2. 1. Solid State
Classification of Solids
Classification of crystalline
solids
3. Unit cells, two and three dimensional
lattices and number of atoms per unit
cell and
Number of Atoms in the unit cell :
Unit cell scc bcc fcc hcp
Number of 1 2 4 3
atoms
5. Relation between radius (r) of an
atom and edge length (a) of cubic
unit cell :
scc bcc fcc
a 3 a
r r a r
2 4 2 2
6. Packing in solids
Density of unit cell
∙ Density of the crystal :
z M
d 3
a NA
7. Packing in voids of ionic solids
Defects in crystal structure
Electrical properties
Magnetic properties
8. 2. Solutions & Colligative
Properties
Types of solution
Concentration of solution of solids
in liquids
W
n
Number ofnmoles, M mol
Molarity = V mol dm-3 (or M)
Normality = gra m e q. gram eq.dm -3
V
9. Solubility of gases in liquids
Solid solution
Colligative properties and
molecular masses
Lowering of vapour pressure
10. n
Molality = W t. of solven t in kg
mol kg -1 (or m)
Raoult’s law: Psoln = x1 P0
P0 P W2 M 1
P0 W1M 2
11. Elevation of boiling point
Tb = Kbm and Tf = kf m
W2 1000
Tb = Kb
W1 M2
12. Depression of freezing point
W2 1000
Tf = Kf W1 M2
Osmotic pressure
2
C2
At constant temperature : C1
1
2
T2
At constant concentration : T1
1
17. 3. Chemical Thermodynamics
& Energetics
Basic concepts in thermodynamics
Nature of Heat and Work
Internal Energy
18. W = - P (V2 – V1) = -P V
(For expansion)
W = P (V2 – V1) – P V
(For compression)
V2
Wmax = - 2.303 nRT log10
V1
P1
Wmax = - 2.303 nRT log10 P2
19. First Law of Thermodynamics
Enthalpy
U=q+W
H = U + PV
H= U+P V
H = U + nRT
20. Enthalpy of physical changes
Thermo chemistry
Spontaneous processes
(Irreversible processes)
Gibbs free energy
S q rev H
T T
G = H – TS
21. G= H-T S
G0 = - 2.303 RT log10K
G = 0, the system is at
equilibrium
G < 0, the process is
spontaneous
G > 0, the process is non-
spontaneous.
Third law of thermodynamics.
23. Potential difference (V)
Resistance (R)
Electric current (I)
1 1
Electrical conductance (G)
R
or S
a
Resistivity ( ) R cm
1
24.
Cell constant = cm-1(or m– 1)
a
C e ll C o n s tan t
Conductivity (k)
R e s is tan ce
Molar conductivity (∧m) = (k in Ω-1
k
m-1 and C in mol m-3) OR C
25. k 1000
∧m
C
(k in Ω-1 m-1 and C in mol m-3)
0 0
Kohlarausch’s law : ∧0
m
Degree of dissociation ( )
0
2
m C
Dissociation constant (ka) (
0 0 m)
26. Electrochemical cells
Electrolytic cells
Galvanic or voltaic cells
Electrode potentials and cells potential
27. 0 0 0
E cell E red (cathode) E red (anode)
0 0.0592 n
EM n / M
E Mn log10 [M ]
/M
n
0 0 .0 5 9 2 [P r o d u c ts]
E c e ll E c e ll lo g1 0
n [R e a c ta n ts]
28. 0 0
G n FE cell
∆G = nFEcell
∆G0 = - RTln K
0 0.0592
E cell log10 K
n
For spontaneous cell reaction :
Ecell > 0; ∆G < 0
29. 5. Chemical Kinetics
Rate of reaction
For a reaction, aA + bB cC + dD
1 [A ] 1 [B] 1 [C] 1 [D ]
a t b t c t d t
Average rate =
Rate law : Rate = k [A]a [B]b
30. Dependence of rate on reactant
concentration
2 .3 0 3 [A ]0
k
t log0 [A ] t
(for first order reaction)
0.693
t ½ = k (for first order
reaction)
31. [A ]0 [A ]t
k=
t
(For zero order reaction)
[A ]0
t½= (For zero order reaction
2k
Molecularity of elementary reactions
Collision theory and activation energy
32. Temperature dependence of
reaction rates (Arrhenius equation)
K = Ae– Ea/RT (Arrhenius equation)
Ea
Log10k = log10A – 2 .3 0 3R T
Log10
33. Effect of catalyst on rates of
reactions
k2 E a ( T2 T1)
k1 2 .3 0 3R T1 T2
34. 6. General & Processes
of Isolation of Elements
Concentration of an ore
Oxidation – reduction
Refining of crude metal
35. Extraction of Zinc
Extraction of Iron
Extraction of Aluminium
Extraction of Copper
36. 7. p–Block Elements
Group 15 elements
Group 16 elements
Group 17 elements
Group 18 elements
37. Reference electrodes
Common types of cells
Fuel cells
Electrochemical series
Corrosion