Chapter 6 Electrochemistry
Transcript of Chapter 6 Electrochemistry
Chapter 6
Electrochemistry
A. Electrolytes & Non-electrolytes
Electrolytes
Substances that can conduct electricity and undergo chemical changes
Non-electrolytes
Substances that cannot conduct electricity
Electrolyte
Non-electrolyte
Why electrolyte at molten and aqueous state can conduct electricity?
BECAUSE
There presence of free moving ions in the electrolyte
B. Electrolysis of Molten Compounds
Electrolysis
A process where compounds in molten or aqueous state are broken down into their constituent elements by passing electricity through them
Electrolytic cell
The set of apparatus needed to conduct electrolysis
Electrolyte
Cathode Anode
+ -
STEPS OCCUR DURING
ELECTROLYSIS
Movement of ions to the
electrodes.
Discharges of ions at the
electrodes.
Graphite or platinum
is usually used as
electrodes because
they are inert.
Important note: Observation Anode (positive electrode)
Electrolysis product Observation Confirmatory test
Chlorine gas Greenish-yellow gas bubbles released
Place moist blue litmus paper into test tube Moist blue litmus paper turn red Bromine gas Brown gas released
Iodine Purple gas released
Oxygen gas Colourless gas bubble released
Place a glow wooden splinter near the mouth of test tube The glowing wooden splinter light up
Metal (all metal) The mass of electrode decreased
Copper metal Brown solid formed
Important note: Observation
Cathode (negative electrode)
Electrolysis product Observation Confirmatory test
Almost all metal (except copper metal)
Grey solid formed The mass of electrode increase
No test for metals
Copper metal Brown solid formed
Hydrogen gas Colourless gas bubbles released
Place a lighted wooden splinter near the mouth of test tube A “pop” sound heard/produced
Electrolysis of molten compound
Electrolysis of molten compound
• PbBr2 • LiCl • MgBr2 • PbI2 • ZnO • CuCl2 • Molten Potassium oxide • Molten Magnesium oxide • Molten Potassium iodide
Electrolysis of Aqueous Solutions
Factors that affect the electrolysis of an aqueous solution
• Position of ions in the Electrochemical Series
• Concentration of ions in the electrolytes
• Types of electrodes used in the electrolysis
Position of ions in the Electrochemical Series
• The ions that are lower in the electrochemical series will be selected discharged
K+
Na+
Ca2+
Mg2+
Al3+
Zn2+
Fe2+
Sn2+
Pb2+
H+
Cu2+
Ag+
F-
SO42-
NO3-
Cl-
Br-
I-
OH-
The Electrochemical Series
Ease of discharge increases
0.01 mol dm-3 of copper(II) sulphate using carbon as electrodes
1 mol dm-3 of
copper(II) sulphate
solution
Carbon Carbon
Concentration of ions
• If the concentration of a particular ions is high, the ions is selectively discharged
TIPS: ANODE Ion selectively discharged based on CONCENTRATION of ions CATHODE Ion selectively discharged based on position of ions in Electrochemical Series
2 mol dm-3 of hydrochloric acid, HCl using platinum as electrodes
2 mol dm-3 of
hydrochloric acid, HCl
Platinum Platinum
Anode : Cathode :
Types of electrodes
• Electrolysis of copper(II) sulphate, CuSO4 solution using copper electrode
• Electrolysis of silver nitrate, AgNO3 solution using silver electrode
0.02 mol dm-3 of copper(II) sulphate, CuSO4
using copper as electrodes
0.02 mol dm-3 of
copper(II) sulphate,
CuSO4
Copper Copper
Anode : Cathode :
0.02 mol dm-3 of silver nitrate, AgNO3
using silver as electrodes
0.02 mol dm-3 of silver
nitrate, AgNO3
Silver Silver
D. Electrolysis in Industries
• The most industrial application of electrolysis:
1. extraction
2. purification
3. electroplating of metals
E. Voltaic Cells
• Chemical energy to electrical energy
• Examples of chemical cell:
simple voltaic cell
Daniell cell
dry cell
alkaline cell
lead-acid accumulator
Simple Voltaic Cell
Two different metals being immersed into an electrolyte and connected by wire
V
Daniell cell – has two types
• Use porous pot
• Use salt bridge
Use porous pot
Use salt bridge
F. The Electrochemical Series
• The Electrochemical Series is series of element, arranged according to the order of decreasing tendency to released electrons.
• Or the greater the tendency to donate electrons, the more electropositive is the metal and the higher it is in the Electrochemical Series.
Principles Used:
• Metals are arranged according to the tendency of their atoms to release electron.
• More the tendency of their atoms to release electron, the higher located it is in the series.
• Elements located at HIGHER part of the Electrochemical Series are more electropositive and have higher tendencies to release electrons to form positive ions.
• Example : magnesium is more electropositive than copper in Electrochemical Series
The Electrochemical Series can be constructed based on:
Metals are arranged according to their tendency to release electrons to form positive ion (cation).
• metal has a higher tendency to release electron placed a the higher position in Electrochemical Series.
• the metal act as negative terminal
The ability of a metal to displace another metal from its salt solution.
• If metal is able to displace another metal from its salt solution, this metal is placed at the higher position in Electrochemical Series
The potential difference between two metals.
• The further apart between two metals in the Electrochemical Series, the greater the potential difference between them.
• The greater the voltage produced by the cell.