ALL REACTION OF IOC in 1 Shot _ Class Notes __ Manzil Legends-JEE.pdf

EACTION OF IOC in 1 Shot

1. Om Pandey
Complete Inorganic Chemistry
Reactions
MANZIL
For JEE Aspirants
ONE SHOT

2. TOPICS TO BE COVERED
NCERT
+
1.

3. Fe
+2
Cl
–
Br
–
I
–
NH
3
H
2O
2
H
2O
NO
Fe
+3
Cl
2
Br
2
I
2
N
2
O
2
O
2
NO
2
SO
2
HNO
2
H
2SO
3
SO
3/SO
4
2–
HNO
3
H
2SO
4
SS
2–
SO
2
Oxidation

4. CO
H
3PO
3
H
2S
Sn
+2
H
2C
2O
4
CO
2
H
3PO
4
S
Sn
+4
CO
2
Base
Neutral
Acid
MnO
4
–
Mild basic
Oxidation Reduction
I
2withH
2O HIO
3

5. Br
2
Cl
2
O
3
H
2O
2
K
2Cr
2O
7/H
+
Fe
+3
Con.HNO
3
Dil.HNO
3
HNO
2
Br
–
Cl
–
H
2O
O
2/O
2–
Cr
+3
Fe
+2
NO
2
NO/N
2O
NO
F
2 F
–
MnO
2 Mn
2+
I
2 I
–
Reduction

6. Pb
+4
Bi
+5
Cu
+2
CaOCl
2
Ag
+
Pb
+2
Bi
+3
Cu
+1
CaCl
2
Ag
Hg
+2
Hg
2
+2
Hg
Hg
2
+2
Reduction

7. OxidisingAgent
ReducingAgent
Metals&Elementswithlowerormin.
oxidationstate
Elementswithmax.oxidationstate
OxidisingAcid
Conc.H
2SO
4
Conc./dil.HNO
3
Conc./dil.HXO
n
Non–OxidisingAcid
Conc./dil.HX
dil.H
2SO
4
Conc./dil.H
2CO
3
Conc./dil.H
3PO
4
Conc./dil.H
3PO
3

8. F
2+Cl
–
Cl
2+I
–
Br
2+I
–
F
2+Br
–
F
2+l
–
Cl
2+Br
–
Oxidising Nature of Halogens

9. O
3CaOCl
2S
2O
8
2–
KMnO
4/H
+
H
2O
2MnO
2 K
2Cr
2O
7/H
+
HNO
3 H
2SO
4
F
2
Cl
2
Br
2
I
2
Bi
+5
Pb
+4
:SOA
Table for Oxidising Power
firozobich-bazarmargyaper-man per man kacontrolnhi
kalnayikregasafayi
baharnitrousfir
HNO
2 Fe
3+
seaayi

