. Complete the following chemical equations


(a) Complete the following chemical equations:

chemical

(b) How would you account for the following?

(i) The value of electron gain enthalpy with negative sign for sulphur is higher than that for oxygen.

(ii) NF3 is an exothermic compound but NCl3 is endothermic compound.

(iii) ClF3 molecule has a T-shaped structure and not a trigonal planar one

                                                     OR

(a) Complete the following chemical reaction equations:

chemical reaction equations

(b) Explain the following observations giving appropriate reasons:

(i) The stability of +5 oxidation state decreases down the group in group 15 of the periodic table.

(ii) Solid phosphorus pentachloride behaves as an ionic compound.

(iii) Halogens are strong oxidizing agents

Best Answer

Hot and conc

(i) Due to smaller size of oxygen the electron cloud is distributed over a small region of space, making electron density high which repels the incoming electrons.

(ii) This is due to lower bond dissociation enthalpy of F2 than Cl2 and comparable size of fluorine and nitrogen.

(iii) ClF3 molecule has a T-shaped structure. This is due to presence of two lone pairs in the outer shell of chlorine in ClF3 molecule which repel the bond pairs.

                                                                      OR

(a) Complete the following chemical reaction equations

P SO Cl 4 + 2 2

(b) (i) The stability of +5 oxidation state decreases down the group in group 15 of the periodic table. The + 3 oxidation state becomes more and more common on moving down the group from N to Bi. This is because of inert pair effect.

(ii) Solid PCl5 behaves as an ionic compound because it is a salt containing the tetrahedral cation [PCl4 ] + and octahedral anion [PCl6 ] .

(iii) Halogens are strong oxidising agents because they have high electron affinities, so, they pick up electrons from other substances.

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