4.2 Alcohols, haloalkanes and analysis Flashcards

1
Q

alkanes vs alcohols polarity and MP/BP

A

alkanes = non-polar
non-polar bonds present as electronegativity of H and C very similar

alcohols = polar
contain polar O-H bond (high difference in electronegativity)

alcohols = higher MP/BP, lower volatility
hydrogen bond between O-H groups as well as London dispersion forces
requires more heat energy to overcome

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2
Q

alkanes vs alcohols solubility

A

alkanes = insoluble
no interactions with water (polar solvent)

alcohols = soluble
can interact with water (polar solvent)
due to polar -OH group
decreases as hydrocarbon chain gets longer (influence of sole -Oh group gets smaller)

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3
Q

classifying alcohols

A

primary alcohol = -OH group attached to carbon attached to just one alkyl group

secondary alcohol = -OH group attached to carbon attached to 2 alkyl groups

tertiary alcohol = -OH group attached to carbon attached to 3 alkyl groups

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4
Q

combustion of alcohols

A

alcohol + oxygen -> carbon dioxide + water

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5
Q

oxidation of alcohols

A

primary and secondary alcohols only
need an oxidising agent [O]
orange solution turns green

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6
Q

oxidation of primary alcohols

A

primary alcohol -> aldehyde -> carboxylic acid

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7
Q

conditions to prepare aldehyde

A

primary alcohol
oxidising agent
gently heat
distill at the same time to prevent further reaction with oxidising agent

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8
Q

conditions to prepare carboxylic acid

A

heated strongly
under reflux (ensures all of alcohol is oxidised)
excess of oxidising agent (e.g. potassium dichromate)

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9
Q

oxidation of secondary alcohols

A

secondary alcohol -> ketone

heated under reflux

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10
Q

oxidation of tertiary alcohols

A

nothing happens

doesn’t undergo oxidation reactions

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11
Q

dehydration of alcohols

A

heated under reflux
in presence of acid catalyst (e.g. concentrated H2SO4/H3PO4
alcohol -[catalyst]-> alkene + water

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12
Q

dehydration definition

A

water molecule is removed from starting material

type of elimination reaction

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13
Q

substitution reaction of alcohols

A

alcohol heated under reflux with sulfuric acid and sodium halide
NaBr(s) + H2SO4(aq) -> NaHSO4(aq) + HBr(aq)
hydrogen halide reacts with alcohol to produce haloalkane
alcohol + hydrogen halide -> haloalkane + H2O

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14
Q

nucleophile definition

A

(group of) atom(s) attracted to an electron deficient centre to form a new covalent bond, electron pair donor

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15
Q

why haloalkanes can attract nucleophiles

A

carbon-halogen bond is polar
carbon atom is partially positive (halogen pulls covalent pair away from carbon)
the centre of the haloalkane is electron deficient

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16
Q

hydrolysis of haloalkane

A

add aqueous sodium hydroxide
nucleophile (OH-) approaches back of carbon atom (attached to halogen) opposite side to halogen
lone pair of electrons on hydroxide attracted and donated to partially positive carbon atom
new bond formed between oxygen and carbon atom
carbon-halogen bond breaks by heterolytic fission
forms alcohol and halide ion

17
Q

rate of hydrolysis and carbon-halogen bond strength

A

bond is weaker due to larger atomic radius of larger halide
lower bond enthalpy
the weaker the bond, the faster the hydrolysis (less energy required to break carbon-halogen bond)

18
Q

measuring rate of hydrolysis of primary haloalkanes

A

complete the reaction in presence of AgNO3(aq)
Ag+ ions react with halide ions produced to form precipitate
also in presence of ethanol solvent (allows water and haloalkane to mix to form single solution)
water bath

19
Q

why rate of reaction increases with haloalkanes with halogens lower down group 7

A

C-halogen bond becomes weaker with halogen lower down the group (larger atom, larger atomic radius, weaker attraction)

20
Q

use of organohalogens

A
general solvent
dry cleaning solvents
making polymers
flame retardants
refrigerants
21
Q

breakdown of ozone layer equations

A

CF2Cl2 → CF2Cl• + •Cl
•Cl + O3 → •ClO + O2
•ClO + O → •Cl + O2
overall equation: O3 + O -> 2O2

22
Q

formation of ozone

A

O2 -> 2O •

O2 + O • ⇌ O3

23
Q

what infra red does to covalent bonds

A

infra red causes covalent bonds to vibrate more and absorb energy

24
Q

factors of what frequency of infrared is absorbed by covalent bonds

A

length of covalent bond

mass of atoms on either side of bond

25
Q

why CO2, CH4 and H2O contribute to greenhouse effect

A

greenhouse gases

as C-H, O-H, C=O bonds absorb infrared radiation

26
Q

uses of IR spectroscopy

A

identify types of bonds present in unknown substances
monitor gases causing air pollution (e.g. CO and NO from car emissions)
breathalysers (measure ethanol in breath)

27
Q

fingerprint region

A

< 1500 cm^-1

contains unique peaks to find a particular molecule

28
Q

molecular ion definition

A

clear peak furthest to the right on mass spectrum
M^+
positive ion formed when a molecule loses an electron
its mass-to-charge ratio (m/z) = Mr of original molecule

29
Q

M + 1 peak

A

very small peak furthest to the right

due to larger isotope of carbon

30
Q

fragmentation definition

A

molecular ions break down into smaller pieces
forms fragment ions and free radicals
only fragment ions shown on mass spectrum as it has positive charge (radicals uncharged so not detected)

31
Q

oxidising agent foralcohols

A

acidified potassium/sodium dichromate

orange

32
Q

how nitrogen (II) oxide formed

A

combustion in engines
lightning
N2(g) + O2(g) -> 2NO(g)

33
Q

effect of nitrogen (II) oxide

A

acid rain

depletion of ozone layer

34
Q

nitrogen (II) oxide reactions for depleting ozone layer

A

•NO + O3 -> •NO2 + O2
•NO2 + O -> •NO + O2
net reaction: O3 + O -> 2O2

35
Q

how to purify organic liquid

A

separate aqueous layer from organic layer using separating funnel
dry using anhydrous salt (e.g. MgSO4, CaCl2)
redistillation

36
Q

esterification

A

when carboxylic acid and alcohol react to form ester + water

37
Q

esterification conditions

A

carboxylic acid group + hydroxyl group

concentrated sulfuric acid catalyst

38
Q

anhydrous salts examples

A

anhydrous:
CaCl2
MgSO4
CaSO4