Transition metals
- Created by: Anjuli.pxtel
- Created on: 11-05-21 13:45
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- Transition metals
- A d-block element that forms one or more stable ions with an incomplete filled d orbital
- complex ions
- A central metal cation surrounded by a dative covalently bonded ligand
- Ligand - an atom, ion or molecule that donates a pair of electrons to a central metal ion
- Coordination number is the number of dative covalent bonds that ligands form from the central metal ion
- The overall charge on the complex ions is the oxidation number
- A central metal cation surrounded by a dative covalently bonded ligand
- Colours
- Copper(II) [Cu(H206]2+ = Blue
- Iron(II) , Chromium(III)= Green
- Iron(III) = Brown/ yellow
- Cobalt(II) = Red/Pink
- Chromate(IV) = Yellow
- Dichromate(VI) = Orange
- Manganate(VII) = Purple
- Reactions with hydroxide
- Copper(II) - blue solution turns into a pale blue precipitate - Precipitate is insoluble in excess NaOH
- Iron(III) Yellow/brown aqueous solution to brown precipitate
- Iron(II) - pale green solution aqueous to a green precipitate
- Cobalt(II) - pink aqueous solution to a blue precipitate
- Chromium(III) - green aqueous solution to green precipitate with excess NaOH precipitate dissolves to green solution
- Reactions with Ammonia
- Copper - blue aqueous solution to blue precipitate, with excess ammonia blue precipitate to dark blue solution
- Iron(II) - pale green aqueous solution to green precipitate
- Iron(III) - yellow/ brown aqueous solution to brown precipitate
- Cobalt(II) - pink aqueous solution to blue precipitate
- Cobalt(II) ligand exchange - blue precipitate to brown aqueous solution
- Chromium - green aqueous solution to green precipitate
- Chromium ligand exchange - green precipitate to purple solution
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