Explanation
Statement (a) is not correct as hybridisation is not a prior phenomenon.
Bond order cannot be negative because number of bonding electrons is always greater than anti bonding electrons.
o-Nitrophenol undergoes intramolecular H –bonding and hence exists as a monomer but p- nitrophenol undergoes intermolecular H – bonding and hence exists as an associated molecule. Therefore, o-nitrophenol is more volatile than p- nitrophenol.
Configuration (c) is correct.
C2H4 has sp2 - hybridization.
[NF3 and H3O+] are pyramidal while [NO3- and BF3] are planar. Hence answer (c) is correct.
F- forms H- Bond with HF, therefore, the species [ H…F- H]- or HF2− exists and hence option (c) is correct.
In H - O - O - H, O - H bonds are polar but O –O bond is non –polar.
Only SO2 has sp2 hybridization while all the remaining molecules, i.e. CO2,N2O and CO have sp- hybridization.
H –bonding interactions.
Since the element X forms XCl3, X2O5 and Ca3X2, therefore, it must be N or P. Since it does form MCl5, therefore, it must be N since it has no d- orbitals to expand its covalency from 3 to 5. Therefore, X must be N.
Metallic lustre is due to oscillation of loose electrons.
Each N atom in N2 molecule shares three electrons, i.e., :N::N:
SF6 has six bond pairs and hence according to VSEPR theory, it should be octahedral.
Since MX4 is tetrahedral, therefore, total number of ∠XMX is six.
Strength of H - bond depends upon the electronegativity of the atom carrying the H - atom. Since O is more electronegative than N, therefore, H- bonding is maximum in ethanol.
Only BCl3 is electron deficient.
sp - Hybridized (O = C= C= C =O).
All are gaseous molecules and do not conform to the octet rule. Thus, option (d) is correct.
Only statement I is correct.
H2O has highest boiling point due to hydrogen bonding.
Hybridization of N in NH3 = sp3, that of Pt2+ in [PtCl4]2- = dsp2, that of P in PCl5 = dsp3and that of B in BCl3 = sp2
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