Cobalt is a metal thus the atoms are bonded together in giant atomic structures and metallic bonds. The atoms attract each other with very strong atomic forces this the resulting structure is giant atomic structures. This provides for the extra strong structure of cobalt.
Answer:
See explanation
Explanation:
From the analysis we have in the question, we must look towards a first row transition metal ion having a d^6 configuration because it yields a paramagnetic complex having four unpaired electrons and a diamagnetic complex having no unpaired electrons.
We have two possible candidates in mind, Fe^2+ and Co^3+. However, Fe^2+ does not form as many coloured complexes as stated in the question so we have to eliminate that option.
We are now left with only Co^3+. Various ligands are going to cause these various colours of Co^3+ to appear in solution.
Hence, we can deduce from all these that the nature of ligands determines the colour of the complex . Don't forget that the colour of a complex arises from crystal field splitting.
I think they are called Faults.
Answer:
B
[(0.75)^3(0.25)]÷[(0.50)^2(0.75)]
Explanation:
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