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Organic chemistry 1002 > Organic chemistry > Flashcards

Organic chemistry Flashcards

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1
Q

All organic compounds

A

contain carbon

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2
Q

examples of organic chemistry

A

Flavours, fragrances, fuels, gases, alcohol drinks, carbonated drinks, pharmaceutical industry etc

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3
Q

organic compounds may be formed from nature but

A

there are also a large number of synthetic compounds

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4
Q

Very first compound synthesised

A

Urea in 1828

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5
Q

Carbon forms covalent bonds

A

forms stable bonds with itself and other atoms in the form of chains and rings

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6
Q

Carbon has 4 valence electrons

A

neither a strong tendency to lose 4 electrons or gain 4 electrons `

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7
Q

Organic chemistry is generally

A

covalent bondings

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8
Q

Carbon is not always bonding to hydrogen

A

it can bond to carbon, nitrogen, oxygen, bromine, chlorine etc

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9
Q

there is always

A

4 bonds to carbon whether they are single or double etc but always 4

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10
Q

Single bond

A

single line (for skeletal structures)

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11
Q

when drawing skeletal structures do not draw

A

hydrogen bonds

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12
Q

Drawing skeletal structure

A
  1. count the number of carbons
  2. number them 1,2,3
    3.draw a zig-zag line which contains 3 points (number this also)
    4.do not draw in the hydrogens
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13
Q

Organic compounds are classified into 4 groups

A

Aliphatic
Alicyclic
Aromatic
Heterocyclic

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14
Q

Aliphatic

A

chains of atoms (skeletal structure zig zag)
not rings
saturated

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15
Q

Alicyclic

A

composed of rings of atoms

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16
Q

Aromatic compounds

A

derivatives of benzene

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17
Q

Heterocyclic

A

composed of rings of atoms that contain at least one atom in the ring the is not carbon example Pyridine

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18
Q

carbon can form

A

single (one line), double bonds (two lines), triple bonds (three lines)

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19
Q

in all organic compounds

A

the carbon atom must have a total of four covalent bonds regardless of how the bonds are arranged

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20
Q

since carbon must always have 4 bonds

A

it means it has a valency of 4

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21
Q

Saturated compounds

A

single bonds

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22
Q

Unsaturated compounds

A

double or triple bonds present

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23
Q

number of valency

A

hydrogen = 1 valency
carbon = 4 valency
nitrogen = 3 valency
oxygen and sulphur = 2 valency
Fluorine, Chlorine, Bromine, Iodine (halogens) = 1 valency

