Other questions in this quiz

2. An aqueous solution of copper(II) ions contains [Cu(H2O)6]2+ complex ions, which have the pale blue colour when ammonia is added the colour changes is

  • From pale blue to dark blue, in the reaction four of the water ligands are replaced by four ammonia ligands [Cu(NH3)4(H2O)2]2+
  • Can form cis/trans
  • A reaction in which one ligand in a complex ion is replaced by another ligand

3. Transition elements are able to form coloured compounds due to

  • Oxidation states, all forming compounds with ions in the 2+ oxidation state (this is usually the result of losing two electrons from 4s orbital, which are lost first as when full 4s is in a higher energy level that 3d)
  • Absorbtion of a specific wavelength of light but reflection or transmission of another wavelength
  • The 4s orbital fills before the orbitals in the 3d sub shell. The d block metals will have filled there 4s orbital before electrons are added to the 3d sub shell

4. Ligands that have two lone pairs are called bidentate as they can form

  • Two coordinate bonds with a metal ion
  • Only one coordinate bonds with a metal ion

5. The reaction of cobalt(II) ions and concentrated hydrocholoric acid is

  • [Co(H2O)6]2+(aq) + 4Cl-(aq) --> [CoCl4]2-(aq) + 6H2O
  • [Cu(NH3)4(H2O)2]2+(aq) + 4H2O(l) (pale blue-->dark blue)




I'm sorry about the last comment, my friend wrote it because he didn't want to accept that he got some answers wrong in this quiz. I just got 100% on this quiz and with it It helped enhance my knowledge on Transition Metals as a whole. Keep up with the resources guys!!! 

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