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chem - chloe > QUARTER 2 EXAM > Flashcards

QUARTER 2 EXAM Flashcards

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1
Q

The area of chemistry concerned with speed, or rates, at which a chemical reaction occurs

A

CHEMICAL KINETICS

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2
Q

refers to the rate of a reaction, or the reaction rate, which is the change in the concentration of a reactant or a product with time (M/s)

A

Kinetics

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3
Q

Any reaction can be represented by the general equation:

A

Reactants → Products

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4
Q

The speed at which a chemical reacts is called reaction rate

A + B → C

A

THE RATE OF REACTION

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5
Q

__________ helps determine how reactions occur, specifically the order in which chemical bonds are broken or formed.

A

Chemical kinetics

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6
Q

Reactants typically _____ in concentration over time, while products ______.

A

decrease ; increase

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7
Q

The more readily molecules collide, the faster they react. Smaller particles with larger surface areas react faster.

In order to react, molecules must come in contact with each other

The more homogeneous the mixture of reactants, the faster the molecules can react

A

PHYSICAL STATE

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7
Q

FACTORS AFFECTING THE RATE OF REACTION

A

PHYSICAL STATE

REACTANT CONCENTRATION

REACTION TEMPERATURE

CATALYST

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8
Q

Higher concentration means more particles are available to collide, increasing the reaction rate.

As reactant concentration increases, the frequency with which the reactant molecules collide increase, leading rates

A

REACTANT CONCENTRATION

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8
Q

Increasing temperature raises kinetic energy, making particles move faster and collide more often.

Reaction rates generally increase as temperature is increased

A

REACTION TEMPERATURE

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9
Q

A _____ speeds up the reaction by changing the reaction mechanism but is not consumed in the process.

A

catalyst

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9
Q

For a reaction to occur:
Particles must _____
_________ to break bonds.
The correct _________ to form new bonds.

A
  1. collide
  2. Sufficient energy
  3. orientation
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10
Q

TRUE OR FALSE

The greater the number of collisions the slower the rate.

A

false

The greater the number of collisions the faster the rate.

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11
Q

true or false

The more molecules present, the greater the probability of collision and the faster the rate.

A

true

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11
Q

In order for reaction to occur the reactant molecules must collide in the correct orientation and with enough energy to form products

true or false

A

true

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12
Q

Reactant rates are denoted with a negative sign to show ______, while products are positive

A

depletion

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13
Q

At any specific time, the rate at which a reaction is proceeding is known as its ________

A

instantaneous rate.

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13
Q

The rate at one single/particular point in time

A

Instantaneous Rate

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13
Q

Rate calculated between 2 points.
: the average between 2 instantaneous reaction rates.

A

Average Rate:

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14
Q

A constant of proportionality between the reaction rate and concentration of reactant

A

RATE CONSTANT

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14
Q

It remains constant regardless of the time point; it does not change over the course of the reaction.

A

RATE CONSTANT

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15
Q

The exponents x and y specify the relationships between the concentrations of reactants A and B and the reaction rate.

A

RATE LAW

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16
Q

For any reaction, the rate law must be determined experimentally

true or false

A

true

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17
Q

A _______reaction is one whose rate depends either on a reactant concentration raised to the second power on the concentrations of two reactants each raised to the first power

A

second-order

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17
Q

Rate expressions are not always determined by experiments

true or false

A

false

Rate expressions are always determined by experiments

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17
Q

It expresses the relationship of the rate of a reaction to the rate constant and the concentration so the reactants raised to some papers:

aA+bBcC+dD

A

rate law

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18
Q

A ______ reaction is one whose rate depends on the concentration of a single reactant raised to the first power

A

first-order

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19
Q

Rate depends on the concentration of one reactant

A

first order

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19
Q

Rate depends on the concentration of one reactant squared or two reactants

A

second-order

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19
Q

is one which rate of disappearance of A is independent of [A]

A

zero-order reaction

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20
Q

Rate is independent of the concentration of reactants

A

zero order

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20
Q

______ Order: The initial rate decreases eightfold when the concentration of the reactant is doubled (1:3 relationship).

A

Third

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21
Q

_____ Order: The initial rate quadruples when the concentration of the reactant is doubled (1:2 relationship).

A

Second

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21
Q

_____ Order: No effect on the initial rate when the concentration of the reactant is changed.

A

Zero

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21
Q

____ Order: The initial rate doubles when the concentration of the reactant is doubled (1:1 relationship).

A

First

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22
Q

The time required for the concentration of a reactant to reach half its initial value

A

THE HALF-LIFE (T ½)

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23
Q

A convenient way to describe how fast a reaction occurs

A

THE HALF-LIFE (T ½)

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24
Q

Drugs with _____ half-lives take longer to take effect but have prolonged action, allowing for less frequent dosing (e.g., once daily, weekly, or monthly).

A

longer

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24
Q

Drugs with _______ half-lives act quickly but wear off rapidly, necessitating multiple doses throughout the day.

