how would the bond length vary in dicarbon species C2, C2+, C2-
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The order of bond length in the dicarbon species, starting with the longest is C2+ > C2 > C2-.
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The bond order of the dicarbon species C2, C2+, C2- is calculated using the formula:-
Bond order = 1/2 (number of electrons in bonding orbitals - number of electrons in antibonding orbitals).
The bond order results show that the C2- has the highest number of valence electrons and highest bond energy. Therefore, C2- supposedly has the shortest bond length.
C2+ has lesser bond energy than C2. Therefore, C2+ has a longer bond length than C2.
---------------------------------------------------------
The bond order of the dicarbon species C2, C2+, C2- is calculated using the formula:-
Bond order = 1/2 (number of electrons in bonding orbitals - number of electrons in antibonding orbitals).
The bond order results show that the C2- has the highest number of valence electrons and highest bond energy. Therefore, C2- supposedly has the shortest bond length.
C2+ has lesser bond energy than C2. Therefore, C2+ has a longer bond length than C2.
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Answer:
Bond order is the number of Chemical bonds between a pair of atoms and indicates the stability of a bond. The bond order results show that the C2- has the highest number of valence electrons and highest bond energy. Therefore, C2- supposedly has the shortest bond length. C2+ has lesser bond energy than C2. Therefore, C2+ has a longer bond length than C2.
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