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, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
At a glance
- What StudyVector is
- An exam-practice platform with board-aligned questions, explanations, and adaptive next steps.
- This topic
- Transition Metals in A-Level Chemistry: explanation, examples, and practice links on this page.
- Who it’s for
- Students revising A-Level Chemistry for UK exams.
- Exam boards
- Practice is aligned to major specifications (AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP).
- Free plan
- Sign up free to use tutor paths and feedback on your answers. Free access is Free while we build toward our first production release. Pricing
- What makes it different
- Syllabus-shaped practice and progress tracking—not generic AI answers.
Topic has curated content entry with explanation, mistakes, and worked example. [auto-gate:promote; score=70.6]
Recommended next topic
Next step: Periodicity
Continue in the same course — structured practice and explanations on StudyVector.
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.
Mini lesson for Transition Metals
1. Understand the core idea
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.
Can you explain Transition Metals without copying the notes?
2. Turn it into marks
A solution containing the [Cu(H2O)6]2+ complex is blue. When excess concentrated HCl is added, the solution turns yellow-green.
Underline the method, evidence, or command-word move that would earn credit in A-Level Inorganic Chemistry.
3. Fix the likely mark leak
Watch for this mistake: Forgetting 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).
Write one correction rule before doing another practice question.
Practise this topic
Jump into adaptive, exam-style questions for Transition Metals. Free to start; sign in to save progress.
Transition Metals practice questions
These are original StudyVector questions for revision practice. They are not official exam-board questions.
Question 1
In one A-Level sentence, explain what Transition Metals is testing.
Answer: 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.
Mark focus: Precise definition and topic focus.
Question 2
A Transition Metals question uses an unfamiliar context. What should the answer do before adding detail?
Answer: It should name the process, variable, equation, particle model, or evidence being tested, then explain the result using precise scientific vocabulary.
Mark focus: Method selection and command-word control.
Question 3
A student makes this mistake: "Forgetting 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)." What should their next repair task be?
Answer: Do one Transition Metals question and review the mistake type.
Mark focus: Error correction and next-step practice.
Transition Metals flashcards
Core idea
What is the main idea in 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, f...
Common mistake
What mistake should you avoid in Transition Metals?
Forgetting 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).
Practice
What is one useful practice task for Transition Metals?
Answer one Transition Metals question and review the mistake type.
Exam board
How should you use board notes for Transition Metals?
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.
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, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP specifications.
Transition Metals exam questionsGet help with Transition Metals
Get a personalised explanation for Transition Metals from the StudyVector tutor. Ask follow-up questions and work through problems with step-by-step support.
Open tutorFree full access to Transition Metals
Sign up in 30 seconds to unlock step-by-step explanations, exam-style practice, instant feedback and on-demand coaching — completely free, no card required.
Try a practice question
Unlock Transition Metals practice questions
Get instant feedback, step-by-step help and exam-style practice — free, no card needed.
Start Free — No Card NeededAlready have an account? Log in
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-).