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24
Q

hydrocarbons

A

organic compounds that contain only the elements carbon and hydrogen

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25
The simplest hydrocarbons
Alkanes
26
Alkanes
1. Have the empirical formula CxHy 2. Can be arranged in straight chains or branched 3. Can write the structure formal of these in short hand 4. eg CH3CH2CH2CH3 -> CH3(CH2)2CH3 5. Can have compounds with the same molecular formal but different structural formula (their arrangement is different) 6. saturated hydrocarbons 7. Methane (CH4), Ethane (C2H6), Propane (C3H8), Butane (C4H10) 8. Molecular formula Cn H2n + 2 9. This series is a homologous series
27
Empirical formula
The ratio of atoms in a molecule It does not tell you how atoms are arranged
28
Molecular formula
tells us the exact number of each kind of atom in the molecule C5H12
29
Structural formula
Tells us the exact number of each kind of atom in the molecule and tells us how they are joined together (their conductivity)
30
Short-hand structural formula
CH3CH2CH2CH2CH3 or CH3(CH2)3CH3
31
Skeletal structure
zig zag lines
32
Homologous series
1. Can write a general molecular formula 2. The members of a homologous series have the same general formula and similar chemical properties 3. They show a graduation of physical properties due to an increase in their size
33
Structural isomers
Compounds with the same molecular formula but different structures or arrangements of atoms
34
STEM names
1 methane 2 ethane 3 propane 4 butane 5 pentane 6 hexane 7 heptane 8 octane 9 nonane 10 decane 11 undecane 12 dodecane
35
IUPAC system of nomenclature
1) Find the longest carbon chain (draw a line through it) 2) Number the carbon atoms in the longest carbon chain consecutively so as to give any side chains the lowest sum of numbers possible 3) Name from the longest chain (stem name) indicating the types and positions of side chains. The number location the particular side chain must appear directly in front of its name (side chain names go in front of stem name)
36
Rules for IUPAC system
1) if two side chains are identical, it is indicated by the prefix "di" 2) 2 groups = di, 3 = tri, 4 = tetra, 5 = penta, 6 = hexa 3)If two or more types of side chains are present they are listed alphabetically, prefixes di and tri are not considered when alphabetically 4) Commas are used between numbers, hyphens are used between numbers and names, no spaces are left
37
Halogen substitutes
Remove 'INE' from the end of the element and replace I with 'O' Fluoro - F Chloro - Cl Bromo - Br Iodo - I
38
Saturated hydrocarbons contain
rings of carbon atoms
39
General formula for the homologous series
CnH2n
40
Longhand vs shorthand structural formula
Longhand includes hydrogens and carbons H and C Shorthand is just lines
41
Cycloalkanes
Has the same stem/root name used for straight or branched alkanes As it is a ring, the prefix 'Cyclo' must be included When there is only one alkyl you don't need to number its position on the ring When there is more than one substituent, numbers are required to locate the position of each substituent on the ring If there is more than one they are labelled alphabetically
42
The physical properties of alkanes
properties that can be observed or measured without changing the composition of the substance include boiling and melting points, smell, colour, density, solubility etc
43
Alkanes solubility in water
Alkanes are insoluble in water as water molecules are polar and alkanes are non-polar
44
A covalent bond
a shared pair of electrons between two atoms
45
Non-polar covalent bond
The sharing of electrons (covalent) but shared evenly (Non-polar)
46
Polar covalent bond
The sharing of electrons (covalent) but shared unevenly (polar)
47
Uneven sharing is due to
large differences in electronegativity between two bonded atoms
48
Electronegativity
The ability of an atom to attract bonding electrons Increases from left to right across periodic table Increases from bottom to top on periodic table
49
The most electronegative element
Fluorine
50
Carbon and Hydrogen have a very small difference in electronegativity so
Their bond is Non-Polar (evenly shared)
51
Hydrogen and Fluorine have a very large difference in electronegativity so
Their bond is Polar (shared un-evenly)
52
Delta negative
electronegative and attracts the electrons in the bonds towards it, making it partially negative (not full charges)
53
Delta positive
slightly electropositive and the electrons are attracted away from it in the bonds, making it partially positive (not full charge)
54
Electronegativity values and bond type
Ionic -> difference is >2 Polar covalent difference is >0.5 Non-Polar covalent difference is <0.5
55
The polarity of a molecule depends on
Th presence of polar bonds and orientation of the polar bonds If we know the shape of a molecule and can identify the polar bonds present, we can determine if the molecule as a whole is Polar or Non-Polar
56
H2O shape
Polar
57
CO2 shape
Non-polar
58
A molecule is non-polar
If it does not have any polar covalent bonds
59
A molecule may be polar if
it has one or more polar covalent bonds
60
Even though a molecule may have polar covalent bonds
It does not mean that t is polar covalent e.g CO2
61
In water
the electronegative oxygen atom attracts th electrons in the O-H bond towards itself therefore the oxygen atom is slightly negative charge and the hydrogen atoms have a slightly positive charge Opposite charges in water are attracted to each other, hydrogen atoms are so small that they can get very close to the oxygen atoms of another water molecule. This allows water molecules to associate closely together
62
Hydrogen bonding
Th attractive interactions between water molecules
63
In alkanes
C-C and C-H bonds are not polarised and so we say that alkanes are Non-polar
64
To dissolve alkanes in water
we would have to mix the alkane molecules between the water molecules break the hydrogen bonds. This would require a lot of energy as hydrogen bonds are relatively strong intermolecular interaction
65
Non-polar C-C and C-H bonds cannot
form hydrogen bonds and so mixing alkanes with water is energetically unfavourable, this is why we get oil slicks
66
The Non-Polar properties of alkanes are useful to us in nature
Waxy coatings on leaves and fruit provide protection and the waxy coating you put on your car when you polish it protects it from the rain. These waxes are all alkanes
67
Physical properties of Alkanes
They are insoluble in water Methane, CH4, Natural gas Propane and Butane, C3H8 and C4H10 "patio" gas, safety lighters Octane, C8H18, petrol

Organic chemistry 1002 (4 decks)

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