-
Redox Reactions-
Reaction the transfer of electrons
involving
"Electrolyte
-
I
: Substance that can conduct electricity i
·
Oxidation Loss of electrons
I
due to the of free
I
:
presence ions when molten
L I
*
Occurs at Anode
↓ or dissolvedinsolution -------
-
+
-
In In + 2e
·
Reduction : Gain of electrons
-
Occurs at cathode
-
(12 + 2e 22 * other substance
gets occidised
-
Oxidising agent Substance that
·
=
accepts electrons
Reducing agent Substance that donates
·
= electron
Oxidation
ositive spontaneous reaction
↑ gradient =
reduction
Cathode
-GalvanicCell- Salt Bridge Anode
·
·
Chemical
Cathode
-
Reduction
energy
is
to
positive :
here
electrical
energy
RED CAT
- Cu2
+ z2 +
occurs
Anode
negative
·
is
-
Oxidation occurs here OX ANODE
·
Anode :
-
Find metal further up on
right side
·
Solution :
-
Stronger reducing agent
Copper cathode -Undergoes oscidation
-
:
+
↳
Ca2 ions
↳
This is Anode
+ +
↳ Cu2 ↳ 2n Ze
gets reduced 2n +
Cu Cu Mass
-
↳
+ Ze decreases
-Zinc anode
·
Cathode :
Int
-Stronger
↳
ions
occidising agent
In Undergoes
gets occidised reduction
In In + Ze ↳
Cu + Ze Cu
Copper forms cathode
-
on mass increases
Electrons
through
·
external circuit
Cathode
-
mass increases
↳
Transferred electrons bond with ions and form atoms
↳
Forms on surface of electrode
Anode looses
-
mass
↳
Electrons leave anode
↳
Atoms become ions in liquid
, -Salt Bridge
Filled
·
with saturated salt solution
HCl NaCl kNOs Isolable
-
, ,
with all ions(
Completes
·
circuit and maintains electrical neutrality
·
Anode :
-
2n levels increase
-
Solution becomes positive
Negative ions enter to keep balance
·
Cathode :
+
-
Cu levels decrease
Solution becomes
negative
-Standard-Hydroge -
HattCell-
Potential
·
of ov
bubbled
Hydrogen platinum
·
over electrode inert
·
Electrolyte is acid (HCl)
-
(e) Notation _
-
Electrodes
·
written outside of cell notation ! Anode
Oxidising
·
·
Single line)) is chase boundry agent -
·
Reduced species
In t
+
2 Cu Ca
bridge
·
= salt
!
·
Formati
!
1) Cathode
Reducing agent
·
Gets occidised
Reducing agent
- ·
2+
In In + Ze
2) Oxidised species
-
Product of Oxidation
3)
Oxidising agent
-
Gets reduced
27
-
Cu + 2e Cu
4) Reduced species
-
Product of reduction
Redox Reactions-
Reaction the transfer of electrons
involving
"Electrolyte
-
I
: Substance that can conduct electricity i
·
Oxidation Loss of electrons
I
due to the of free
I
:
presence ions when molten
L I
*
Occurs at Anode
↓ or dissolvedinsolution -------
-
+
-
In In + 2e
·
Reduction : Gain of electrons
-
Occurs at cathode
-
(12 + 2e 22 * other substance
gets occidised
-
Oxidising agent Substance that
·
=
accepts electrons
Reducing agent Substance that donates
·
= electron
Oxidation
ositive spontaneous reaction
↑ gradient =
reduction
Cathode
-GalvanicCell- Salt Bridge Anode
·
·
Chemical
Cathode
-
Reduction
energy
is
to
positive :
here
electrical
energy
RED CAT
- Cu2
+ z2 +
occurs
Anode
negative
·
is
-
Oxidation occurs here OX ANODE
·
Anode :
-
Find metal further up on
right side
·
Solution :
-
Stronger reducing agent
Copper cathode -Undergoes oscidation
-
:
+
↳
Ca2 ions
↳
This is Anode
+ +
↳ Cu2 ↳ 2n Ze
gets reduced 2n +
Cu Cu Mass
-
↳
+ Ze decreases
-Zinc anode
·
Cathode :
Int
-Stronger
↳
ions
occidising agent
In Undergoes
gets occidised reduction
In In + Ze ↳
Cu + Ze Cu
Copper forms cathode
-
on mass increases
Electrons
through
·
external circuit
Cathode
-
mass increases
↳
Transferred electrons bond with ions and form atoms
↳
Forms on surface of electrode
Anode looses
-
mass
↳
Electrons leave anode
↳
Atoms become ions in liquid
, -Salt Bridge
Filled
·
with saturated salt solution
HCl NaCl kNOs Isolable
-
, ,
with all ions(
Completes
·
circuit and maintains electrical neutrality
·
Anode :
-
2n levels increase
-
Solution becomes positive
Negative ions enter to keep balance
·
Cathode :
+
-
Cu levels decrease
Solution becomes
negative
-Standard-Hydroge -
HattCell-
Potential
·
of ov
bubbled
Hydrogen platinum
·
over electrode inert
·
Electrolyte is acid (HCl)
-
(e) Notation _
-
Electrodes
·
written outside of cell notation ! Anode
Oxidising
·
·
Single line)) is chase boundry agent -
·
Reduced species
In t
+
2 Cu Ca
bridge
·
= salt
!
·
Formati
!
1) Cathode
Reducing agent
·
Gets occidised
Reducing agent
- ·
2+
In In + Ze
2) Oxidised species
-
Product of Oxidation
3)
Oxidising agent
-
Gets reduced
27
-
Cu + 2e Cu
4) Reduced species
-
Product of reduction
