Transition Metal

Key Stage 4

Transition Metals (also known as transition elements) are a block of elements on the Periodic Table between Group 2 and Group 3.

Transition Metals usually have high melting points because metallic bonds are very strong, keeping the atoms vibrating in fixed positions.

The transition metal melting points measured in Kelvin are written below each chemical symbol.

N.B. The Period 7 elements have not been included as they do not occur naturally and have not been made in large enough quantities to find their melting points.

Transition Metals have a high density compared to other elements. However, many of the Actinides also have a density.

The transition metal densities measured in kilograms per metre cubed are written below each chemical symbol.

N.B. The Period 7 elements have not been included as they do not occur naturally and have not been made in large enough quantities to find their [density\|densities]].

Most of the Transition Metals react slowly with Oxygen, Water and the Halogens at room temperature and some will not react at all.

For combustion to occur the Transition Metals must be heated to very high temperatures. However, some Transition Metals will not combust at all.

Transition Metals can form several different charge ions and these different charges can determine the physical properties of the compounds they are in. Specifically this affects the colour of those compounds.

In compounds the charge of the Transition Metal ion is given in Roman Numerals after the name of the metal

Copper (I) Sulphate: +1 Ion of Copper giving the compound a light green colour.
Copper (II) Sulphate: +2 Ion of Copper giving the compound a blue colour.
Manganese (II) Chloride: +2 Ion of Manganese giving the compound a pale pink colour.
Manganese (IV) Oxide: +4 Ion of Manganese giving it a very dark brown colour, often appearing black.
Iron (II) Sulphate: *2 Ion of Iron giving the compound a pale green colour.
Iron (III) Sulphate: *3 Ion of Iron giving the compound a redish-brown colour.

Gem stones with various colours (red rubies, green emeralds, blue sapphires) get their colour from the Transition Metal ions they contain.

Catalysts can increase the rate of reaction and lower the temperature needed to start a reaction.

Catalysts are not used up in the chemical reaction so can be used over and over again.

Transition Metal catalysts can increase the rate of reaction by either accepting or donating electrons so that not as much energy is needed for a reaction to happen.

These are some Transition Metal catalysts you may know:

Iron: Used as a catalyst for Hydrogen and Nitrogen reacting to produce Ammonia.
Platinum: Used in the production of Nitric Acid.
Manganese: Used in the form of Manganese Dioxide as a catalyst for the decomposition of Hydrogen Peroxide.