Download Oxidation of Cyclohexanol to Cyclohexanone Notes

Reminder: These notes are meant to supplement, not replace, the laboratory manual.
Oxidation of Cyclohexanol to Cyclohexanone Notes
History and Application:
Oxidation reactions are incredibly important in the chemical and biochemical
sciences. Re-dox reactions are critical in the NADH-NAD+ couple with ATP which
provides energy to all cellsi. The same reaction we are doing today, the transformation
of cyclohexanol to cyclohexanone, is a commercially important process. In large
chemical plants a catalytic dehydrogenation process is used instead of bleach.
This process was used to make 1.1 trillion pounds of cyclohexanone in the US in 1995.ii
BASF is the largest North American manufacturer. They have a large plant just outside
Houston in Freeport Texas iii.
Most of the commercial cyclohexanone goes on to make an oxime (similar to a
later experiment in 2240), then it undergoes a rearrangement to form caprolactam which
is the starting material of Nylon 6.
Nylon-6 is one of the most widely used nylons in the world. This polymer goes into such
materials as nylon windbreakers, shoe strings, automobile components and automobile
tire cordiv.
Safety considerations for this experiment:
Cyclohexanol is an irritant. Avoid contact with skin, eyes, and clothing.
Glacial acetic acid is a dehydrating agent, an irritant, and corrosive which means
it causes burns. Handle it with care. Dispense it in a fume hood and avoid
contact with skin, eyes, and clothing.
Sodium hypochlorite solution emits chlorine gas, which is a respiratory and eye
irritant. Handle it with care, and dispense it in a fume hood.
Keep the reaction in the hood until all of the excess oxidizing agent has been
quenched with sodium thiosulfate.
1. Some terminology related to oxidation-reduction reactions:
Oxidation: In organic chemistry, increasing the oxygen content of an organic
molecule or decreasing its hydrogen content. Also creating a C-Z bond,
where Z is an element that is more electronegative than C such as N,
Halogen, etc. More generally, the process of removing electrons from a
substance.
Reduction: In organic chemistry, increasing the hydrogen content of an organic
molecule or decreasing its oxygen content. Also removing C-Z bonds.
More generally, the process of adding electrons to a substance.
Oxidizing agent: A substance that causes an oxidation by accepting one or more
electrons from a substrate. The oxidizing agent is reduced in the reaction.
Reducing agent: A substance that causes a reduction by donating one or more
electrons to a substrate. The reducing agent is oxidized in the reaction.
Exothermic reaction: A reaction in which energy is released from the system as
the reaction proceeds (–ΔH). Typically the reaction container heats up as
the reaction proceeds.
Endothermic reaction: A reaction in which energy is absorbed into the system as
the reaction proceeds (+ΔH). Typically the reaction container cools as the
reaction proceeds.
Solubility: The amount of one material that will dissolve in a liquid. Typically
solubility is discussed as grams of solute per 100 grams of solvent.
Something is soluble when 3 or more grams of it will dissolve in 100 g of a
solvent. v Insoluble is defined as less than 0.001g of material will dissolve
in 100 g of solvent. Slightly and sparingly soluble are in between these
levels.
2.
The balanced equation for the cyclohexanol oxidation with NaOCl is:
3. Reagents used in this experiment are:
Sodium hypochlorite: NaClO, Bleach solution. This is the oxidizing agent.
Acetic Acid, CH3CO2H. This further activates the sodium hypochlorite and forms
hypochlorous acid.
Sodium thiosulfate: Na2S2O3, is a reducing agent that reacts with and quenches
any remaining oxidizing agent. (This is similar to sodium sulfate with one
O replaced with a S, hence the name thiosulfate.)
Sodium Sulfate: Na2SO4, a drying agent. This removes the residual water from
the organic product.
Sodium bicarbonate or Sodium hydrogen carbonate: NaHCO 3. This is baking
soda. This is a weak base which neutralizes any remaining acetic acid.
Sodium Chloride, NaCl, table salt. This reduces the solubility of the organic
product in the aqueous phase thus increasing the amount of product
isolated.
Potassium iodide-starch test paper: indicates the presence of oxidizing agents by
the formation of a colored I2-starch complex, as shown here:
I
oxidation
I2
starch
blue-black starch-iodine
complex
iodide
molecular
ion
iodine
4. Ordinary household bleach is the source of the oxidizing agent, NaOCl. Most bleach
is prepared by the addition of chlorine gas to aqueous sodium hydroxide, as
shown here:
Cl2 + NaOH
NaOCl + H2O + NaCl
Standard bleach is an approximately 0.74 M solution of Sodium hypochlorite in water.
A new commercial concentrated bleach is 1.11 M. Make note of the type (regular or
concentrated) of bleach used during the experiment.
5. The acetic acid is a catalyst which transforms the sodium hypochlorite into
hyprochlorous acid, which is believed to be the active oxidizing agent. The acetic
acid is regenerated in this cycle. It does not react in a stoichiometric manner with
the reagents. Notice that oxidation state of chlorine in HOCl is +1, and the
deficiency of electrons in the valence shell of Cl+ makes it more reactive than
chloride ion.
