Complex Ions and Ligands

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Questions and Answers

What is the co-ordination number of the complex [Ag(NH3)2]+?

  • 1
  • 6
  • 2 (correct)
  • 4

All ligands must be negatively charged in order to bond with metal ions.

False (B)

Define a ligand.

A particle with a lone pair of electrons that bonds to metals by a co-ordinate bond.

The complex ion [CuCl4]2- has a co-ordination number of ______.

<p>4</p> Signup and view all the answers

Match the following complexes with their shapes:

<p>[Cu(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup> = Octahedral [PtCl<sub>4</sub>]<sup>2-</sup> = Square planar [CuCl<sub>4</sub>]<sup>2-</sup> = Tetrahedral [Ag(NH<sub>3</sub>)<sub>2</sub>]<sup>+</sup> = Linear</p> Signup and view all the answers

Which of the following ligands is a bidentate ligand?

<p>Ethanedioate ion (C<sub>2</sub>O<sub>4</sub><sup>2-</sup>) (C)</p> Signup and view all the answers

Haemoglobin binds oxygen more strongly than carbon monoxide.

<p>False (B)</p> Signup and view all the answers

What is the coordination number of the complex [Cu(EDTA)]2-?

<p>6</p> Signup and view all the answers

The ligand _________ forms four bonds in a complex with iron in haemoglobin.

<p>porphyrin</p> Signup and view all the answers

Match the following ligands with their types:

<p>Cl<sup>-</sup> = Unidentate EDTA<sup>4-</sup> = Multidentate 1,2-diaminoethane = Bidentate Porphyrin = Multidentate</p> Signup and view all the answers

Which complex represents a coordination sphere involving a unidentate ligand?

<p>[Fe(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup> (A)</p> Signup and view all the answers

Cyanide ions will bond to haemoglobin in preference to oxygen.

<p>True (A)</p> Signup and view all the answers

What is the oxidation state of chromium in the complex [Cr(NH3)6]3+?

<p>+3</p> Signup and view all the answers

Flashcards

Ligand

Particle with lone pair that bonds to metals via a co-ordinate bond.

Complex

Metal ion combined with co-ordinately bonded ligands.

Co-ordination number

Number of co-ordinate bonds from ligands to a metal ion.

Lewis base

A species that donates a lone pair of electrons.

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Lewis acid

A species that accepts a lone pair of electrons.

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Unidentate ligands

Ligands that form one coordinate bond to a metal ion.

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Examples of Unidentate ligands

Includes Cl-, OH-, CN-, H2O, and NH3.

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Bidentate ligands

Ligands that form two coordinate bonds to a metal ion.

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Examples of Bidentate ligands

Includes 1,2-diaminoethane and ethanedioate ion (C2O42-).

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Multidentate ligands

Ligands that form more than two coordinate bonds to a metal ion.

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Example of Multidentate ligand

EDTA4- forms 6 bonds with a metal ion.

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Haemoglobin

A globular protein with four Fe2+ centers, enabling oxygen transport.

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Toxicity of CO and CN-

CO and CN- are better ligands than O2, preventing oxygen transfer.

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Study Notes

Complex Ions Definitions

  • Ligand: A particle with lone pairs of electrons that bonds to a metal ion via a coordinate bond.
  • Complex: A metal ion with co-ordinately bonded ligands.
  • Coordination number: The number of coordinate bonds from ligands to a metal ion.
  • Lewis base: A lone pair donor.
  • Lewis acid: A lone pair acceptor.

Complex Ion Formation

  • Common ligands include H₂O, NH₃, and Cl⁻ ions, which have lone pairs of electrons.
  • Complexes form when ligands use their lone pairs to form coordinate bonds with a metal ion.
  • In the example of [CuCl₄]²⁻, four chloride ions act as ligands, each donating a lone pair to the Cu²⁺ ion.
  • Ligands act as Lewis bases because they donate lone pairs to transition metals to form coordinate bonds.
  • The metal ion acts as a Lewis acid because it accepts lone pairs.

Shapes of Complexes

  • Common shapes include linear (2), square planar (4), tetrahedral (4), and octahedral (6).
  • Coordination number reflects the number of ligands surrounding the metal ion.
  • Linear complexes (e.g., [Ag(NH₃)₂]⁺) are common with Ag⁺ ions, while square planar complexes (e.g., [PtCl₄]²⁻) are common with Pt²⁺ and Ni²⁺ and when ligands are too big for 6 to fit.
  • Tetrahedral complexes (e.g., [CuCl₄]²⁻) are common with small ligands (e.g., H₂O, NH₃).
  • Octahedral complexes (e.g., [Cu(H₂O)₆]²⁺) are also common with small ligands.

Types of Ligands

  • Unidentate ligands: Form one coordinate bond to a metal ion (e.g., Cl⁻, OH⁻, CN⁻, H₂O, NH₃).
  • Bidentate ligands: Form two coordinate bonds to a metal ion (e.g., 1,2-diaminoethane, ethanedioate ion (C₂O₄²⁻)).
  • Multidentate ligands: Form more than two coordinate bonds to a metal ion (e.g., EDTA⁴⁻, porphyrin).
    • EDTA⁴⁻ can form 6 bonds.
    • Porphyrin can form 4 bonds.

Haemoglobin

  • Haemoglobin is a protein containing four iron(II) (Fe²⁺) centres, each with a porphyrin ligand.
  • One of the coordination sites in the Haemoglobin is available to bind oxygen.
  • Oxygen is transported in blood bound to iron in haemoglobin.
  • Cyanide ions (CN⁻) and carbon monoxide (CO) are better ligands than oxygen (O₂), so they bind to haemoglobin in preference to oxygen, preventing oxygen transfer.

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