transitional metals

transition element

• empty vacant d orbitals that are energetically accessible

• more than 1 stable oxidastion state

copper and chrommium

3d5 4s1, 3d10 4s1

scandium n zinc

• not transitional elemtents

• Sc3+ has an empty d-subshell as it is not partially filled, it isn't a transition element.

• Only 1 stable ion - sc3+ n zn2+

• Has a full d subshell 

properties of trasnitional metals

• varaible oxidastion states

• coloured ions in solution

• good catalysts

• form complex ions

variable oxidastion states

• because electrons sit on 4s and 3d energy levels which are really close

• 3d and 4s atomic orbitals are similar in energy

• Electrons can jump easily

• As a result, electrons are gained and lost using a similar amount of energy when they form ions / remove or add electrons 

• When they form ions electrons in 4s is lost first then 3d

behave as catalysts

• have more than 1 stable oxidastion state

• have vacant d orbitals that are energeticaly accessible

• Dative bonds can form between transition element ion and ligands

complex ions

• A central transition metal ion surrounded by ligands, bonded by dative covalent (coordinate) bonds. 

• Ligands have a lone pair of electrons, that donate electrons that are used in dative bonds 

• So the transition central ion accepts the electrons. 

• Transition elements form easily as they have empty d orbitals and are energetically accessible 

• Not too high in energy and can accommodate lone pair of electrons

s block element calcium compared to transition elements

• calcium has a larger ionic radius

• has a lower melting point

• lower density

ligand

• An ion atom or molecule that has at least 1 lone pair of electrons 

• Can be mono, bio or poly dentate 

mono, bi, n poly dentate

• 1 lone pair - h20, nh3, cl, oh

• 2 lone pair - ethanedioate, ethan-1,2-diamine

• more than 1 - EDTA4-