Discuss the shape of the following molecules | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(N/A) $BeCl_2$: The central atom has no lone pair and two bond pairs ($AB_2$ type). Hence,it has a linear shape.$BCl_3$: The central atom has no lone

Vedclass · Accepted Answer

Vedclass · Answer

(N/A) $BeCl_2$: The central atom has no lone pair and two bond pairs ($AB_2$ type). Hence,it has a linear shape.
$BCl_3$: The central atom has no lone pair and three bond pairs ($AB_3$ type). Hence,it is trigonal planar.
$SiCl_4$: The central atom has no lone pair and four bond pairs ($AB_4$ type). Hence,it is tetrahedral.
$AsF_5$: The central atom has no lone pair and five bond pairs ($AB_5$ type). Hence,it is trigonal bipyramidal.
$H_2S$: The central atom has two lone pairs and two bond pairs ($AB_2E_2$ type). Hence,it is bent or $V$-shaped.
$PH_3$: The central atom has one lone pair and three bond pairs ($AB_3E$ type). Hence,it is trigonal pyramidal.

Discuss the shape of the following molecules using the $VSEPR$ model: $BeCl_2, BCl_3, SiCl_4, AsF_5, H_2S, PH_3$.

Similar Questions

The $H-N-H$ angle in ammonia is $107.6^{\circ}$ while the $H-P-H$ angle in phosphine is $93.5^{\circ}.$ Relative to phosphine, the $p$-character of the lone-pair on ammonia is expected to be

The $F-Br-F$ bond angles in $BrF_5$ and the $Cl-P-Cl$ bond angles in $PCl_5$,respectively,are

Identify the number of molecules in which the central atom has one lone pair of electrons from the following list:
$PbCl_2, PH_3, ClF_3, SF_4, BF_3, SnCl_2$

The species having a pyramidal shape according to $VSEPR$ theory is:

The shapes of $XeF_4$,$XeF_5^-$ and $SnCl_2$ are

Vedclass Test Series

Exam Paper Generator

Online Exam Module