A co-ordinate bond formed between two species by sharing of an electron pair where shared pair electron is given by one but shared by both.
ILLUSTRATIVE EXAMPLE (1):
ILLUSTRATIVE EXAMPLE (1):
ILLUSTRATIVE EXAMPLE (1):
ILLUSTRATIVE EXAMPLE (1):
ILLUSTRATIVE EXAMPLE (1):
CONCLUSIONS:
(1) Atoms of second period elements follow octed rule in doing so either they accept co-ordinate bond or they form co-ordinate bond. However atoms of 3rd period elements perfectly form double bond (pi bond) in the place of co-ordinate bond if direction of co-ordinate bond is from centre to substituent.
(2) If maximum covalency rule applied and pi bonds have formed then back bond is not considered in species
For example H2SO4 and HClO4 have no back bond there is double bond.
Why all the
tetrahedral Complexes are high spin Complexes?
Why Fe(CO)5 is colourless
while Fe(bipy)(CO)3 is intensely purple in colour ?
Why [Mn(H2O)6]+2 is colourless
although in which Mn+2 ion had five unpaired electrons ?
Why [FeF6]3– is colourless whereas [CoF6]3–
is coloured?
Why [Ni(CN)4]-2 is colourless
while [Ni(H2O)4]-2 is colour although both have +2
oxidation state and 3d8 configuration ?
No comments:
Post a Comment