Topic 13: The periodic table—the transition metals

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.

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.

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.

[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.

[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.

What is the overall charge, $x$, of the chromium (III) complex?

$\left[\mathrm{Cr}\right({\mathrm{H}}_2\mathrm{O}{)}_4{\mathrm{Cl}}_2{]}^x$

A.  0

B.  1+

C.  2−

D.  3+

What is the overall charge, $x$, of the chromium (III) complex?

$\left[\mathrm{Cr}\right({\mathrm{H}}_2\mathrm{O}{)}_4{\mathrm{Cl}}_2{]}^x$

A.  0

B.  1+

C.  2−

D.  3+

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.

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.

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.

[Cr(OH)₆]³⁻ forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.

[Cr(OH)₆]³⁻ forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.

[Cr(OH)₆]³⁻ forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.

Describe the bond formation when urea acts as a ligand in a transition metal complex ion.

Describe the bond formation when urea acts as a ligand in a transition metal complex ion.

Describe the bond formation when urea acts as a ligand in a transition metal complex ion.

Explain why transition metals exhibit variable oxidation states in contrast to alkali metals.

Explain why transition metals exhibit variable oxidation states in contrast to alkali metals.

Explain why transition metals exhibit variable oxidation states in contrast to alkali metals.

Which complex ion contains a central ion with an oxidation state of +3?

A.  [PtCl₆]²⁻

B.  [Cu(H₂O)₄(OH)₂]

C.  [Ni(NH₃)₄(H₂O)₂]²⁺

D.  [Co(NH₃)₄Cl₂]⁺

Which complex ion contains a central ion with an oxidation state of +3?

A.  [PtCl₆]²⁻

B.  [Cu(H₂O)₄(OH)₂]

C.  [Ni(NH₃)₄(H₂O)₂]²⁺

D.  [Co(NH₃)₄Cl₂]⁺

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.

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.

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.

State and explain the magnetic property of iron(II) and iron(III) ions.

State and explain the magnetic property of iron(II) and iron(III) ions.

State and explain the magnetic property of iron(II) and iron(III) ions.

Which is correct for the complex ion in [Fe(H₂O)₅Cl]SO₄?

Which is correct for the complex ion in [Fe(H₂O)₅Cl]SO₄?

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.

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.

[Cr(OH₂)₆]³⁺ is violet and [Cr(NH₃)₆]³⁺ is yellow. What is correct?

The Colour Wheel

[Cr(OH₂)₆]³⁺ is violet and [Cr(NH₃)₆]³⁺ is yellow. What is correct?

The Colour Wheel

Explain why, when ligands bond to the iron ion causing the d-orbitals to split, the complex is coloured.

Explain why, when ligands bond to the iron ion causing the d-orbitals to split, the complex is coloured.

Explain why, when ligands bond to the iron ion causing the d-orbitals to split, the complex is coloured.

Identify the colour of the emission spectrum of lithium using section 17 of the data booklet.

Identify the colour of the emission spectrum of lithium using section 17 of the data booklet.

Identify the colour of the emission spectrum of lithium using section 17 of the data booklet.

Predict two other chemical properties you would expect rhenium to have, given its position in the periodic table.

Predict two other chemical properties you would expect rhenium to have, given its position in the periodic table.

Predict two other chemical properties you would expect rhenium to have, given its position in the periodic table.

Which electrons are removed from iron (Z = 26) to form iron(II)?

A. two 3d electrons

B. two 4s electrons

C. one 4s electron and one 3d electron

D. two 4p electrons

Which electrons are removed from iron (Z = 26) to form iron(II)?

A. two 3d electrons

B. two 4s electrons

C. one 4s electron and one 3d electron

D. two 4p electrons

What is the oxidation state of the metal ion and charge of the complex ion in [Co(NH₃)₄Cl₂]Cl?

What is the oxidation state of the metal ion and charge of the complex ion in [Co(NH₃)₄Cl₂]Cl?

Describe how the blue colour is produced in the Cu(II) solution. Refer to section 17 of the data booklet.

Describe how the blue colour is produced in the Cu(II) solution. Refer to section 17 of the data booklet.

Describe how the blue colour is produced in the Cu(II) solution. Refer to section 17 of the data booklet.

Examine the relationship between the Brønsted–Lowry and Lewis definitions of a base, referring to the ligands in the complex ion [CuCl₄]²⁻.

Examine the relationship between the Brønsted–Lowry and Lewis definitions of a base, referring to the ligands in the complex ion [CuCl₄]²⁻.

Examine the relationship between the Brønsted–Lowry and Lewis definitions of a base, referring to the ligands in the complex ion [CuCl₄]²⁻.

Deduce why the Cu(I) solution is colourless.

Deduce why the Cu(I) solution is colourless.

Deduce why the Cu(I) solution is colourless.

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.

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.

Outline the magnetic properties of iron by referring to its electron configuration.

Outline the magnetic properties of iron by referring to its electron configuration.

Outline the magnetic properties of iron by referring to its electron configuration.

Copper(II) ion solutions are blue. Suggest, giving your reason, a suitable wavelength of light for the analysis.

Copper(II) ion solutions are blue. Suggest, giving your reason, a suitable wavelength of light for the analysis.

Copper(II) ion solutions are blue. Suggest, giving your reason, a suitable wavelength of light for the analysis.

Which of these statements are correct?

I. Zinc is not a transition element.
II. Ligands are Lewis bases.
III. Manganese(II) chloride is paramagnetic.

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Which of these statements are correct?

I. Zinc is not a transition element.
II. Ligands are Lewis bases.
III. Manganese(II) chloride is paramagnetic.

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

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.

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.

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.

Determine the standard enthalpy of reaction ($\text{Δ}{H}_{\text{r}}^{⦵}$), in kJ mol⁻¹, for the oxidation of SO₂ to SO₃.

Determine the standard enthalpy of reaction ($\text{Δ}{H}_{\text{r}}^{⦵}$), in kJ mol⁻¹, for the oxidation of SO₂ to SO₃.

Determine the standard enthalpy of reaction ($\text{Δ}{H}_{\text{r}}^{⦵}$), in kJ mol⁻¹, for the oxidation of SO₂ to SO₃.

State the oxidation state of sulfur in copper (II) sulfate.

State the oxidation state of sulfur in copper (II) sulfate.

State the oxidation state of sulfur in copper (II) sulfate.

State the oxidation state of sulfur in copper (II) sulfate.

State the oxidation state of sulfur in copper (II) sulfate.

State the oxidation state of sulfur in copper (II) sulfate.