Account for the following : (i) Tendency to show –3 oxidation sta

1.	Account for the following : (i) Tendency to show –3 oxidation state decreases from N to Bi in group 15. (ii) Acidic character increases from H2O to H2Te. (iii) F2 is more reactive than CIF3, whereas CIF3 is more reactive than Cl2.
Answer» (i) The tendency to exhibit –3 oxidation state decreases down the group due to increase in size and metallic characters. (ii) Acidic character increases from H₂O to H₂Te because decrease in bond enthalpy for the dissociation of H – E bond down the group. (iii) F – F bond is weaker than Cl–F bond due to small size and high electron density, more repulsion between fluorine atoms therefore F₂ is more reactive than ClF₃. Where as When we compare to Cl₂, with ClF₃,Cl – Cl bond is stronger than ClF₃. Therefore ClF₃ is more reactive than Cl₂

Account for the following : (i) Tendency to show –3 oxidation state decreases from N to Bi in group 15. (ii) Acidic character increases from H2O to H2Te. (iii) F2 is more reactive than CIF3, whereas CIF3 is more reactive than Cl2.

Answer»

(i) The tendency to exhibit –3 oxidation state decreases down the group due to increase in size and metallic characters.

(ii) Acidic character increases from H₂O to H₂Te because decrease in bond enthalpy for the dissociation of H – E bond down the group.

(iii) F – F bond is weaker than Cl–F bond due to small size and high electron density, more repulsion between fluorine atoms therefore F₂ is more reactive than ClF₃. Where as When we compare to Cl₂, with ClF₃,Cl – Cl bond is stronger than ClF₃. Therefore ClF₃ is more reactive than Cl₂

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