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organic chemistry Flashcards

1
Q

define homologous series

A

series of organic compounds having the same functional group

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2
Q

define structural isomer

A

same molecular formula but different structural formula

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3
Q

define functional group

A

part of an organic molecule that is largely responsible for the molecules chemical properties

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4
Q

alcohol functional group/prefix/suffix

A

-OH/hydroxy-/-ol

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5
Q

haloalkane functional group/prefix

A

-Cl,Br,I/chloro,bromo,iodo

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6
Q

aldehyde functional group/suffix

A

-CHO/al

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7
Q

ketone functional group/suffix

A

-C(CO)C-/one

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8
Q

carboxylic acid functional group/suffix

A

-COOH/oic acid

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9
Q

ester functional group/suffix

A

-COOC-/oate

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10
Q

acyl chloride functional group/suffix

A

-COCl/oyl chloride

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11
Q

amine functional group/prefix/suffix

A

-NH2/amino/amine

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12
Q

nitrile functional group/suffix

A

-CN/nitrile

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13
Q

How is a sigma bond formed

A

Carbon has 4 electrons in its outer shell. S orbital is filled. 2 of the p orbitals are half-filled and one is completely empty so they overlap

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14
Q

How is a pi bond formed

A

There is 1 electron in each carbon not involved, this electron is in the p orbital. The pi bond is formed by the sideways overlap of the p orbitals. Each carbon contributes one electron to the electron pair. Weaker bond

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15
Q

can pi bonds rotate

A

no because of the double carbon to carbon bond, would otherwise break.

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16
Q

How do you get E/Z isomerism

A

2 different groups attached to the carbons. A double carbon bond. Occurs due to restricted rotation

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17
Q

z / cis isomers

A

non H groups on the same side of the double bond

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18
Q

E/trans isomers

A

non H groups on different sides of the double bond

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19
Q

define stereoisomers

A

same structural formula but a different arrangement of the atoms in space

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20
Q

what is optical isomerism

A

can occur in a wide range of compounds including alkanes with no functional group

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21
Q

order the elements with increasing priority

A

H, C, N, O, Cl, Br

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22
Q

pattern with boiling points as the length of the chain increases

A

Longer the chain, the higher the boiling point because there is more surface contact so there are stronger London forces so more energy is needed to overcome these forces.

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23
Q

pattern with boiling points as the branching of the chain increases

A

The more branching, the lower the boiling point because there are fewer points of contact and the molecules are not as close together so there are weaker London forces meaning less energy is needed to overcome the forces.

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24
Q

why are alkanes unreactive

A

the sigma bonds are strong, C-C is non polar, and there is a small difference in electronegativity between C and H

