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Revision:Transition Metals
From The Student RoomTSR Wiki > Study Help > Subjects and Revision > Revision Notes > Chemistry > Transition Metals
Transition ElementsA transition element is a metal with an ion or a compound with a partially filled d subshell. Zinc is not a transition metal but is a d block element because it has a full d subshell. This is shown because its compounds are usually white. Properties of transition elements
ComplexesA complex is formed when a transition metal ion is surrounded by ligands which dative covalent bond with it by donating lone pairs of electrons into vacant d orbitals. The d electrons of the metal ion do not take part in ligand bonding. Definitions
Electronic ConfigurationTransition metals have full 1s, 2s, 2p, 3s and 3p orbitals. i.e. 18 electrons. Hence, they are sometimes written as: E.g. Sc [Ar] 3d1 4s2 - since Ar has 18 electrons. NOTE: the 4s electrons are lost and gained BEFORE the 3d orbitals.Vanadium Vanadium, like many other transition metals can form various oxidation states. This means it can be used as a catalyst because it can readily gain or lose electrons i.e. be reduced or oxidised i.e. undergo redox. Oxidation States of Vanadium+5 in VO2+ (yellow) +4 in VO2+ (blue) +3 in V3+ (green) +2 in V2+ (lavender) NOTE: If the question mentions the reduction of vanadium and notes the colour change as being yellow to green to blue to green to lavender, the first green is simply a mixture of the yellow VO2+ and the blue VO2+ ions. Comments |
















