1The difference of Electronegativity of C=2.1 and O=2.5(According to Pauling Scale)
Thus the difference should be 0.4 rather than 0.1
In in formation of the metal carbonyl compounds the dipole moment of the CO group should be considerable regarding the electronegativity difference of C and O but on the experimental basis the dipole moment comes out to be 0.1D!!!!!!!!!!! comment why!!!!!!!!!
By Professor R. Kapoor(Indian Institute of Science Education and Research)
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6 Answers
1
106maybe because of the double bond the length of the C=O bond becomes small resulting in a smaller dipole moment.
p = qd (q is large and invariable but maybe the d becomes small as the C is sp2 hybridised)
1It is because of the co-ordinate bond between C & O. When the electron pair is donated to C by O
via the co-ordinate bond, the partial negative charge on O decreases and that of C increases which
result in lower difference of effective electronegativity between the atoms in the compound, which
in turn suppresses the dipole moment.
106abhi coordinate bond is the same as covalent bond (atleast thats wat is written in ur fav. buk)
1coordinate bond is treated same as covalent bond with respect to equivalence in energy levls of
the bonds n their characterstics. but,der r few exceptions in which coordinate bond becomes
dative i.e. acquires partial double bond characters ( normally due to p(pi)-d(pi) back bonding and
normal backbonding)
(my fav. buk also mentions dat )
6well i further searched the answer and found that due to the coordinate/dative bond the ∂+ve charge on carbon reduces and that too on Oxygen the ∂-ve charge too decrease which leads to a dipole moment much small as 0.1 D!!!!!!!!!!!!