Directly related questions
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20N.2.hl.TZ0.6b:
The electron configuration of copper makes it a useful metal.
Explain why a copper(II) solution is blue, using section 17 of the data booklet.
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20N.2.hl.TZ0.6b:
The electron configuration of copper makes it a useful metal.
Explain why a copper(II) solution is blue, using section 17 of the data booklet.
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20N.2.hl.TZ0.b:
The electron configuration of copper makes it a useful metal.
Explain why a copper(II) solution is blue, using section 17 of the data booklet.
- 21M.1.hl.TZ2.8: Which factor does not affect the colour of a complex ion? A. temperature of the solution B. ...
- 21M.1.hl.TZ2.8: Which factor does not affect the colour of a complex ion? A. temperature of the solution B. ...
- 18M.1.hl.TZ2.8: Part of the spectrochemical series is shown for transition metal complexes. I−< Cl− < H2O...
- 18M.1.hl.TZ2.8: Part of the spectrochemical series is shown for transition metal complexes. I−< Cl− < H2O...
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22M.1.hl.TZ2.8:
[Cr(OH2)6]3+ is violet and [Cr(NH3)6]3+ is yellow. What is correct?
The Colour Wheel
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22M.1.hl.TZ2.8:
[Cr(OH2)6]3+ is violet and [Cr(NH3)6]3+ is yellow. What is correct?
The Colour Wheel
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22M.2.hl.TZ1.4e:
Mg(OH)+ is a complex ion, but Mg is not regarded as a transition metal. Contrast Mg with manganese, Mn, in terms of one characteristic chemical property of transition metals, other than complex ion formation.
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22M.2.hl.TZ1.4e:
Mg(OH)+ is a complex ion, but Mg is not regarded as a transition metal. Contrast Mg with manganese, Mn, in terms of one characteristic chemical property of transition metals, other than complex ion formation.
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22M.2.hl.TZ1.e:
Mg(OH)+ is a complex ion, but Mg is not regarded as a transition metal. Contrast Mg with manganese, Mn, in terms of one characteristic chemical property of transition metals, other than complex ion formation.
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19M.2.hl.TZ1.6b:
Explain why, when ligands bond to the iron ion causing the d-orbitals to split, the complex is coloured.
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19M.2.hl.TZ1.6b:
Explain why, when ligands bond to the iron ion causing the d-orbitals to split, the complex is coloured.
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19M.2.hl.TZ1.b:
Explain why, when ligands bond to the iron ion causing the d-orbitals to split, the complex is coloured.
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19N.2.hl.TZ0.6f(i):
Describe how the blue colour is produced in the Cu(II) solution. Refer to section 17 of the data booklet.
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19N.2.hl.TZ0.6f(i):
Describe how the blue colour is produced in the Cu(II) solution. Refer to section 17 of the data booklet.
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19N.2.hl.TZ0.f(i):
Describe how the blue colour is produced in the Cu(II) solution. Refer to section 17 of the data booklet.
- 19N.1.hl.TZ0.8: What is the effect of a stronger ligand?
- 19N.1.hl.TZ0.8: What is the effect of a stronger ligand?
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22N.1.hl.TZ0.6:
Which best explains why complexes of d-block elements are coloured?
A. Light is absorbed when electrons are promoted between d orbitals.B. Light is emitted when electrons are promoted between d orbitals.
C. Light is absorbed when electrons return to lower energy d orbitals.
D. Light is emitted when electrons return to lower energy d orbitals.
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22N.1.hl.TZ0.6:
Which best explains why complexes of d-block elements are coloured?
A. Light is absorbed when electrons are promoted between d orbitals.B. Light is emitted when electrons are promoted between d orbitals.
C. Light is absorbed when electrons return to lower energy d orbitals.
D. Light is emitted when electrons return to lower energy d orbitals.
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17N.1.hl.TZ0.10:
[CoCl6]3– is orange while [Co(NH3)6]3+ is yellow. Which statement is correct?
A. [CoCl6]3– absorbs orange light.
B. The oxidation state of cobalt is different in each complex.
C. The different colours are due to the different charges on the complex.
D. The different ligands cause different splitting in the 3d orbitals.
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17N.1.hl.TZ0.10:
[CoCl6]3– is orange while [Co(NH3)6]3+ is yellow. Which statement is correct?
A. [CoCl6]3– absorbs orange light.
B. The oxidation state of cobalt is different in each complex.
C. The different colours are due to the different charges on the complex.
D. The different ligands cause different splitting in the 3d orbitals.
- 18M.1.hl.TZ1.8: Which complex has the greatest d orbital splitting?
- 18M.1.hl.TZ1.8: Which complex has the greatest d orbital splitting?
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18N.3.hl.TZ0.1c:
Copper(II) ion solutions are blue. Suggest, giving your reason, a suitable wavelength of light for the analysis.
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18N.3.hl.TZ0.1c:
Copper(II) ion solutions are blue. Suggest, giving your reason, a suitable wavelength of light for the analysis.
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18N.3.hl.TZ0.c:
Copper(II) ion solutions are blue. Suggest, giving your reason, a suitable wavelength of light for the analysis.
