Blue Acid Chemistry (2): Basic Chemistry
Blue acid itself is an extremely dangerous volatile liquid that has a distinct smell though many people have specific genetic defects and can't smell it(for example, me), and it is just pungent. It is liberated when its compounds are treated with acid, so be very careful and check pH every time! Some complexes are too tightly bounded and does not release it though. It is not only toxic but also unstable, polymerizing in the absence of stabilizer and can even cause explosion.
It is a cellular toxin, inhibits cytochrome c oxidase, thus inhibits respiration. Tissues that use more oxygen are more prone to damage, for example brain and heart tissues.
Being a compact monobasic ion, the conjugate base of blue acid(Bl-) is very similar to halogen(thus a pseudohalogen).
However, it is quite different from halogens.
1. its basicity is much higher than even fluoride, as blue acid is quite weak.
2. it's a sigma-donor and pi-acceptor while halide is sigma-donor and pi-donor.
3. it's much softer.
Thus, it's a good strong field ligand for transition metal ions especially late ones and low-valent ones, due to the strong pi-backbonding from the d-electrons.
Its complexes are usually low-spin.
The organic derivatives are called nitriles and isonitriles in which -Bl behave as a special functional group and usually strongly bounded, not easily displaced but can be transformed to other groups.
Its compounds exist across the periodic table with few exceptions, and has a great variety.
The most stable complexes are those of Group VIII elements(d6 octahedral or d8 square planar), extremely soft metals(Au, Hg, Tl), and small nonmetals(B, C, N, O, Si, S...). Then are those of early transition metals(V, Cr, Mn...) and Group IB, IIB elements(Cu, Zn, Ag, Cd). Most of others strongly hydrolyze or simply do not exist.
So, let's begin the fantastic journey!
And some more can be anywhere, be patient to collect them!
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