A

shorter

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24
Q

Drugs reach a _______—where the amount of drug eliminated equals the amount administered—typically after five half-lives. This is crucial for maintenance medications (e.g., for hypertension, diabetes, and antibiotics).

A

steady state

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24
Q

Constant quantity per time
For every minute, 5mg of the drug is eliminated

A

THE HALF-LIFE: ZERO ORDER

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25
Q

The concentration of the reactant decreases by one-half in each of a series of regularly spaced time intervals, each interval equal to +½

A

THE HALF-LIFE: FIRST ORDER

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25
Q

It is used to calculate the remaining concentration of a substance after a given time period.

A

INTEGRATE RATE LAW: 1ST ORDER

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25
Q

Is the minimum amount of energy required for a chemical reaction to process. It is essentially a barrier that molecules overcome before they can react and form products.

A

ACTIVATION ENERGY

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25
Q

Release energy, making the energy of the products lower than that of the reactants. The activation energy in these reactions is less compared to the total energy released.

A

EXOTHERMIC

26
Q

Constant fraction per time unit
For every minute, 5% of the drug is eliminated

A

THE HALF-LIFE: FIRST ORDER

26
Q

The final state or endpoint of the reaction.

A

PRODUCTS

27
Q

The starting substances in a reaction.

A

REACTANTS

27
Q

Absorb energy, resulting in products with higher energy than the reactants. The activation energy here is greater than the overall energy absorbed.

A

ENDOTHERMIC

28
Q

The energy barrier that must be overcome for a reaction to proceed.

A

Energy Activation (Ea)

29
Q

The intermediate state between the reactants and products, where bonds of the reactants are breaking, and bonds of the products are forming.

A

Transition State (AB)

29
Q

tell you the components of the overall reaction; how will the reaction proceed.

A

REACTION MECHANISM

30
Q

These are the individual, simple steps that make up the overall reaction. They can be unimolecular (involving a single molecule) or bimolecular (involving two molecules)

A

Elementary Steps

31
Q

These are species that are formed during the reaction but are not present in the overall equation. They are often highly reactive and short-lived

A

Intermediates

32
Q

The slowest step in a reaction mechanism, which dictates the overall rate of the reaction. The activation energy for this step is higher than that of other steps, making it the most crucial step in controlling the reaction rate.

A

Rate-Determining Step (RDS)

33
Q

The energy barrier that must be overcome for each elementary step to proceed

A

Activation Energy

34
Q

_______ refers to the number of molecules or ions that collide simultaneously to form a product in a single elementary step of a reaction mechanism. It is an important concept in understanding the kinetics of chemical reactions.

A

Molecularity

34
Q

true or false

Higher molecularity beyond termolecular are very rare due to the low probability of molecules colliding simultaneously

A

true

35
Q

A reaction involving a single molecule

A

UNIMOLECULAR

36
Q

A reaction involving a two molecules

A

BIMOLECULAR

37
Q

A reaction involving a three molecules

A

TERMOLECULAR

37
Q

A catalyst that is present in the same phase as the reactants in a reaction mixture

A

HOMOGENEOUS CATALYST

37
Q

It provides an alternative reaction pathway with lower activation energy, allowing the reaction to occur faster.

A

CATALYSIS

38
Q

Is a substance that increases the rate of a chemical reaction without itself being consumed

A

CATALYSIS

38
Q

An advantage if heterogenous catalysis is that the catalyst mixes into the reaction mixture, allowing a very high degree of interaction between catalyst and reactant molecules

true or false

A

false

An advantage if homogenous catalysis is that the catalyst mixes into the reaction mixture, allowing a very high degree of interaction between catalyst and reactant molecules

39
Q

They allow for an increase in reaction rate without an increase in temperature

A

HOMOGENEOUS CATALYST

40
Q

Mixes well with reactants, ensuring a high degree of interaction, thus increasing the reaction rate without the need for increased temperature.

A

HOMOGENEOUS CATALYST

41
Q

This involves the use of catalyst in a different phase from the reactants
Liquids or gases

A

HETEROGENEOUS CATALYST

41
Q

One or more of the reactants are absorbed on to the surface of the catalyst at the active sites

A

HETEROGENEOUS CATALYST

42
Q

After absorption, the reaction happens and the product molecules are desorbed

A

HETEROGENEOUS CATALYST

43
Q

Good catalyst needs to absorb the reactant molecules strongly enough for them to react, but nor so strongly that the product molecules stick more or less permanently to the surface

true or false

A

true

44
Q

A natural catalyst that accelerates biological reactions in organisms.

A

ENZYMATIC CATALYST

45
Q

The enzyme’s active site is highly specific, following a lock-and-key model. Only substrates that match the active site can bind, lowering activation energy and facilitating the reaction. After the reaction, the products are released.

