Total number of species from the following which can undergo disproportionation reaction _______.
$\text{H}_2\text{O}_2, \text{ClO}_3^-, \text{P}_4, \text{Cl}_2, \text{Ag}, \text{Cu}^{+1}, \text{F}_2, \text{NO}_2, \text{K}^+$
$\text{H}_2\text{O}_2, \text{ClO}_3^-, \text{P}_4, \text{Cl}_2, \text{Ag}, \text{Cu}^{+1}, \text{F}_2, \text{NO}_2, \text{K}^+$
Correct Answer: 6
Solution and Explanation
A disproportionation reaction is a type of redox reaction where a single substance is simultaneously oxidized and reduced, forming two different products. Only species in an intermediate oxidation state can undergo such reactions.
The given species are analyzed as follows:
- H2O2 (Hydrogen peroxide) undergoes disproportionation to form water (H2O) and oxygen (O2).
- ClO3- (Chlorate ion) does not commonly undergo disproportionation.
- P4 (Phosphorus) can undergo disproportionation, forming phosphoric acid and phosphine in acidic conditions.
- Cl2 (Chlorine) can disproportionate to form chloride (Cl-) and hypochlorite (ClO-).
- Ag (Silver) in metallic form does not undergo disproportionation.
- Cu+ (Copper(I) ion) undergoes disproportionation to form copper(II) (Cu2+) and copper metal (Cu).
- F2 (Fluorine) does not undergo disproportionation as it is the most electronegative element.
- NO2 (Nitrogen dioxide) undergoes disproportionation to form nitric acid (HNO3) and nitric oxide (NO).
- K+ (Potassium ion) does not undergo disproportionation as it is already in a stable oxidation state.
From the list, the species that can undergo disproportionation reactions are:
H2O2, P4, Cl2, Cu+, NO2
Total number of species = 6.
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