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25
why is carbon monoxide deadly
combines with haemoglobin to form carboxyhaemoglobin which prevent haemoglobin from transporting oxygen.
26
what are addition reactions
2 reactants join together to make one product
27
what are substitution reactions
an atom or group of atoms are replaced by a different atom or group of atoms
28
what are elimination reactions
removal of a small molecule from a large one
29
what is heterolytic fission
where 1 atom takes both electrons from the covalent bond
30
what is homolytic fission
where each atom take one electron from the covalent bond
31
what conditions are needed for free radical substitution
UV light
32
what are the different stages of free radical substitution
initiation, propagation and termination
33
what is made in initiation give an example
molecule --- radical+radical | e.g. Cl2 -- Cl. + Cl.
34
what is made in propagation give an example
radical + molecule ---- radical + molecule Cl. + CH4 ---- Ch3. + HCl CH3. + Cl2 ---- CH3Cl + Cl.
35
what is made in termination give an example
radical + radical ----- molecule CH3. + CH3. ---- C2H6 CH3. + Cl. ---- CH3Cl Cl. + Cl. ----- Cl2
36
Why are alkenes more reactive
pi bond has a lower enthalpy than a sigma bond so it is broken more easily
37
reactants/conditions for hydrogenation
hydrogen/nickel + heat
38
reactants/conditions for halogenation
any halogen/room temperature - used as a test for saturation
39
reactants/conditions for hydrogenated halides
gaseous or concentrated solution of a hydrogenated halide - can form 2 products
40
reactants/conditions for hydration
steam/phosphoric acid - can form 2 products
41
Describe electrophilic addition
the double bond in an alkene represents a region of high electron density because of the presence of a pi electron. The high density attracts electrophiles which accepts an electron pair
42
What is a nucleophile
electron pair donors
43
what is an electrophile
electron pair acceptors
44
what is markownikoff's rule
addition of a hydrogen halide etc to an unsymmetrical alkene forms the major product through the most stable carbocation
45
order of carbocation stability starting with least stable
primary (2 H), secondary (1 H), tertiary (0 H)
46
Primary alcohol
carbon with OH is attached to one alkyl group
47
Secondary alcohol
carbon with OH is attached to two alkyl group
48
Tertiary alcohol
carbon with OH is attached to three alkyl group
49
during oxidation what does a primary alcohol produce
aldehyde then carboxylic acid
50
during oxidation what does a secondary alcohol produce
ketone
51
during oxidation what does a tertiary alcohol produce
no reaction
52
what is used to oxidize alcohols
potassium dichromate (K2Cr2O7) and sulfuric acid (H2SO4)
53
what color change is observed during oxidation
orange to green
54
How can you make sure an aldehyde is produced from oxidation of a primary alcohol
distillation - aldehydes have a lower boiling points than alcohols, the aldehyde evaporates before it can react with anymore oxidizing agent
55
Describe heating under reflux
allows you to boil a liquid. The vapor condenses in a vertical condenser and returns to the reaction vessel so no substance is lost.
56
dehydration of alcohols
H3PO4 or H2SO4 as a catalyst. Water is also produced. Heated under reflux
57
substitution of alcohols. Give example equation
heated under reflux with H2SO4 and sodium halide. e.g. C3H7OH + NaBr + H2SO4 ---- C3H7Br + NaHSO4 +H2O.
58
examples of nucleophiles
:OH-, H2O: and :NH3
59
describe nucleophilic substitution hydrolysis
nucleophile approaches carbon atoms attached to halogen on the opposite side of the molecule from the halogen atom. Direction minimizes repulsion between nucleophile and negative halogen. Lone pair of electrons on OH- is attracted and donated to positive carbon. Carbon - halogen bond breaks via heterolytic fission. Alcohol plus halide ion formed. Heated under reflux and aqueous sodium hydroxide is used.
60
cl. reacting with ozone
1. Cl. + O3 ----- ClO. + O2 2. ClO. + O ---- Cl. + O2 3. O3 + O ---- 2O2
61
what is the ozone molecule
O3
62
breakdown of ozone NO.
1. NO. + O3 ---- NO2+O2 2. NO2. + O ----- NO. + O2 3. O3+ O ---- 2O2
63
when is NO. formed
During lightening strikes and a result of aircraft travel in the stratosphere
64
CFC properties
stable due to string carbon to halogen bond. UV light provides sufficient energy to break carbon halogen bond. As C-Cl bond is lowest enthalpy a CL. is formed
65
properties of aerosols
non-toxic, Low BP, low reactivity
66
ozone formation formula
O2 + O ---- O3
67
consequences of ozone breakdown
skin cancer, cataracts, low crop yield, famine as high food prices, more sunburn
68
what is a sigma bond
overlap of orbitals between atoms
69
what is optical isomerism
same structural formula but are non-superimposable mirror images of each other
70
Describe how to purify an organic product
1. Ensure that the tap of the separating funnel is closed. 2. Pour the mixture of liquids into the separating funnel, place a stopper in the top of the funnel, and invert to mix the contents. 3. Allow the layers to settle. 4. Add some water to see which layer increases in volume - this is the aqueous layer. 5. Place a conical flask under the separating funnel, remove the stopper and open the tap until the whole of the lower level has left the funnel. 6. Place a second conical flask under the separating funnel to collect the other layer. 7. You will now have one conical flask containing the aqueous layer and the other containing the organic layer.
71
How can you remove acid impurities when purifying an organic product
Add aqueous sodium carbonate to the separating funnel and invert the mixture. Carbon dioxide is produced and the tap needs to be slowly opened, holding the stoppered separating funnel upside down, to release any gas pressure that may have been built up. Aqueous sodium carbonate layer is removed and organic layer is washed with water before running both layers off into separate conical flasks.
72
How do you dry an organic product
1. Add organic liquid to a conical flask 2. using a spatula, add some of the drying agent (e.g.CaSO4) to the liquid and gently swirl the contents to mix together. 3. Place a stopper on the flask to prevent the mixture from evaporating away. Leave for about 10 minutes. 4. If the solid has all stuck together in a lump, there is still some water present. Add more drying agent until some solid it's dispersed in the solution as a fine powder. 5. Decant the liquid from the solid into another flask. If the liquid is dry it should be clear.
73
Why is a tertiary carbocation more stable than a primary carbocation
Because there are more alkyl groups around the carbon. Alkyl groups electron releasing/positive inductive effect.
74
Reflux:
The continual boiling and condensing of a reaction mixture back into the original container to ensure that the reaction takes place without the contents of the flask boiling dry.

Chemistry (24 decks)

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