S3.1 The periodic table: Classification of elementsIB Chemistry HL: Flashcards

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Configuration of Fe³⁺?

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Configuration of Fe³⁺?: [Ar]3d⁵ (4s electrons lost first).
Configuration of Cu²⁺?: [Ar]3d⁹.
Why is B's first IE lower than Be's?: B's electron is removed from 2p, which is higher in energy than 2s.
Why is O's first IE lower than N's?: O's electron comes from a paired 2p orbital; repulsion raises its energy.
How do IE discontinuities show sublevels exist?: The 2, 3, 3 pattern across a period matches filling s, then singly filling p, then pairing in p.
List six characteristic properties of transition elements.: Variable oxidation states, high melting points, magnetic properties, catalytic activity, coloured compounds, complex ions.
Why do transition elements show variable oxidation states?: Their successive ionisation energies (4s and 3d) are close in value.
What is a ligand?: A species that donates a lone pair to a central metal ion via a coordination bond.
Why are transition metal complexes coloured?: Ligands split the d orbitals; an electron is promoted by absorbing visible light and the complementary colour is seen.
A complex absorbs orange light. What colour does it appear?: Blue.
Why are Zn²⁺ complexes colourless?: 3d¹⁰: the d-sublevel is full, so no d–d promotion can occur.
What makes a species paramagnetic?: Unpaired electrons.
Which period 3 oxide is amphoteric?: Al₂O₃.
Oxidation state of Mn in KMnO₄?: +7.