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LC Chemistry > Organic Chemistry > Flashcards

Organic Chemistry Flashcards

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1
Q

Functional group

A

An atom or group of atoms which is responsible for the characteristic properties of a series of organic compounds

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2
Q

Substitute reaction

A

A chemical reaction in which an atom or group of atoms in a molecule is replaced by another atom or group of atoms

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3
Q

Mechanism for substitute reaction

A

free radical substitution
initiation (homolytic fission)
propagation
termination

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4
Q

Addition reaction

A
  • A chemical reaction in which two substances react together forming a single substance
  • Only happens to unsaturated compounds
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5
Q

Mechanism for addition reaction

A

ionic addition

apparoach/polarisation/heterolytic fission/carbonium ion/ product formation

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6
Q

Polymers

A

long chain molecules made by joining together many small molecules called monomers

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7
Q

Elimination reaction

A

one in which a small molecule is removed from a larger molecule to leave a double bond in the larger molecule

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8
Q

Organic synthesis

A

The process of making organic compounds from simpler starting materials

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9
Q

Chloroalkane

A

a compound in which one or more of the hydrogen atoms in an alkane molecule have been replaced by chlorine atoms

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10
Q

Example of a chloroalkane

A

chloroform (CHCL₃)

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11
Q

Use of chloroalkanes

A
  • As solvents for removing oil + grease marks from machinery

- In dry cleaning of clothes - remove substances without harming the fabric

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12
Q

Examples of chloroalkanes

A

Monochloromethane
Dichloromethan
Trichloromethane (chloroform)
Tetrachloromethane

1-Chloropropane
1,2-dichloropropane
1,1,1-trichloroethane

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13
Q

Chloroalkane notes

A

have same basic tetrahedral shape as corresponding alkanes

not a hydrocarbon - contains Cl

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14
Q

Physical properties of chloroalkanes

A
  • Solubility: do not dissolve in water, readily dissolve with non-polar solvents eg. cyclohexane, methylbenzene
  • Physical state: liquids at room temp
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15
Q

Polar

A

dissolves in water

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16
Q

Non-polar

A

needs an organic solvent

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17
Q

Alcohols functional group

A

-OH group (the hydroxyl/hydroxide group)

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18
Q

General formula of alcohols

A

Cₙ H₂ₙ₊₁ OH

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19
Q

Naming alcohols

A

change the -e ending to -ol

eg. methane –> methanol

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20
Q

Examples of alcohols

A 
methanol (methyl alcohol)
ethanol (ethy alcohol)
propan-1-ol
propan-2-ol
butan-1-ol
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21
Q

Classifications of alcohols

A

primary
secondary
tertiary

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22
Q

Primary alcohol

A

one where carbon atom joined to the -OH group is attached to only one other carbon atom

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23
Q

Secondary alcohol

A

One where the carbon atom joined to the -OH group is attached to two other carbon atoms

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24
Q

Tertiary alcohol

A

one where the carbon atom joined to the -OH group is attached to three other carbon atoms

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25
Q

Ethanol

A

ethanol for alcoholic drinks is produced by a process known as fermentation

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26
Q

Glucose fermenting equation

A

C₆H₁₂O₆ –(yeast)–> 2C₂O₅OH ₊ 2CO₂

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27
Q

Methanol property

A

particularly toxic

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28
Q

Use of methanol

A

added to industrial alcohol to prevent people from drinking it (used as a denaturing agent)

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29
Q

methylated spirits

A

mixture which consists of approx. 90% ethanol and 10% methanol

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30
Q

ethanol’s effects on the body

A
  1. Relax muscles, loosening inhibitions
  2. V. toxic chemical if taken in large quantities (ethanol poisoning)
  3. Excess - cause unconsciousness, vomitting. Can lead to death (drowning in vomit) + liver failure
  4. Depresses activity of the central nervous system - shows reaction time, makes us less vigilant, impairs judgement
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31
Q

uses of ethanol

A
  • Used in alcoholic drinks
  • Main use as a fuel
  • Used as a solvent
  • Used in perfumes, after-shave lotions, deodorants, hair sprays
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32
Q

physical properties of alcohols

A
  • Boiling points: alcohols have higher boiling points than corresponding alkanes (effect of hydrogen bonding)
  • Solubility in water: methanol, ethanol, propan-1-ol are completely miscible w/ water (infinitely soluble). Solubility decreases w/ length of carbon chain.

