Transition Elements are elements whose atoms, or ions, have an incompletely filled d-subshell. They occupy the d-block of the Periodic Table, spanning Groups 3 to 12.
d-block: Groups 3–12.
Variable Oxidation State: Key characteristic.
Exception: Zinc (Zn) — d¹⁰ configuration — some argue it is NOT a true transition element.
Catalyst Examples: Fe (Haber process), V₂O₅ (Contact process).
They are located between the s-block (alkali and alkaline earth metals) and the p-block (non-metals). There are four series of transition elements (3d, 4d, 5d, 6d).
Iron (Fe), Copper (Cu), Zinc (Zn), Nickel (Ni), Chromium (Cr), Manganese (Mn), Cobalt (Co), Silver (Ag), Gold (Au).
Transition elements are elements with incompletely filled d-subshells in their atoms or common ions, located in the d-block (Groups 3–12) of the periodic table.
Because the energy difference between ns and (n-1)d subshells is small, electrons from both can be lost during bonding, giving multiple oxidation states.
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