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Transition metal properties: Cr to Cu

Atomic structure and the periodic table • Properties of transition metals

Key concepts

What you'll likely be quizzed about

  • A transition metal is defined as an element that forms at least one ion with a partially filled d subshell.
  • Elements like scandium (Sc3+, empty d subshell) and zinc (Zn2+, full d subshell) do not qualify as transition metals because they do not possess partially filled d orbitals.
  • The presence of these orbitals dictates the chemical behavior that differentiates transition metals from s- and p-block elements.

Flashcards

Test your knowledge with interactive flashcards

What is a notable high-oxidation-state manganese compound and its colour?

Click to reveal answer

Permanganate (MnO4−) appears purple due to strong charge-transfer and d–d transitions.

Key notes

Important points to keep in mind

Transition metal forms at least one ion with a partially filled d subshell.

Variable oxidation states arise from available 3d and 4s electrons.

Coloured ions result from d–d and charge-transfer electronic transitions.

Catalytic activity depends on variable oxidation states and surface adsorption.

High melting points and conductivity arise from strong metallic bonding with d electrons.

Iron, cobalt, and nickel exhibit ferromagnetism due to unpaired d electrons and domain alignment.

Chromium(VI) compounds are strong oxidizing agents; permanganate is significant in manganese chemistry.

Copper features excellent electrical conductivity and forms blue Cu2+ aqueous ions.

Not all d-block elements are transition metals; only those forming partially filled d-ion states qualify.

Alloying modifies mechanical properties by distorting the metallic lattice and altering electron interactions.

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