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organic chemistry bsc > organic chemistry (knight) > Flashcards

organic chemistry (knight) Flashcards

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1
Q

What is R?

A

any alkyl group

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2
Q

What is i-Pr?

A

isopropyl

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3
Q

What is i-Bu?

A

isobutyl

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4
Q

What is s-Bu?

A

sec-butyl

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5
Q

What is t-Bu?

A

tert-butyl

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6
Q

What is Ac an abbreviation for?

A

acetyl group

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7
Q

What is Ar an abbreviation for?

A

an aryl group meaning any aromatic ring

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8
Q

What is Ph an abbreviation for?

A

a phenyl group

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9
Q

What is Bn an abbreviation for?

A

Benzyl

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10
Q

How are orbitals represented?

A

they are represented by a single contour within which there is a 90% chance of finding the electron

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11
Q

What are the three different type of p orbitals?

A

there are 3 degenerate p-orbitals all 90 degrees to each other
Px, Py, Pz

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12
Q

What are the patterns that the energies of atomic orbitals show?

A
  • each orbital can hold a maximum of 2 electrons
  • electrons are placed in orbitals from the lowest energy upwards
  • electrons do not pair if there is an empty degenerate orbitals
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13
Q

describe the two ways that 1s orbitals overlap

A

the 1s orbitals can either overlap in phase and become the bonding orbital the electrons will occupy the bonding (sigma) resulting in an energy drop. Or 1s orbitals can overlap out of phase and become the antibonding orbital and this antibonding orbital if empty does not contribute to the energy

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14
Q

Why doesn’t helium form He2?

A

the four electrons in helium would fully occupy both the bonding orbital and the antibonding orbital resulting in an overall energy increase so it is energetically unfavorable

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15
Q

describe a sigma orbital and how they are formed.

A

sigma orbitals are cylindrically symmetrical
a sigma bond can be formed by an overlap of 2 s orbitals or by one side on p and one s in the same phase to make the bonding orbital or a p orbital side on and an s orbital in different phases to make the antibonding orbital. this is the same logic with 2 p orbitals end on

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16
Q

how do u produce pi orbitals

A

side on overlap of p orbitals in phase will produce the bonding pi orbital and out of phase overlap of 2 end on p orbitals will produce the antibonding pi orbitals

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17
Q

describe sp3 hybridization

A

mixing 1 s orbital and 3 p orbitals this we generate 4 hybrid orbitals which point to the corners of a tetrahedral in order to be as far apart as possible this means there are no remaining p orbitals and it can for 4 sigma bonds

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18
Q

describe sp2 hybridization

A

mixing one s orbital and 2 p orbitals will generate 3 identical sp2 hybrid orbitals which will be trigonal planar structure in order to be as far apart as possible there will be 1 remaining p orbital. and these can for 3 sigma bonds and one pi bond

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19
Q

describe sp hybridisation

A

when one s orbital and one p will generate 2 hybrid orbitals which will take a linear structure containing 2 remaining p orbitals which can for 2 sigma bonds and 2 pi bonds

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20
Q

draw an n-propyl group

A

see one note

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21
Q

draw an iso-propyl group

A

see one note

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22
Q

draw an n-butyl group

A

see one note

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23
Q

draw an iso-butyl group

A

see one note

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24
Q

draw a sec- butyl group

A

see one note

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25
Q

draw a tert-butyl group

A

see one note

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26
Q

draw formic acid structure

A

methanoic acid see one note

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27
Q

draw formaldehyde

A

methanal see one note

28
Q

draw acetic acid

A

ethanoic acid see one note

29
Q

draw acetaldehyde

A

ethanal see one note

30
Q

draw acetyl chloride

A
31
Q

draw ethyl acetate

A
32
Q

draw benzene

A
33
Q

draw toluene

A
34
Q

draw pyridine

A
35
Q

draw phenol

A
36
Q

draw acetone

A
37
Q

draw diethyl ether

A
38
Q

draw THF

A
39
Q

what does THF stand for

A

tetrahydrofuran

40
Q

draw DMF

A
41
Q

what does DMF

A

dimethylformamide

42
Q

draw DMSO

A
43
Q

what does DMSO stand for

A

dimethylsulfoxide

44
Q

what is an orbital

A

Orbitals describes energy and distribution of an electron, orbitals are represented by a single contour where there is a 90% chance of finding the electron

45
Q

what are the 3 degenerate p orbitals of equal energy

A

Px, Py, Pz
all at 90 degrees to each other

46
Q

What brings molecules together

A
  • Cations and anions
  • Ions and dipoles
  • Dipoles and dipoles
47
Q

how can reactions still happen if there are no charges or dipoles

A

Reactions involve changes in the bonding: bonds are made and broken, and this is caused by a flow of electrons
One reactant donates electrons the nucleophile and the other reactant accepts electrons the electrophile
Electrons reside in orbitals

48
Q

how do we form molecular orbitals

A

We should use filled-empty orbital overlap and the most favourable is between the nucleophile HOMO and the electrophile LUMO

49
Q

define HOMO

A

highest occupied molecular orbitals

50
Q

define LUMO

A

lowest unoccupied molecular orbitals

51
Q

what is the pKa of HI

A

-10

52
Q

what is the pKa of HCl

A

-7

53
Q

what is the pKa of H2SO4

A

-3

54
Q

what is the pKa of H3O+

A

-2

55
Q

what is the pKa of HSO4-

A

2

56
Q

what is the pKa of acetic acid

A

5

57
Q

what is the pKa of H2S

A

7

58
Q

what is the pKa of NH4+

A

9

59
Q

what is the pKa of a phenol

A

10

60
Q

what is the pKa of MeOH

A

15

61
Q

what is the pKa of H20

A

15

62
Q

what is the pKa of propanone

A

20

63
Q

what is the pKa of alkyne

A

25

64
Q

what is the pKa of NH3

A

33

65
Q

what is the pKa of CH4

A

48

66
Q

what factors affect pKa and acidity

A

1) Weak A-H bonds lead to stronger acid
2) Stability of the conjugate base A- due to the charge being on an electronegative atoms
3) Delocalization of the - charge makes A- more stable HA more acidic
4) Inductive effects can stabilize A- and increase the acidity of HA
5)Hybridisation can affect pKA - the more s character the more stable s

organic chemistry bsc (5 decks)

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