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Basic Concepts Flashcards

(72 cards)

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1
Q

Homologous Series

A

Organic compounds with the same functional group and general formula

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2
Q

Functional Group

A

A group of atoms in a molecule responsible for the characteristics of a compound

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3
Q

Nomenclature

A

Naming of organic compounds

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4
Q

Aromatic

A

Contain benzene ring

not aliphatic or alicyclic

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5
Q

Alicyclic

A

Aliphatic with non-aromatic ring

aliphatic and alicyclic

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6
Q

Aliphatic

A

Straight chains, branched chains or non-aromatic rings

only aliphatic

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7
Q

Saturated

A

Single carbon-carbon bonds only

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8
Q

Unsaturated

A

Can have carbon-carbon double bonds, triple bonds or aromatic groups

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9
Q

Structural Isomers

A

Same molecular formula, different structural formula

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10
Q

Stereoisomers

A

Same structural formula but different arrangement in space

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11
Q

Chain Isomers

A

Structural
Carbon skeleton can be arranged differently(straight chain, branched)
Similar chemical properties but different physical properties (like boiling point because of shape)

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12
Q

Positional Isomers

A

Structural
Functional group attached to a different carbon atom
Different physical properties, chemical might be different too

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13
Q

Functional Group Isomers

A

Structural
Same atoms can be arranged into different functional groups
Very different chemical and physical properties

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14
Q

Alkanes

A

Saturated hydrocarbons

General formula is CnH2n+2

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15
Q

What shape are alkanes around the carbon atom?

A

Tetrahedral (109.5°)

Four bonding electrons

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16
Q

What state(s) are alkanes at room temperature and pressure?

A

Short hydrocarbons are gases at rtp as they have low boiling points
Larger alkanes are liquids at rtp as they have high boiling points

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17
Q

What bonds are present in alkanes and what intermolecular forces are between the molecules?

A

Alkanes have covalent bonds within the molecule and induced dipole-dipole interactions between molecules

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18
Q

Do long or short chain hydrocarbons have higher boiling points and why?

A

The longer the carbon chain, the stronger the induced dipole-dipole interactions as there is more surface contact and there are more electrons to interact. This causes more energy to be needed to overcome the interactions so the boiling point rises

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19
Q

Do branched or straight chain isomers have lower boiling points?

A

Branched isomers have lower boiling points than their straight chain isomers as there is a smaller molecular surface area so induced dipole-dipole interactions are reduced

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20
Q

Why are alkanes unreactive?

A

They are non-polar

C-C and C-H bonds are strong covalent bonds

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21
Q

What is produced in
(1) complete
(2)incomplete
combustion?

