Test 2 Flashcards

1
Q

Describe the two different types of isomers

A

Constitutional isomers: isomers with different atomic connectivity
Stereoisomers: isomers with the same atomic connectivity but with differed 3D arrangement

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2
Q

define an isomer

A

different compounds with the same molecular formula

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3
Q

define chirality

A

the ability of objects to exist as non-superposable mirror images of each other.
- an object that contains a mirror plane and can be superimposed with its mirror image is achiral
- an objects that does not have a mirror plane and cannot be superimposed with its mirror image

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4
Q

define enantiomers

A

chiral molecules and their non-superimposable mirror images

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5
Q

what does chirality often originate from?

A

an atom that is connected to four different substituents - called a stereogenic centre, chirality centre, or stereo centre

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6
Q

do enantiomers have identical physical and chemical properties?

A

yes; melting points, boiling points, and density are identical. The IR and NMR spectra of enantiomers are also identical

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7
Q

how can enantiomers be differentiated from each other?

A
  1. interactions with other chiral molecules
  2. optical activity (rotation of plane-polarised light by same angle but in opposite directions, + or -)
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8
Q

optical rotation α

A

the angle that a sample rotates plane-polarised light
- clockwise rotation (α > 0): dextrorotary (+ or d)
- counterclockwise rotation (α < 0) levorotary (- or l)

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9
Q

define a racemic mixture

A

a 1:1 mixture of two enantiomers

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10
Q

does a racemic mixture rotate polarised light?

A

no; the single enantiomers rotate light in opposite directions and cancel each other out

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11
Q

how do you determine the absolute configuration of a chirality centre?

A
  1. identify the chirality centre
  2. determine the priorities of attached groups
  3. rotate the molecule to put the lowest priority group (number 4) at the back
  4. determine the direction of priority group numbers 1,2, and 3

if clockwise -> R (right)
if counter-clockwise -> S (left)

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12
Q

define diastereomers

A

stereoisomers that are non-superimposable, non-mirror images

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13
Q

how do diastereomers differ from enantiomers?

A

enantiomers: changing configuration at all stereocenters
diastereomers: changing configuration at some stereocenters

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14
Q

do diastereomers differ in their physical and chemical properties?

A

yes; boiling point, melting point, IR and NMR spectra, solubility, etc

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15
Q

maximum number of stereoisomers =

A

2^n, where n = number of chirality centres

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16
Q

define a meso compound

A
  • a molecule that has chirality centres but is a chiral due to an internal mirror plane
  • the molecule and its mirror image are superimposable = achiral
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17
Q

double bond isomerism

A

E = highest priority groups are trans
Z = highest priority groups are cis

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18
Q

chirality depends on

A

whether the molecule lacks a plane of symmetry and has a non-superimposable mirror image.

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19
Q

do diastereomers have optical activity?

A

yes - diastereomers have different physical properties including optical activity

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20
Q

Define a nucleophile

A

an electron rich species (with a lone pair or pi bond) that reacts by donating an electron pair to an electron-poor species

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21
Q

Define an electrophile

A

an electron poor species (polarised bond or empty orbital) that reacts by accepting an electron pair from a nucleophile

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22
Q

Is a carbonyl carbon a nucleophile or an electrophile?

A

Overall, the molecule is an electrophile.

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23
Q

Electron pairs always move from

A

a nucleophile (high electron density) to an electrophile (low electron density)

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24
Q

when a bond is broken, bonding electrons tend to move toward which atom

A

the more electronegative atom

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25
Q

define polarisability

A

the ability to shift bonding or nonbonding electrons in response to nearly nucleophile or electrophile

26
Q

as you go down a group

A

size increases and polarisability increases (more reactive bonds)

27
Q

as you go across a period

A

size decreases and electronegativity increases (stabilizes negative charge better)

28
Q

why do reactions often involve polar bonds?

A

due to polarisability and differences in electronegativity

29
Q

intermolecular reactions

A

reactions that occur between two or more molecules

30
Q

intramolecular reactions

A

reactions that occur between two functional groups on the same molecule

31
Q

state the equation for the equilibrium constant

32
Q

K(eq) < 1

A

reactants are more favoured

33
Q

K(eq) > 1

A

products are more favoured

34
Q

how is the equilibrium constant K related to the Gibbs free energy change?

