Experiment shows that $H_2O$ has a dipole moment while $CO_2$ does not. Point out the structures which best illustrate these facts.
- A$O=C=O$ ; $H-O-H$ (Bent)
- B$O=C=O$ ; $H-O-H$
- C$O=C=O$ (Bent) ; $H-O-H$
- D$O=C=O$ (Bent) ; $H-O-H$ (Bent)
Explore More
Similar Questions
If $H-X$ bond length is $2 \ \mathring{A}$ and $H-X$ has dipole moment $5.12 \times 10^{-30} \ C \cdot m$,the $\%$ of covalent character of the molecule is ............. $\%$
Medium
View SolutionThe correct order of dipole moments of $NH_3$,$H_2O$ and $NF_3$ is
Explain the dipole moment of a triatomic molecule $(AB_2)$.
Difficult
View SolutionIf $Q$ is the magnitude of charge and $r$ is the distance between the centres of positive and negative charges,then the dipole moment $(\mu)$ is given by:
Match the compounds given in List-$I$ with their dipole moments given in List-$II$.
List-$I$ List-$II$ $(1)$ ${\rm{HBr}}$ $(A)$ $0.23$ $(2)$ ${{\rm{H}}_2}{\rm{S}}$ $(B)$ $1.04$ $(3)$ ${\rm{N}}{{\rm{F}}_3}$ $(C)$ $1.07$ $(4)$ ${\rm{CC}}{{\rm{l}}_4}$ $(D)$ $0.79$ $(5)$ ${\rm{CHC}}{{\rm{l}}_3}$ $(E)$ $0.00$ $(F)$ $0.95$
| List-$I$ | List-$II$ |
| $(1)$ ${\rm{HBr}}$ | $(A)$ $0.23$ |
| $(2)$ ${{\rm{H}}_2}{\rm{S}}$ | $(B)$ $1.04$ |
| $(3)$ ${\rm{N}}{{\rm{F}}_3}$ | $(C)$ $1.07$ |
| $(4)$ ${\rm{CC}}{{\rm{l}}_4}$ | $(D)$ $0.79$ |
| $(5)$ ${\rm{CHC}}{{\rm{l}}_3}$ | $(E)$ $0.00$ |
| $(F)$ $0.95$ |
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