Question

Total number of species from the following which can undergo disproportionation reaction _______.
$\text{H}_2\text{O}_2, \text{ClO}_3^-, \text{P}_4, \text{Cl}_2, \text{Ag}, \text{Cu}^{+1}, \text{F}_2, \text{NO}_2, \text{K}^+$

Answer 1

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:

• H 2O2 (Hydrogen peroxide) undergoes disproportionation to form water (H2O) and oxygen (O2).
• ClO 3- (Chlorate ion) does not commonly undergo disproportionation.
• P 4 (Phosphorus) can undergo disproportionation, forming phosphoric acid and phosphine in acidic conditions.
• Cl 2 (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).
• F 2 (Fluorine) does not undergo disproportionation as it is the most electronegative element.
• NO 2 (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:

H 2O2, P4, Cl2, Cu+, NO2

Total number of species = 6.