Despite the fact that atomic radius generally increases with period, the palladium-chlorine distance — Descriptive Chemistry Chemistry Question
Question
Despite the fact that atomic radius generally increases with period, the palladium-chlorine distance in PdCl42- is essentially identical to the platinum-chlorine distance in PtCl42- (2.30 Å). Which is the best explanation of why the two bond lengths are the same?
A.✓ Correct
The presence of the 14 lanthanides between Pd and Pt makes Pt unexpectedly small.
B.
PdCl42- is tetrahedral, while PtCl42- is square planar and so has shorter bonds than expected.
C.
The metal-chlorine bonds are highly covalent and so are insensitive to the trend in atomic radius.
D.
The large negative charge on the complex ions makes the chloride-chloride repulsions, not the metal-chloride attractions, the dominant factor in determining the bond distance.
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