Which of the following contain a maximum number of electrons in the antibonding molecular orbitals?

1.  ${O_2}^{2-}$

2.  $O_2$

3.  ${O_2}^{-}$

4.  ${O_2}^{+}$

Which of the following compounds has the least tendency to form hydrogen bonds between molecules?

1.  ${\mathrm{NH}}_3$

2.  ${\mathrm{H}}_2\mathrm{NOH}$

3.  HF

4.  ${\mathrm{CH}}_3\mathrm{F}$

Assuming that Hund's rule is violated by the diatomic molecule $B_2$, its bond order and magnetic nature will be respectively

1.  1, diamagnetic

2.  1, paramagnetic

3.  2, diamagnetic

4.  2, paramagnetic

In the Lewis structure of ozone $\left({\mathrm{O}}_3\right)$ the formal charge on the central oxygen atom is:  

1.  +1

2.  -1

3.  0

4.  -2

The types of hybrid orbitals of nitrogen in ${\mathrm{NO}}_2^{+}, {\mathrm{NO}}_3^{-},\mathrm{and} {\mathrm{NH}}_4^{+}$ respectively are expected to be 

1. $\mathrm{sp}, {\mathrm{sp}}^{3 } \mathrm{and} {\mathrm{sp}}^2$

2. $\mathrm{sp}, {\mathrm{sp}}^2 \mathrm{and} {\mathrm{sp}}^3$

3. ${\mathrm{sp}}^2, \mathrm{sp} \mathrm{and} {\mathrm{sp}}^3$

4. ${\mathrm{sp}}^{2 }, {\mathrm{sp}}^3 \mathrm{and} \mathrm{sp}$

Which of the following species has tetrahedral geometry(shape)?

1. ${\mathrm{BH}}_{4_{}}^{-}$

2. ${\mathrm{NH}}_2^{-}$

3. ${\mathrm{CO}}_3^{2-}$

4. ${\mathrm{H}}_3{\mathrm{O}}^{+}$

Which molecule /ion out of the following does not contain unpaired electrons?

1. ${\mathrm{N}}_2^{+}$

2. ${\mathrm{O}}_2$

3. ${\mathrm{O}}_2^{2-}$

4. ${\mathrm{B}}_2$

Which of the following order of energies of molecular orbitals of  ${\mathrm{N}}_2$  is correct?

1. $\left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right) < \left(\sigma 2p_z\right) < \left({\mathrm{\pi }}^{*}2{\mathrm{p}}_{\mathrm{x}}\right) \approx \left({\mathrm{\pi }}^{*}2{\mathrm{p}}_{\mathrm{y}}\right)$

2. $\left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right) > \left(\sigma 2p_z\right) > \left({\mathrm{\pi }}^{*}2{\mathrm{p}}_{\mathrm{x}}\right) \approx \left(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{y}}\right)$

3. $\left(\mathrm{\pi }2{\mathrm{P}}_{\mathrm{y}}\right) < \left(\sigma 2p_z\right) > \left(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{x}}\right) \approx \left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right)$

4. $\left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right) > \left(\sigma 2p_z\right) < \left(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{x}}\right) \approx \left(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{y}}\right)$

Match the species in Column I with the 5 types of hybrid orbitals in Column II.

   Column I                                      Column II

1.${\mathrm{SF}}_4$                                            (a) ${\mathrm{sp}}^3{\mathrm{d}}^2$

2. ${\mathrm{IF}}_5$                                              (b) ${\mathrm{d}}^2{\mathrm{sp}}^3$

3. ${\mathrm{NO}}_2^{+}$                                            (c) ${\mathrm{sp}}^3\mathrm{d}$

4.${\mathrm{NH}}_4^{+}$                                             (d) ${\mathrm{sp}}^3$  

                                                       (e) sp 

1. (1) → (a), (2) → (b), (3) → (e), (4) → (d)

2. (1) → (c), (2) → (a), (3) → (e), (4) → (d)

3. (1) → (d), (2) → (a), (3) → (e), (4) → (c)

4. (1) → (e), (2) → (b), (3) → (c), (4) → (d)

Match the species in Column I with the shape in Column II.

1. (1) → (d), (2) → (a), (3) → (b), (4) → (c)

2. (1) → (b), (2) → (a), (3) → (e), (4) → (c)

3. (1) → (e), (2) → (a), (3) → (b), (4) → (c)

4. (1) → (c), (2) → (a), (3) → (b), (4) → (d)