Untitled Flashcards Set

Transition Metal Halides

Compounds formed by transition metals and halogens, showing various oxidation states and reacting behavior.

Fluoride Stability

Fluorine stabilizes higher oxidation states in transition metals due to higher lattice energy or bond enthalpy.

Cupric Ion (Cu2+)

The copper ion in the +2 oxidation state, known to oxidize iodide ions to iodine.

Magnetic Properties

Behavior of substances in a magnetic field, categorized as diamagnetic, paramagnetic, or ferromagnetic.

Paramagnetism

Magnetic behavior resulting from unpaired electrons in atoms or ions, causing attraction to a magnetic field.

Coloured Ions Formation

Occurs when electrons in d-orbitals are excited to higher energy d-orbitals, absorbing visible light.

Complex Compounds

Chemical species formed by the coordination of metal ions with ligands, exhibiting unique properties.

Catalytic Activity

The ability of transition metals to speed up chemical reactions by forming various oxidation states.

Interstitial Compounds

Compounds formed when small atoms like H, C, or N are trapped in metal crystal lattices, exhibiting unique properties.

Alloy Formation

The blending of metals to create solid solutions, enhancing properties such as hardness and melting points.

Oxidation State Stabilization

The ability of oxygen and fluorine to stabilize transition metals in high oxidation states through bonding.

Hydrolysis of Halides

The reaction of halides with water resulting in the formation of oxohalides.

High Oxidation States of Mn

The highest manganese fluoride is MnF4, while the highest oxide is Mn2O7.

Disproportionation Reaction

A reaction in which a single substance is transformed into two different products, such as 2Cu+ → Cu2+ + Cu.

Metal Reactivity

Transition metals exhibit varying reactivity patterns, with many dissolving in acids and some being 'noble'.

E V Values

Electrode potential values indicating the tendency of transition metals to form cations.

Spin-Only Formula

Calculates magnetic moments based solely on the number of unpaired electrons.