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Chemistry > Organic Chemistry 1 > Flashcards

Organic Chemistry 1 Flashcards

1
Q

hydrocarbon

A

compound of hydrogen and carbon only

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2
Q

A homologous series has

A
  • compounds with the same general formula
  • members which have similar chemical properties
  • members which show a trend in physical properties
  • members which differ from each other by a CH2 unit
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3
Q

Alkene

A

name ends in -ene

CnH2n

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4
Q

Alcohol

A

name ends in -ol

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5
Q

Aldehyde

A

name ends in -al

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6
Q

Ketone

A

name ends in -one

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7
Q

Carboxylic acid

A

ends in -oic acid

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8
Q

Amine

A

name ends in -amine

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9
Q

Nitrile

A

ends in -nitrile

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10
Q

if molecule contains alcohol and carboxyic acid eg.

A

name starts with hydroxyl- for alcohol and ends with -oic acid

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11
Q

stereoisomerism

A

illustrated by E/Z isomerism

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12
Q

structural isomerism

A

same molecular formula, different structural, displayed, skeletal formula.

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13
Q

eg. of saturated hydrocarbons

A

alkanes and cycloalkanes

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14
Q

alkane fuels are obtained from

A

the fractional distillation, cracking

and reforming of crude oil

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15
Q

reforming

A

the processing of straight-chain hydrocarbons into

branched-chain alkanes and cyclic hydrocarbons for efficient combustion

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16
Q

pollutants formed during the combustion of alkane fuels

A

carbon monoxide, oxides of nitrogen and sulfur,

carbon particulates and unburned hydrocarbons

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17
Q

carbon monoxide problems

A

toxic, poisonous in that it combines almost irreversibly with haemoglobin so preventing it carrying oxygen around the body

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18
Q

sulfur oxides and nitrogen oxides problems

A
  • Fuels often contain some sulfur and nitrogen
  • when combusted, sulfur dioxide and oxides of nitrogen
  • then reacts with water vapour in the atmostphere forming acid rain of sulfuric acid and nirtic acid
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19
Q

use of a catalytic converter to solve problems of pollutants

A

catalyst provides the surface enabling oxidisers such as oxides of nitrogen to react with reductants such as unburnt hydrocarbons to form less harmful carbon dioxide and nitrogen

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20
Q

use of alternative fuels

A
  • biodiesel and alcohols formed from renewable resources
  • biofuel is formed by plants that take up carbon dioxide from the air to make the plant material which is then converted into fuel, and when the fuel is burnt, it simply puts back into the air the carbon dioxide it originally removed, so is carbon-neutral
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21
Q

radical

A
  • is a species with an unpaired electron and is represented in mechanisms by a single dot
  • is formed by homolytic fission of a covalent bond and results in the formation of radicals
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22
Q

limitations of radical substitutions of alkanes

A

further substitution reactions and the

formation of a mixture of products

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23
Q

eg. of unsaturated hydrocarbons

A

alkenes and cycloalkenes

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24
Q

electrophile

A

a species attracted to an area of negative charge and is an electron pair acceptor

