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organic chemistry Flashcards

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1
Q

what is an atomic orbital

A

a region around the nucleus that can hold up to two electrons with opposite spins

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2
Q

what are the different types of orbital

A

s f d p

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3
Q

how many s orbitals are there in one sub level

A

1

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4
Q

how many p orbitals are there in one sub level

A

3

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5
Q

how many d orbitals are there in one sub level

A

5

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6
Q

how many f orbitals are there in one sub level

A

7

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7
Q

what is Aufbau’s principle

A

electrons enter at the lowest energy orbital available

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8
Q

what is Hund’s rule?

A

electrons prefer to occupy orbitals on their own and only pair up when no empty orbitals of the same energy level are available

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9
Q

explain how the electronic configuration for an ion would work

A

highest energy electrons are lost when and ion is formed
4s lost before 3d

  1. remove outer shell electrons first
  2. remove p-electrons, then s , then d
  3. remove paired electrons before unpaired electrons in the same sub lvl
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10
Q

what is an ionic bond?

A

electrostatic attraction between oppositely charged ions which are formed from the transfer of electrons

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11
Q

what is a covalent bond

A

strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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12
Q

what is a dative covalent bond?

A

a pair of electron shared between two atoms, one of which provides both electrons to the bond

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13
Q

what is a sigma bond

A

a bond resulting from the direct overlap of two orbitals along the internuclear axis or between the two bonding nuclei

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14
Q

what is a pi bond

A

a bond resulting from overlap of adjacent atomic orbitals above and below the two bonding nuclei

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15
Q

define electronegativity

A

relative ability of an atom to attract the two electrons in a covalent bond

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16
Q

what are the factors which affect electronegativity

A
  • nuclear charge
  • atomic radi
  • shielding
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17
Q

how does nuclear charge impact electronegativity

A

more protons=stronger attraction between nucleus and bonding pair of electronsh

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18
Q

how does atomic radi impact electronegativity

A

closer to nucleus=stronger attraction between nucleus and bonding pair of electrons

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19
Q

how does shielding impact electronegativity

A

less shells of electrons between nucleus and electrons=less shielding=stronger attraction between nucleus and bonding pair of electrons

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20
Q

how does electronegativity change down a group and why

A

it decreases

atomic radi increases=more shielding=less attraction between nucleus and bonding pair electrons

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21
Q

how does electronegativity change across a period and why

A

it increases

atomic radi decreases=increased nuclear charge = stronger attraction between nucleus and bonding pair of electrons

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22
Q

describe non polar covalent bonds

A
  • two atom in a covalent bond have the same electronegativity (less than 0.4 difference in electronegativity)
  • two electrons are shared equally as both atoms attract with a similar power therefore the electrons are midway in the bond
  • eg cl2
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23
Q

describe polar covalent bonds

A
  • two atoms in a covalent bond have different electronegativity

-covalent bond where the two electrons are not shared equally (one has greater attraction)

-the more electronegative atom will have a greater share and become slightly negative, the other, slightly positive

  • eg hcl
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24
Q

what is a bond dipole moment

A

measure of the strength and direction of the polarity in the bond

the bigger the difference in electronegativity, the bigger the bond dipole moment

