Increasing order of bond length is:

1. $N{O}^{-}$ $<$ $NO$ $<$ $N{O}^{+}$ $<$ $O_2^{-}$

2. $O_2^{-}$ $<$ $NO$ $<$ $N{O}^{-}$ $<$ $N{O}^{+}$ $$

3. $O_2^{-}$ $<$ $N{O}^{-}$ $<$ $NO<$ $N{O}^{+}$ $$

4. $N{O}^{+}$ $<$ $NO$ $<$ $N{O}^{-}$ $<$ $O_2^{-}$

H₂O is dipolar, whereas BeF₂ is not. It is because:
 

In a regular octahedral molecule, MX₆, the number of X–M–X bonds at 180º is:

The lone pairs in the BrF₃ molecule, occupy equatorial positions to minimize:

The dipole moment of compound AB is 10.92 D and that of compound CD is 12.45 D. If the bond length of AB is 2.72 A° and that of CD is 2.56 A°, then for these compounds the correct statement is:
1.  More ionic nature in AB
2.  More ionic nature in CD
3.  Equal in both
4.  Cannot be predicted

Among the following, iso-electronic species are:

1. CO₂, NO₂

2. $N{O}_2^{-}$, CO₂

3. CN^–, CO

4. SO₂, CO₂

 ${\mathrm{p}}_{\mathrm{\pi }}-{\mathrm{d}}_{\mathrm{\pi }}$ bonding is present in:

1. ${\mathrm{NO}}_3^{-}$

2. ${{\mathrm{SO}}_3}^{-2}$

3. ${{\mathrm{BO}}_3}^{-3}$

4. ${{\mathrm{CO}}_3}^{-2}$

In NO₃^– ion, the number of bond pair and lone pair of electrons on nitrogen atom are respectively:

Incorrect statement about peptide bond is:
 

1.	C–N bond length in proteins is longer than the usual bond length of N-bond.
2.	Spectroscopic analysis shows the planar structure of  group.
3.	C–N bond length in proteins is smaller than the usual bond length of the C–N bond.
4.	None of the above.

Which of the following two species in the pair are isostructural:

1.  $Xe{F}_2$ $,$ $I{F}_2^{-}$

2. $N{H}_3$ $,$ $B{F}_3$

3. $$ $C{O}_3^{-2}$ $,$ $S{O}_3^{-2}$

4. $PC{l}_5$ $,$ $IC{I}_5$