Chemical bonding & molecular structure practice · Mixed difficulty

Which species has lone pair on central atom?

Consider the following statements.

I. In $F_2$ molecule $F - F\,\,\,\sigma - {\text{bond}}$ is formed by axial overlapping of two p-orbitals.

II. In $O_2$ molecule one $\sigma - {\text{bond}}$ is formed by axial overlap of p-orbitals and one $\pi - {\text{bond}}$ is formed by lateral overlap of p-orbitals.

III. In $N_2$ molecule one $\sigma$ and two $\pi - {\text{bonds,}}$ i.e., all the three bonds are formed by lateral overlap of p-orbitals.

Which of the above statements are incorrect?

The correct order of hybridization of the central atom in the following species $\mathrm{N}{\mathrm{H}_3},{\left[ {\mathrm{PtC}{\mathrm{l}_4}} \right]^{2 - }},\mathrm{PC}{\mathrm{l}_5}$ and $\mathrm{BC}{\mathrm{l}_3}$ is:

In which of the following dative bond is not present

In the formation of a molecule by an atom

Which of the following set contains same bond angle around central atom?

In case of $\mathrm{H}_2 \mathrm{O}$ molecule, the enthalpy needed to break the two $\mathrm{O}-\mathrm{H}$ bonds is not the same, i.e.

$\begin{aligned} & \mathrm{H}_2 \mathrm{O}(\mathrm{g}) \longrightarrow \mathrm{H}(\mathrm{g})+\mathrm{OH(g}) ; \Delta_\mathrm{a} \mathrm{H}_1^{\mathrm{S}}=502 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \mathrm{OH}(\mathrm{g}) \longrightarrow \mathrm{H}(\mathrm{g})+\mathrm{O}(\mathrm{g}) ; \Delta_\mathrm{a} \mathrm{H}_2^{\mathrm{S}}=427 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$

What should be the mean bond enthalpy of $\mathrm{O}-\mathrm{H}$ bonds in case of $\mathrm{H}_2 \mathrm{O}$ molecule?

Which statement is wrong?

Among the following, the molecule expected to be stabilised by anion formation is ${C_2},\,{O_2},\,NO,\,{F_2}.$

Among the following molecules which one have smallest bond angle

The number of species below that have two lone pairs of electrons in their central atom is.
$S{F_4},\,\,\,BF_4^ - ,\,\,\,Cl{F_3},\,\,\,As{F_3},\,\,\,PC{l_5},\,\,\,Br{F_5},\,\,\,Xe{F_4},\,\,\,S{F_6}$

The bond strength in $\mathrm{O}_2^ + ,{\mathrm{O}_2},\mathrm{O}_2^ -$ and $\mathrm{O}_2^{2 - }$ follows the order:

Select which type of overlapping is responsible for $\pi$-character in ${Si}-{N}$ bond of ${H}_3 {SiNCO}$

The pair having similar geometry is:

In which of the following compound $s{p^2}$ hybridisation is absent?

Dipole moment is shown by

Given below are two statements:

Statement I: $\mathrm{PF}_5$ and $\mathrm{BrF}_5$ both exhibit $\mathrm{sp}^3 \mathrm{d}$ hybridisation.

Statement II: Both $\mathrm{SF}_6$ and $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+}$ exhibit $\mathrm{sp}^3 \mathrm{d}^2$ hybridisation.

In the light of the above statements, choose the correct answer from the options given below:

The decreasing order of bond dissociation energies of $\mathrm{C}-\mathrm{C}, \mathrm{C}-\mathrm{H}$ and $\mathrm{H}-\mathrm{H}$ bonds in

Among the following the molecule with the highest dipole moment is

Which of the following is a polar molecule?

Which one of the following constitutes a group of the isoelectronic species?

The value of electronegativity of atoms A and B are 1.20 and 4.0 respectively. The percentage of ionic character of $\mathrm{A}-\mathrm{B}$ bond is:

In allene structure, three carbon atoms are joined by:

Some of the properties of the two species, $\mathrm{NO}_3^ -$ and ${\mathrm{H}_3}{\mathrm{O}^ + }$ are described below. Which one of them is correct?

Which is expected to have linear structure?

Which does not use $s{p^3}$-hybrid orbitals in its bonding?

In which of the following crystals of ionic compounds would you expect maximum distance between the centres of cotions and anions

Which of the following pairs are isostructural?

Assertion : The ${O}-{O}$ bond length in ${H}_2 {O}_2$ is shorter than that of ${O}_2 {~F}_2$.

Reason: ${H}_2 {O}_2$ is an ionic compound.

Bond formed due to complete transfer of electron is