Transcript Chapter 7 Electrochemistry What is electrochemistry?

Chapter 7 Electrochemistry
What is electrochemistry?
A science that studies the relation between electric and
chemical phenomena and the disciplines that govern the
conversion between electric and chemical energies.
Chapter 7 Electrochemistry
Main contents
• Section 1: Electrolyte and electrolytic solution
• Section 2: Electrochemical Thermodynamics:
• Section 3: Irreversible electrochemical system
• Section 4: Applied electrochemistry
§7.1 Electrolyte and electrolytic solution
Main contents:
1) Electrolyte: origin of the concept
2) Existence of ions in solution
3) Hydration theory:
4) Interionic interaction
5) Motion under electric field
6) Conducting mechanism
7) Faraday’s law and its application
7.1.1 Origin of the concept – electrolyte
1) Definition of electrolyte
An electrolyte is a substance that, when dissolved in
solvent, produces a solution that will conduct electricity.
2) Dissociation of substance
In 1886, Van’t Hoff published his
quantitative research on the colligative
properties of solution.
For sucrose, the osmotic pressure ()
can be expressed as:
=cRT
But for some other kind of solvates such
as NaCl, the osmotic pressure had to be
expressed as:
=icRT
i , Van’t Hoff factor, is larger than 1.
In the paper written in Achieves Neerlandaises (1885) and Transactions of the Swedish.
Academy (1886), van't Hoff showed analogy between gases and dilute solutions.
The equation for freezing point depression and boiling
point elevation contains the letter i. i stands for the van’t
Hoff Factor.
∆T = imKf
Since freezing point depression and boiling point elevation
depend only on the number of particles ( it does not matter
what the particles are), we need only determine the total m of
the particles.
If a solution is 0.2 m NaCl, the i would be about 2. The
true van’t Hoff factor is not exactly 2, but is close enough to
call it 2.
http://en.wikipedia.org/wiki/Van_'t_Hoff_factor
3) Dissociation theory for weak electrolytes
In 1887, Svant August Arrhenius
postulated that, when dissolved in
adequate solvent, some substances can
split into smaller particles, the process
was termed as dissociation.

+
AB
molecule


 +

A+
cation
positive ion
+
B–
anion
negative ion
The charged chemical species are named as ions and the
process is termed as ionization.
Therefore, the number of particles present in solution is
actually larger than that predicted by van’t Hoff, which
resulted van’t Hoff factor.
New definitions:
Dissociation, ionization
Weak / strong electrolyte? True and potential?
Theory of Electrolytic Dissociation
Acid-base theory
Greenhouse effect
Cf. Levine p.295
7.1.2 State of ion in solution
In what state do ions exist in solution?
Solvated (hydrated) ion
+

Solvation shells
The interaction between ions and water molecules
disturb the structure of liquid water.
Primary hydration shell
ion
secondary hydration shell
Disordered layer
Bulk solution
The water molecules in the hydration sphere and bulk water have
different properties which can be distinguished by spectroscopic
techniques such as nuclear magnetic resonance (NMR), infrared
spectroscopy (IR), and XRD etc.
Hydration of ion
Coordination number:
Li+: 4, K+: 6
Primary solvation shell:
4-9, 6 is the most common number
Secondary slovation shell:
6-8, for Al3+ and Cr3+: 10-20
7.1.3 Hydration Theory / Solvation Theory
Why does NaCl only melt at higher temperature, but dissolve
in water at room temperature?
H / kJ mol-1
Na+(g) + Cl(g)
hydration energy:
784 kJ mol-1
788
784
Na+(aq) + Cl(aq)
NaCl(s)
4
1948, Robinson and Storks
F 
q1 q 2
4 r  0 r
2
Long-range forces
The interionic distance for NaCl crystal is 200 pm, while for 0.1
moldm-3 solution is 2000 pm.
To draw Na+ and Cl apart from 200 nm to 2000 nm, the work
is: W (/kJ) = 625 / r
for melting: r =1, W = 625 kJ, m.p. = 801 oC。
for dissolution in water: r = 78.5, W = 8 kJ.
Therefore, NaCl is difficult to melt by easy to dissolve in
water at room temperature.
7.1.4 Interaction between cation and anion
F 
+

