Transition Metals — A-Level Chemistry Revision
Revise Transition Metals for A-Level Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel and OCR.
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Go to PeriodicityWhat is Transition Metals?
Transition metals are elements in the d-block of the periodic table that form at least one stable ion with a partially filled d-orbital. This gives rise to their characteristic properties: variable oxidation states, formation of coloured ions in solution, and catalytic activity. Their ability to form complex ions with ligands, which are molecules or ions that donate a pair of electrons to the central metal ion, is a key feature of their chemistry.
Board notes: All boards require knowledge of the characteristic properties of transition metals. AQA often includes questions on catalysis, including examples like the use of iron in the Haber process. Edexcel places a strong emphasis on ligand substitution reactions and the associated colour changes. OCR frequently tests the different shapes of complex ions (e.g., octahedral, tetrahedral, square planar) and isomerism in complexes (cis-trans and optical).
Step-by-step explanationWorked example
A solution containing the [Cu(H2O)6]2+ complex is blue. When excess concentrated HCl is added, the solution turns yellow-green. Explain this observation. Step 1: The initial blue colour is due to the hexaquacopper(II) complex ion. Step 2: Chloride ions are larger ligands than water molecules and can replace them in a ligand substitution reaction. Step 3: The equation for the reaction is [Cu(H2O)6]2+(aq) + 4Cl-(aq) <=> [CuCl4]2-(aq) + 6H2O(l). The new complex, tetrachlorocuprate(II), has a different shape (tetrahedral) and a different d-orbital splitting, causing it to appear yellow-green.
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Common mistakes
- 1Forgetting that scandium and zinc are d-block elements but not technically transition metals. Scandium only forms the Sc3+ ion (with an empty d-orbital) and zinc only forms the Zn2+ ion (with a full d-orbital).
- 2Confusing coordination number with oxidation state. The coordination number is the number of coordinate bonds to the central metal ion, while the oxidation state is the charge on the metal ion.
- 3Incorrectly predicting the colours of complex ions. While students need to know some specific examples (e.g., Cu2+(aq) is blue, Fe2+(aq) is pale green, Fe3+(aq) is yellow/brown), the exact colour arises from d-orbital splitting and is complex to predict without more information.
Transition Metals exam questions
Exam-style questions for Transition Metals with mark-scheme style solutions and timing practice. Aligned to AQA, Edexcel and OCR specifications.
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Transition Metals
Core concept
Transition metals are elements in the d-block of the periodic table that form at least one stable ion with a partially filled d-orbital. This gives rise to their characteristic properties: variable ox…
Frequently asked questions
Why do transition metal compounds have colour?
When ligands bond to a transition metal ion, the d-orbitals are split into different energy levels. Electrons can be promoted from a lower to a higher d-orbital by absorbing light of a specific frequency from the visible spectrum. The colour we see is the complementary colour, made up of the frequencies of light that are not absorbed.
What is a ligand?
A ligand is a molecule or ion that can donate a pair of electrons to a central transition metal ion to form a coordinate (or dative covalent) bond. Examples include water (H2O), ammonia (NH3), and chloride ions (Cl-).