Compare the net dipole moment of ${\mathrm{NH}}_3$ and ${\mathrm{NF}}_3$.

Important Questions on Chemical Bonding and Structure

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

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: $1\mathrm{\text{D}}={10}^{-18}\text{esu}\text{cm}$]

MEDIUM

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

The polarity of $\left(\text{i}\right){\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}\text{P}{\left({\text{CF}}_{\text{3}}\right)}_{\text{3}}$ and $\left(\text{ii}\right){\left({\text{CH}}_{\text{3}}\right)}_{\text{3}}\text{P}{\left({\text{CF}}_{\text{3}}\right)}_{\text{2}}$ respectively are?

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Which of the following is an example of a planar molecule having a net dipole moment to be zero?

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

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

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Compare the theoretical dipole moments of BF₂Cl and BCl₂F.

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

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

MEDIUM

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

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

MEDIUM

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

The decreasing order of the bond moment of E-H bond in NH₃ , PH₃ , AsH₃ and SbH₃ is given by

MEDIUM

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Compare  the polarities on COCl₂ and COBr₂ ?

MEDIUM

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Select correct statement :

EASY

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Which are non-polar molecules?

I : ${\mathrm{NCl}}_3$;      II :${\mathrm{SO}}_3$;      III : ${\mathrm{PCl}}_5$

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Draw the shapes of $\mathrm{BeClF}$ and $\mathrm{BeBrF}$ and predict whether they are polar or non-polar. Compare the polarity of these two molecules.

MEDIUM

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

In the molecules ${\mathrm{BF}}_3$ and ${\mathrm{NF}}_3$, ${\mathrm{BF}}_3$ is non-polar and ${\mathrm{NF}}_3$ is polar. The reason is that

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

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:

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Which of the following species is non-polar ?

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Discuss the dipole moment of

EASY

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Cotyledons are also called-

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

Choose the correct statement from the following

HARD

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

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 $\cos \mathrm{\theta }=-0.24)$

EASY

Chemistry>Inorganic Chemistry>Chemical Bonding and Structure>Covalent Bond

The molecule which does not exhibit dipole moment is