Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Organic Chemistry > Chemical reactivity and mechanisms > Flashcards

Chemical reactivity and mechanisms Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Heterolytic bond cleavage

A

Results in forming ions & use only a single head curved arrow

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Enthaply (ΔH)

A

Heat at constant pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Bond dissociation energy

A

The energy required to break a covalent bond through hommolytic bond cleavage

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Homolytic Bond cleavage

A

Results in forming two uncharged radicals (Use two half curved arrows)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

The ΔH0 is known as the ______________

A

Standard bond dissociation (under standard conditions like 1 atm)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Heat of reaction

A

The total change in enthaply for a reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Entropy

A

Measure of disorder associated with a system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Spontaneous reaction

A

Increases total entropy (ΔStot = Ssys + Ssurr) (ΔStotal has to be positive for a reaction to be spontaneous)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Between liquids, solids, & gases list it in increasing entropy

A

Ssolid < Sliquid gas (from least to greatest)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Under constant pressure what is the equation used for ΔSsurr ?

A

ΔSsurr = -ΔHsys / T

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the equation for Gibbs free energy?

A

ΔG = ΔH - TΔS (ΔG must be negative for a reaction to be spontaneous)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Exergonic

A

A reaction where ΔG is negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Endergonic

A

A reaction where ΔG is positive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Equilibrium constant (Keq)

A

Keq = [Products] /[Reactants]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Equation relating equilibrium constant to ΔG

A

ΔG = -RTlnKeq

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

With the equation relating ΔG & Keq if ΔG is negative then the __________ are favored (Keq > 1) & if ΔG is positive the _________ will be favored (Keq < 1)

A

Products, Reactnats

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the rate equation?

A

R = k[Reactants] (R = k[A] *[B]*)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are the factors that affect the rate constant?

A
  1. Energy Activation (Ea)
  2. Temperature
  3. Steric Considerations
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

How does Ea (activation energy) affect the rate of a reaction?

A

The activation energy is the minium energy required for a reaction to occur so the lower the Ea the faster the reaction & the larger the Ea the slower the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

How does the temperature affect the rate of a reaction?

A

The rate constant (k) is directly proportional to temp. & the rate of a reaction so increase the temp will increase the rate constant & speed up the rate of the reaction & vis versa when decreased

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Catalysts

A

Speeds up the reaction without being consumed (Enzymes are a type of calalysts)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Transition state on a energy diagram

A

Highest peaks on the graph

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Intermediate on a energy diagram

A

Peaks where it concaves up on the graph

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

The transition state is where the ____________ occurs where bonds are broken & formed

A

Reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What is the Hammond Postulate?

A

States that if the reactants are close in energy to the transition state then the transition state will look like the reactants (exothermic reaction) & if the products are close in energy to the transition state then the transition state will look like the products (endothermic reaction)

26
Q

Nucleophile

A

Reacts with a positive charged atom & donates electrons (has a high electron density)

27
Q

Electrophile

A

Reacts with a negative charged atom & accepts electrons (Low electron density)

28
Q

A ____________ shows how a reaction takes place using a curved arrows to show the flow of electrons (The tail shows where the electrons coming from & the head shows where its going to)

A

Mechanism

29
Q

What are the patterns of a mechanism?

A
  1. Nucleophilic Attack
  2. Loss of a leaving group
  3. Proton Transfer
  4. Rearrangments
30
Q

Nucleophilic Attack

A

A nuclepphile attacking (donating electrons) to an electrophile

31
Q

Loss of a leaving group

A
32
Q

Proton Transfer

A

For a compound to lose a proton (transfer a proton (H) a base must be present to deprontonate the compound)

33
Q

Rearrangment (Carbocation arrangement)

A

Carbocation are stabilized by neigboring alkyl groups & a prcoess calles hyperconjugation- stablizes the P orbitial

34
Q

What are the two types of rearrangments to stablize the carbocations?

A
  1. Hydride shift (involves moving a hydrogen)
  2. Methyl shift (involves moving a methyl group)
35
Q

The terms primary, secondary, tertiary, represents the number of ________ groups attached directly to the positively charged atom

A

Alkyl

36
Q

___________ carbocation are the most stable, & __________ are the least stable (secondary carbocation is in between the two)

A

Tertiary, primary

37
Q

For a mehyl or hydride shift to occur they must be attacthed to a carbon atom that is ____________ to the carbocation

A

Adjacent

38
Q

All mechanism are just a combination of the __________

A

4 patterns

39
Q

When drawing the curved arrow the tail must either be on a bond or _________ & can never be on a __________

A

Lone pair, positive charge

40
Q

The head of the curved arrow shows where the electrons are going to form a _________ or _________

A

Bond or lone pair (Have to make sure dont break the octect rule)

41
Q

When predicting if a carbocation rearrangement (shift) can occur must determine wheteher the carbocation can become more ________ if a methyl or hydride shift was to occur

A

Stable

42
Q

Reversible arrows

A

Equilibrium arrows

43
Q

Irreverisble reaction arrows

A

Forward arrows

44
Q

A reversible arrow is used if the nucleophile is capable of functioning as a _____________ after the nucleophilic attack

A

A good leaving group

45
Q

A irrversible arrow is used if the nucleophile is a _______________

A

Poor leaving group

46
Q

For a loss of a leaving group a reversible arrow is mostly used for the reaction but its used only if the leaving group is capable of functioning as a _____________

A

Good nucleophile

47
Q

For a proton transer they are mostly drawn with a reversible arrow if the ________ difference is low

A

pKa

48
Q

Irreversible arrows are used for a proton transfer when the pKa difference is greater than ______

A

10 pKa

49
Q

Carbocation rearrangment are always drawn with an __________________ arrow

A

Irreversible arrow (Beacuse stabilzing a secondary carbocation into a tertiary one)

50
Q

Free energy diagram gives us information on the ____________ & ________ of a reaction

A

Spontaneity & Rate of reaction

51
Q

Stability & reactivity have a ___________ relationship

A

Inverse relationship (increase the stability decreases the reactivity & vis versa)

52
Q

What are the 4 common indicators of a compound being reactive?

A
  1. Formal charges
  2. net dipoles (partial charges)
  3. π bonds (have a good source of free electrons & wants give away)
  4. Steric affect (Ring strains)
53
Q

Negative charged atoms are called _____________

A

Nucleophiles (donates electrons)

54
Q

Positive charged atoms are called ___________

A

Electrophiles (Accepts electrons)

55
Q

The side of the dipole with the _______________ preference can be used to predict nucleophile or electrophile whenever there is no formal charges present

A

Highest bond (whatever atom can form the most bonds)

56
Q

If a compound is not __________ then its neither nucleophile or electrophile

A

Reactive

57
Q

_____________ can be both a nucleophile or electrophile depending on the atom its reacting with

A

Water

58
Q

Reactive molecules react to become more ___________ & share two electrons

A

Stable

59
Q

Electrons flow from regions of ____________ electron denisty to regions of ______________electron denisty

A

High electron denisty (Nucleophile) , low electron density (Electrophile)

60
Q

________________ always attacks ___________ & the curved arrows shows 2 electrons being shared & an arrow will then be repalced with a sigma bond & bond breaking is only needed to protect the octect rule

A

Nucleophile, electrophile

61
Q

Ring expansion (a type of carbocation rearrangment)

A

Occurs when a carbocation is adjacent to a 3,4,5 or small ring & turns it into a larger ring

Organic Chemistry (47 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions