The Valence Shell Electron Pair Repulsion (VSEPR) Theory

Give an example of a compound which has six bond pairs and one lone pair.

The shape of ${\mathrm{XeF}}_6$ is 

Explain the Geometry of ${\mathrm{XeF}}_6$.

The $F-Br-F$ bond angles in $Br{F}_5$ and the $Cl-P-Cl$ bond angles in $PC{l}_5$, respectively, are

Which of the molecules has trigonal bipyramidal geometry with bond angles 120 ° and 90 °?

Due to_____ the deviations occurs from idealized shape of ${\mathrm{H}}_2\mathrm{O}$ and ${\mathrm{NH}}_3$ molecules. (attractive effect/repulsive effect)

Which statement about noble gases is not correct?

Identify the molecule which contains lone pair of electrons on the sulphur atom

Which set of the following molecules has only one lone pair of electrons on their respective central atoms?

a) ${\mathrm{SO}}_2$

b) ${\mathrm{XeF}}_4$

c) ${\mathrm{PbCl}}_2$

d) ${\mathrm{SF}}_4$

e) ${\mathrm{ClF}}_3$

Identify the correct statements

Among

(i) ${\mathrm{XeO}}_3,$ 

(ii) ${\mathrm{XeOF}}_4$ and

(iii) ${\mathrm{XeF}}_6,$ those having the same number of lone pairs on the central atom are _________

Which of the following species has a square planar geometry?

The shape of ${\mathrm{XeF}}_4$ molecule is based on the fact that it has

According to VSEPR theory, the correct order of repulsion is

Molecular shapes of ${\mathrm{SF}}_4, {\mathrm{CF}}_4, {\mathrm{XeF}}_4$ are

Assertion. $\mathrm{H}-\mathrm{S}-\mathrm{H}$ bond angle in ${\mathrm{H}}_2\mathrm{S}$ is closer to $90°$ but $\mathrm{H}-\mathrm{O}-\mathrm{H}$ bond angle in ${\mathrm{H}}_2\mathrm{O}$ is $104.5°$.

Reason. lp-lp repulsion is stronger in ${\mathrm{H}}_2\mathrm{S}$ than in ${\mathrm{H}}_2\mathrm{O}$.

Non-linear species among the following is:

Consider the structure of ${\mathrm{ClF}}_3$, the number of significant repulsion $\mathrm{lp}-\mathrm{lp}=x, \mathrm{lp}-\mathrm{bp}=y, \mathrm{bp}-\mathrm{bp}=z\mathit{,}$ then $\mathrm{x}+\mathrm{y}+\mathrm{z}=?$

The option having the correct order of bond angle is:

For ${\mathrm{XeOF}}_4$, calculate x+y+z if $x$ is the total number of bond pairs around $\mathrm{Xe}$, $\mathrm{y}$ is the total number of lone pairs on all atoms and $z$ is the total number of ${90}^{° }\mathrm{OXeF}$ angles.