Question
Which of the following statement is wrong?
A.
The stability ofhydride increases from $$N{H_3}\,{\text{to}}\,Bi{H_3}$$ in group $$15$$ of the periodic table.
B.
Nitrogen cannot form $$d\pi - p\pi $$ bond.
C.
Single$$N - N$$ bond is weaker than the single $$P - P$$ bond.
D.
$${N_2}{O_4}$$ has two resonance structures.
Answer :
The stability ofhydride increases from $$N{H_3}\,{\text{to}}\,Bi{H_3}$$ in group $$15$$ of the periodic table.
Solution :
The ease of formation and stability of hydrides decreases rapidly from $$N{H_3}\,{\text{to}}\,Bi{H_3}.$$ This is evident from their dissociation temperature which decreases from $$N{H_3}\,{\text{to}}\,Bi{H_3}.$$ As we go down the group the size of central atom increases and thus metal-hydrogen bond becomes weaker due to decreased overlap between the large central atom and small hydrogen atom.
$$\mathop {N{H_3} > P{H_3}}\limits_{{\text{(most stable)}}} > As{H_3} > Sb{H_3} > \mathop {Bi{H_3}}\limits_{{\text{(least stable}})} $$