but I have a doubt how i can confirmed whether formed one is the complex crystal or others means starting material
I would recomend that you dont do your coordination chemistry in water as Schiff-base ligands hydrolyse in water. I am not entirely sure what you are asking but if you formed a copper(II) complex it will likely be blue or green whereas your starting material will be colourless. You could use IR to see if your C=N str is still present and if its shifted in relation to your ligand, UV-Vis might be useful to check to see if you have a charge transfer band, or if you have a crystal you could measure the crystal structure then you will know what you have. If you are in water though it is likely your ligand has hydrolyzed.
I would recomend that you dont do your coordination chemistry in water as Schiff-base ligands hydrolyse in water. I am not entirely sure what you are asking but if you formed a copper(II) complex it will likely be blue or green whereas your starting material will be colourless. You could use IR to see if your C=N str is still present and if its shifted in relation to your ligand, UV-Vis might be useful to check to see if you have a charge transfer band, or if you have a crystal you could measure the crystal structure then you will know what you have. If you are in water though it is likely your ligand has hydrolyzed.
Melanie is right, try to avoid water. Schiff base Copper(II) complexes are normally red so your crystals should be red coloured: observe them on an optical microscope and see. Of course if you have crystals, as you said, perform an x-ray analysis if you can. IR and UV are good as Melanie said.
Try also mass spectrometry. Your complex could easily undergoes fragmentation, so ESI(+)-MS can be better than other techniques: even though your complex should be neutral and sould be not acid-base responsive, if you are lucky the Cu(II) metal center might oxidize to Cu(III) (nozzle potential may promote the oxidation) and so you might see the peak at m/z = MW of the complex. Cu(II)-dithiocarbamate complexes, for example, have this behaviour.
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