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Questions and Answers
What is the color of the solution when Cr³⁺ reacts with excess NH₃?
What is the color of the solution when Cr³⁺ reacts with excess NH₃?
Which Fe ion forms a yellow solution?
Which Fe ion forms a yellow solution?
What is the color of Cu²⁺ in solution?
What is the color of Cu²⁺ in solution?
Which ion forms a pale pink solution?
Which ion forms a pale pink solution?
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What is the charge on the Fe ion that can be oxidized with MnO₄⁻ in acidic conditions?
What is the charge on the Fe ion that can be oxidized with MnO₄⁻ in acidic conditions?
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Which transition metal forms a purple solution with excess NH₃?
Which transition metal forms a purple solution with excess NH₃?
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Which transition metal forms a brown precipitate with OH⁻ ions?
Which transition metal forms a brown precipitate with OH⁻ ions?
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What happens to the color of Fe²⁺ when oxidized to Fe³⁺?
What happens to the color of Fe²⁺ when oxidized to Fe³⁺?
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What is the color of the precipitate formed by Cu²⁺ with OH⁻ ions?
What is the color of the precipitate formed by Cu²⁺ with OH⁻ ions?
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Which ion forms a green solution followed by a green precipitate when reacting with NH₃?
Which ion forms a green solution followed by a green precipitate when reacting with NH₃?
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Study Notes
Transition Elements Properties
- Transition metals are elements in the d-block of the periodic table that form one or more stable ions with a partially filled d-orbital.
- They lose electrons to form positive ions, with the s-orbital electrons being removed first.
- Transition metals have similar physical properties, including similar atomic radius, high densities, and high melting points.
- They also have special chemical properties: forming complexes, forming colored ions in solution, having variable oxidation states, and being good catalysts.
Variable Oxidation States
- Transition metals have variable oxidation states because the 4s and 3d orbitals are very close in energy levels.
- This makes it possible for electrons to be lost from both orbitals relatively easily, and the remaining electrons can form stable configurations.
Catalysts
- Cu²⁺ is used as a catalyst for the reaction of Zn with acids.
- MnO₂ is used as a catalyst for the decomposition of H₂O₂.
- Using catalysts in industry reduces energy usage, but there is also an increased risk from toxicity of many transition metals.
Complexes and Ligands
- Transition metals form complexes, consisting of a central metal ion surrounded by ligands.
- Ligands are molecules or ions with a lone electron pair that is able to form a dative (coordinate) bond to the central metal ion by donation of this electron pair.
- Common ligands include Cl⁻, H₂O, and NH₃.
Types of Ligands
- Monodentate ligands each form one coordinate bond (e.g., H₂O, Cl⁻, NH₃).
- Bidentate ligands each form two coordinate bonds (e.g., NH₂CH₂CH₂NH₂).
- Hexadentate ligands each form six coordinate bonds (e.g., EDTA⁴⁻).
- Polydentate and multidentate ligands are general terms for any ligands that form more than one coordinate bond.
Coordination Number
- The coordination number of a transition metal complex is the total number of coordinate bonds formed with the central metal ion.
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Description
Detailed notes for Module 5.3 on Transition Elements in OCR A Chemistry A-level. The notes cover properties of transition elements, such as forming stable ions with partially filled d-orbitals and losing electrons to form positive ions. Licensed under CC BY-NC-ND 4.0.
