Transition metals

• what is a transition element?

  a d-block element that can form at least one stable ion with a partially filled d-subshell
• 6 general physical properties of transition elements

  Good conductors of heat and electricity.

  Hard

  Strong

  Shiny

  High melting points

  High boiling points
• 4 general chemical properties of transition elements

  Form complex ions

  Form coloured ions

  Good catalysts

  Variable oxidation states
• are transition metals more or less reactive than group 1 or 2 metals?


  less
• does the 4s or 3d subshell fill first? why?


  4s as it is lower energy
• when ions form, from which subshell are electrons lost first?

  4s
• write the full electron configuration of copper

  1s2 2s2 2p6 3s2 3p6 3d10 4s1
• write the short hand electron configuration of chromium

  [Ar] 3d5 4s1
• why are scandium and zinc not considered transition metals?

  do not have a partially filled d subshell
• what is the only ion scandium forms?

  Sc3+
• why is scandium not a transition metal?

  only forms Sc3+, so forms anemptyd subshell
• what is the only ion zinc forms?

  Zn2+
• why is zinc not a transition metal?

  forms Zn2+, which has full d-orbital
• what is a ligand?

  a molecule or ion that forms a co-ordinate bond with a transition metal by donating a pair of electrons.
• what do ligands have to have?

  a lone pair of electrons
• 4 examples of ligands

  H2O NH3 CN- Cl-
• what is a complex?

  A central metal atom or ion surrounded by ligands
• what is coordination number?

  thenumberofcoordinatebondstoligandsthat surround the d-block metal ion
• what is a lewis acid?

  electron pair acceptor
• what is a lewis base?

  electron pair donor
• what type of bonds do ligands form with metal ions?

  coordinate bonds
• what is a coordinate bond?

  A covalent bond in which both electrons in the shared pair come from the same atom (ligand)
• ligands act as lewis? becasue?

  bases because theydonatea lone pair to form a coordinate bond
• metal ions act as lewis? because?


  acids because they accept the lone pair
• do ligands around the central ion have to all be the same?

  no2 multiple choice options
• are all ligands the same size?


  no
• what happens when some ligands are bigger than others?

  can fit less around the central metal ion
• what are uni/monodentate ligands?


  ligands which form1coordinate bond to a metal ion
• examples of monodentate ligands

  :NH3 H2O: :Cl- :CN-
• why are H2O and NH3 ligands similar?


  similar in size, relatively small, and uncharged
• how many coordinate bonds can H2O and NH3 produce aroudd a metal ion?

  6
• :Cl- is a larger ligand, how many coordinate bonds can it form?

  Only 4 ligands can fit round the metal ion
• what are bidentate ligands?

  ligands which form2coordinate bonds to a metal ion
• examples of bidentate ligands

  1,2-diaminoethane and ethanedioate ion
• structural formula of ethane-1,2-diamine

  NH2CH2CH2NH2

  
• how does ethane-1,2-diamine form around a metal ion?

  octahedral, each N has lone pair that forms coordinate boond, 6 bonds, 2 from each ligand

  
• structural formula of ethanedioate

  C2O4 2-

  
• how does ethanedioate form around a metal ion?

  octahedral, each N has lone pair that forms coordinate boond, 6 bonds, 2 from each ligand

  
• what are multidentate ligands?

  ligands which formmore than 2coordinate bonds to a metal ion
• example of a multidentate ligand

  EDTA4-