Chemical Bonding Questions

Lattice energy of an ionic compound depends upon:

The molecular shapes of ${\text{SF}}_4$, ${\text{CF}}_4$ and ${\text{XeF}}_4$ are:

The number and type of bonds between two carbon atoms in calcium carbide are:

The structure of diborane (${\text{B}}_2{\text{H}}_6$) contains:

Which one of the following species is diamagnetic in nature?

In which of the following ionization processes, the bond order has increased and the magnetic behaviour has changed?

The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species, ${\text{K}}^{+},{\text{Ca}}^{2+},{\text{Mg}}^{2+},{\text{Be}}^{2+}$?

Which of the following species exhibits diamagnetic behaviour?

Which of the following hydrogen bonds is the strongest?

Which one of the following has a square planar geometry?

In which of the following molecules/ions are all the bonds not equal?

Which of the following molecules/ions does not contain unpaired electrons?

The maximum number of $90^{\circ }$ angles between bond pair of electrons is observed in:

Which one of the following has a regular tetrahedral structure?

The states of hybridization of boron and oxygen atoms in boric acid (${\text{H}}_3{\text{BO}}_3$) are respectively:

The bond order in $\text{NO}$ is $2.5$ while that in ${\text{NO}}^{+}$ is $3$. Which of the following statements is true for these two species?

The correct order of bond angles (smallest first) in ${\text{H}}_2\text{S},{\text{NH}}_3,{\text{BF}}_3$ and ${\text{SiH}}_4$ is:

Four species are listed below:(i) ${\text{HCO}}_3^{-}$ (ii) ${\text{H}}_3{\text{O}}^{+}$ (iii) ${\text{HSO}}_4^{-}$ (iv) ${\text{HSO}}_3\text{F}$ Which one of the following is the correct sequence of their acid strength?

Which one of the following pairs of species have the same bond order?

Using MO theory predict which of the following species has the shortest bond length?

The bond dissociation energy of $\text{B}-\text{F}$ in ${\text{BF}}_3$ is $646{\text{kJ mol}}^{-1}$ whereas that of $\text{C}-\text{F}$ in ${\text{CF}}_4$ is $515{\text{kJ mol}}^{-1}$. The correct reason for higher $\text{B}-\text{F}$ bond dissociation energy as compared to that of $\text{C}-\text{F}$ is:

Among the following the maximum covalent character is shown by the compound:

The hybridization of orbitals of N atom in ${\text{NO}}_3^{-}$, ${\text{NO}}_2^{+}$ and ${\text{NH}}_4^{+}$ are respectively:

The structure of ${\text{IF}}_7$ is:

The molecule having smallest bond angle is:

In which of the following pairs the two species are not isostructural?