10. FeSO
4+H
2SO
4+Cl
2
Na
2SO
3+Cl
2+H
2O
SO
2+ Cl
2+H
2O
I
2+ Cl
2+H
2O
Chlorine as Oxidising agent
Na
2S
2O
3+Cl
2

11. C+H
2SO
4
S+H
2SO
4
Cu+H
2SO
4
H
4SO
4as Oxidising agent

12. HCl
KMnO
4/H
+
Pb
3O
4
O
2
Deacon’s
Process
PbO
2
K
2Cr
2O
7/H
+
H
2SO
4
MnO
2
CaOCl
2
O
3
CuCl
2

13. HBr
K
2Cr
2O
7/H
+
H
2SO
4
MnO
2
CaOCl
2
KMnO
4/H
+
O
3
Pb
3O
4
PbO
2

14. HI
K
2Cr
2O
7/H
+
H
2SO
4
MnO
2
CaOCl
2
KMnO
4/H
+
O
3
Pb
3O
4
PbO
2
HNO
3
HNO
2
FeCl
3
K
2S
2O
8
HIO
3

15. O
3
PbS
NO
2
–
SO
3
2-
Sn
+2
K
2MnO
4
l
–
C
NO
I
2
(moist)
H
2S

16. Oxalic acid
Fe
2+
(Green)
KI
H
2S
C
2O
4
2–
H
2SO
3
SO
3
2–
NO
2
–
KMnO
4 / H
+

17. S
2O
3
2–
I
–
Mn
2+
ZnO as catalyst
MnO
4
–
Neutral
Mild basic

18. H
2S
Sn
2+
Fe
2+
I
–
K
2Cr
2O
7/H
+
Potassium Dichromate in Acidic Medium

19. MnO
4
–
VsMnO
4
2–
MnO
4
2–
AcidicNeutral
Mild basic
Mn
2+
+ S
2O
8
2–
+ H
2O
Preparation of KMnO
4

20. MnO
2+ KOH + O
2
Acidic Solution
Electrolytic oxidation
in alkaline solution
MnO
2+ KOH + O.A.
Air / KNO
3 / KClO
3
Preparation of KMnO
4
From MnO
2( Pyrolusite )

21. ➢From Chromite Ore : FeCr
2O
4
FeCr
2O
4 + Na
2CO
3 + O
2
Na
2CrO
4
H
2SO
4 KCl
Preparation of Potassium Dichromate

