The relative order of stability of the following species: \(\mathrm{O}_2,\mathrm{O}^+_2,\mathrm{O}^-_2~\mathrm{and}~\mathrm{O}^{2-}_2\) is -

1.	\(\mathrm{O}^+_2>\mathrm{O}_2>\mathrm{O}^-_2>\mathrm{O}^{2-}_2\)	2.	\(\mathrm{O}^{2-}_2>\mathrm{O}_2>\mathrm{O}^-_2>\mathrm{O}^{+}_2\)
3.	\(\mathrm{O}_2>\mathrm{O}^+_2>\mathrm{O}^-_2>\mathrm{O}^{2-}_2\)	4.	\(\mathrm{O}_2>\mathrm{O}^{2-}_2>\mathrm{O}^-_2>\mathrm{O}^{+}_2\)

$\mathrm{}$

Which of the following is represented by the positive (+) and negative (−) signs shown on the lobes of atomic orbitals?

1. Sign (phase) of the wave function

2. Probability density of an electron

3. Quantum number of the orbital

4. Frequency of the orbital

${\mathrm{AlCl}}_3$ $+$ ${\mathrm{Cl}}^{-}$ $\to$ ${\mathrm{AlCl}}_4^{-}$

1. \(s p^{2} \text { to } s p^{3}\)
2. \(\mathrm{sp}^{3} \text { to } s p^{2}\)
3. \(\mathrm{sp}^{3} \text { to } \mathrm{dsp}{ }^{2}\)
4. \(\operatorname{sp}^{2} \text { to } d s p^{2}\)

Considering the X-axis as the internuclear axis, a sigma bond will not be formed in:

$1.$ $1\mathrm{s}$ $\mathrm{and}$ $2\mathrm{s}$
$2.$ $1\mathrm{s}$ $\mathrm{and}$ $2{\mathrm{p}}_{\mathrm{x}}$
$3.$ $2{\mathrm{p}}_{\mathrm{y}}$ $\mathrm{and}$ $2{\mathrm{p}}_{\mathrm{y}}$
$4.$ $1\mathrm{s}$ $\mathrm{and}$ $1\mathrm{s}$

The set of oxides of nitrogen that are paramagnetic in nature is:

1. NO, N₂O

2. N₂O₃, NO

3. NO, NO₂

4. N₂O, NO₂

Which of the compounds given below will exhibit a linear structure?

Match the compounds of Xe in Column I with the molecular structure in Column II.

Match the coordination number and type of hybridization with the distribution of hybrid orbitals in space based on Valence bond theory.

The potential energy (y) curve for H₂ formation as a function of internuclear distance (x) of the H atoms is shown below.

The bond energy of H₂ is: