15 - transition metals
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transition metal definition
a d-block element that can form at least one stable ion with a partially filled d-subshell
which 2 d-block elements are not classified as transition metals?
scandium and zinc dont form a stable ion with an incomplete d-subshell
think 4s orbital how do chromium and copper behave differently from other transition metals?
an electron from the 4s orbital moves into the 3d orbital to create a more stable full / half full 3d sub-shell
energy levels why do transition metals have variable oxidation states?
electrons in 4s and 3d energy levels which are very close, and electrons are gained and lost using a similar amount of energy
colour of V²⁺
violet
colour of V³⁺
green
colour of VO²⁺
blue
colour of VO₂⁺
yellow
colour of Cr³⁺
green / violet
colour of Cr₂O₇²⁻
orange
colour of Fe²⁺
pale green
colour of Fe³⁺
yellow
colour of Co²⁺
pink
colour of Cu²⁺
blue
what is a complex ion?
where a central transition metal ion is surrounded by ligands bonded by dative covalent bonds
have a pair what is a ligand?
atoms, ions or molecules that have at least 1 lone pair of electrons can be monodentate, bidentate or multidentate
(2) monodentate ligands
• only have 1 lone pair of electrons • H₂O܃, ܃NH₃, ܃Cl⁻, ܃OH⁻
(2) bidentate ligands
• have 2 lone pairs of electrons • ethanedioate - C₂O₄²⁻, ethane-1,2-diamine - NH₂CH₂CH₂NH₂
complex shape (2) what is the shape dependent on?
• size of the ligands • the coordination number
what is the coordination number?
number of dative bonds in a complex NOT the number of ligands
what shape do complexes w a co-ord number of 6 form?
octahedral bond angle - 90°
what shape do complexes with a co-ord number of 4 form?
tetrahedral bond angle - 109.5°
think redox? what is the overall charge of a complex the same as?
the total oxidation state
when electrons absorb light energy where do they move?
ground state to the excited state