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25
describe electron pair repulsion
bonding pairs -involved in boning and repel e/o equally lone pairs -not involved in bonding - repel e/o more than bonding pairs (more electron dense) - each lone pair reduces the bond angle by 2.5 degrees
26
what is meant by 'shrinking the octet'
in the outer shell neither beryllium nor boron have enough electrons to form an octet - unpaired electrons will pair up and so the element will not achieve an octet
27
what is meant by the 'expansion of octet'
phosphorus can have 5 bonds - another expansion: sulphur
28
what are london forces
electrons in a molecule are in a state of constant motion - the distribution of electrons will not be symmetrical there is likely to be a slight surplus on one of the atoms - this is known as temporary dipole (lasts for a short time as electrons constantly move)
29
what is an induced dipole
electrons on adjacent molecules are repelled by the negative parts of the dipole and attracted to the positive part and move accordingly ---> this results in an attraction between the 2 molecules (london forces)
30
which two factors affect the strength of london forces
- number of electrons in the molecule - surface are of the molecule
31
what is a permanent dipole
- polar molecules have polar bonds - in polar molecules the dipoles cancel out
32
explain how hydrogen's lack of electron density allows it to form dipole bonds
as hydrogen has almost no electron density it is able to approach electronegative atoms on adjacent molecules very closely and form strong intermolecular dipole bonds
33
how do you draw hydrogen bonds
1. relevant dipoles 2. dashed hydrogen bond between the lone pair and hydrogen 3. h bond and covalent bond have an angle of 180
34
describe the arrangement of water molecules in ice
- water molecules arrange themselves in order to maximise the amount hydrogen bonding between the molecules - the results in a very open hexagonal structure with large spaces within crystals, this accounts for its low density
35
describe the arrangement of water molecules as ice melts
the structure collapses into the open spaces , this causes water to occupy less space and thus becoming more dense
36
describe how the surface area of molecules can impact the strength of london forces
- the larger the surface area of a molecule, the more contact it will have with adjacent molecules - the more contact, the greater the ability to induce a dipole in an adjacent molecule and the greater the london force and therefore greater melting and boiling points
37
describe how the number of electrons in a molecule can impact the strength london forces
- the greater the number of electrons in a molecule, the greater the likelihood of a distortion - the greater the frequency and magnitude of the temporary dipoles - the London Forces between the molecules are stronger and the melting and boiling points are larger
38
how can you decide if a bond is polar or non polar
if the difference in electronegativity is: - 0.4 or less = non polar - 0.4 - 1.8 = polar
39
what is a polar molecule
- has polar bonds - the dipoles from the polar bond do not cancel out
40
what is dipole-dipole bonding
an attraction between a permanent dipole on one molecule and permanent dipole on another molecule
41
define first ionisation energy
the energy required to remove one electron from each atom in one mole of gaseous atoms to produce one mole of gaseous 1+ ions
42
how does ionisation energy differ across a period
it increases because NC increases, AR decreases and shielding stays the same , increase attraction and so increased energy to remove
43
why does the ionisation energy of aluminium dip
group 2 = s block, group 3= p block , this means group 2 is closer to the nucleus than group 3, therefore 3 requires less energy to remove
44
Why does the ionisation energy of sulphur dip?
group 5 electrons lose from orbital with 2 electrons, rest lose from orbital with 1 and due to electron-electron repulsion, group 5 is easier to lose
45
explain the difference in boiling points from silicon to argon
si- macromolecular, giant covalent structure, covalent bonds, lots of energy to break bonds ar- monoatomic, very weak london forces, noble gas
46
name the shape and angle of the molecule with 2 electron pairs
linear, 180
47
name the shape and angle of the molecule with 3 bonding pairs and 0 lone pairs
trigonal planar, 120
48
name the shape and angle of the molecule with 4 bonding pairs and 0 lone pairs
tetrahedral, 109.5
49
name the shape and angle of the molecule with 5 bonding pairs and 0 lone pairs
trigonal bipyramidal, 120 and 90
50
name the shape and angle of the molecule with 6 bonding pairs and 0 lone pairs
octahedral, 90
51
name the shape and angle of the molecule with 2 bonding pairs and 1 lone pairs
bent v shape, 118
52
name the shape and angle of the molecule with 3 bonding pairs and 1 lone pairs
trigonal pyramidal, 107
53
name the shape and angle of the molecule with 2 bonding pairs and 2 lone pairs
bent v shape, 104.5
54
name the shape and angle of the molecule with 4 bonding pairs and 1 lone pair
trigonal pyramidal, 119 and 89
55
name the shape and angle of the molecule with 3 bonding pairs and 2 lone pairs
trigonal planar, 120 or 89
56
name the shape and angle of the molecule with 5 bonding pairs and 1 lone pair
square pyramidal, 89
57
What is the mechanism needed to go from an alkene to an alkane
electrophillic addition
58
what is the condition required to go from alkene to alkane
H2 or Ni catalyst
59
what is the mechanism to go from alkane to haloalkane
freeradical substitution
60
what are the conditions needed to go from alkane to haloalkane
- uv light - halogen
61
whta is the mechanisms to go from an alkene to a haloalkane
halogenation alkenes decolourise bromine water
62
what are the conditions required for halogenation
hydrogen halide
63
what is the mechanism to go from an alkene to an alcohol
hydration
64
what are the conditions required for hydration
water (steam), alkene reacted with steam H3PO4 catalyst
65
what is the reaction to form an alkene from an alcohol
dehydration
66
what are the condition for dehydration
● Heated under reflux ● Requires sulfuric or phosphoric acid
67
What is the mechanism to form an aldehyde from a primary alcohol
distillation
68
what are the conditions of a distillation
- acidified potassium dichromate or sulfuric acid
69
What is the mechanism to form an carboxylic acid from a primary alcohol
- reflux
70
what are the conditions required for refulx
strong heat excess K2Cr2O7 or sulfuric acid
71
what does a secondary alcohol form
ketone
72
what is the mechanism to form a ketone
REFLUX
73
what is the mechanism to form nitriles from haloalkanes
NUCLEOPHILIC SUBSTITUTION OF HALOALKANES (reflux)
74
what is the mechanism to form an amine from a haloalkane
heat with ammonia in ethanol

chemistry (2 decks)

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