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1
Solubility in
Water
2
Reaction with
Sodium
The Hydroxyl Group: Reactions
of Alcohols and Phenols
Alcohols and phenols are organic analogs of water, HOH, in which one
hydrogen is replaced by an aliphatic (R—OH) group in the alcohols and by
an aromatic (Ar—OH) group in the phenols. The following tests and experi-
ments illustrate some properties and reactions of alcohols and phenols.
Alcohols and phenols, like water, form strong intermolecular hydrogen bonds:
R R A
\ \ A
O— H----0O—H and O—H----O--H
The lewer-molecular-weight alcohols can readily replace water molecules in
the hydrogen-bonded network of water.
aA R H
\ \ \
O— H-~--O—H--~-0-H
This hydrogen bonding accounts for he solubility of many alcohols in water.
In this part of this experiment, you will test the solubility of several alcohols
in water.
Procedure In separate test mbes, place 0.5 mL of each of the following
alcohcls: ethanol, 1-butanol, 2-methyl-2-propanol, i-hexanol, cyclohexanol,
and ethylene glycol. Add 2 mL of water to each test tube, mix, and observe.
Record your results for each alcohol on the report sheet.as very soluble,
moderately soluble, slightly soluble, or insoluble.
Just as with water, the hydrogen atom of the hydroxyl group in alcohols and
phenols can be replaced by sodium.
2 HOH + 2Na‘
An
<— 2a OH + Hat
N 27” sedis bydrozide
\
2 ROH +2Nae ——>%e onatoR + Hot
ae todium alkoxide
The evolution of hydrogett can be taken‘as evidence for the presence of a
hydroxy! group, or other acidic group, in the ‘molecule. Metal alkoxides (like
metal hydroxides) are strong bases. :
CAUTION
: 3
The Lucas Test
In this expeciment you will observe the relative reactivity of several alcohola
toward * godium,
Be extremely careful when handling sodium, Be sire that all your test
tubes are clean and dry.* :
Sodium: redets violently with water. Never dispose of sodium in the sink.
When you havé\completed all your observations, add sufficient methanol
to each tube to react completely with any wireacted sodium metal. Only
when all the sodiurh, has reacted may y; a discard the contents of each
tube in a waste bottle) provided by we instructor.
Procedure In separate, dry test tubes, place 2 ml of each of the following
alcchols: methanol, 1- -butanal\g- -betanol, and 2-methyl-2-propanol In a fifth
test tube, place 2 mL of hexane Xs a comparison control.
Using a tweezers (do net hb ‘dle* ‘sodium metal with your fingers), add one
smau piece (a sphere 2 mm ir’ diametéxor a cube 2 mm on an edge) of sodium
metal to each tube, and note, the result In Same cases, it may be necessary to heat
. the mube over a steam bedi i initiate reactién. Record your results,
To the methanol m5 /onty, after all the sGdjum has dissolved, add a few
drops of phenolphiheléi in indicator solution (this indicator is colorless in acid,
pink in bese). Recor your result.
Waste Dispose” When you have finished the tests, ae ely add 1 mL of
methanol to’ each tube to destroy the excess sodium. Wien nO more so-
dium can be observed, pour the contents of the tubes into a waste bottle for
organic solvents, provided by your instructor.
Alcohols are classified as primary, secondary, or tertiary, depending on
whether the hydroxyl-bearing carbon is bound to one, two, or three carbon
atoms. When treated with a particular reagent, alcohols may differ in the
rates at which they react, or indeed even in the type of product obtained,
depending on the class to which they belong. Tests that distinguish among
the three classes can be useful in determining the structure of an unknown
alcohol.
H H R
n—b-ox n—b-on n—b—on
x b A
pemary secondary terdary
The Lucas reagent is a solution of zinc chloride in concemtrated hydro-
chloric acid. The Lucas test is based on the different rates at which primary,
secondary, and tertiary zlcohcls are converted to chlorides with this reagent.
ZaQh
ROH +HQ ————} R~-C!l + H—-OH
The lower alcohols ali dissolve in the reagent to form oxonium salts.
"AU xcobols to be tetted should be previeudly dried over molecnlar siever,
a
The Hydroxyl Group:
Solubility in
Water
Reaction with
Sodium
The Lucas Test
MAME SECTION
Report
Compound Swructure
Ethanol
1-Butanol
2-Methy!-2-propanol
1-Hexanol
Cyclohexmol
Ethylene glycol
Compound Structure
Methanol
1-Butanol
2-Butanol
2-Methyl-2-proparol
Hexane control
Addition of phenolphthzlein to the methanol solution:
DATE
Solubility in warer
Observation
Compound Structure
1-Butanol
2-Butanol
Cyclohexanol
2-Methyl-2-prepanol
Consol
Tine for Reaction
Esters Ethanol:
Isopentyl! alcohot
Compound Structure
Acidity of YHetsset
Phenols Phenol
p-Chlorophenol
Compound
Reaction of Phenol
Phenols and
Enols with Resorcinol
Ferric Chloride 2,4-Pentanedione
2-Propanol
Control
Solubilizy
Water
NaOH Solution
Stracture
Questions 1. What general conclusions can you draw about the solubility of alcohols in
‘water on the basis of your results in Sec. 17
2. Which is less soluble in water, 1-pentanol or i-heptanoi?
Explain.
3. Write an <quation for the reaction of methanol with sodium.
4, What experimental evidence did you observe for the products of the reac-
tion of methanol with sodium?
5. What would you expect to happen if sodium methoxide were added to
water? Write the equation.
6. Write am equation for the reaction of 2-butanol with the Lucas reagent
7. What would be the result of treating each of the follawing compounds with
the Lucas reagent? Explain.
a. 2-Methyl-1-propanol
b. Cyclopentanol
e 1-Methylcyclopentanal
9. Describe the odor of the product derived from mixing isopentyl alcohol
and acetic acid (Sec. 5), and write the equation for its formation.