Calculation of Net Dipole Moment and its Applications

Which compounds exhibits maximum dipole moment among the following?

The percent ionic character in $\mathrm{HCl}$ is $22.05 .$The observed dipole moment is $1.08 \mathrm{D}$. Find the inter-nuclear distance in $\mathrm{HCl}$.

Give the nearest integer as the answer.

What is the $\%$ covalent character if the bond length and dipole moment of $\mathrm{HBr}$ are $1.41\stackrel{\mathrm{o}}{\mathrm{A}}$ and $2.6\times {10}^{-30}\mathrm{ }\mathrm{e}.\mathrm{s}.\mathrm{u} \mathrm{cm}$ respectively?

Dipole moment of a bond is a vector and physical quantity to calculate the percentage ionic character in a covalent bond. It is expressed as:

Dipole moment $\left(\mathrm{\mu }\right)=\underset{\mathrm{\delta }\times \mathrm{d}}{\to }$ where, $\delta$ is dipole moment and $d$ is the bond length. It is usually expressed in terms of C.G.S. unit known as Debye (D) $1\mathrm{D}={10}^{-18}$ esu cm. In S.I. unit it is expressed in coulomb metre. Resultant dipole moment $\left({\mathrm{\mu }}_{\mathrm{R}}\right)$of two bond moments $\left({\mathrm{\mu }}_1 \mathrm{and} {\mathrm{\mu }}_2\right)$ acting at an angle $\mathrm{\theta }$, is given by:

${\mathrm{\mu }}_{\mathrm{R}}=\sqrt{{{\mathrm{\mu }}_1}^2+{{\mathrm{\mu }}_2}^2+2{\mathrm{\mu }}_1{\mathrm{\mu }}_2\cos \left(\mathrm{\theta }\right)}$

$\text{ If }{\mathrm{\mu }}_1={\mathrm{\mu }}_2,\text{ Also if }\mathrm{cos\theta }=-1,\text{ ie, }\mathrm{\theta }=180°,\text{ then }\mathrm{\mu }=0$ (molecule is non-polar)

If $\mu \neq 0$ molecule is polar. Dipole moment plays an important role in deciding the stability order of alkanes,i.e., a more stable alkane has less dipole moment. The dipole moment of a molecule can predict the geometrical and position isomers as well as orientations in benzene nucleus and polarity of molecule.

Dipole moment of $\mathrm{HCl}$ molecule is found to be $0.816 \mathrm{D}$. Assuming $\mathrm{HCl}$ bond length to be equal to $1 \mathrm{\AA }$, the '$\%$ ionic character of $\mathrm{HCl}$ molecule is:

The dipole moment of  is 1.5 D . The dipole Moment  ofin Debye is $\mathrm{\lambda }. \mathrm{Then} \mathrm{the} \mathrm{value} \mathrm{of} 2\mathrm{\lambda } \mathrm{is}$

Choose the correct statement from the following

The experimental value of the dipole moment of $\mathrm{HCl}$ is $1.03\hspace{0.17em}\mathrm{D}$. The length of the $\mathrm{H}-\mathrm{Cl}$ bond is $1.275\mathrm{Å}$ . The percentage of ionic character in $\mathrm{HCl}$ is:
[Given: $1\mathrm{\text{D}}={10}^{-18}\text{esu}\text{cm}$]

The net dipole moment of $\mathrm{A}-{\mathrm{C}\mathrm{H}}_2-{\mathrm{C}\mathrm{H}}_2-\mathrm{A}$ , if the dipole moment of its gauche form is 5D and mole fraction of anti-form is 0.7 is:

Experiment shows that $H_{2}O$ has a dipole moment while $C{O}_2$ has not. Point out the structure which best illustrates these facts

${\mathrm{H}}_2\mathrm{O}$ is dipolar, whereas ${\mathrm{BeF}}_2$ is not. It is because:

The dipole moment of $\mathrm{\prime }\mathrm{O}-\mathrm{H}\mathrm{\prime }$ bond and $\mathrm{\prime }\mathrm{O}-\mathrm{D}\mathrm{\prime }$ bond is 'X' and 'Y' respectively. If ${\mathrm{\mu }}_{\mathrm{n}\mathrm{e}\mathrm{t}}$ of ${\mathrm{H}}_2\mathrm{O}{=}^{\mathrm{\prime }}{\mathrm{Z}}^{\mathrm{\prime }}$ Debyes, then ${\mathrm{\mu }}_{\mathrm{n}\mathrm{e}\mathrm{t}}$ of ${\mathrm{D}}_2\mathrm{O}$ will be? Consider the same effect of lone pair on dipole moment of both molecules. (Assuming bond angle of ${\mathrm{H}}_2\mathrm{O}$ and ${\mathrm{D}}_2\mathrm{O}=\mathrm{\theta }$ and $\cos \mathrm{\theta }=-0.24)$

You have been given two species $\mathrm{N}\mathrm{O}\mathrm{F}$ and ${\mathrm{N}\mathrm{O}}_2\mathrm{F}$ and two dipole moments $1.81\mathrm{ }\mathrm{D}$ and $0.47\mathrm{ }\mathrm{D}$. The correct set is:

Calculate the dipole moment $\left(\text{μ}\right)$ of

If ${\text{μ}}_{\text{C}-\text{Cl}}=\text{1.55}D\; and{\text{μ}}_{\text{C}-{\text{NO}}_2}=\text{3.95 D}$.

You have given two species$–\mathrm{N}\mathrm{O}\mathrm{F}$ and ${\mathrm{N}\mathrm{O}}_2\mathrm{F}$ and two dipole moments 1.81 D and 0.47 D :

Increasing order of dipole moment is-

Which of the following compounds are non-polar ?

Which of the following compounds has dipole moment approximately equal to that of chlorobenzene?

The dipole moment of $\mathrm{H}\mathrm{B}\mathrm{r}$ is $1.6\times {10}^{-30}$C-m and interatomic spacing is $1Å$. The % ionic character of HBr is

If the dipole moment of Toluene and Nitro-benzene are $0.43$ D and $3.93$D respectively, then what is the expected dipole moment of p-Nitrotoluene?

If the molecule of $\mathrm{HCl}$ were totally polar, the expected value of dipole moment is $6.12 \mathrm{D}$ (debye). However, the experimental value of dipole moment was $1.03 \mathrm{D}$. Calculate the percentage ionic character