6.
One accepted mechanismvi for this oxidation is shown below. The hypochlorite is
transformed into hypochlorous acid by the acetic acid.
The hypochlorite ion acts as the nucleophile. Subsequently the carbonyl is formed and
chloride leaves as a chloride ion Cl-:
Notice that the chlorine atom that is transferred to the substrate as part of
hypochlorite ion is in the +1 oxidation state. This same chlorine leaves as Cl-1.
The chlorine has undergone a reduction (from Cl+1 to Cl-1) by accepting two
electrons from cyclohexanol. The cyclohexanol is thereby oxidized to
cyclohexanone.
7. You are required to calculate a theoretical and a percent yield for this experiment. For
instructions and examples on how to do this, see the examples in the Percent
Yield Instruction sheet. Note that one of the starting materials was added as a
neat liquid, the other material was added as an aqueous solution. The density of
cyclohexanol is 0.962 g/mL. The molarity of the bleach is necessary for this
calculation.
8. Cyclohexanol and cyclohexanone have different solubilities in water. This allows the
product to be isolated without distillation. The roughly 2 mL of cyclohexanol is
soluble in the 30 mL of bleach (sodium hypochlorite in water) and acetic acid.
When bleach and cyclohexanol are mixed, one homogenous solution results.
Cyclohexanone has a lower solubility in this system than cyclohexanol. vii The
cyclohexanone which forms is slightly soluble in the water so it separates and
forms a new layer. Cyclohexanol is a hydrogen bond donor and a hydrogen bond
acceptor. Cyclohexanone is a hydrogen bond acceptor but is not a hydrogen
bond donor. Alcohol groups are more polar and more readily solubilized in water
than carbonyl groups. Hence cyclohexanol is more soluble in water than
cyclohexanone. Cyclohexanone has a density of 0.9478 g/mLviii which is lower
than the density of water. This causes the new layer to float on the surface of the
water. If cyclohexanone had a density greater than water this new layer would be
on the bottom of the flask. As the reaction proceeds, and cyclohexanone forms, a
new separate liquid layer should become apparent. If a new layer is not
observed, there is a problem and it indicates the reaction is not progressing.
9.
The product will be analyzed by Infrared Spectroscopy. A table summarizes the
more important IR active bonds found in starting cyclohexanol and product
cyclohexanone.
Cyclohexanol
Cyclohexanone
-O-H, ~ 3300cm-1
-x-
Sp3 C-H, 2800-3000cm-1
-x-C-O, ~1100cm-1
Sp3 C-H, 2800-3000cm-1
C=O, ~1720cm-1
Cyclohexanol
Cyclohexanone
ix
x
A disappearance of the –O-H absorbance, and the development of a strong C=O
absorbance in the IR of the cyclohexanone, is evidence for the successful synthesis of
cyclohexanone from cyclohexanol.
10.
Alcohols can form a variety of oxidation products depending up on their structure.
Some alcohols cannot be oxidized.
Primary alcohols are easily oxidized to carboxylic acids.
Primary alcohols can under special conditions (PCC) be oxidized only to
aldehydes. Typically primary alcohols when oxidized do not stop at aldehydes, but go
directly onto carboxylic acids.
Secondary alcohols are readily oxidized to ketones.
Tertiary alcohols are impervious to most oxidation.
Carboxylic acids and ketones are already highly oxidized and hence are impervious to
further oxidation.
References
i
Lehninger, Principles of Biochemistry, Worth, New York, 1982, p 472-475
Weissermel, K, Arpe, H.-J., Industrial Organic Chemistry, 3rd Completely Revised Edition, VCH, New York ,
1997
iii
BASF Optimizes Plant Performance, http://www.chemicalprocessing.com/articles/2003/299.html (September 27,
2011)
iv
Raghavendra R. Hegde, Atul Dahiya, M. G. Kamath, Nylon Fibers,
http://www.engr.utk.edu/mse/Textiles/Nylon%20fibers.htm (September 27, 2011)
v
Formulation in Pharmacy Practice.Appendix B
http://www.pharminfotech.co.nz/manual/Formulation/mixtures/pages/solubilities.html (September 27, 2011)
vi
Mohrig, J.R, Nienhuis, D.M, Linck, C.F., Van Zoeren, C. Fox, B. G, Mahaffy, P.G., Journal of Chemical
Education, 1985, 62, 519-521
vii
ICSC Cyclohexanone, http://www.inchem.org/documents/icsc/icsc/eics0425.htm (February 1, 2012) Chemical
book, Cyclohexanol, http://www.chemicalbook.com/ChemicalProductProperty_EN_CB7852772.htm (October 22,
2013)
viii
CRC Handbook of Chemistry and Physics, 65th, CRC Press, 1984, ppC-251
ii
http://sdbs.db.aist.go.jp/sdbs/cgibin/direct_frame_disp.cgi?sdbsno=581 (Accessed March 27,
2017)
ix
x
SBDS Database, http://sdbs.db.aist.go.jp/sdbs/cgi-
bin/direct_frame_disp.cgi?sdbsno=571
Revised March 27, 2017 S.L. Weaver
( Accessed March 27, 2017)