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25
double bond is made up of
sigma and pi bond
26
heterolytic bond fission of a covalent bond
Electron pair split unevenly, both electrons in the bonding pair going to one atom, formation of ions
27
test for alkenes
bromine water is added to an unsaturated compound, an addition reaction occurs fairly rapidly and the bromine water changes from orange to colourless
28
addition polymerisation
alkenes form polymers
29
waste polymers can be separated into specific types of polymer for
recycling incineration to release energy use as a feedstock for cracking
30
more sustainable use of materials
Remove any waste gases produced during incineration | Make plastics which are biodegradable, such as polyethenol
31
chemists can contribute to the more sustainable use of materials
Materials and energy used to make them Materials and energy used to maintain them Materials, space and energy used to dispose of them
32
halogenoalkanes can be classified into
primary secondary and tertiary
33
E-Z isomerism
Zay are on Ze Zame Zide | look at the RFM to see the most significant
34
homolytic fission
Electron bonding pair split evenly, one electron going to each of the bonded atoms forming radicals
35
carbocation stability
primary=>tertiary the stability increases
36
nucleophile
a species attracted towards a region of positive charge and is an electron pair donor
37
alkene + H => alkane conditions
presence of a nickel catalyst
38
Alkene => alcohols conditions
steam, in the presence of an acid catalyst
39
alkene => diol conditions
potassium manganate(VII), in acid conditions, to oxidise the double bond
40
hydrolysis of halogenoalkanes conditions
RX + H2O → ROH + H+ + X- Ag+(aq) + X-(aq) → AgX(s) precipitate aqueous silver nitrate in ethanol, acts as an emulsifier allowing water and halo to mix and collide to react
41
two reasons why halogenoalkanes are reactive
The electronegativity of the Halogen causing the carbon partially positive and making it susceptible to nucleophilic attack The halogen is a good leaving group; being readily broken away from the carbon forming a halide ion
42
halogenoalkanes => alcohols reagent type of reaction nucleophile
C3H7Br + OH- → C3H7OH + Br - Aqueous potassium hydroxide Nucleophilic substitution Hydroxide ion
43
halogenoalkanes => alkene reagent type of reaction nucleophile
RCH2CH2Br + OH- > RCH=CH2 + Br- + H2 Ethanolic potassium hydroxide Elimination Hydroxide ion
44
halogenoalkanes => Nitrile reagent type of reaction nucleophile
RX + CN- → RCN + X- Potassium cyanide Nucleophilic substitution Cyanide ion
45
halogenoalkanes => amine reagent type of reaction nucleophile
C2H5Cl + 2NH3 → C2H5NH2 + NH4Cl Ammonia Nucleophilic substitution Ammonia molecule
46
experimental observations used to compare the relative rates of hydrolysis of primary, secondary and tertiary halogenoalkanes
The quicker the precipate forms the faster the rate tertiary halide produces a precipitate almost instantly secondary and primary take longer keeping the halogen constant
47
experimental observations used to compare the relative rates of hydrolysis of chloro-, bromo-, and iodoalkanes
``` A primary iodo compound produces a precipitate quite quickly and the bromo then chloro keeping the class of halogeno constant ```
48
trend in reactivity of primary, secondary and tertiary halogenoalkanes
increasing reactivity as u go from primary to tertiary | Rate of SN1 is faster so tertiary
49
the trend in reactivity of chloro-, bromo-, and iodoalkanes
reactivity decreases down the group | bond enthalpy is lowest on C-I so it is the weakest, most easily broken so most reactive
50
uses of halogenoalkanes
fire retardants and refrigerants as they are unreactive and non-combustible
51
alcohol classification
primary etc. number of carbon groups attached to the carbon with the OH group
52
alcohol => chloroalkanes
PCl5
53
alcohol => bromoalkanes
50% concentrated sulfuric acid and potassium bromide
54
alcohol => iodoalkanes
red phosphorus and iodine
55
oxidising primary alcohols
potassium dichromate(VI) in dilute sulfuric acid firstly form aldehyde distilled off as it forms further oxidation forms carboxylic acid
56
alcohol => alkenes by elimination
concentrated phosphoric acid
57
oxidising secondary alcohols
``` potassium dichromate(VI) in dilute sulfuric acid forms ketones heated under reflux ```
58
heating under reflux
vertical condenser | keeps vapours trapped but allows oxygen in so mixture can be heated for a long time
59
extraction with a solvent in a separating funnel
organic on the top layer-non polar | aqueous on the bottom- polar and ions
60
distillation
bp range 47-51=purity | anti-bumping granules heat distributed evenly
61
drying with an anhydrous salt
cloudy wet>cloudy dry anhydrous salt:Cacl2 CaSO4 NaSO4 filter/decant
62
boiling temperature determination
water bath | measure temp when it starts to boil and then when its gone
63
Why can’t tertiary alcohols oxidise using potassium dichromate
No hydrogen atoms attached to adjacent carbon atoms
64
Colour change of oxidation of alcohols
Orange (Cr2O7-2) to green (Cr+3)

Chemistry (19 decks)

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