1 / 6

A2 Chemistry transition metal complexes a visual guide

A2 Chemistry transition metal complexes a visual guide. VERSION 1. Designed by Samuel Millar. NOTES. Black text – CORE KNOWLEDGE Red text – EXCEPTIONS TO THE PATTERNS Grey text – EXTENSION

aldon
Download Presentation

A2 Chemistry transition metal complexes a visual guide

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. A2 Chemistrytransition metal complexesa visual guide VERSION 1 Designed by Samuel Millar

  2. NOTES • Black text – CORE KNOWLEDGE • Red text – EXCEPTIONS TO THE PATTERNS • Grey text – EXTENSION The colour and formula are given for the complex formed by each ion with each • reagent, starting with the aqueous complex. In the case of NaOH and NH3, the hydroxide precipitate produced is given, followed by the complex formed (if any) when excess (“xs”) of the reagent is added. The colours are named as CCEA wants them in the exam! The colour boxes hopefully give some indication of the actual shade. Most of the complexes involve six ligands and so are octahedral. However, chloride complexes take tetrahedral or square planar shapes.

  3. Copper (II) and Cobalt (II) • ion • aq • NaOH • NH3 • concHCl • Cu2+ • blue soln[Cu(H2O)6]2+ • blue ppt[Cu(OH)2(H2O)4]insoluble in xs • blue ppt[Cu(OH)2(H2O)4]soluble – deep blue soln[Cu(NH3)4(H2O)2]2+ • yellow-green soln[CuCl4]2- • Co2+ • pink soln[Co(H2O)6]2+ • blue ppt[Co(OH)2(H2O)4]insoluble in xs • blue ppt[Co(OH)2(H2O)4]soluble – yellow soln[Co(NH3)6]2+ • blue soln[CoCl4]2-

  4. Iron (III) and Iron (II) • ion • aq • NaOH • NH3 • SCN-thiocyanate • Fe2+ • green soln[Fe(H2O)6]2+ • green ppt*2[Fe(OH)2(H2O)4]insoluble in xs • green ppt*2[Fe(OH)2(H2O)4]insoluble in xs • Fe3+ • yellow/orange soln[Fe(H2O)6]3+*1 • rust/brown ppt[Fe(OH)3(H2O)3]insoluble in xs • rust/brown ppt[Fe(OH)3(H2O)3] insoluble in xs • blood-red soln[Fe(SCN)(H2O)5]2- *2NB: Iron (II) hydroxide slowly oxidises to iron (III) hydroxide, so a rust/brown colour is observed after some time. *1[Fe(H2O)6]3+is actually pale violet. The high charge density on the metal ion causes some deprotonation and the yellow-orange colour is actually due to [Fe(OH)(H2O)5]2+

  5. Chromium (III) and Manganese (II) • ion • aq • NaOH • NH3 • Cr3+ • green soln[Cr(H2O)6]3+ • green-blue ppt[Cr(OH)3(H2O)3]soluble – green soln[Cr(OH)6]3- • green-blue ppt[Cr(OH)3(H2O)3]soluble – violet soln[Cr(NH3)6]3+ • Mn2+ • pink soln[Mn(H2O)6]2+ • white ppt*[Mn(OH)2(H2O)4]insoluble in xs • white ppt*[Mn(OH)2(H2O)4] insoluble in xs *NB: Manganese (II) hydroxide slowly oxidises to manganese (III) oxide, so the white (off-white) precipitate slowly turns brown/black. • aq • Chromium (VI) CrO42-yellow soln • Chromium (VII) Cr2O72-orange soln • Chrome alumKCr(SO4)2 violet crystals

  6. Nickel (II) and Vanadium • ion • aq • NaOH • NH3 • concHCl • edta • en • Ni2+ • green soln[Ni(H2O)6]2+ • green ppt[Ni(OH)2(H2O)4]insoluble in xs • green ppt[Ni(OH)2(H2O)4]soluble – blue soln[Ni(NH3)6]2+ • yellow soln[NiCl4]2- • blue soln[Ni(edta)]2- • purple soln[Ni(en)3]2+ • aq • Vanadium (II) V2+violet • Vanadium (III) V3+green • Vanadium (IV) VO2+blue • Vanadium (III) VO2+yellow

More Related