The following are properties of transition metals except

Explanation

Transition metals are elements found in the d-block of the periodic table (groups 3 to 12). They include metals like iron (Fe), copper (Cu), zinc (Zn), and chromium (Cr). These metals share several special properties that set them apart from other metals.

Variable oxidation states: Transition metals can lose different numbers of electrons when they form compounds. For example, iron can exist as Fe²⁺ or Fe³⁺. This happens because the energy difference between their 3d and 4s electrons is small, so different numbers of electrons can be removed.

Tendency to form complex ions: Transition metal ions can bond with molecules or ions called ligands. For example, Cu²⁺ forms a deep blue complex with ammonia (NH₃). The partially filled d-orbitals allow them to accept electron pairs from ligands.

Formation of coloured ions: Most transition metal compounds are coloured in solution. This is because their partially filled d-orbitals can absorb certain wavelengths of visible light. For example, copper(II) compounds are blue, and iron(III) compounds are yellow-brown.

Low melting points is NOT a property of transition metals. In fact, transition metals generally have very HIGH melting points. This is because they have strong metallic bonding due to the involvement of d-electrons. For example, iron melts at 1,538°C and tungsten at 3,422°C. Low melting points are characteristic of alkali metals like sodium (98°C) and potassium (63°C).