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Inorganic and Organic Chemistry > Organic Derivatives of Water > Flashcards

Organic Derivatives of Water Flashcards

1
Q

can be classified based on
the number of alkyl groups attached
to the carbon that contains the
hydroxyl group

A

alcohol

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2
Q

react with various oxidizing agents

A

primary and secondary alcohol

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3
Q

alcohols that are
unreactive, but most reactive to
nucleophilic substitution in Lucas
reagent

A

tertiary alcohol

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4
Q

quite reactive
to nucleophilic substitution

A

secondary alcohol

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5
Q

unreactive to
nucleophilic substitution

A

primary alcohol

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6
Q

only oxidized only by the
strongest oxidative agents

A

phenol

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7
Q

useful chemical
test for determining phenols from
alcohols

A

ferric chloride test

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8
Q

generally unreactive as it
has a very stable bond

A

ethers

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9
Q

organic derivatives of water include

A

hydroxyl
carbonyl
carboxyl
amine
ester
ether
thiol

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10
Q

materials and reagent needed for test of organic derivatives of water

A

1-butanol
2-butanol
2-methyl-2-propanol
cyclohexanol
ethylene glycol
Phenol
2-napthtol

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11
Q

Bayer’s reagent

A

KmnO4

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12
Q

Sodium dichromate

A

Na2Cr2O7

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13
Q

sulfuric acid

A

H2SO4

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14
Q

reagents needed

A

lucas reagent
Bayer’s reagent
1.00M Sodium dichromate
Sulfuric acid
Ferric Chloride
Distilled Water
1.00M NaOH
Iodine solution
sodium metal

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15
Q

equipment needed

A

Test tube
Pasteur pipettes

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16
Q

corrosive substances used

A

phenol
conc. sulfuric acid
sodium dichromate
NaOH

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17
Q

what to do
with corrosive substances

A

avoid skin contact

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18
Q

its vapor is toxic, so
avoid inhalation

A

diethyl ether

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19
Q

how many drops of the following are placed on separate dry test tube:

A

➢ 1-butanol
➢ 2-butanol
➢ 2-methyl-2-propanol
➢ Cyclohexanol
➢ Ethylene glycol
➢ Phenol
➢ 2-napthtol

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20
Q

procedures of solubility in water

A

2 mL of distilled water
shake and observe

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21
Q

procedures of acidic properties of alcohols (using sodium metal)

A

add a small piece of dry sodium metal
add 2 mL of each sample,
observe the rate of evolution of
hydrogen gas

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22
Q

test for solubility in NaOh

A

5 drops of NaOH
shake and observe solubility

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23
Q

Bayer’s oxidation

A

5 drops of Bayer’s reagent,
shake and observe

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24
Q

chromic acid oxidation

A

add 5 mL of Na2Cr2O7
2 drops of conc. H2SO4,
and add 2 drops of sample, observe.

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25
Q

lucas test

A

add 2mL of Lucas reagent,
add sample,
seal the test tube
shake and observe reaction

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26
Q

ferric chloride test

A

add small amount of sample
add 1 mL of deionized water
and add several drops of 2.5 M aqueous ferric chloride solution
shake and observe reaction.

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27
Q

compounds tested that are soluble in water

A

1-butanol
2-methyl-2propanol
ethylene glycol

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28
Q

what bonds do 1- butanol, 2-methyl-2-propanol and
ethylene glycol have with water
molecules

A

hydrogen bonds

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29
Q

where the water has a
slightly positive charge on this

A

hydrogen

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30
Q

where the water has a
slightly negative charge on these

A

oxygen

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31
Q

contains hydroxyl (-OH)
group, which is the functional group
responsible for its solubility in water,
the oxygen atom in the hydroxyl
group can form hydrogen bonds with
water molecules, allowing 1-butanol
to dissolve in water

A

1-butanol

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32
Q

contains a
hydroxyl group, enabling it to form
hydrogen bonds with water
molecules. The presence of a
branched alkyl group does not
significantly affect its solubility since
the hydroxyl group is the main
determining factor

A

2-methyl-2-propanol

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33
Q
  • is a diol, meaning it
    contains two hydroxyl groups. These
    hydroxyl groups can also form
    hydrogen bonds with water
    molecules, facilitating its solubility.
    Additionally, ethylene glycol has a
    small molecular size, further
    enhancing its solubility in water
A

ethylene glycol

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34
Q

not soluble in water
compared to other alcohols due to it
having a bulky cyclohexyl group attached to the hydroxyl (-OH)
functional group.

A

cyclohexanol

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35
Q

introduces a
significant nonpolar component to
the molecule, making it less
compatible with the polar nature of
water

A

cyclohexyl group

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36
Q

The nonpolar nature
of the cyclohexyl group makes this
more hydrophobic, or waterrepellent.

A

cyclohexanol

37
Q

qualities that can influence solubility and insolubility in water

A

presence of polar functional groups
size and shape
hydrophobicity

38
Q

results of acidic properties of alcohol using sodium metal

A

1-butanol - positive
2-butanol - positive
2-methyl-2-propanol - positive

39
Q

is an organic compound
with a hydroxyl group bound to an
aliphatic carbon atom

40
Q

this character of alcohol is
revealed through its reactions with
active metals.

