Summary JEE mains & Advance chemistry mind map

PHYS
OXIDISING AGENT
OXIDATION
REDOX REACTIONS
(OXIDANTS):
NUMBER
WAL
A reagent which
can increase
RULES TO ASSIGN OXIDATION NUMBER the oxidation
1) Oxidation number of an element in free elemental number.
state or Uncombined state zero REDUCING AGENT
2) In polyatomic ion, the algebraic sum of all the
(REDUCTANTS):
oxidation numbers of atoms of the ion must equal OXIDATION: A reagent which REDOX REACTIONS:
the charge on the ion Increase in the can decrease Reactions which
3) The oxidation number of oxygen in most oxidation number the oxidation involve change
number.
of the compounds is -2 in oxidation number
In peroxides -1
REDUCTION: of the
In superoxides -1/2
In O2 F2 +1 Decrease in the interacting species
In OF2 +2 oxidation number
4) Oxidation number of hydrogen is +1 in
most of its compounds(In metal hydrides -1)
5) Oxidation number of fluorine is always -1 in its
compounds
6) Alkali metals have oxidation number +1 and
alkaline earth metals have oxidation number +2 always
in its compounds
REDOX REACTION
7) The algebraic sum of the oxidation number of all
the atoms in a compound must be zero. TYPES OF REDOX REACTIONS
>
+1 x -2
KMnO4 1 + x + 4x(-2) = 0 x = +7




DECOMPOSITION REACTION DISPLACEME
COMBINATION REACTION
Reaction leads to the breakdown of a An ion (or an atom
POINTS TO A redox reaction in the form
compound into two or more components is replaced by an
REMEMBER A+B→C
at least one of which must be in the another element.

Either A and B or both A and B must be in elemental state. X + YZ →
the elemental form for such a reaction to be eg: H2O → H2 + O2
Carbon suboxide Fe3O4 CaOCl2 a redox reaction.
+2 O +2 +2 +3 +1 -1
O = C = C = C = O FeO. Fe2O3 Ca(OCl)Cl eg: H2 + Cl2 → 2HCl