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Chemistry
Redox
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Created by
Shriya Shivakumar
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Cards (18)
Reducing agents
Electron donors
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Oxidising
agents
Electron
acceptors
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Oxidation
1. Process of electron loss
2. Involves an
increase
in oxidation number
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Reduction
1. Process of
electron
gain
2. Involves a decrease in
oxidation
number
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Rules for assigning oxidation numbers
All uncombined elements have an oxidation number of
zero
The oxidation numbers of the elements in a compound
add
up to
zero
The oxidation number of a monoatomic ion is
equal
to the ionic charge
In a polyatomic ion, the sum of the individual oxidation numbers of the elements
adds
up to the
charge
on the ion
Several elements have
invariable
oxidation numbers in their
common
compounds
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Note the oxidation number of Cl in CaCl2 = -1 and not
-2
because there are
two
Cl's
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Always work out the
oxidation
per one atom of the
element
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Oxidation number of Fe in FeCl3
+3
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Redox equations and half equations
1.
Br2
(aq) +
2I-
(aq) → I2 (aq) + 2 Br- (aq)
2
.
Br2
(aq) + 2e- → 2 Br- (aq)
3.
2I-
(aq) →
I2
(aq) + 2 e-
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Oxidising agent
Bromine water.
It is an
electron acceptor
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Reducing agent
Iodide
ion. It is an
electron
donor
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Oxidising
agent (or
oxidant
)
The species that causes another element to
oxidise.
It is itself
reduced
in the reaction.
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Reducing agent
(or
reductant
)
The
species
that causes another
element
to reduce. It is itself oxidised in the reaction.
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Reduction half equation
Only shows the parts of a chemical equation involved in
reduction.
The electrons are on the
left.
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Oxidation
half equation
Only shows the parts of a chemical equation involved in oxidation. The
electrons
are on the right.
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Balancing redox equations
1. Work out
oxidation
numbers for element being oxidised/
reduced
2. Add
electrons
equal to the change in
oxidation
number
3. Check to see that the sum of the
charges
on the reactant side equals the sum of the
charges
on the product side
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Writing half equations (more complex)
1. Balance the change in
O.N.
with
electrons
2. Add
H2O
in products to
balance
O's
3. Add H+ in reactants to
balance
H's in
H2O
4. Check to see that the sum of the
charges
on the reactant side equals the sum of the
charges
on the product side
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Combining half-equations
1. To make a full redox equation combine a
reduction half
equation with an
oxidation half
equation
2. To combine two half equations there must be equal numbers of
electrons
in the two half equations so that the electrons
cancel
out
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