Among the following species, the H - X - H bo | vedclass

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(D) The bond angles for the given species are as follows:$1$. $PH_3$: The bond angle is approximately $93.5^\circ$ due to the absence of hybridization

Vedclass · Accepted Answer

$PH_3 < NH_3 < NH_4^+$

Vedclass · Answer

(D) The bond angles for the given species are as follows:$1$. $PH_3$: The bond angle is approximately $93.5^\circ$ due to the absence of hybridization and the presence of a lone pair.$2$. $NH_3$: The bond angle is $107^\circ$ due to $sp^3$ hybridization with one lone pair.$3$. $NH_4^+$: The bond angle is $109.5^\circ$ due to $sp^3$ hybridization with no lone pair, resulting in a perfect tetrahedral geometry.$4$. $BF_3$: This molecule does not contain $H - X - H$ bonds, so it cannot be compared in this series.Comparing the bond angles of the hydrides: $PH_3 (93.5^\circ) Therefore, the correct order is $PH_3 < NH_3 < NH_4^+$.

Among the following species, the $H - X - H$ bond angle $(X = B, N, \text{ or } P)$ follows the order:

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