Explanation
Because of the triple bond, the carbon –carbon bond distance in ethyne is shortest.
H – O – N = O does not have ionic and coordinate bonds.
Percentage of s–character decreases as sp (50%) > sp2 (33.3%) > sp3 (25.0%).
SiF4 is a symmetrical tetrahedral molecule and hence its dipole moment is zero.
Molecular solids have van der Waal’s forces of attraction and hence usually have low heats of fusion, i.e., melting points.
HCl does not have H-bonding but H-F has extensive H- bonding. Therefore, boiling point of HCl is lower than that of HF. Amongst HCl, HBr and Hl the molecular size of HCl is the smallest and has the weakest van der Waal’s interactions and thus has the lowest b. p.
Si(CH3)4 has sp3 - hybridization and is thus tetrahedral.
Amongst the molecules listed, in NH3, the electronegativity difference between N (3.0) and H (2.1) is the maximum and hence NH3 has the highest dipole moment.
Because of highest electronegativity of F, F - H…F hydrogen bond is the strongest.
Electronegative difference in KI is more.
ACC to V.B.T, O2 contain all e- paired. So they are diamagnetic.
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