Higher alcohols ave poor solubility in water + readily dissolve in solvents eg. cyclohexane

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33
Q

miscible

A

mix with

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34
Q

absolute alcohol

A

pure ethanol

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35
Q

aldehydes functional groups

A

contain the -CHO functional group

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36
Q

aldehydes general formula

A

Cₙ H₂ₙ₊₁ CHO

37
Q

aldehydes naming

A

named from parent alkane by changing -e ending to -al

eg. methane becomes methanal

38
Q

placement of functional group in aldehydes

A

adlehyde functional group must always occur at end of the carbon chain

39
Q

carbonyl group

A
  • the carbon connected to the O by double bond is called the carbonyl group
  • The carbonyl group + atoms it is bonded to all lie in one plane w/ all bond angles of 120 degrees
40
Q

examples of aldehydes

A

methanal (CHCHO) - formaldehyde
ethanal (CH3CHO) - acetaldehyde
propnanal (C2H5CHO) - propioaldehyde
butanal (2 isomers)

41
Q

physical properties of aldehydes

A

-Boling points:
•Methanal - gas at room temp
•Ethanal - v. volatile liquid

-Solubility - solubility in water decreases w/ length of carbon chain. All aldehydes are quite soluble in organic solvents. Lower members of aldehyde - v soluble in water

42
Q

volatile

A

Unstable

43
Q

use of aldehydes

A
  • Methanal - used for preserving biological specimens + as embalming fluid
  • Main use of benzaldehyde is as a flavouring agent in cooking
44
Q

benzaldehye

A

benz + aldehyde

45
Q

ketones functional groups

A

> C=O functional group (Attached to two alkyl groups)

46
Q

ketones general formula

A

RCOR’

47
Q

Difference between aldehydes + ketones

A

Diff. in structural formula is the replacement of the hydrogen atoms in aldehydes by an alkyl group, R’

48
Q

examples of ketones

A

propanone (Acetone)

butanone (methylethyl ketone)

49
Q

alkyl

A

w/o one hydrogen atom

50
Q

naming ketones

A

change final -e of parent alkane to -one

eg. propane - propanone

51
Q

example of a ketone + its use

A

propanone

used as an organic solvent, eg. nail varnish remover

52
Q

physical properties of ketones

A

-Have higher boiling points than corresponding alkanes

-Solubility: Lower members - v soluble in water, eg. propanone + butanone completely miscible w/ water
C5+ not soluble in water

53
Q

uses of propanone + butanone

A

widely used as solvents in industry - cna act as solvents for both polar + non-polar substances

54
Q

carboxylic acids functional groups

A

Contain the carboxyl group, -COOH

55
Q

carboxylic acids general gormula for aliphatic monocarboxylic acids

A

Cₙ H₂ₙ₊₁COOH or RCOOH

R is an alkyl group

56
Q

carboxylic acids naming

A

named from parent alkane by changing -e ending to

-oic acid

57
Q

carboxylic acids examples

A

methanoic acid
Ethanoic acid
propanoic acid

58
Q

methanoic acid

A

found in stings of nettles + ants

59
Q

ethanoic acid

A

used to make cellulose acetate, used in varnishes, lacquers, rayon (a type of textile)

60
Q

propanoic acid

A

inhibits growth of mould + used as food preservative

61
Q

benzoic acid

A

used as food preservative, in antiseptic medicines, as a fungicide for treating skin problems (eg. ringworm + athelet’s foot)

62
Q

carboxylic acids properties

A

have characteristic odours

63
Q

carboxylic acids physical properties

A
  • Ethanoic acid is liquid at room temp, solid at 17°C
  • Methanoic, ethanoic, propanoic, butanoic acid are all liquids at room temp + completely soluble in water
  • Solubility: in water, decreases w/ increasing length of the carbon chain
  • Higher members more soluble in organic solvents eg. cyclohexane
64
Q

glacial acetic acid

A

pure ethanoic acid is often referred to as glacial acetic acid as the solid material looks like ice