A

ΔG = -RTlnK(eq)

K(eq)>1 and ΔG<0: products are favoured (reaction is exergonic)
K(eq)<1 and ΔG>0: reactants are favoured (reaction is endergonic)

35
Q

exergonic

A
  • reactions where there is a net release of free energy
  • spontaneous
  • ΔG<0
36
Q

exothermic

A
  • reactions where there is a net release of heat
  • ΔH<0
37
Q

when ΔH is negative:

A
  • exothermic (heat released)
  • bonds formed in product are stronger (more stable) than bonds broken in reactants
38
Q

when ΔH is positive:

A
  • endothermic (heat absorbed)
  • bonds formed in products are weaker (less stable) than bonds broken in reactants
39
Q

bond dissociation energy

A

the amount of energy required to symmetrically break a covalent bond

40
Q

define entropy (ΔS)

A

measure of freedom of movement or disorder

41
Q

what is the effect of ΔS being positive on ΔG?

A

there is more movement/disorder and ΔG becomes more negative

42
Q

ΔS<0

A

entropically unfavourable

43
Q

ΔS>0

A

entropically favourable

44
Q

transition state

A
  • highest energy structure
  • in-between reactants and products
  • from transition state, reaction can go in either direction
  • cannot be isolated or observed
45
Q

ΔG‡

A
  • activation energy
  • energy required to reach transition state
  • determines the rate of reactions (higher activation E = slower process)
46
Q

what is the rate-determining step of the reaction?

A

the slowest elementary step

47
Q

what is the effect of a catalyst?

A

increase reaction rate without changing ΔG of the overall reaction
- catalyst not consumed during the reaction
- activation energy lowered by providing a new reaction mechanism

48
Q

define a Bronsted acid and a Bronsted base

A

Bronsted acid: proton (H+) donor
Bronsted base: proton (H+) acceptor

49
Q

how can the position of an acid-base equilibrium be determined?

A

by comparing the acid strengths. strong acids dissociate more readily than weak acids, so the equilibrium will lie in the direction of the weaker acid and base

50
Q

draw two free energy graphs for strong and weak acids

51
Q

what is the ΔG for strong/weak acids?

A

strong acids have a negative ΔG
weak acids have a positive ΔG

52
Q

how does pKa relate to acid strength?

A

the lower the pKa value, the stronger the acid

53
Q

how does stability of a conjugate base relate to the strength of an acid?

A

conjugate bases that are stabilised have lower free energy than similar bases without the stabilising effect (->strong acid)

54
Q

how does electronegativity impact acid strength?

A

conjugate bases in which the atom carrying the negative charge is more electronegative are more stable (weaker base). this leads to a stronger acid.

high electronegativity -> increase ability to accomodate negative charge

55
Q

how does induction impact acid strength?

A

removal of electron density from an atom by a strongly electronegative atom nearby increases the ability to accommodate negative charge and increases stability. this leads to a stronger acid.

56
Q

how does hybridisation impact acid strength?

A
  • orbitals with higher ‘s’ character are lower in energy because s orbitals experience a greater effective nuclear charge
  • conjugate bases with unpaired electrons in orbitals with greater ‘s character’ are more stable
  • this leads to a stronger acids
57
Q

s character

A

sp = 50%
sp2 = 33%
sp3 = 25%

58
Q

how does resonance impact acid strength?

A
  • charge delocalisation increases the ability to accommodate negative charge and increases stability for the conjugate base
  • this leads to a stronger acid
59
Q

common acids and their pKa values

A

strongest acid
HCl (-7)
H3O+ (0)
carboxylic acid (5)
phenol (10)
water (16-18)
CH4 (>45)
weakest

60
Q

define a Lewis acid and base

A

Lewis acid: electron pair acceptor
Lewis base: electron pair donor

61
Q

examples of Lewis acids

A
  • tricoordinate B and Al
  • cations such as Li+, Mg2+
62
Q

examples of Lewis bases

A
  • lone-pair donors
  • benzene