Question
Choose the correct option as directed.
A.
$$CsH < KH < NaH < LiH$$ ( Order of reducing strength )
B.
$${H_2}O < N{H_3} < C{H_4}$$ ( Order of dipole moment )
C.
$$P{H_3} < As{H_3} < N{H_3} < Sb{H_3}$$ (Order of boiling point)
D.
$$X - H - X,X = O > F > N > S > Cl$$ ( Order of strength of $$H$$ - bonding )
Answer :
$$P{H_3} < As{H_3} < N{H_3} < Sb{H_3}$$ (Order of boiling point)
Solution :
$$CsH > KH > NaH > LiH$$
The reducing strength of the alkali metal hydrides increases down the group.
$$C{H_4} < N{H_3} < {H_2}O$$
Dipole moment depends upon the difference between the electronegativities of the bonded atoms, and the internuclear separation.
$$P{H_3} < As{H_3} < N{H_3} < Sb{H_3}$$
Boiling point increases with an increase in molecular mass,
$$N{H_3}$$ being an exception because of strong hydrogen bonding.
$$Cl < S < N < O < F$$
The strength of hydrogen bonding depends upon the electronegativity and the size. Higher electronegativity and smaller size increases the strength of hydrogen bonding.