Which of the following statement is true with respect to H2O, NH3 and CH4 ?
(A) The central atoms of all the molecules are sp3 hybridized.
(B) The H–O–H, H–N–H and H–C–H angles in the above molecules are
104.5°, 107.5° and 109.5°, respectively.
(C) The increasing order of dipole moment is CH4 < NH3 < H2O.
(D) Both H2O and NH3 are Lewis acids and CH4 is a Lewis base.
(E) A solution of NH3 in H2O is basic. In this solution NH3 and
H2O act as Lowry–Bronsted acid and base respectively.
Explanation
In H2O, NH3 and CH4, the central atom is sp3 hybridized.
Bond angles decrease due to lone pair–lone pair and lone pair–bond pair repulsions.
CH4 is non-polar, NH3 is polar and H2O has the highest dipole
moment.
NH3 acts as a Bronsted base and H2O acts as a Bronsted acid,
hence statement (E) is incorrect.