State the hybridization and draw the structures of $PCl_3$ and $PCl_5$.
(N/A) For $PCl_3$: The central phosphorus atom is $sp^3$ hybridized. It has $3$ bond pairs and $1$ lone pair,resulting in a trigonal pyramidal geometry.
For $PCl_5$: The central phosphorus atom is $sp^3d$ hybridized. It has $5$ bond pairs and $0$ lone pairs,resulting in a trigonal bipyramidal geometry.
For $PCl_5$: The central phosphorus atom is $sp^3d$ hybridized. It has $5$ bond pairs and $0$ lone pairs,resulting in a trigonal bipyramidal geometry.
Explore More
Similar Questions
What is the state of hybridisation of carbon in $(a)$ $CO_3^{2-}$,$(b)$ diamond,and $(c)$ graphite?
Medium
View SolutionThe geometry of the molecule with $sp^3d^2$ hybridised central atom is
Easy
View SolutionIn which of the following molecules/ions $BF_3$,$NO_2^-$,$NH_2^-$ and $H_2O$,the central atom is $sp^2$ hybridised?
DifficultAIPMT 2009
View SolutionIn which of the following molecules is the $N$ atom not $sp^2$ hybridized?
Medium
View SolutionWhich of the following pairs has the same bond angle?
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo