Interactions | Reactions | Processes

Classified as: Disproportionation

An internal redox reaction where a specific centre, X, is an intermediate oxidation state splits to become both more oxidised and more reduced.

4
H2N–OH
  +  
H+
         
N2O
  +  
2
NH3
  +  
3
H2O

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3
H2N–OH
  +  
[OH]–
         
N2
  +  
NH3
  +  
3
H2O

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2
  +  
H2O
  +  
[OH]–
         
  +  

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3
HN3
  +  
2
Na
         
2
NaN3
  +  
NH3
  +  
N2

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5
PF3
  +  
5
Br2
         
3
PF5
  +  
2
PBr5

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2
HOOH
         
2
H2O
  +  
O2

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Cl2
  +  
H2O
         
HClO
  +  
HCl

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Cl2
  +  
[OH]–
         
[ClO]–
  +  
Cl–
  +  
H+

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3
[IO]–
         
[IO3]–
  +  
2
I–

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3
[ClO]–
         
[ClO3]–
  +  
2
Cl–

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3
[BrO]–
         
[BrO3]–
  +  
2
Br–

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5
[ClO2]–
  +  
4
H+
         
4
ClO2
  +  
Cl–
  +  
2
H2O

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4
HClO3
         
4
ClO2
  +  
O2
  +  
2
H2O

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6
NaOH
  +  
3
Cl2
         
NaClO3
  +  
5
NaCl
  +  
3
H2O

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4
KClO3
         
3
KClO4
  +  
KCl

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2
Na+
  +  
2
[HXeO4]–
  +  
2
NaOH
         
4
Na+
  +  
[XeO6]4–
  +  
Xe
  +  
O2
  +  
2
H2O

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2
Rb+
  +  
2
[XeF7]–
         
2
Rb+
  +  
[XeF8]2–
  +  
XeF6

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2
Cs+
  +  
2
[XeF7]–
         
2
Cs+
  +  
[XeF8]2–
  +  
XeF6

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2
HCHO
  +  
NaOH
  +  
H2O
         
CH3OH
  +  
HCOONa

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2
  +  
NaOH
  +  
H2O
         
  +  
  +  
Na+

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  +  
HCHO
  +  
NaOH
  +  
H2O
         
  +  
HCOONa

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  +  
2
H+
         
S
  +  
SO2
  +  
H2O

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Na2S2O3
  +  
2
HCl
         
S
  +  
SO2
  +  
2
NaCl
  +  
H2O

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4
         
  +  
  +  
2

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  +  

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3
SiF4
  +  
2
H2O
         
2
H2SiF6(aq)
  +  
SiO2

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3
Br2
  +  
6
[OH]–
         
[BrO3]–
  +  
5
Br–
  +  
3
H2O

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3
Br2
  +  
3
Na2CO3
         
5
NaBr
  +  
NaBrO3
  +  
3
CO2

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2
CH3–CH=CH2
         
H2C=CH2
  +  
  +  

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2
K+
  +  
2
  +  
CO2
         
  +  

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2
NH4NO3
  +  
C
         
2
N2
  +  
CO2
  +  
4
H2O

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3
[MnO4]2–
  +  
4
H+
         
2
[MnO4]–
  +  
MnO2
  +  
2
H2O

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© Mark R. Leach 1999 –

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