reaction
an elementary reaction that involves the decomposition or rearrangement of a single particle
34
equilibrium constant (K)
the value obtained when equilibrium concentrations are substituted into the reaction quotient
35
haber process
an industrial process used to form ammonia from its elements
36
law of chemical equilibrium/law of mass action
the law stating that, when a system reaches equilibrium at a given temperature, the ratio of quantities that make up the reaction quotient has a constant numerical value
37
le châteliers principle
a principle stating that, if a system in a state of equilibrium is disturbed, it will undergo a change that shifts its equilibrium position in a direction that reduces the effect of one disturbance
38
reaction quotient (Q)/ mass-action expression
a ratio of terms for a given reaction consisting of product concentrations multiplied together and divided by reactant concentrations multiplied together, with each concentration raised to the power of its balancing coefficient. the value of Q changes until the system reaches equilibrium, at which point it equals K
39
van't hoff equation
an equation for calculating the change in equilibrium constant that occurs with a change in temperature
40
define equilibrium in terms of reaction rates
at equilibrium: rate fwd = rate rev
41
acid-base indicator
an organic molecule whose colour is different in acid and in base; the colour is used to monitor the equivalence point of a titration or the pH of a solution
42
acid-dissociation (acid-ionization) constant (Ka)
an equilibrium constant for the dissociation of an acid (HA) in H2O to yield the conjugate base (A-) and H3O+
43
adduct
the product of a lewis acid-base reaction, species that contains a new covalent bond
44
amphiprotic
a substance that can either donate or accept a proton (H+)
45
arrhenius acid-base definition
a model of acid-base behaviour in which an acid is a substance that has H in its formula and dissociated in water to yield H3O+, and a base is a substance that has OH in its formula and produces OH- in water
46
autoionization/self-ionization
a reaction in which two molecules of a substance react to give ions. the most important example is for water
47
base-dissociation (base-ionization) constant (Kb)
an equillibrium constant for the reaction of a base (B) with H2O to yield the conjugate acid (BH+ and OH-):
48
brønsted-lowry acid-base definition
a model of acid-base behaviour based on proton transfer, in which an acid and a base are defined, respectively, as a species that donates a proton and one that accepts a proton
49
conjugate acid-base pair
two species related to each other through the gain or loss of a proton; the acid has one more proton than its conjugate base
50
hydronium ion (H3O+)
a proton covalently bonded to a water molecule
51
ion-product constant for water (Kw)
the equilibrium constant for the autoionization of water; equal to 1.0x10^-14 at 298K
52
leveling effect
the inability of a solvent to distinguish the strength of an acid/base that is stronger than the conjugate acid/base of the solvent
53
lewis acid-base definition
a model of acid-base behaviour in which acids and bases are defined, respectively, as species that accept and donate an electron pair
54
neutralization
the process that occurs when an H+ ion from an acid combines with an OH- ion from a base to form H2O
55
pH
the negative common logarith of [H3O+]
56
proton acceptor
a species that accepts an H+ ion; a Brønsted-lowry base
57
proton donor
a species that donates an H+ ion; a Brønsted-lowry acid
58
acid-base buffer
a solution that resists changes in pH when a small amount of either stronf acid or strong base is added
59
acid-base titration curve
a plot of the pH of a solution of acid/base versus the volume of base/acid added to the solution
60
buffer capacity
a measure of the ability of a buffer to resist a change in pH; related to the total concentrations and relative proportions of buffer components
61
buffer range
the pH range over which a buffer acts effectively
62
common-ion effect
the shift in the position of an ionic equilibrium away from an ion invlved in the process that is caused by the addition or presence of that ion
63
complex ion
an ion consisting of a central metal ion covalently bonded to two or more anions or molecules, called ligands
64
end point
the point in a titration at which the indicator changes colour permanently
65
equivalence point
the point in a titration when the number of moles of the added species is stoichiometrically equivalent to the original number of moles of the other species
66
formation constant (Kf)
an equilibrium constant for the formation of a complex ion from the hydrated metal ion and ligands
67
henderson-hasselbalch equation
an equation for calculating the pH of a buffer system:
68
ligand
a molecule or an anion bonded to a central metal ion in a complex ion
69
selective precipitation
the process of seperating ions through differences in the solubility of their compounds with a given precipitating ion
70
solubility product constant (Ksp)
an equilibrium constant for a slightly soluble ionic compound dissolving in water

CHM135 (3 decks)

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