Chemistry

2.15 - Transition Metals

4 min

note 1 of 3

What the transition metals are like

The transition metals (also called transition elements) are the block of metals in the centre of the periodic table, between Group 2 and Group 3.
Most metals in the periodic table belong to this block, including iron, copper, chromium, manganese, cobalt, nickel, silver, and gold.

Periodic table with the central block of metals between Group 2 and Group 3, three rows running from scandium to zinc, yttrium to cadmium, and hafnium to mercury, highlighted in blue.

Typical metal properties

They behave as typical metals: relatively hard, strong, and shiny, and good conductors of heat and electricity.

How they compare with Group 1 metals

High melting points - Iron melts at about 1,540 °C, while sodium melts at only 98 °C (mercury is the exception, being a liquid at room temperature).
High densities - Copper is 9.0 g/cm³ and iron 7.9 g/cm³, against 0.9 g/cm³ for potassium.
Stronger and harder - Group 1 metals are soft enough to be cut with a knife.
Far less reactive - They react only slowly with water and oxygen, and slowly or not at all with the halogens. Copper doesn't react with water at all, and iron rusts slowly, whereas alkali metals react vigorously with cold water and lose their shine within seconds in air.

note 2 of 3

Ions of more than one charge

Most elements form an ion with only one charge. Sodium is always Na⁺ and magnesium is always Mg²⁺, so each forms just one chloride.
Transition metals are different: the same metal can form ions carrying more than one charge, so it forms more than one compound with the same partner element.

Examples of variable charges

Iron - Forms Fe²⁺ and Fe³⁺ ions.
Copper - Forms Cu⁺ and Cu²⁺ ions.
Chromium - Forms Cr²⁺ and Cr³⁺ ions.

Naming with Roman numerals

To show which ion a compound contains, the charge is written into the metal's name as a Roman numeral in brackets:
- Iron(II) means Fe²⁺ and iron(III) means Fe³⁺.
- Copper(I) and copper(II) mean Cu⁺ and Cu²⁺.
Because the charges differ, the compounds differ:
- Iron(II) chloride is FeCl₂ - two chloride ions balance the 2+ charge.
- Iron(III) chloride is FeCl₃ - three chloride ions balance the 3+ charge.

note 3 of 3

Coloured compounds and catalysts

Compounds of the transition metals are coloured, which sets them apart from most other metal compounds.
The colour comes from the metal ion itself: transition metal ions are coloured, so most compounds containing one are coloured too - both as a solid and when dissolved in solution. There are exceptions: anhydrous copper(II) sulfate is white, and turns blue only when water is added.

Which colour depends on the ion

The colour depends on which transition metal ion the compound contains:
- Compounds containing Fe²⁺ ions are usually pale green.
- Compounds containing Fe³⁺ ions are orange-brown.
- Compounds containing Cu²⁺ ions are typically blue.
Across the block: chromium(III) is green, manganese(II) is pale pink, manganate(VII) is deep purple, cobalt(II) is pink, and nickel(II) is green.

Catalytic activity

Many transition metals, and many of their compounds, are useful as catalysts.
A catalyst is a substance that speeds up a chemical reaction without being used up by it.
A transition metal can act as a catalyst either as the element itself or in one of its compounds - iron is the standard example.

key terms

TermDefinition

Transition metalsThe block of metals in the centre of the periodic table, between Group 2 and Group 3.

CatalystA substance that speeds up a chemical reaction without being changed or used up.

end of notes

Key points to remember

Ions of more than one charge

Most elements form an ion with only one charge. Sodium is always Na⁺ and magnesium is always Mg²⁺, so each forms just one chloride.

Transition metals are different: the same metal can form ions carrying more than one charge, so it forms more than one compound with the same partner element.

Examples of variable charges

Iron - Forms Fe²⁺ and Fe³⁺ ions.

Copper - Forms Cu⁺ and Cu²⁺ ions.

Chromium - Forms Cr²⁺ and Cr³⁺ ions.

Naming with Roman numerals

To show which ion a compound contains, the charge is written into the metal's name as a Roman numeral in brackets:

Iron(II) means Fe²⁺ and iron(III) means Fe³⁺.
Copper(I) and copper(II) mean Cu⁺ and Cu²⁺.

Because the charges differ, the compounds differ:

Iron(II) chloride is FeCl₂ - two chloride ions balance the 2+ charge.
Iron(III) chloride is FeCl₃ - three chloride ions balance the 3+ charge.

Coloured compounds and catalysts

Compounds of the transition metals are coloured, which sets them apart from most other metal compounds.

The colour comes from the metal ion itself: transition metal ions are coloured, so most compounds containing one are coloured too - both as a solid and when dissolved in solution. There are exceptions: anhydrous copper(II) sulfate is white, and turns blue only when water is added.

Which colour depends on the ion

The colour depends on which transition metal ion the compound contains:

Compounds containing Fe²⁺ ions are usually pale green.
Compounds containing Fe³⁺ ions are orange-brown.
Compounds containing Cu²⁺ ions are typically blue.

Across the block: chromium(III) is green, manganese(II) is pale pink, manganate(VII) is deep purple, cobalt(II) is pink, and nickel(II) is green.

Catalytic activity

Many transition metals, and many of their compounds, are useful as catalysts.

A catalyst is a substance that speeds up a chemical reaction without being used up by it.

A transition metal can act as a catalyst either as the element itself or in one of its compounds - iron is the standard example.