Predict the correct order among the following.

(1) lone pair-lone pair>bond pair-bond pair>lone pair-bond pair

(2) bond pair-bond pair>lone pair-bond pair>lone pair-lone pair

(3) lone pair-bond pair>bond pair-bond pair>lone pair-lone pair

(4) lone pair-lone pair>lone pair-bond pair>bond pair-bond pair

The pair of electrons in the given carbanion, CH₃C≡C^-, is present in which of the following orbitals?

The incorrect statement among the following regarding the molecules of CH_4, NH₃, and H₂O is:

Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

1. Cl₂ > Br₂ > F₂ > I₂

2. Br₂ > I₂ > F₂ > Cl₂

3. F₂ > Cl₂ > Br₂ > I₂

4. I₂ > Br₂ > Cl₂ > F₂

Which of the following species contains equal number of $\mathrm{\sigma }$ and $\mathrm{\pi }$ bonds?

1. ${\mathrm{HCO}}_3^{-}$                                   

2. XeO₄

3. (CN)₂                                     

4. CH₂(CN)₂

Find the correct decreasing order of bond order among the following species:

The total number of $\mathrm{\pi }$-bond electrons in the following structure is :

1. 4       

2. 8         

3. 12         

4. 16

In which of the following pairs, both the species are not isostructural?

1. ${\mathrm{SiCl}}_4,<mspace\; width="1em"></mspace>{\mathrm{PCl}}_4^{+}$

2. Diamond, silicon carbide

3. ${\mathrm{NH}}_3,<mspace\; width="1em"></mspace>{\mathrm{PH}}_3$

4. ${\mathrm{XeF}}_4,<mspace\; width="1em"></mspace>{\mathrm{XeO}}_4$

Decreasing order of stability of ${\mathrm{O}}_2,<mspace\; width="1em"></mspace>{\mathrm{O}}_2^{-},<mspace\; width="1em"></mspace>{\mathrm{O}}_2^{+}<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{O}}_2^{2-}<mspace\; width="1em"></mspace>\mathrm{is:}$

1. ${\mathrm{O}}_2^{+}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{-}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{2-}$

2. ${\mathrm{O}}_2^{2-}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{-}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{+}$

3. ${\mathrm{O}}_2^{}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{+}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{2-}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{-}$

4. ${\mathrm{O}}_2^{-}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{2-}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{+}<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>{\mathrm{O}}_2^{}$

A molecule having the maximum dipole moment among the following is -

1. CO₂

2. CH₄

3. NH₃

4. NF₃