65
Q

Esters functional group

A

-COO- group

66
Q

Esters general formula

A

RCOOR’

67
Q

Esters & carboxylic acids

A

Esters may be considereds as being derives from carboxylic acids by replacing te H of the -OH group by an alkyl group

68
Q

Condensation reaction

A

A chemical reaction in which two molecules combine to form a larger molecule w/ loss of a smaller molecule such as water

69
Q

Examples of Esters

A

Methyl1methanoate
Methyethanoate
Ethylmethanoate

70
Q

Esters physical properties

A
  • Lower members are volatile liquids w/ pleasant fruit smells
  • Low boiling points
  • Solubility: lower members - soluble in water, solubility in water decreases as length of carbon chain increases. Soluble in organic solvents.
71
Q

Esters uses

A
  • commonly used in fruit flavourings + in manufacture of perfumes and cosmetics
  • used as solvents for varnishes + spray paints + also as solvent in some perfumes
72
Q

polyester

A

consist of millions of ester molecules linked together

73
Q

bonding in benzene/aromatic compounds

A

contain a benzene ring structure in their molecules

74
Q

properties in benzene

A

all carbon-carbon bonds in benzene ring are identical + are intermediate in length between a double + single bond

75
Q

Sigma bonds in benzene

A
  • Carbon atom has four electrons in its outer shell,
  • Of these four, each carbon atom uses three of them to form sigma (σ) bonds by head-on overlap if atomic orbitals
  • Two of these single, sigma bonds are formed between each carbon atom + two adjacent carbon atoms
  • Third sigma bond formed w/ an atom of hydrogen
76
Q

bond angles in benzene

A

120 degrees

77
Q

orbitals

A
  • Remaining electron in outer energy level of each carbon atom is in a p orbital
  • These six singly-occupied p orbitals overlap sideways to form two doughtnut-shaped electron clouds
  • Pi bond is more correctly referred to as a pi-bonding system
78
Q

delocalised electrons

A

6 electrons in the pi bond do not belong to any particular atom. These are described as six delocalised electrons.
Delocalisation of electrons explains why alternating double + single bonds do not exist in benzene. Give extra stability.

79
Q

Summary of important points about chemical bonding in benzene molecule

A
  • All c-c bonds are identical, ie. c-c single covalent bonds containing a shared pair of electrons. May be described as sigma bonds formed by head-on overlap of singly-occupied atomic orbitals
  • All c-c bonds intermediate in length between c-c single bonds + c=c double bonds
  • 6 singly-occupied p atomic orbitals overlap sideways to form a pi bonding system containing six delocalised electrons
  • C-H bonds are all identical single convalent bonds containing a shared pair of electrons. These bonds may also be described as sigma bonds formed by head-on overlap of singly-occupied atomic orbitals
80
Q

properties of benzene

A
  • Benzene is a planar molecule
  • Non-polar
  • Carcinogenic
81
Q

uses of benzene

A

Many aromatic compounds are not dangerous despite benzene being carcinogenic. They form basis of many pharmaceutical compounds, dyes, detergents, insectides, herbicides, disinfectants

82
Q

Uses of benzene in insecicides + hebicides

A

Napthalene (found in mothballs)

83
Q

Uses of benzene in Dyes

A

2-amino-4-nitrophenol (yellow hair colourant)

84
Q

Uses of benzene in narcotics

A

Cocaine

Heroin

85
Q

Uses of benzene in food flavourings

A

Vanillin (vanilla)

86
Q

Organic Natural Products - examples

A 
Benzaldehyde (in almonds)
Caffein (In tea + coffee)
Nicotine (in tobacco)
Opium (in poppies)
Limonene (in orange peel)
Penicillin (in bread mould)
87
Q

test to show ethene is unsaturated

A
  • add a few drops of bromine water to ethene in a test tube + shake well
  • will turn brown Br water colourless
88
Q

organic synthesis table

A

learn off

LC Chemistry (26 decks)

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