. Complete the following chemical reaction equations


(a) Complete the following chemical reaction equations

chemical reaction equations

(b) Explain the following observations:

(i) Sulphur in vapour state exhibits paramagnetic behaviour.

(ii) The stability of +3 state increases down the group in group 15 of the periodic table.

(iii) XeF2 has a linear shape and not a bent structure

                                                                         OR

(a) Complete the following chemical reaction equations:

chemical reaction equations

(b) Explain the following observations:

(i) H2S is less acidic than H2Te

(ii) Fluorine is a stronger oxidising agent than chlorine

(iii) Noble gases are the least reactive elements

Best Answer

equations

(b) (i) Sulphur in vapour state exhibits paramagnetic behaviour because it forms S2 molecules like O2 which contains two unpaired electrons.

     (ii) The stability of +3 state increases down the group in group 15 due to inert pair effect.

    (iii) This is due to presence of two bond pairs and three lone pairs of electrons in XeF2

                                                                                                 OR

equations

(b) (i) This is because bond dissociation enthalpy of H–Te bond is less than H–S as the size of Te is larger than S.

(ii) Fluorine is a stronger oxidising agent than chlorine due to low dissociation enthalpy of F–F bond and high hydration enthalpy of F ions.

(iii) Noble gases are the least reactive elements due to fully filled outermost shells and zero electron gain enthalpy.

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