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CORE ORGANIC CHEMISTRY Flashcards

1
Q

Nomenclature

A

set of rules outlining how organic compounds should be named and their formula

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2
Q

the 10 prefixes and the alkane example

A

1.meth- (methane)
2.Eth-(ethane)

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3
Q

alkane suffix

A

-ane

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4
Q

alkene suffix

A

-ene

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5
Q

alcohol suffix

A

-ol

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6
Q

carboxylic acid suffix

A

-oic acid

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7
Q

ketone suffix

A

-one

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8
Q

aldehyde suffic

A

-al

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9
Q

ester suffix

A

-oate

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10
Q

Hydrocarbons

A

compounds containing only hydrogen and carbon atoms only

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11
Q

Halogen functional group prefix

A

-fluorine-fluoro
chlorine-chloro
Bromine-Bromo
iodine-iodo

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12
Q

side chains that are branched are

A

represented by a prefix(methy,Ethyl)

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13
Q

General IUPAC rules (4)

A
  1. functional groups and side chains are given with the corresponding number
    2.numbers are separated by commas
  2. numbers and words separated by hyphens
  3. go in alphabetical order for functional groups
  4. when counting carbpns go on either the left or right side making sure you have the smallest number as possible
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14
Q

saturated meaning

A

a hydrocarbon containing single bonds . fully saturated with hydrogens. (methane )

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15
Q

Unsaturated meaning

A

a hydrocarbon containing carbon to carbon multiple bonds (propene,but-2-ene)

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16
Q

general formula

A

simplest algebraic formula of the homologous series

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17
Q

Displayed formula meaning

A

relative positioning of atoms and the bonds between them

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18
Q

skeletal formula

A

simplified organic formula of just a carbon skeleton or functional group. the corners count for carbons

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19
Q

cyclic compound/benzene ring

A

a compound with one or more series of atoms in an elemnt in a ring

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20
Q

Homologous series meaning

A

a series of roganic compounds witty the same functional group . all members follow a general formula

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21
Q

functional group is

A

responsible for the charactersitics and reactions of a compound .they differ by CH2

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22
Q

Aliphatic

A

carbon atoms are joined to each other in unbranched(straight,branched or non-aromatic rings

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23
Q

Aromatic

A

an organic copound conaining a benzene ring . contains delocalised electrons .

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24
Q

Alicyclic

A

aliphatic compound arranged in non-aromatic rings

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25
alkanes
single carbon to carbon bonds
26
alkenes
double carbon to carbon bonds
27
alkynes
contains triple carbon to carbon bonds
28
Alcohol structure
-OH functional group
29
Haloalkanes structure
-halogen and alkane bonded with one another -Cl -Br -i -F
30
Aldehyde structure
-CHO
31
Ketone
-C(CO)C
32
Carboxylic acid structure
-COOH
33
Ester structure
-COOC-
34
Acyl chloride
-COCL
35
Amine structure
-NH2
36
Nitrite structure
-CN
37
Structural isomers
Molecules with the same molecular formula but different arrangement of atoms
38
The three types of structural isomers
1. Chain isomers 2. Position isomers 3.functional group isomers
39
Chain isomers
Have the same molecular formula but a different arrangement of atoms
40
position isomers
Have the same functional group in a different position . Propan-1-ol and proan-2-ol
41
Functional group isomers
Have the same molecular formula but the molecules have a different functional group . Hexene and cyclohexane
42
Reaction mechanisms
Are a series of steps that represent the overall reaction by showing the breaking and forming of bonds
43
Heterolytic fission
A covalent bond breaks one bonding atom and receives the pair of electrons from a bonding pair leads to the formation of a positive and negative ion . Unequal .
44
Homolytic fission
When a covalent bond breaks each bonding atom receives one electron forming two radicals . It is equal splitting of electron pair
45
Radicals
Unstable molecules ions or atoms with unpaired electrons . Key condition=UV light
46
Addition reactions
Start with two reactants and end up with 1 product .
47
Substitution reactions
One functional group is replaced by a different functional group
48
Polymerisation reaction
A reaction in which many small molecules of repeating units to form a polymer
49
Elimination reaction
A small molecule is removed from a larger molecule . Start with 1 end up with 2
50
Alkanes
Saturated hydrocarbons containing single carbon=Caron bonds
51
Sigma bonds
Are the single bonds held in alkanes
52
Each carbon atom in an alkane
Is surrounded by 4 electron pairs in four sigma bonds
53
All alkanes are a type of shape …
Tetrahedral . 109.5’
54
Cycloalkanes contain the general formula
CnH2n
55
Less branched gives
More surface contact
56
The larger the molecule the more
London forces and the ore energy is needed to overcome these London forces
57
Alkanes must be separated by
Fractional distillation
58
Steps of fractional distillation
1. Mixture of hydrocarbons is vaporised 2.the vapours rise.cool and condense at different boiling points 3. Column is hotter at the bottom than at the top
59
Short chain hydrocarbons rise to
The top as they have lower boiling points
60
London forces in organic chains are affected by
Chain length and branching
61
Branching of alkane chains gives
Weaker London forces as they are less compact
62
Higher boiling point gives stronger
Intermolecular forces
63
An increase in chain length gives
An increase in surface contact and therefore an increase in London forces
64
Alkanes do not react with common reagents due to
-Strong sigma bonds betwee C-C And C-H -C-C bonds are non polar
65
Complete combustion of alkanes
plentiful supply of oxygen
66
Incomplete combustion
Forms carbon monoxide which is dangerous as it bids to haemoglobin in our blood
67
Free radical substitution involves 3 steps
1. Initiation 2.propagation 3. Termination
68
Free radical substitution is caused by
Homocysteine fission as two free radicals are formed
69
1. Initiation stage
Radicals are produced by using visible ignition or uv light . Bond breaks equally producing two radicals .
70
2. Propagation stage
1.Halogen radical reacts with alkane molecule to make an alkyl radical 2.alkyl radical reacts with halogen to form . Possibly chloromethane and CL* radical 3. The halogen can now start its chain reaction . Product must correlate with the reactant .
71
3. Termination
Propagation may stop when 2 radicals collide . When two radicals collide the radicals are removed stopping the reaction all stable
72
Freee radical
A reactive species which has unpaired electrons
73
Limitations of radical substitution
-we get multiple substitution I’d,tri,tetra -these all need to be separated -to stop all this substitution we need to add an excess of alkanes
74
Alkenes
Unsaturated hydrocarbons part if a homologous series with the general formula cnH2n
75
Pi-bonds
Sideways overlap of p orbitals from each carbon atom
76
Sigma bonds
Overlap of orbitals directly between bonding atoms
77
What is the shape of Alkenes and explain this
Trigonal planar due to -there are three regions of high electron density around each carbon atom -the three regions repel each other meaning bond angle is 120.
78
Stereoisomers
Compounds with the same structural formula but different arrangement in space .
79
E/Z isomerism
A type of stereoisomerism that is restricted by rotation around a double bond
80
Cis-trans isomerism
A type of E/Z isomerism in which two f the same groups are attached to the same carbon
81
CIP rules
Rules that are used to decide whether a Hydrocarbon is E or Z
82
steps to CIP rules
1. Number the carbons it’s double bonds 2. Calculate the highest atomic number of the first lemon directly bonded . HIGHEST ATOMIC NUMBER = HIGHEST PRIORITY
83
E means
Different groups .EOPPISITE
84
Z means
The same . ZAME

CHEMISTRY (9 decks)

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