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The six transition metals to know are chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni) and copper (Cu). Free notes and 11 questions answered.
Transition Metal Examples: From Chromium to Copper is part of Properties of transition metals (chemistry only) in GCSE AQA Higher Chemistry.
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The six transition metals to know are chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni) and copper (Cu). Free notes and 11 questions answered.
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Use this lesson to stay inside Properties of transition metals (chemistry only) while connecting the detail back to the wider Topic 1: Atomic structure and the periodic table topic.
Read the core explanations from Transition Metal Examples: From Chromium to Copper before testing yourself from memory.
Chromium makes stainless steel rust-proof. Iron carries oxygen in your blood. Copper wires power your phone. These aren't random facts — they're all transition metals with special properties that make modern life possible.
The six transition metals you need to know — chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni), and copper (Cu) — all share the same fundamental characteristics. But each has its own personality that determines how we use it.
All transition metals share four key properties that set them apart from other elements. Think of these as their 'superpowers' that make them so useful in industry and biology.
Property 1: Ions with different charges. Unlike Group 1 metals that usually form +1 ions, many transition metals can form ions with different charges. For example, iron can form Fe²⁺ and Fe³⁺ ions.
Property 2: Coloured compounds. Many transition metal compounds are coloured. Copper sulphate is blue, chromium oxide is green, and potassium permanganate is purple.
Property 3: Catalytic activity. Many transition metals speed up reactions without being used up. Iron catalyses the Haber process for making ammonia. Nickel catalyses the hydrogenation of alkenes.
Property 4: GCSE focus. At GCSE, focus on the properties named in the specification: many transition metals form ions with different charges, form coloured compounds, and are useful catalysts.
Now let's see how each of our six transition metals shows these general properties in their own unique way. You'll spot patterns, but also key differences that explain their different uses.
Chromium (Cr): The 'chameleon' metal. Forms Cr³⁺ (green compounds like Cr₂O₃) and Cr⁶⁺ (orange compounds like K₂Cr₂O₇). Used in stainless steel because chromium oxide forms a protective layer that prevents rusting.
Manganese (Mn) is one of the named transition metals you may meet in examples of coloured compounds and catalysts.
Iron (Fe): The 'biological workhorse'. Forms Fe²⁺ (pale green) and Fe³⁺ (yellow/brown). Fe²⁺ in haemoglobin carries oxygen in blood. Fe³⁺ in rust (Fe₂O₃) shows why iron corrodes easily.
Cobalt (Co) is another transition metal. Its compounds can be coloured, and cobalt is used in rechargeable batteries and as a catalyst in industry.
Nickel (Ni): The 'hydrogenation specialist'. Ni²⁺ forms green compounds. Metallic nickel catalyses the addition of hydrogen to alkenes (margarine production). Also used in rechargeable batteries and stainless steel.
Copper (Cu): The 'conductor'. Forms Cu⁺ (colourless compounds) and Cu²⁺ (blue compounds like CuSO₄·5H₂O). Excellent electrical conductor — used in all electrical wiring. Also has antimicrobial properties.
Looking across our six metals, you can spot some trends that help predict their behaviour. This is where chemistry becomes less about memorising and more about understanding patterns.
At GCSE, you do not need detailed trends in charges across the transition metals.
At GCSE, it is enough to know that many transition metal compounds are coloured and to learn valid examples.
At GCSE, you do not need detailed stability patterns across the transition metals.
The unique properties of these transition metals aren't just academic curiosities — they're the reason these elements are essential to modern technology and life itself.
Catalysis in industry: Iron catalyses ammonia production (Haber process), feeding billions through fertiliser. Nickel catalyses margarine production by adding hydrogen to vegetable oils. These reactions would be impossibly slow without transition metal catalysts.
Biological roles: Iron in haemoglobin remains as Fe²⁺ and uses its coordination chemistry to reversibly bind oxygen. Cobalt sits at the centre of vitamin B₁₂. These metals literally keep us alive.
Materials science: Chromium's protective oxide layer makes stainless steel possible. Copper's conductivity powers our electrical world. Nickel's strength and corrosion resistance make it perfect for coins and marine applications.
Transition metal questions often test your ability to link properties to uses. Examiners love asking why a particular metal is chosen for a specific application — the answer always comes back to the four key properties.
Common exam mistakes to avoid: focus on the properties in the specification - coloured compounds, useful catalysts, and ions with different charges.
At GCSE, use straightforward wording: many transition metals form ions with different charges, many of their compounds are coloured, and many are useful catalysts.
Worked example: Step-by-Step: Ions with Different Charges in Transition Metals
Use iron as an example to show that transition metals can form ions with different charges. [4 marks]
Answer: Iron is a transition metal because it can form Fe²⁺ and Fe³⁺ ions.
Published by Revise Right. Use the official specification reference to check the requirements for your course. Content updated: 2026-03-19.
Move to the related lessons or back to the topic page when you need the wider sequence before exam-style practice.
Cobalt is used in rechargeable batteries and as a catalyst in industry, and its compounds can be coloured. Cobalt also sits at the centre of vitamin B₁₂.
Metallic nickel catalyses the hydrogenation of alkenes, the addition of hydrogen, which is used to turn vegetable oils into margarine. Ni²⁺ forms green compounds, and nickel is also used in rechargeable batteries and stainless steel.
The six transition metals to know are chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni) and copper (Cu). They are metals in the central part of the periodic table that form ions with different charges, form coloured compounds and are useful catalysts.
Iron forms Fe²⁺ ions, which give pale green compounds, and Fe³⁺ ions, which give yellow/brown compounds. Fe²⁺ in haemoglobin carries oxygen in blood, while Fe³⁺ is found in rust (Fe₂O₃).
Chromium is used in stainless steel because chromium oxide forms a protective layer that prevents rusting. Chromium forms Cr³⁺, which gives green compounds like Cr₂O₃, and Cr⁶⁺, which gives orange compounds like K₂Cr₂O₇.
Copper forms Cu⁺ ions, which give colourless compounds, and Cu²⁺ ions, which give blue compounds such as CuSO₄·5H₂O. Copper is an excellent electrical conductor, used in all electrical wiring, and also has antimicrobial properties.
Chromium forms Cr³⁺ compounds that are green, such as Cr₂O₃, and Cr⁶⁺ compounds that are orange, such as K₂Cr₂O₇. Chromium is used in stainless steel because chromium oxide forms a protective layer that prevents rusting.
Copper compounds with Cu²⁺ ions are blue, such as CuSO₄·5H₂O, while Cu⁺ compounds are colourless. Copper is an excellent electrical conductor, used in all electrical wiring, and has antimicrobial properties.
Transition metals form ions with different charges, many of their compounds are coloured, and many are useful catalysts. These named properties, such as iron forming Fe²⁺ and Fe³⁺, are the ones to focus on.
Iron in haemoglobin, as Fe²⁺, reversibly binds oxygen so blood can carry it around the body. Fe³⁺ is found in rust (Fe₂O₃), which shows why iron corrodes easily.
Iron can be shown to be a transition metal because it forms ions with different charges, Fe²⁺ and Fe³⁺. Giving two ions of the same metal demonstrates this defining property.