pBlock ElementsII 1 Question 64
59. Among the following, the correct statement is
(a) Between $\mathrm{NH}{3}$ and $\mathrm{PH}{3}, \mathrm{NH}_{3}$ is a better electron donor because the lone pair of electrons occupies spherical ’ $s$ ’ orbital and is less directional
(b) Between $\mathrm{NH}{3}$ and $\mathrm{PH}{3}, \mathrm{PH}_{3}$ is a better electron donor because the lone pair of electrons occupies $s p^{3}$-orbital and is more directional
(c) Between $\mathrm{NH}{3}$ and $\mathrm{PH}{3}, \mathrm{NH}_{3}$ is a better electron donor because the lone pair of electrons occupies $s p^{3}$-orbital and is more directional
(d) Between $\mathrm{NH}{3}$ and $\mathrm{PH}{3}, \mathrm{PH}_{3}$ is a better electron donor because the lone pair of electrons occupies spherical ’ $s$ ’ orbital and is less directional
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Solution:
- $\mathrm{NH}{3}$ is stronger Lewis base than $\mathrm{PH}{3}$. In a group of hydrides, basic strength decreases down the group.
