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Chemistry > Organic Chemistry 1 > Flashcards

Organic Chemistry 1 Flashcards

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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
Q

double bond is made up of

A

sigma and pi bond

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26
Q

heterolytic bond fission of a covalent bond

A

Electron pair split unevenly, both electrons in the bonding pair going to one atom, formation of ions

27
Q

test for alkenes

A

bromine water is added to an unsaturated compound, an addition reaction occurs fairly rapidly and the bromine water changes from orange to colourless

28
Q

addition polymerisation

A

alkenes form polymers

29
Q

waste polymers can be separated into specific types of polymer for

A

recycling
incineration to release energy
use as a feedstock for cracking

30
Q

more sustainable use of materials

A

Remove any waste gases produced during incineration

Make plastics which are biodegradable, such as polyethenol

31
Q

chemists can contribute to the more sustainable use of materials

A

Materials and energy used to make them
Materials and energy used to maintain them
Materials, space and energy used to dispose of them

32
Q

halogenoalkanes can be classified into

A

primary secondary and tertiary

33
Q

E-Z isomerism

A

Zay are on Ze Zame Zide

look at the RFM to see the most significant

34
Q

homolytic fission

A

Electron bonding pair split evenly, one electron going to each of the bonded atoms forming radicals

35
Q

carbocation stability

A

primary=>tertiary the stability increases

36
Q

nucleophile

A

a species attracted towards a region of positive charge and is an electron pair donor

37
Q

alkene + H => alkane conditions

A

presence of a nickel catalyst

38
Q

Alkene => alcohols conditions

A

steam, in the presence of an acid catalyst

39
Q

alkene => diol conditions

A

potassium manganate(VII), in acid conditions, to oxidise the double bond

40
Q

hydrolysis of halogenoalkanes conditions

A

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
Q

two reasons why halogenoalkanes are reactive

A

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
Q

halogenoalkanes => alcohols
reagent
type of reaction
nucleophile

A

C3H7Br + OH- → C3H7OH + Br -
Aqueous potassium hydroxide
Nucleophilic substitution
Hydroxide ion

43
Q

halogenoalkanes => alkene
reagent
type of reaction
nucleophile

A

RCH2CH2Br + OH- > RCH=CH2 + Br- + H2
Ethanolic potassium hydroxide
Elimination
Hydroxide ion

44
Q

halogenoalkanes => Nitrile
reagent
type of reaction
nucleophile

A

RX + CN- → RCN + X-
Potassium cyanide
Nucleophilic substitution
Cyanide ion

45
Q

halogenoalkanes => amine
reagent
type of reaction
nucleophile

A

C2H5Cl + 2NH3 → C2H5NH2 + NH4Cl
Ammonia
Nucleophilic substitution
Ammonia molecule

46
Q

experimental observations used to compare the relative rates of hydrolysis of primary, secondary and tertiary halogenoalkanes

A

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
Q

experimental observations used to compare the relative rates of hydrolysis of chloro-, bromo-, and iodoalkanes

A 
A primary iodo compound produces a precipitate quite quickly and the bromo then chloro
keeping the class of halogeno constant
48
Q

trend in reactivity of primary, secondary and tertiary halogenoalkanes

A

increasing reactivity as u go from primary to tertiary

Rate of SN1 is faster so tertiary

49
Q

the trend in reactivity of chloro-, bromo-, and iodoalkanes

A

reactivity decreases down the group

bond enthalpy is lowest on C-I so it is the weakest, most easily broken so most reactive

50
Q

uses of halogenoalkanes

A

fire retardants and refrigerants as they are unreactive and non-combustible

51
Q

alcohol classification

A

primary etc. number of carbon groups attached to the carbon with the OH group

52
Q

alcohol => chloroalkanes

A

PCl5

53
Q

alcohol => bromoalkanes

A

50% concentrated sulfuric acid and potassium bromide

54
Q

alcohol => iodoalkanes

A

red phosphorus and iodine

55
Q

oxidising primary alcohols

A

potassium dichromate(VI) in dilute sulfuric acid
firstly form aldehyde distilled off as it forms
further oxidation forms carboxylic acid

56
Q

alcohol => alkenes by elimination

A

concentrated phosphoric acid

57
Q

oxidising secondary alcohols

A 
potassium dichromate(VI) in dilute sulfuric acid
forms ketones heated under reflux
58
Q

heating under reflux

A

vertical condenser

keeps vapours trapped but allows oxygen in so mixture can be heated for a long time

59
Q

extraction with a solvent in a separating funnel

A

organic on the top layer-non polar

aqueous on the bottom- polar and ions

60
Q

distillation

A

bp range 47-51=purity

anti-bumping granules heat distributed evenly

61
Q

drying with an anhydrous salt

A

cloudy wet>cloudy dry
anhydrous salt:Cacl2 CaSO4 NaSO4
filter/decant

62
Q

boiling temperature determination

A

water bath

measure temp when it starts to boil and then when its gone

63
Q

Why can’t tertiary alcohols oxidise using potassium dichromate

A

No hydrogen atoms attached to adjacent carbon atoms

64
Q

Colour change of oxidation of alcohols

A

Orange (Cr2O7-2) to green (Cr+3)

Chemistry (19 decks)

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