41
Q

reason of acidity of
alcohol which decreases as the
electron density on the oxygen atom
increases

A

polarity of OH

42
Q

primary alcohol that is
more acidic than secondary and
tertiary alcoho

43
Q

exhibit a faster
reaction when combined with the
sodium metal and the evident release
of hydrogen gas

A

primary alcohol

44
Q

in this, there is a
decrease in acidity strength due to
the addition of alkyl group on carbon

A

tertiary alcohol

45
Q

result of chromic acid oxidation

A

1-butanol - positive
2-butanol - positive
2-methyl-2-propanol - negative

46
Q
  • To test the oxidation of alcohol, the
    following are mixed together for the chromic oxidation test:
A

sodium dichromate (NaCr2O7)
sulfuric acid (H2SO4)

47
Q

products on oxidation depend on the
type of alcohol:

A

primary
secondary
tertiary

48
Q

tested positive in the chromic acid oxidation
due to the disappearance of the redorange color of chromic acid and the formation of a blue-green color of the Cr (III) ion

A

1-butanol, 2-butanol,

49
Q

formed if a sample is positive in the chromic acid
oxidation

A

chromium (III) ion

50
Q

as this oxidizes the C2O7 ions in the solution are reduced to chromium (III)

51
Q

showed resistance to oxidation by
to the oxidizing agent

A

2-methyl-2-propanol

52
Q
  • demonstrated by
    the retention of the solution’s original
    color in chromic acid oxidation
A

negative reaction

53
Q

process where the
hydrogen atom in the -OH and the αhydrogen atom on the carbon atom to
which the -OH is attached are
removed to form a C=O bond

54
Q

does not contain an
α-hydrogen, the C=O cannot be
formed.

55
Q
  • formed via the oxidation of
    secondary alcohols
56
Q

formed via the oxidation of primary alcohols

57
Q

result of lucas test

A

1-butanol - negative
2-butanol - positive
2-methyl-2-propanol - positive

58
Q

its reactivity determines
whether they are classified as
primary, secondary, or tertiary. This
is due to the substitution of a
hydroxyl group produced from the
provided alcohol in place of the
chloride (Cl-) in the zinc-chloride
bond.

A

Lucas test

59
Q

after mixing the Lucas reagent with
this, a change of color from colorless
to slightly clear and white,
respectively, was seen.

A

2-butanol and 2-methyl-2-propanol

60
Q

remains colorless (no
reaction) in Lucas test

61
Q

the change of color of
the solution from clear to cloudy
suggests that this has been formed
and therefore indicates a positive
reaction for the Lucas test.

A

chloroalkane

62
Q
  • are the most
    reactive to nucleophilic substitution
    in the Lucas reagent
A

tertiary alcohol

63
Q

are moderately
reactive in Lucas reagent

A

secondary alcohol

64
Q

are unreactive in
Lucas reagent

A

primary alcohol

65
Q

its
mechanism starts when the OH
group of alcohol is protonated by
hydrochloric acid

A

nucleophilic substitution

66
Q

is a stronger
nucleophile than water (H₂O),

67
Q

formed in the
nucleophilic substitution in the Lucas
test

A

carbocation

68
Q

immediately attacks
the carbocation in the lucas test

A

chloride anion

69
Q

formed after the
chloride anion attacking the
carbocation

A

alkyl chloride

70
Q

is insoluble, making the
solution murky

A

alkyl chloride

71
Q

result of iodoform test

A

1-butanol - negative
2-butanol - positive
2-methyl-2-propanol - negative

72
Q

is used to
differentiate the ability of primary,
secondary, and tertiary alcohols to
undergo oxidation and form a yellow
precipitate called iodoform (CHI3)

A

iodoform test

73
Q

yellow precipitate that was
formed in the iodoform test

A

iodoform (CHI3)

74
Q

sample that has visible
yellow precipitate

75
Q

has no visible precipitate in the test

A

1-butanol and 2-methyl-2-propanol

76
Q

did not show iodoform because of them lacking a
methyl ketone group next to the carbonyl
group

77
Q

when iodine
(I2) was allowed to react with these
two compounds, it only produced a
colorless solution without any
precipitate.

78
Q

the solution
turning into a yellow color without
any visible precipitate in it and thus
inferring that tertiary alcohols does
not give the iodoform reaction

A

2-methyl-2-propanol

79
Q
  • has shown a positive
    result indicated by the cloudy yellow
    precipitate seen in the test tube.
    Unlike 1-butanol, this has a methyl
    ketone group, which is essential for
    the iodoform to occur.
80
Q

result of ferric chloride test

A

phenol - positive
2-napthol - negative

81
Q

are organic
substances that have an aromatic
ring and a hydroxyl group directly
connected

82
Q

due to the phenol having
this, phenol reacts with ferric
chloride to produce colored
compounds

A

enol group

83
Q

what the phenol group
interacts with to generate a colored
complex, which is violet in color

A

ferric ion

84
Q

is created in the
ferric chloride test, , which results in
various colored water soluble
complex compounds, phenols react with ferric chloride solution to yield
blue, violet, or green coloring.

A

ferric phenoxide

85
Q

this hue in ferric
chloride test suggest that it is
produced by ortho, meta, or paracresol with resorcinol

A

violet or blue

86
Q

gives green color

A

beta-naphthol

87
Q
  • gives pink color.
A

alpha-naphthol

88
Q

forms a
deep red colo

A

acetic acid and formic acid

89
Q

demonstrated a
negative reaction, as seen by its clear
yellowish hue, ferric chlorideoriginal color.

A

2-naphthol

Inorganic and Organic Chemistry (19 decks)

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