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Chemistry > Test 3 > Flashcards

Test 3 Flashcards

1
Q

collision theory

A

A model that explains reaction rate as based on the number, every, and orientation of colliding particles.

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2
Q

Arrhenius equation

A

An equation that expresses the exponential relationship between temperature and the rate constant.

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3
Q

activation energy

A

The minimum energy with which molecules must collide to react.

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4
Q

effective collision

A

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

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5
Q

frequency factor

A

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

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6
Q

transition state theory

A

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

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7
Q

transition state

A

An unstable species formed in an effective collision of reactants that exists momentarily when the system is highest in energy and that can either form products or re-form reactants

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8
Q

reaction energy diagram

A

A graph that shows the potential energy of a reacting system as it progresses from reactants to products

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9
Q

reaction mechanism

A

A series of elementary tips that sum to the overall reaction and is consistent with the rate law

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10
Q

elementary reaction

A

A simple reaction that describes a single molecular event in proposed reaction mechanism

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11
Q

molecularity

A

The number of reactant particles involved in a elementary step

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12
Q

unimolecular reaction

A

An elementary reaction that involves the decomposition or rearrangement of a single particle.

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13
Q

bimolecular reaction

A

An elementary reaction involving the collision of two reactant species

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14
Q

rate-determining step

A

The slowest step in a reaction mechanism and therefore the step that limits the overall rate.

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15
Q

reaction intermediate

A

A substance that is formed and used up during the overall reaction and therefore does not appears int he overall equation

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16
Q

catalyst

A

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

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17
Q

homogeneous catalyst

A

A catalyst that exists in the same phase as the reactants.

18
Q

heterogeneous catalyst

A

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

19
Q

hydrogenation

A

The addition of hydrogen to a carbon-carbon multiple bond to form a carbon-carbon single bond.

20
Q

enzyme

A

A biological macromolecule that acts as a catalyst

21
Q

active site

A

The region of an enzyme formed by specific amino acid side chains at which catalysis occurs.

22
Q

equilibrium constant

A

The value obtained when equilibrium concentrations are substituted into the reaction quotient.

23
Q

law of chemical equilibrium

A

The law stating that when a system reaches equilibrium a given temperature, the ratio of quantities that make up the reaction quotient has a constant numerical value

24
Q

reaction of quotient

A

A ratio of terms for a given reaction consisting of product concentrations multiplied together and divided by reactant concentrations multiplied together, each raised to the power of their balancing coefficient. The value of Q changes until the system reaches equilibrium, at which point it equals K.

25
Q

Le Chatelier’s principle

A

A principle stating that if a system in a stat of equilibrium is disturbed, it will undergo a change that shifts its equilibrium position in a direction that reduces the effect of the disturbance

26
Q

Haber process

A

An industrial process used to form ammonia from its elements

27
Q

hydronium ion

A

A proton covalently bonded to a water molecule

28
Q

Arrhenius acid-base definition

A

A model of acid-base behavior in which an acid is a substance that has H in its formula and dissociates in water to yield H3O+, and a base is a substance that has OH in its formula and produces OH- in water

29
Q

neutralization

A

Process that occurs when an H+ ion from an acid combines with an OH- ion from a base to from H2O

30
Q

acid-dissociation constant

A

An equilibrium constant for the dissociation of an acid in H2O to yield the conjugate base and H3O+

31
Q

autoionization

A

A reaction in which two molecules of a substance react to give ions

32
Q

ion-product constant for water

A

The equilibrium constant for the auto ionization of water; equals to 1.00x10^-14 at 298K

33
Q

pH

A

The negative common logarithm of H3O+

34
Q

acid-base indicator

A

An organic molecule whose color is different in acid and in base and is used to monitor the equivalence point of a titration or the pH of a solution

35
Q

Bronsted-Lowry acid-base definition

A

A model of acid-base behavior baed on proton transfer in which an acid and a base are defined, respectively, as species that donate and accept a proton.

36
Q

proton donor

A

A substance that donates an H+ ion

37
Q

proton acceptor

A

A substance that accepts and H+ ion

38
Q

conjugate acid-base pair

A

Two species related to each other through the gain or loss of a proton; the acid has one more proton that its conjugate base.

39
Q

polypro tic acid

A

An acid with more than one ionized proton.

40
Q

base-dissociation constant

A

An equilibrium constant for the reaction of a base with H2O to yield the conjugate acid and OH-

41
Q

Lewis acid-base definition

A

A model of acid-base behavior in which acids and bases are defined, respectively, as species that accept and donate an electron pair.

42
Q

adduct

A

The product of a Lewis acid-base reaction characterized by the formation of a new covalent bond.

Chemistry (25 decks)

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