The document consists of clear and simple explanations of how to approach redox reactions and how to balance redox in acidic conditions. Everything needed to understand how to perform redox reactions is in the document and there are step-by-step fully solved problems in addition.
*HDDAAITH REEDDUUCCTT
" "
Short for redox reaction
considered transfer of electrons
e-
- →
A B
oxidation :
reduction :
loss of electron
gain of electron
due to transfer the ions get
charged and At B- come
together
In equation expression : HALF REACTION
REDUCTION ( gain electron) OX1DATO1aosselectron)_
+
B + e- → B- A → A- + e-
↳ written on the
losing so getting t
right-side "
spit out
"
you need to write
it on the side separated
right
from the ion
example : catty, #
0022 →
¢0022 # THE
hydrogen bonded to nonmetal >
r
=
positive charge
-
( (4) to ( (4-1) meaning oxidation of methane as
goes from
a whole
, -11 #
ccuuccllzz -
☒ A- 1181133 # Ccuu
gaining
pure element
electrons
☐
-
compound
= reduction RED#
+2 -2 +3 -3
-
I +
Cuclz -1>
Alclztcu
1
losing electrons
= oxidation
$0033 80033¥
5+1-67=04 C. + C- 6) = -67
50g COZZ
-
5=+6
↳ -2.3=-6 ↳ -2.3=-6
11¥04 Birra
11-+1-21=2 # Br -1C D= It
-
Hath Bra
↳ -1.2=-2 Li> -1.1=-1
HzPOy+(+ 1) = -
l
or
cause Ogmore electronegative Na:/ +
[Rule6:sum=O
Poy 1.1=1 7
all# $0044
-0-2
13+(1-1) -14.23+(-2-4)=0
P -11+2-8--0
H :
p :g+
it
To aHzpOg 10=+5 0:3 -
P-14C 2) =-3 -
↳ 1.2=2
Pt -8 =-3
D= -15
ALLREDOX SOMETIMES NEVER
Combustion Synthesis Double Replacement
Single Replacement combination
•
Acid Base
-
Decomposition •
Precipitation
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