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1.
Cuprous oxide
The reduction of Cu(Ⅱ) solution with glucose in alkaline medium can easily get red Cu 2 O precipitation
.
This reaction is used in medicine to detect sugar in urine samples
Cu 2 O can also be obtained by the decomposition of CuO at high temperature
.
Cu 2 O has high thermal stability and melts at 1244°C but does not decompose
Cu 2 O+2H + =Cu+Cu 2+ +H 2 O
Cu 2 O dissolves in ammonia water to generate colorless complex ions.
Due to the oxidation of oxygen in ammonia water , Cu 2 O dissolves in ammonia water to obtain a blue [Cu(NH 3 ) 4 ] 2+ solution
.
2.
Halides and sulfides
CuCl, CuBr, and Cul are all white insoluble compounds with successively reduced solubility, which can be obtained by the reduction of +2 valent copper ions in the presence of corresponding halide ions
.
It was diluted with water [CuCl 2 ] - solution, resulting precipitate insoluble CuCl
.
Using reducing agents such as SnCl 2 and Na 2 SO 3 to react with copper halide can also obtain cuprous halide
CuCl is dissolved in ammonia, concentrated hydrochloric acid and alkali metal chloride solution to form coordination compounds
.
Cuprous sulfide Cu 2 S, black, hardly soluble in water, soluble in hot concentrated nitric acid or CN - solution
.
3.
Coordination Compound
Due to the different ligand concentration, Cu + and the single-base ligand form a coordination compound with a coordination number of 2 to 4.
These complex ions are colorless, such as [Cu(NH 3 ) 2 ] + , [Cu(NH 3 ) 3 ] + , [Cu(NH 3 ) 4 ] + , [CuCl 2 ] - , [CuCl 3 ] 2- , [CuCl4]3-, [Cu(CN) 2 ] - , [Cu(CN) 3 ] 2- , [a Cu (the CN) .
4 ] 3- and the like
[Cu(NH 3 ) 2 ] + is unstable and will be oxidized to dark blue [Cu(NH 3 ) 4 ] 2+ when it encounters air .
This property can remove trace O 2 in the gas
.
The complex formed by Cu + and Cl - or CN - is stable in the air
.
[Cu(NH 3 ) 2 ] + can absorb CO gas
.