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 given  in Column II:

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)

Which of the following species absorb maximum energy in its HOMO-LUMO electronic tranistion ?

$1. {\mathrm{O}}_2$
$2. {\mathrm{N}}_2^{-}$
$3. {\mathrm{C}}_2$
$4. {\mathrm{N}}_2$

Which of the following facts given is not correct/

(I) Bond length order : ${\mathrm{H}}_2^{-} = {\mathrm{H}}_2^{+} > {\mathrm{H}}_2$

(II) ${\mathrm{O}}_2^{+}, \mathrm{NO}, {\mathrm{N}}_2^{-}$ have same bond order of $2\frac{1}{2}$

(III) Bond order can assume any value including zero upto four

(IV) ${\mathrm{NO}}_3^{-}$ and ${\mathrm{BO}}_3^{3-}$ have same bond order for X - O bond (where X is central atom)

1. I, II & III

2. I & IV

3. II & IV

4. I & II

${\mathrm{N}}_2$ and ${\mathrm{O}}_2$ are converted to monocations ${\mathrm{N}}_2^{+}$ and ${\mathrm{O}}_2^{+}$ respectively, which is wrong statements:

1. In ${\mathrm{N}}_2^{+}$, the $\mathrm{N}-\mathrm{N}$ bond weakens

2. In ${\mathrm{O}}_2^{+}$, the $\mathrm{O}-\mathrm{O}$ bond order increases

3. In ${\mathrm{O}}_2^{+}$, the paramagnetism decreases

4. ${\mathrm{N}}_2^{+}$ becomes diamagnetic