At low
concentration
q1 q 2
4 r  0 r 2
+

At medium
concentration
In equilibrium -- Bjerrum
+

At high
concentration
Cf. Levine, p. 304
Owing to the strong interaction, ionic pair forms in concentrated
solution.
ionic pair vs free ion
In an ionic pair, the cation and anion are close to each other,
and few or no solvent molecules are between them. Therefore,
HCl does not ionize and NaCl does not dissociate completely in
solvents.
Some facts about strong electrolytes
solution
present species
0.52 mol·dm-3 KCl
95% K+ + 5% KCl
0.25 mol·dm-3 Na2SO4
76 % Na+ + 24% NaSO4¯
0.1 mol·dm-3 CuSO4
44% CuSO4
For concentration-dependence of ion pair, see Levine p. 305, Figure 10.10
Degree of association
Activity coefficient is essential for quite dilute solutions
7.1.5 Conducting mechanism of electrolyte
(1) Category of conductor:
Charge carriers: electron; ion; hole; Cooper electron pair; polaron.
Conductor
Charge carrier
samples
1st
electron
2nd
ion
3rd
Semiconductor
4th
Electron and
hole
polaron
5th
electron pair
Superconductors
Mixed conductor
Ion and electron
Metals, carbonous materials, some metal
oxides
Electrolytic solution, solid-state electrolyte
(Al2O3, ZrO2)
Conducting polymers
PbO2, NiOOH
(2) Conducting mechanism

+
I
+
+
+
+
+
+
+
E
+
•Electric transfer of ion in
solution under electric field
How can current cross the
electrode / solution interface ?
Motion of ions in the solution:
1) diffusion: due to difference in
concentration
2) convection: due to the difference in
density
3) transfer: due to the effect of electric
field
e
e
e
Cl
Cl
H+
Cl
e
H+
Cl
H+
Cl
Cl
Cl
e
H+
H+
Cl
H+
e
H+
H+
Cl
H+
Cl
H+
At anode:
At cathode:
2Cl  2e  Cl2
2H+ + 2e  H2
Conducting mechanism:
1) Transfer of ion in solution under electric field;
2) electrochemical reaction at electrode/solution interface.
7.1.7 Law of electrolysis
For quantitative electrolysis:
Q
m 
M
zF
Faraday’s Law
where m is the mass of liberated matter; Q the
electric coulomb, z the electrochemical equivalence,
F a proportional factor named as Faraday constant,
M the molar weight of the matter.
Faraday’s constant
Micheal Faraday
Great Britain 1791-1867
Invent the electric motor
and generator, and the
principles of electrolysis.
F = (1.6021917  10-19  6.022169  1023 ) C·mol-1
= 96486.69 C·mol-1 usually round off as 96500
C·mol-1, is the charge carried by 1 mole of
electron.
Current efficiency ()
Qtheoretical

Qeffective

meffective
mtheoretical
Current efficiency is lower than 100% due to side-reactions.
For example, evolution of hydrogen occur during electrodeposition of copper.
Application of Faraday’s law
1) Definition of ampere:
IUPAC: constant current that would deposit 0.0011180 g of
silver per second from AgNO3 solution in one second: 1
ampere.
2) Coulometer: copper / silver / gas (H2, O2) coulometer
3) Electrolytic analysis – electroanalysis
Q ↔m ↔ n ↔ c
Exercise-1:
A 0.100 molality (mol/kg) solution of NaCl has a freezingpoint depression of -0.348 oC, whereas the expected decrease in
the freezing point is -0.186 oC. The van’t Hoff factor in this case
is 1.87. If there were no ion pairing, we would expect the van’t
Hoff factor for NaCl to be 2.00. Similarly, acetic acid in a 0.100
molal solution has a van’t Hoff factor of 1.05. Calculate the
concentration of NaCl ion pairs and also the percent ionization of
acetic acid form the above information.
Exercise-2:
A current of 2.34 A is delivered to an electrolytic cell for 85
min. how many grams of (a) Au from AuCl3, (b) Ag form
AgNO3, and (c) Cu from CuCl2 will be plated out?
Exercise-3
Levine: p.317 10. exercise 48
Exercise -4
Yin: p. 217 exercise 1.
Outside class reading
Ira N. Levine, Physical Chemistry, 5th Ed., McGraw-Hill, 2002.
pp. 294-310
Section 10.6 solutions of electrolytes
Section 10.9 ionic association
pp. 512-515
Section 16.6 electrical conductivity of electrolyte solutions.