What are the successes and failures of the Lewis theory in explaining chemical bonding?
(N/A) The Lewis approach is successful in explaining the sharing of electrons between atoms to form covalent bonds and the formation of simple molecules.
However,it fails to explain the following:
$1$. It does not explain the shape of polyatomic molecules.
$2$. It does not provide information about the energy of the bond (bond enthalpy) or the bond length.
$3$. It fails to explain the stability of molecules based on the electronic configuration.
However,it fails to explain the following:
$1$. It does not explain the shape of polyatomic molecules.
$2$. It does not provide information about the energy of the bond (bond enthalpy) or the bond length.
$3$. It fails to explain the stability of molecules based on the electronic configuration.
Explore More
Similar Questions
Assertion : The $S-S-S$ bond angle in $S_8$ molecule is $105^o$.
Reason : $S_8$ has a $V$-shape.
Reason : $S_8$ has a $V$-shape.
In the following electron-dot structure, calculate the formal charge from left to right for the nitrogen atoms: $: \ddot{N} = N = \ddot{N} :$
MediumWBJEE 2011
View Solution$XeF_4$ has a total of $36$ valence electrons. Select the correct statement regarding the use of valence electrons in $XeF_4$.
Medium
View SolutionWhich of the following is $NOT$ likely to act as a Lewis base?
Easy
View SolutionThe number of sigma $(\sigma)$ and pi $(\pi)$ bonds in peroxodisulphuric acid are, respectively:
Vedclass 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