22. SO
3
Cr
2O
7
2–
MnO
4
–
V
2O
5/O
2
P
4
l
–
C
PCl
5
I
2
(moist)
Fe
+3
SO
2
PbO
2
Cl
2

23. K
2Cr
2O
7/H
+
HCl
NaCl
NaBr
HBr
SO
2
+H
2S
P
4+ SOCl
2
P
4+ SO
2Cl
2
OxidisingPower : SOCl
2 SO
2Cl
2

24. H
2O
2
MnO
4
-
Fe
2+
Mn
2+
I
2
PbS
Fe
2+
MnO
4
-
HOCl
H
2O
2 / H
+ H
2O
2 / OH
-

25. AB
H
2O
Oxides
Peroxides
Superoxides
Hydrolysis

26. N
2O
5
Na
2O
Na
2ON
2O
5+
Hydrolysis of Oxide
P
4O
10
P
4O
6

27. Hydride
Silicide
NaH
CaH
2
Ca
2Si + SiH
4
H
2O
NitridesLi
3N
Mg
3N
2
PhosphideCa
3P
2
Ca
3P
2+CaC
2
:Holme’s Signal

28. Sulphide ZnS
Ionic Carbide CaC
2+H
2O
(Acetilide)
Al
4C
3+
(Methanide)
H
2O

29. Nucleophilic Sub
n
PCl
3+H
2O
PCl
5+H
2O
SO
2Cl
2+H
2O
SOCl
2+H
2O
Hydrolysis
SF
6:No hydrolysis

30. NCl
3
PCl
3
AsCl
3
SbCl
3
BiCl
3
Hydrolysis of Group –15 Halides

31. F
2+H
2O
Br
2+
I
–
+H
+
H
2O
+O
2
Cl
2+H
2O
Hydrolysis of Halogens

32. NonMetal+Alkalisolution DisproportionationReaction
F
2
NaOH
Cl
2
R.T.
Hot
Br
2
R.T.
Hot
l
2
Hot
R.T.

33. P
4
H
2O NaOH
S
8
H
2O NaOH

34. Sn, Al, Pb, Zn, B, Si
Reaction of NaOH(aq)
NaOH
(aq)
Elements
NaOH
(aq)
M+ H
2Na
xMO
y+NaOH

35. IF
5
IF
7
ICl
CIF
3
Hydrolysis of Interhalogen Compounds

36. H
2O
XeF
6
H
2O H
2O
XeF
2
XeF
6
XeF
4
H
2O
H
2O
H
2O
H
2O
Hydrolysis of Xe Fluorides

37. XeF
4+O
2F
2
XeF
2+PF
5F
–
donor
NaF+XeF
6F
–
Acceptor
Pu +O
2F
2
PuisremovedasPuF
6fromspentnuclearfuel

38. NH
3+HClNH
3asBase
NH
3+H
2SO
4
(i)
(ii)
NH
3+H
2O(ii)
Ammonia NH
3

39. NH
4Cl
(NH
4)
2SO
4
Heat
Urea+Water
+Ca(OH)
2
+NaOH
N
2
Haber’sprocess +H
2
IronOxide
Ammonia NH
3

40. Detectionofdblockmetalion:
NH
4OH+ZnSO
4
NH
4OH+FeCl
3
AgCl
(s)+NH
3
Cu
2+
+NH
3(i)
Ag
+
+Cl
–(ii)
Reaction of NH
3

41.  (NH
4)
2Cr
2O
7
NH
4NO
3
NH
4NO
2

42. Inlaboratory
NH
4Cl
(aq)+NaNO
2(aq)
(NH
4)
2Cr
2O
7
Heat
Ba(N
3)
2
Heat
NaN
3
Heat
Nitrogen : N
2

43. Ostwald’sProcess
NH
3+O
2
500K
Pt/Rh
NO
2+H
2O
NO+O
2
HNO
3(Nitric acid)

44. HNO
3+Nonmetals –icacid+NO
2
HNO
3+S
HNO
3+I
2
HNO
3+P
4
HNO
3+C
Oxidising agent

45. M+Conc.HNO
3
Zn+Conc.HNO
3
M(NO
3)
y+NO
2
Cu+Conc.HNO
3
M+dil.HNO
3
Zn+dil.HNO
3
M(NO
3)
y+N
2O/NO
Cu+dil.HNO
3
Au,Pt:DonotdissolveinHNO
3

46. Somemetalsdonotdissolveinconcentratednitricacidbecauseof
theformationofapassivefilmofoxideonthesurface.
Fe Cr Co Ni AlBe
Pb
3O
4
Conc. HNO
3

47. Au,Pt:DonotdissolveinHNO
3
Aqua Regia
HNO
3+HCl
Chloroauric Acid Au+[Cl]
Pt+[Cl] Chloroplatinic Acid

48. Testfornitrates⟹
+
H
2SO
4
FeSO
4
NO
3
–
NO
3
–
[Fe(H
2O)
6]
2+
+Fe
2+
+NO
Brown Ring Test

49. N
2O NH
4NO
3
Heat
NaNO
2+FeSO
4+H
2SO
4NO
N
2O
3
NO+N
2O
4
250K
Formula
Oxidation
State
Preparation
Physical /
chemical
Oxides of Nitrogen

50. NO
2
PbNO
3
673K
N
2O
4
HNO
3+P
4O
10N
2O
5
NO
2
Cool
Heat
Formula
Oxidation
State
Preparation
Physical /
chemical
Nitronium cations[NO
2]
+
andNitrate anions[NO
3]
−N
2O
5
(Solid)

51. Formula Oxidation State Preparation
H
3PO
2
WhiteP
4+alkali
PCl
3+H
3PO
3
H
3PO
3
H
4P
2O
5
P
2O
3+H
2O
Oxoacids of Phosphorus

52. Formula Oxidation State Preparation
redP
4+alkali
H
4P
2O
7
P
4O
10+H
2O
H
4P
2O
6
H
3PO
4
(HPO
3)
n
H
3PO
4
heat
H
3PO
3
Br
2 / heat
Sealed tube

53. H
3PO
4 H
3PO
3 H
3PO
2
Basicity:
AcidicNature:
AgNO
3+H
2O+H
3PO
2
H
3PO
2
NN
+
Cl
–
Reducing Properties of Oxoacids of Phosphorus
ReducingAgent:

54. ByHeating:
KClO
4
KMnO
4
K
2Cr
2O
7
Dioxygen
KClO
3
MnO
2
DecompositionofH
2O
2
H
2O
2(aq.)
Ag
2O/HgO
Pb
3O
4
PbO
2/

55. Contact Process
Sulphuric Acid

56. Thank You !