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19M.3.hl.TZ1.3b(i):
Identify the colour of the emission spectrum of lithium using section 17 of the data booklet.
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19M.3.hl.TZ1.3b(i):
Identify the colour of the emission spectrum of lithium using section 17 of the data booklet.
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19M.3.hl.TZ1.b(i):
Identify the colour of the emission spectrum of lithium using section 17 of the data booklet.
- 19M.1.hl.TZ2.6: How is colour produced in transition metal complexes? A. Light is absorbed when electrons are...
- 19M.1.hl.TZ2.6: How is colour produced in transition metal complexes? A. Light is absorbed when electrons are...
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19N.2.hl.TZ0.6f(ii):
Deduce why the Cu(I) solution is colourless.
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19N.2.hl.TZ0.6f(ii):
Deduce why the Cu(I) solution is colourless.
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19N.2.hl.TZ0.f(ii):
Deduce why the Cu(I) solution is colourless.
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19N.2.hl.TZ0.6f(iv):
Examine the relationship between the Brønsted–Lowry and Lewis definitions of a base, referring to the ligands in the complex ion [CuCl4]2−.
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19N.2.hl.TZ0.6f(iv):
Examine the relationship between the Brønsted–Lowry and Lewis definitions of a base, referring to the ligands in the complex ion [CuCl4]2−.
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19N.2.hl.TZ0.f(iv):
Examine the relationship between the Brønsted–Lowry and Lewis definitions of a base, referring to the ligands in the complex ion [CuCl4]2−.
- 21M.2.hl.TZ1.3f: Outline why, unlike typical transition metals, zinc compounds are not coloured.
- 21M.2.hl.TZ1.3f: Outline why, unlike typical transition metals, zinc compounds are not coloured.
- 21M.2.hl.TZ1.f: Outline why, unlike typical transition metals, zinc compounds are not coloured.
- 21M.2.hl.TZ1.3g: Transition metals like iron can form complex ions. Discuss the bonding between transition metals...
- 21M.2.hl.TZ1.3g: Transition metals like iron can form complex ions. Discuss the bonding between transition metals...
- 21M.2.hl.TZ1.g: Transition metals like iron can form complex ions. Discuss the bonding between transition metals...
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21M.2.hl.TZ2.2b(iii):
Deduce, giving a reason, which complex ion [Cr(CN)6]3− or [Cr(OH)6]3− absorbs higher energy light. Use section 15 of the data booklet.
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21M.2.hl.TZ2.2b(iii):
Deduce, giving a reason, which complex ion [Cr(CN)6]3− or [Cr(OH)6]3− absorbs higher energy light. Use section 15 of the data booklet.
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21M.2.hl.TZ2.b(iii):
Deduce, giving a reason, which complex ion [Cr(CN)6]3− or [Cr(OH)6]3− absorbs higher energy light. Use section 15 of the data booklet.
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21M.2.hl.TZ2.2b(iv):
[Cr(OH)6]3− forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.
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21M.2.hl.TZ2.2b(iv):
[Cr(OH)6]3− forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.
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21M.2.hl.TZ2.b(iv):
[Cr(OH)6]3− forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.
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21N.2.hl.TZ0.9b(iii):
Copper is a transition metal that forms different coloured complexes. A complex [Cu(H2O)6]2+ (aq) changes colour when excess Cl− (aq) is added.
Explain the cause of this colour change, using sections 3 and 15 from the data booklet.
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21N.2.hl.TZ0.9b(iii):
Copper is a transition metal that forms different coloured complexes. A complex [Cu(H2O)6]2+ (aq) changes colour when excess Cl− (aq) is added.
Explain the cause of this colour change, using sections 3 and 15 from the data booklet.
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21N.2.hl.TZ0.b(iii):
Copper is a transition metal that forms different coloured complexes. A complex [Cu(H2O)6]2+ (aq) changes colour when excess Cl− (aq) is added.
Explain the cause of this colour change, using sections 3 and 15 from the data booklet.
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22M.1.hl.TZ1.8:
Why is hydrated copper (II) sulfate blue?
A. Blue light is emitted when electrons return to lower d-orbitals.
B. Light complimentary to blue is absorbed when electrons return to lower d-orbitals.
C. Blue light is emitted when electrons are promoted between d-orbitals.
D. Light complimentary to blue is absorbed when electrons are promoted between d-orbitals.
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22M.1.hl.TZ1.8:
Why is hydrated copper (II) sulfate blue?
A. Blue light is emitted when electrons return to lower d-orbitals.
B. Light complimentary to blue is absorbed when electrons return to lower d-orbitals.
C. Blue light is emitted when electrons are promoted between d-orbitals.
D. Light complimentary to blue is absorbed when electrons are promoted between d-orbitals.
- 22M.2.hl.TZ2.7d: Explain why transition metal cyanide complexes are coloured.
- 22M.2.hl.TZ2.7d: Explain why transition metal cyanide complexes are coloured.
- 22M.2.hl.TZ2.d: Explain why transition metal cyanide complexes are coloured.