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4.55. N₂O is more polar than CO₂.

This is because CO₂ is linear and symmetrical. Its net dipole moment is zero.

N₂O is linear but not symmetrical.

4.54. This is because ethyl alcohol forms H-bonds with water.

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4.53. The electron pairs involved in the bond formation are known as bond pairs or shared pairs.

4.52.  (i) Linear

(ii) Tetrahedral

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4.51. CH₄= sp³

C₂H₄ = sp²

C₂H₂ = sp

4.50.  (c) Higher the bond order, greater is the stability.

4.49.  (d) 2-nitrophenol

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4.48.  (a) NO⁺

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4.47.  (a) sigma bond

4.46.  (c) sharing of electrons contributed by one atom only

4.44.  (c) R is an incorrect statement. Electrons placed in a bonding molecular orbital tend to hold the nuclei together and stabilise a molecule. Therefore, a bonding molecular orbital alwayspossesses lower energy than either of the atomic orbitals that have combined to form it.In contrast, the electrons placed in the antibonding molecular orbital destabilise the molecule.

This is because the mutual repulsion of the electrons in this orbital is more than the attraction between the electrons and the nuclei, which causes a net increase in energy.

4.43.  (d) Basically the strength of a bond depends uponthe extent of overlapping. In case of sigma bond, the overlapping of orbitals takes place to alarger extent. Hence, it is stronger as comparedto the pi bond where the extent of overlappingoccurs to a smaller extent. Further, it isimportant to note that in the formation ofmultiple bonds between two atoms of amolecule, pi bond (s) is formed in addition to asigma bond.