A

ENZYMATIC CATALYST

46
Q

Key
They bind to the active side of the enzyme, the lock, as it is highly selective, will allow the lowering of activation energy

A

Substrate

47
Q

Hydrolyze the bonds, and break molecules into smaller components by adding water

A

Hydrolases

47
Q

Break the bonds and catalyze the reaction allowing the reaction to proceed, releasing the product
Enzymes’ active side are very specific for a specific substrate

A

Enzyme-Substrate Complex

47
Q

Catalyze oxidation-reduction

A

Oxidoreductases

48
Q

Catalyze the transfer of molecules

A

Transferases

49
Q

Catalyze the cleavage of bonds without the use of water or oxidation; responsible for forming octaval bonds

A

Lyases

50
Q

Help the rearrangement of atoms

A

Isomerases

51
Q

Join two or more molecules together

A

Ligases

52
Q

The state of a chemical reaction when the concentrations of the products and reactants are unchanged over time

A

CHEMICAL EQUILIBRIUM

52
Q

It is also known as Dynamic Equilibrium

A

CHEMICAL EQUILIBRIUM

52
Q

When a reaction reaches equilibrium, the rate of the forward reaction equals the rate of the backward reaction.

A

Equilibrium Condition:

53
Q

all reaction can have an equilibrium

true or false

A

Only a reversible reaction can have an equilibrium

false

54
Q

Reactions at equilibrium are represented by a______________, indicating the reaction is reversible

A

double-headed (equilibrium) arrow (⇌)

55
Q

Reactants (A and B) combine to form products (C and D).

A

Forward Reaction

56
Q

Products (C and D) recombine to reform the reactants (A and B).

A

Reverse Reaction

57
Q

FACTORS AFFECTING EQUILIBRIUM

A

Temperature, Pressure, and Concentration

58
Q

When a system is at equilibrium, a constant value is established by the multiplicative product of the concentrations of the products’ concentrations (each raised first to the power of its coefficient), then divided by the multiplicative product of the reactants’ concentrations (each raised first to the power of its coefficient).

A
  • Law of Mass Action (Cato Maximilian Guldberg and Peter Waage)
59
Q

A ____________ has everything present in the same phase. The usual examples include reactions where everything is a gas, or everything is present in the same solution.

A

homogeneous equilibrium

59
Q

The _________ represents the ratio of the concentrations of the products raised to their stoichiometric coefficients to the concentrations of the reactants raised to their stoichiometric coefficients.

A

equilibrium constant Kc​

59
Q

All reactants and products are in the same phase (all solid, all gas, all aqueous, or all liquid).

A

homogeneous equilibrium

59
Q

A ____________ has things present in more than one phase. The usual examples include reactions involving solids and gases, or solids and liquids.
Reactants and products are in different phases (e.g., gas, aqueous).

A

heterogeneous equilibrium

59
Q

true or false

for equilibrium, the value of K remains constant if temperature is unchanged.

A

true

59
Q

true or false

equilibrium is not affected by: Changes in pressure or addition of a catalyst.

A

true

60
Q

A K value between 0.01 and 100 indicates that the reaction is _________ or _______

A

incomplete or reversible.

61
Q

t or f

The equilibrium constant always has the same value (provided you don’t change the temperature), irrespective of the amounts of A, B, Cand D you started with. It is also unaffected by a change in pressure or whether or not you are using a catalyst.

A

t

62
Q

Measures the relative amount of products and reactants present during a reaction at a particular point in time.

A

THE REACTION QUOTIENT

63
Q

Aids in figuring out which direction a reaction is likely to proceed, given the pressures or the concentrations of the reactants and the products.

A

THE REACTION QUOTIENT

64
Q

If a chemical system at equilibrium experiences a change in concentration, Temperature or pressure (either the reactant or product side), the equilibrium will shift in order to minimize that change.

A

LE CHATELIER’S PRINCIPLE

64
Q

helps to predict what a change in temperature, concentration or pressure will have on the position of the equilibrium in a chemical reaction.

A

LE CHATELIER’S PRINCIPLE

64
Q

If the concentration of a substance is increased, the equilibrium will shift so that the concentration increase.

true or false

A

false

If the concentration of a substance is increased, the equilibrium will shift so that the concentration decreases.

65
Q

If the concentration of a reactant is increased, the equilibrium would shift in the direction of the reaction that used up the reactants

true or false

A

true

66
Q

If the concentration is increased, the equilibrium will shift so that the concentration decreases.

true or false

A

true

67
Q

When the pressure of a system increases, there are less particles in a particular space. The equilibrium will shift in a direction that reduces the number of gas particles so that the pressure is reduced.

true or false

A

false

When the pressure of a system increases, there are more particles in a particular space. The equilibrium will shift in a direction that reduces the number of gas particles so that the pressure is reduced.

68
Q

The chemical system must be in equilibrium first.

t or f

A

t

69
Q

The changes will involve increasing or decreasing something which affects the equilibrium.

t or f

A

t

70
Q

The old equilibrium will not change itself without rearranging the Keq value.
t or f

A

The old equilibrium will change itself without rearranging the Keq value.

71
Q

Keq value changes when pressure is involved.

t or f

A

Keq value changes when temperature is involved.

false

72
Q

If something is increased, the induced change will be for something to decrease.

true or false

A

true

chem - chloe (3 decks)

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