(a)     (i) Write the disproportionation reaction of H_{3}PO_{3}.

          (ii) Draw the structure of XeF_{4}

(b) Account for the following:

        (i) Although Fluorine has less negative electtron gain enthalpy yet F2 is styrong oxidizing agent.

        (ii) Acidic character decreases from N2O3 to Bi2O3 in group 15.

(c) Write a chemical reaction to test sulphur dioxide gas. Write chemical eqaution involved.

 

 

 

 

 
 
 
 
 

Answers (1)

(a) (i) 4H_{3}PO_{3}\rightarrow 3H_{3}PO_{4}+PH_{3}

(ii) 

(b) (i) Fluorine is the strongest oxidising agent because of:

  • F2 has low enthalpy of dissociatiation.
  • F2 has high free energy of hydration.

(ii) The oxides E2O3 of N and P are acidic. As amphoteric and those of Bi basic beacuse the metallic character of the element and hence the basicity of its oxide increases with increasing atomic number.

(c) K_{2}Cr_{2}O_{7}+3SO_{2}+H_{2}SO_{4}\rightarrow Cr_{2}(SO_{4})_{3}+K_{2}SO_{4}+H_{2}O

SO2 turns a filter paper moistened with acidified potassium dichromate solution green, due to the formation of Cr^{3+} and acts as a reducing agent.

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