Valence Bond Theory

Which of the following plot represents potential energy of a pair of nuclei as a function of their separation:

In which of the following species, the underlined carbon atom is  ${\mathrm{sp}}^{\text{3}}$ hybridised?

$\mathrm{Pz}$ and $\mathrm{dyz}$ form which bond at $\mathrm{x}$ axis?

The number of $\sigma$ bonds, $\mathrm{\pi }$ bonds and lone pair of electrons in pyridine, respectively.

The species having ${\mathrm{sp}}^3\mathrm{d}$ hybradisation is/are:

How does percentage $\mathrm{s}$character afftect the bond angle?

$\mathrm{What} \mathrm{is} \mathrm{the} \%\mathrm{p} \mathrm{character} \mathrm{in} \mathrm{carbon} \mathrm{which} \mathrm{is} \mathrm{bonded} \mathrm{doubly} \mathrm{with} \mathrm{another} \mathrm{carbon}.$

Explain valance bond theory.

Identify the orbital hybridization at the two indicated carbons in the molecule below:

Draw the sigma bond structure for ${\mathrm{NH}}_3 \mathrm{and} {\mathrm{CH}}_4$

Find the % of  ${\mathrm{p}}_{\mathrm{x}}$ orbital in $\mathrm{sp}$ hybridisation.

The molecule which contains ${\mathrm{\sigma }}_{{\mathrm{sp}}^3-{\mathrm{sp}}^3}$ and ${\mathrm{\sigma }}_{{\mathrm{sp}}^3-\mathrm{p}}$ bonds in it is

In which of the following $\mathrm{N}$ is in the ${\mathrm{sp}}^2$ hybridised state.

There are $\mathrm{x}$ number of $\mathrm{\pi }$ bonds and $\mathrm{y}$ number of $\mathrm{\sigma }$ bonds present in the compound given below :

The value of $\frac{\mathrm{x}+\mathrm{y}}{2}$ is

Match the following.

The correct match is

Find the number of molecules or ions in which d orbitals is/are not used in hybridisation

${\mathrm{PCl}}_6^{-}, {\mathrm{PCl}}_4^{+}, {\mathrm{IF}}_{4,}^{-} {\mathrm{IF}}_5^{}, {\mathrm{XeO}}_3{\mathrm{F}}_2, {\mathrm{ICl}}_2^{+}, {\mathrm{SF}}_{2,} {\mathrm{SF}}_6, {\mathrm{ASF}}_4^{+}, {\mathrm{SiF}}_4$

A single bond is always a '$\mathrm{\sigma }$' bond where as multiple bonds contain bolh $\mathrm{\sigma }$ and $\mathrm{\pi }$ bonds. A double bond contains one $\mathrm{\sigma }$ and and one $\mathrm{\pi }$ bond whereas a triple bond contain one $\mathrm{\sigma }$ and $2 \mathrm{\pi }$ bonds. On basis of this statement calculate $\mathrm{\sigma }$ and $\mathrm{\pi }$ bonds in $\mathrm{HC}\equiv \mathrm{C}-\mathrm{CH}={\mathrm{CH}}_3$.