In which of the following pairs, the two species are iso-structural?

1. $S{F}_4<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>Xe{F}_4$

2. $S{O}_3^{2-}<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>N{O}_3^{-}$

3. $B{F}_3<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>N{F}_3$

4. $Br{O}_3^{-}<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>Xe{O}_3$

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

Which of the following species has a linear shape?

1. $N{O}_2^{-}$

2. $S{O}_2$

3. $N{O}_2^{+}$

4. $O_3$

Which of the following is not a correct statement?

The number of unpaired electrons in a paramagnetic diatomic molecule of an element with atomic number 16 is:

1. 2

2. 3

3. 4

4. 1

Which of the following is not isostructural with SiCl₄?

1. $SC{l}_4$

2. $S{O}_4^{2-}$

3. $P{O}_4^{3-}$

4. $N{H}_4^{+}$

According to Molecular Orbital Theory (MOT), which of the following diatomic species contains only \(\pi\) bonds in its ground state?

The correct order of C-O bond length among \(CO\), \(CO_ 3^ {2 -}\), and \(CO_2\) is:

1. $C{O}_2<C{O}_3^{2-}<CO$

2. $CO<C{O}_3^{2-}<C{O}_2$

3. $C{O}_3^{2-}<C{O}_2<CO$

4. $CO<C{O}_2<C{O}_3^{2-}$

The correct order of increasing bond order among the following is:

1. ${\mathrm{O}}_2^{-}$ $<$ $\mathrm{NO}$ $<$ ${\mathrm{C}}_2^{2-}$ $<$ ${\mathrm{He}}_2^{+}$

2. $\mathrm{NO}$ $<$ ${\mathrm{C}}_2^{2-}$ $<$ ${\mathrm{O}}_2^{-}$ $<$ ${\mathrm{He}}_2^{+}$

3. ${\mathrm{C}}_2^{2-}$ $<$ ${\mathrm{He}}_2^{+}$ $<$ $\mathrm{NO}$ $<$ ${\mathrm{O}}_2^{-}$

4. ${\mathrm{He}}_2^{+}$ $<$ ${\mathrm{O}}_2^{-}$ $<$ $\mathrm{NO}$ $<$ ${\mathrm{C}}_2^{2-}$