Basic concepts on redox reactions.. Get full control over these reactions by paying full attention. All reagents are included.

1. NAME;
MuAMMADJamil
ROLLNO;
16309
ASSIGNMENTTOPIC;
OXIDIZINGAGENTS
SUBMITTEDTO
AMJADHUSSAIN
SEMESTER
6th

2. Oxidation:
i. Oxidation is a loss of electrons
ii. gain of oxygen
iii. loss of electrons
A loses electrons B gains electrons
Electrons are moving fromA to B. so, A being oxidized and B is reduced
Oxidizing Agents definition
Those species which has capibilty to oxidize the other
chemical reagent or get away electrons. An oxidizing agent
ejects electrons from other atom .in Oxidation reduction
reaction oxidizing agents are very important.
Oxidizing agents accept electrons and reduced .They are also
called electrons gainers this is due to they have high oxidation
agents.

3. Oxidizing agents have low oxidation state because they
oxidize other substance and reduced itself.
Oxidizing agents are also called electron acceptor. Because they accept
electrons
Atom transfer reagent
Most commonly said that oxygen atom is trasfered by
oxidizing agents therefore mostly it also said oxygenation
reagent .
 Perchlorate
 Osmium tetraoxide
 Chromate
Dangerous material definition
Oxidizing agents also cause combustion of material that is
why they are called dangerous material. Chemist classified the
oxidizing agents but they are not called oxidizing agents
according to dangerous material sense. For example
potassium dichromate is unable to classify in dangerous
material sense.
Common oxidizing agents and products formed
ClO-
CL-
, H2O

4. SO2 Ultramarine production,
more commonly reducing
agent
RuO4 In organic laboratory
CrO3-
CrO2-
Cr-
Cr+3
F2
F-
Br2 Br-
HNO3 NO
NO2
H2O2 Oxides and H2O
Types of oxidizing agents
There are many types of oxidizing agents some of them are as follows:
 Oxygen
 Ozone
 Hydrogen peroxide, fenton’s reagent
 Halogens
 Nitric acid and nitrate compounds
 Sulfuric acid
 Peroxydisulfuric acid
 Peroxymonosulfuric acid

5. Common oxygen transfer reagents
 Chromic acid, potasaium permanganate,
 Oxygen
 Hydrogen peroxide
 Potassium nitrate
 Sodium perborate
 Sodium bismuthate
 Ozone
 Hypochlorite
 Peroxydisulpuric acid
 Fluorine, chlorine
 Chromium trioxide
 Nitrous oxide
 Peroxydisulpuric acid
Example
In this example focus on role of oxidizing agent. Potassium
permanganate role in equation.
2 MnO4
-
(aq) + 5 H2C2O4 (aq) + 6 H+
(aq) 10 CO2(g) + 2
Mn2+
(aq) + 8 H2O(l )
This equation shows that oxidation takes place at oxalic acid
and in this process permagnate get reduced.
Oxidation: H2C2O4 CO2
+3 +4
Reduction: MnO4
-
Mn2+
+7 +2

6. Removal of electrons takes place from oxalic acid so this
process oxidizes oxalic acid. During this reaction reduction
takes place at oxidizing agent. While on other side oxalic acid
is reducing agent by changing its oxidation state.
Those atomic species which have good affinity for electrons
are mostly act as good oxidizing agent. In periodic table
fluorine is best electronegative element in other words it has
good attraction for electrons so its presence can burn metals,
quartz and water. Oxygen is also very good electronegative
element and third one chlorine above these also use to oxidize
the other species.
Mostly it is noticed that high oxidation state elements like
sulphuric acid, dichromate, permanganate, chromate and nitric
acid act as good oxidizing agents.
By increasing oxidation state their oxidizing becomes
increase. Some species act as both oxidizing and reducing
agents. E.g. hydrogen gas, hydrogen peroxide, hydrogen
chloride.
Inorganic oxidizing agent
MnO2: Ketonic and alcoholic group get oxidized by this
reagent and Mn change its oxidation state
Sodium hypochlorite: Secondary alcohol converted to
ketones by help of this oxidizing agent
Organic oxidizing agents

7. Peroxycarboxylic acid: This is used in converting
formation of ester by oxidation of alcohol. Mostly peracids
are used commonly in oxidation as oxidizing agrnts like
perbenzoic, peracetic, monoperphathalic, m-chlorobenzoic
and triflouroacetic acid.
Others oxidizing agents are:
 𝐾𝑀𝑛𝑂4
KMnO4 IS A STRONG OXIDIZING AGENT. Potassiumpermanganate
oxidizes the aldehydes, alcohols, alkenes andalkynes andmany other
compounds. 𝑲𝑴𝒏𝑶 𝟒 oxidizes the carbonatoms if they containsufficiently
weak bonds.
Examples:





8.  Potassium dichromate:
In organic chemistry potassiumdichromate is usedtooxidize the primary
alcohols intoaldehyde and secondary alcohol intoketone. Whenheatedit
oxidizes the alcohol andchanges the color, as is reduced to Cr3
.
EXAMPLE:
It is used in breathalyzers.
Application
Oxidizing agents play very important role in industries as
bleaching of different fabrics, purification of water, storage of
energy. Much biological process takes place in presence of
oxidizing agents like reaction of photosynthesis and
metabolization of body. In breakage of glucose
C6H12O6+2ADP+2P+2NAD+→2CH3COCO2H+2ATP+2N
ADH(1)(1)C6H12O6+2ADP+2P+2NAD+→2CH3COCO2H+
2ATP+2NADH

9. Combustion which is takes place in industries is also due to
oxidizing agent. Combustion is very important process of
industries.
2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g)(2)(2)2C8H18(l)
+25O2(g)→16CO2(g)+18H2O(g)
Reference
 https://www.organicchemistry.org/chemicals/oxidations
 www.cod.edu/people/faculty/jarman/richenda/1105.../Redox_1105-
notes.pdf
 www.idconline.com/technical_references/pdfs/.../Oxidizing_and_reducing
_agents.pdf...
 Organic Organic chemistry by paula Bruice
 Organic chemistry by clayden
 https://www.chegg.com/homework-help/definitions/oxidizing-and-
reducing-agents-6