IB Chemistry Topic 3 Periodicity HL 13.1 First-row d-block elements

IB Chemistry Topic 3 Periodicity HL 13.1 First-row d-block elements
Explanation of why transition metals have split d orbitals and produce different colours and how the ligands influence this

IB update: In the new 2016 syllabus scandium is now considered a transition metal. Even though it is colourless it does have d electrons in the atomic and rarer Sc2+ ionic state even though not in the more common Sc3+ ionic state.

13.1 First-row d-block elements HL
• Transition elements have variable oxidation states, form complex ions with ligands, have coloured compounds, and display catalytic and magnetic properties.
• Zn is not considered to be a transition element as it does not form ions with incomplete d-orbitals.
• Transition elements show an oxidation state of +2 when the s-electrons are removed.
• Explanation of the ability of transition metals to form variable oxidation states from successive ionization energies.
• Explanation of the nature of the coordinate bond within a complex ion.
• Deduction of the total charge given the formula of the ion and ligands present.
• Explanation of the magnetic properties in transition metals in terms of unpaired electrons.
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[mcalex]

Hasn't scandium been defined as a transition metal by the IB now?