A

(1) carbon dioxide and water

(2) carbon monoxide and water

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22
Q

Hydrocarbon

A

A compound existing of carbon and hydrogen atoms only

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23
Q

Mechanism

A

Shows the movement of electrons in a reaction

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24
Q

What does a
(1)double headed
(2) single headed
arrow represent

A

(1) movement of two electrons

(2) movement of one electron

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25
Free Radical
A species with an unpaired electron
26
Where and how are free radicals formed?
Formed in the upper atmosphere by UV light
27
Homolytic Fission
Bond is broken evenly and each atom receives an unpaired electron from the bonded pair. Two electrically charged radicals are formed
28
What are the four steps of the mechanism for free radical substitution
1) Overall reaction 2) Initiation 3) Propagation 4) Termination
29
How do you prevent polysubstitution in free radical substitution?
Use excess of the alkane
30
Alkenes
Unsaturated hydrocarbons | General formula is CnH2n (same as cycloalkanes)
31
What reactions do alkanes take part in?
Combustion and Halogenation (free radical substitution)
32
Heterolytic Fission
The bond breaks unevenly with one of the bonded atoms receiving both electrons from the bonded pair. A positively charged cation and a negatively charged anion are formed
33
What are photochemical reactions?
Reactions started by light. | Free radical substitution needs UV light to start.
34
What happens in the initiation reaction in free radical substitution
Free radicals are produced: Sunlight provides enough energy to break the halogen-halogen bond (photodissociation) The bond splits equally and each atom gets to keep one electron (homolytic fission). The atom becomes a highly reactive free radical because of it’s unpaired electron.
35
What happens in the propagation reactions in free radical substitution?
Free radicals are used up and created in a chain reaction: Free radical attacks the alkane molecule The new alkane free radical can attack another halogen molecule The new halogen free radical can attack another alkane molecule until all the halogen and alkane molecules are wiped out.
36
What happens in the termination reactions of free radical substitution?
Free radicals are mopped up: If two free radicals join together they make a stable molecule There are multiple possible termination reactions
37
What are the two problems with free radical substitution?
A mixture of products is formed so the desired product has to be separated from the unwanted by-products Free radical substitution can take place at any point along the carbon chain so a mixture of isomers can be formed
38
What reactions do alkenes undergo?
Addition reactions where a small molecule is added across the double bond to form one saturated product (pi bond breaks)
39
When do sigma bonds form?
When two s orbitals overlap in a straight line This gives the highest possible electron density between the two nuclei This is a single covalent bond
40
When do pi bonds form?
When two adjacent p orbitals overlap
41
Describe the bond enthalpy of sigma bonds
They have a high bond enthalpy (strongest type of covalent bond) This is because the high electron density between the nuclei means there’s a strong electrostatic attraction between the nuclei and the shared pair of electrons
42
Describe the bond enthalpy of pi bonds
They have a relatively low bond enthalpy as the electrostatic attraction between the nuclei and the shared pair or electrons is weaker This is because pi bonds are much weaker than sigmas bonds as the electron density is spread out above and below the nuclei
43
What does a pi bond do?
Fixes the C atoms in place so there is no free rotation around the carbon-carbon double bond Creates an area of electron density above and below the plane of the molecule
44
What shape do the electron pairs in the three sigma bonds produce?
They repel and produce a trogon always planar shape with a bond angle of 120°
45
Which type of bond is broken when alkenes take part in addition reactions?
The weaker pi bond (pi is more reactive than sigma) The electron rich carbon-carbon double bond is attacked by an electrophile
46
Which are more reactive alkanes or alkenes and why?
Alkenes are more reactive the carbon-carbon double bonds contain both a pi and a sigma bond The double bond contains four electrons so it has a high electron density and the pi bond is above and below the molecule so is likely to be attacked by electrophiles
47
Why can alkenes form stereoisomers?
There is restricted rotation around the carbon-carbon double bond This allows them to form stereoisomers
48
Describe an E isomer
The E isomer has the same groups positioned across the double bond (opposites)
49
Describe a Z isomer
The Z isomer has the same groups either above or below the double bond
50
How does the Cahn Ingold Prelog Priority Naming system work?
Atoms with a larger atomic number is given a higher priority e.g an ethyl group is higher priority than a methyl group
51
What are cis-trans isomers?
E/Z isomers with carbon atoms that have at least one group in common
52
What’s a cis isomer?
Same group on same side of double bond
53
What’s a trans isomer?
Same group on opposite sides of the double bond
54
Hydrogenation of alkenes
Reacts with hydrogen to form an alkane Nickel Catalyst 150°C
55
Halogenation of alkenes
Forms a dihaloalkane Electrophilic addition Bromine tests for double bond (orange to colourless)
56
Hydration of alkenes
``` Forms an alcohol Phosphoric acid High temp (300°C) Pressure (60-70 atm) Steam ```
57
Adding a hydrogen halide to a non symmetrical alkene
Produces a minor and major product
58
Why is a major product formed when adding a hydrogen halide to a non symmetrical alkene?
The intermediate is a stable secondary carbocation
59
What’s a major product from the addition of a hydrogen halide?
The one where hydrogen adds to the carbon with the most hydrogens already attached
60
Electrophile
A lone pair acceptor (to form a new covalent bond)
61
Addition polymers
Double bonds in alkenes break to form monomers which join together to form polymers
62
Problem with polymers
They’re very unreactive so aren’t biodegradable
63
Ways of getting rid of polymers and when are they used?
Landfill (when plastic is difficult to difficult to separate from other waste, not in sufficient quantities to make separation financially worthwhile, too difficult technically to recycle) Reused (some plastics can be recycled by melting and re-moulding them, some plastics can be cracked into monomers and these can be used as an organic feedstock to make more plastics out of the chemicals) Burned (this heat can be used to generate electricity, this process needs to be carefully controlled to reduce toxic gases waste gases from the combustion are passed through scrubbers which can neutralise gases allowing them to react with a base)
64
Describe biodegradable polymers
Biodegradable polymers decompose pretty quickly in certain conditions because organisms can digest them They can be made from renewable raw materials such as starch or oil fractions They are more expensive than non-biodegradable equivalents
65
What type of polymers have scientist started to develop and how do they decompose
Photodegradable polymers which decompose when exposed to light
66
What can polyethylene terephthalate (PET) be used for?
Fizzy drink bottles and oven ready meal trays
67
What can high-density polyethylene (HDPE) be used for?
Bottles for milk and washing up liquids
68
What can polyvinylchloride (PVC) be used for?
Food trays, clingfilm, bottles for squash, mineral water and shampoo
69
What can low-density polyethylene (LDPE) be used for?
Carrier bags and binliners
70
What can polypropylene (PP) be used for?
Margarine tubs, microwaveable meal trays
71
What can polystyrene (PS) be used for?
Yoghurt pots, phone meat or fish trays, hamburger boxes and egg cartons, vending cups, plastic cutlery, protective packaging for electronic goods and toys
72
What are some benefits of plastics?
Extreme versatility, lighter weight than competing materials, extreme durability, resistance to chemicals water and impact, good safety and hygiene properties for food packaging, excellent thermal and electrical installation properties, relatively inexpensive to produce

Organic Chemistry (3 decks)

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