Short notes of chemistry class 11, 12

INDEX
S.No. Topic Page No.
PHYSICAL CHEMISTRY
1. Atomic Structure 1
2. Stoichiometry 2
3. Gaseous State 6
4. Thermodynamics 8
5. Chemical Equilibrium 12
6. Ionic Equilibrium 15
7. Electrochemistry 18
8. Solution & Colligative Properties 22
9. Solid State 27
10. Chemical Kinetics & Radioactivity 30

INORGANIC CHEMISTRY
11. Periodic Table & Periodicity 34
12. Chemical Bonding 42
13. Coordination Compounds 53
14. Metallurgy 66
15. s-Block Elements & their compounds 73
16. p-Block Elements & their compounds 77
17. d-Block Elements & their compounds 95
18. Qualitative Analysis 101

ORGANIC CHEMISTRY
Points to remember in
19. Nomenclature 109
20. Structure Isomerism 114
21. General Organic Chemistry 119
22. Alkane 126
23. Alkene & Alkyne 126
24. Alkyl Halide 127
25. Alcohol 127
26. Grignard Reagent 129
27. Reduction 130
28. Oxidation Reaction 132
29. Aldehyde & Ketones 135
30. Carboxylic acid & Derivatives 139
31. Aromatic Compounds 141
32. Polymers 145

, PHYSICAL CHEMISTRY
ATOMIC STRUCTURE
Planck's Quantum Theory :
hc
Energy of one photon = h =


Photoelectric Effect :
1
h = h0 + m 2
2 e
Bohr’s Model for Hydrogen like atoms :
h
1. mvr = n (Quantization of angular momentum)
2

E1 z2 z2
2. En = – 2 z2 = –2.178 × 10–18 2 J/atom = –13.6 eV
n n n2

 2 2 me 4
E1 =
n2
2
n2 h 0 . 529  n2
3. rn = × 2 2 = Å
Z 4 e m Z

2 ze 2 2 .18  10 6  z
4. v= = m/s
nh n
De–Broglie wavelength :
h h
=  (for photon)
mc p

Wavelength of emitted photon :

1 
 1

1 
=  = RZ2  2  2 
 n
 1 n2 




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,No. of photons emitted by a sample of H atom :
n ( n  1)
2
Heisenberg’s uncertainty principle :
h h h
x.p > or m x.v  or x.v 
4 4 4m
Quantum Numbers :
* Principal quantum number (n) = 1, 2, 3, 4 .... to .
nh
* Orbital angular momentum of electron in any orbit = .
2
* Azimuthal quantum number () = 0, 1, ..... to (n – 1).
* Number of orbitals in a subshell = 2 + 1
* Maximum number of electrons in particular subshell = 2 × (2 + 1)
h
* Orbital angular momentum L = ( 1) =   (  1)
2
 h 
  2  
 

STOICHIOMETRY
Mass of one atom of an element
 Relative atomic mass (R.A.M) =
1
 mass of one carbon atom
12
= Total Number of nucleons
 Y-map

Number lt Volume at STP
2.4
×N
A 2
 × lt
N
A 2 2.4

Mole



 mol. wt. × mol. wt.
 At. wt. × At. wt.

Mass

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, Density :
density of the subs tance
Specific gravity = density of water at 4C

For gases :
Molar mass of the gas
Absolute density (mass/volume) = Molar volume of the gas

PM
 =
RT

dgas PMgas RT Mgas M gas
Vapour density V.D.= d = PM = M =
H2 H2 RT H2 2
Mgas = 2 V.D.
Mole-mole analysis :

At. wt. / Mol. Wt. Mole-mole
Mass Mole relationship Mole
of equation t.
t. w
t./A × 22.4 lt
l. w
× mo

Mass Volume at STP


Concentration terms :
Molarity (M) :
w  1000
 Molarity (M) = (Mol. wt of solute )  V
inml
Molality (m) :
number of moles of solute
Molality =  1000 = 1000 w / M w
mass of solvent in gram 1 1 2


Mole fraction (x) :
n
 Mole fraction of solution (x1) =
nN
N
 Mole fraction of solvent (x2) =
nN
x1 + x 2 = 1


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