Explain the difference between 1,2- and 1,3- chelating amines? Show example.

Denticity refers to the number of donor groups in a single ligand that bind to a central atom in a coordination complex. In many cases, only one atom in the ligand binds to the metal, so the denticity equals one, and the ligand is said to be monodentate (sometimes called unidentate).

Get eRawanna/Transit-Pass Details: Get eRawanna/Transit-Pass Details: Screen reader Access; A A+ A-; rs rs rs; Hindi. Dimethylglyoxime (dmg) is a bidentate ligand chelating large amounts of metals. Only two dmg molecules per metal center are needed, because Ni (dmg)22 + has a square-planar geometry. To the aqueous array, add 1 per cent dmg. What is the role of DMG in analytical chemistry?

Dimethylglyoxime (DMG) is a complexing ligand. D Dimethylglyoxime forms a number of mixed ligand complexes with N -acetylglycine with metals such as VO (IV), Ni (II), Zn (II), Pd (II), Cd (II) and Pb (II). It is a useful reagent for the spectrophotometric determination of Co (II), Fe (II), Ni (II), Pd (II) and Re (VII). DMG N,N-DIMETHYLGLYCINE Find entries where: DMG is present as a standalone ligand. DMG as a non-polymer is covalently linked to polymer or other heterogen groups.

1 Answer

1,2-DIIMINE LIGANDS (CHELATING AGENTS)

An example of a 1,2-diimine is the dimethylglyoximato ligand (which somewhat resembles a conjugated diene for Diels-Alder reactions).

Name:

bis-(DMG)nickel(II)

As a general rule, 'bis' is used to indicate two of the same, complicated ligand.

Chemical formula:

#'Ni'('DMG')_2#

If we call one of the imine carbons 'carbon-1', then the other imine carbon is one atom away (meaning, on 'carbon-2'). Hence, we can call this a 1,2-diimine.

Each dimethylglyoximato ligand (abbreviated DMG in compound names) has a net charge of #mathbf(-1)#, and each nitrogen acts as a binding site due to their lone pairs of electrons.

If you recall the chelate effect, it essentially states that the binding of more than one 'tooth' is entropically favored, relative to binding with one 'tooth'.

This two-'tooth' binding mode requires that the ligand's binding sites be cis (same-side). Therefore, DMG is a bidentate ligand, binding preferentially cis.

1,3-DIIMINE LIGANDS (CHELATING AGENTS)

An example of this that I can find in my book is the N,N'-diphenyl-2,4-pentanediiminato ligand.

Name:

dichloro(nacnac)nickel(II)

As a general rule, complicated ligands tend to be in parentheses.

Chemical formula:

#['Ni'('nacnac')'Cl'_2]^(-)#

Fortunately, this ligand has a simple 'nickname': nacnac.

Dmg Molecule

Like DMG, nacnac is a bidentate ligand, and its two binding sites are the two nitrogens, each using their lone pair of electrons. However, its imine carbons are 1,3 to each other instead.

This ligand also has a net charge of #mathbf(-1)#.

It substantially favors binding cis to the metal, again due to the chelate effect favoring the binding of both 'teeth' rather than only one of them.

Related questions

Coordination compounds, such as the FeCl₄^- ion and CrCl₃ 6 NH₃, are called such because they contain ions or molecules linked, or coordinated, to a transition metal. They are also known as complex ions or coordination complexes because they are Lewis acid-base complexes. The ions or molecules that bind to transition-metal ions to form these complexes are called ligands (from Latin, 'to tie or bind'). The number of ligands bound to the transition metal ion is called the coordination number.

Although coordination complexes are particularly important in the chemistry of the transition metals, some main group elements also form complexes. Aluminum, tin, and lead, for example, form complexes such as the AlF₆^3-, SnCl₄^2- and PbI₄^2- ions.

Alfred Werner developed a model of coordination complexs which explains the following observations.

• At least three different cobalt(III) complexes can be isolated when CoCl₂ is dissolved in aqueous ammonia and then oxidized by air to the +3 oxidation state. A fourth complex can be made by slightly different techniques. These complexes have different colors and different empirical formulas.

• The reactivity of the ammonia in these complexes has been drastically reduced. By itself, ammonia reacts rapidly with hydrochloric acid to form ammonium chloride.

NH₃(aq) + HCl(aq) NH₄⁺(aq) + Cl^-(aq)

These complexes don't react with hydrochloric acid, even at 100^oC.

• Solutions of the Cl^- ion react with Ag⁺ ion to form a white precipitate of AgCl.

Ag⁺(aq) + Cl^-(aq) AgCl(s)

When excess Ag⁺ ion is added to solutions of the CoCl₃ 6 NH₃ and CoCl₃ 5 NH₃ H₂O complexes, three moles of AgCl are formed for each mole of complex in solution, as might be expected. However, only two of the Cl^- ions in the CoCl₃ 5 NH₃ complex and only one of the Cl^- ions in CoCl₃ 4 NH₃ can be precipitated with Ag⁺ ions.

• Measurements of the conductivity of aqueous solutions of these complexes suggest that the CoCl₃ 6 NH₃ and CoCl₃ 5 NH₃ H₂O complexes dissociate in water to give a total of four ions. CoCl₃ 5 NH₃ dissociates to give three ions, and CoCl₃ 4 NH₃ dissociates to give only two ions.

Werner explained these observations by suggesting that transition-metal ions such as the Co³⁺ ion have a primary valence and a secondary valence. The primary valence is the number of negative ions needed to satisfy the charge on the metal ion. In each of the cobalt(III) complexes previously described, three Cl^- ions are needed to satisfy the primary valence of the Co³⁺ ion.

The secondary valence is the number of ions of molecules that are coordinated to the metal ion. Werner assumed that the secondary valence of the transition metal in these cobalt(III) complexes is six. The formulas of these compounds can therefore be written as follows.

Dmg Ligand

The cobalt ion is coordinated to a total of six ligands in each complex, which satisfies the secondary valence of this ion. Each complex also has a total of three chloride ions that satisfy the primary valence. Some of the Cl^- ions are free to dissociate when the complex dissolves in water. Others are bound to the Co³⁺ ion and neither dissociate nor react with Ag⁺.

The [Co(NH₃)₆]Cl₃ complex dissociates in water to give a total of four ions, and all three Cl^- ions are free to react with Ag⁺ ion.

One of the chloride ions is bound to the cobalt in the [Co(NH₃)₅Cl]Cl₂ complex. Only three ions are formed when this compound dissolves in water, and only two Cl^- ions are free to precipitate with Ag⁺ ions.

Once again, the three Cl^- ions are free to dissociate when [Co(NH₃)₅(H₂O)]Cl₃ dissolves in water, and they precipitate when Ag⁺ ions are added to the solution.

Two of the chloride ions are bound to the cobalt in [Co(NH₃)₄Cl₂]Cl. Only two ions are formed when this compound dissolves in water, and only one Cl^- ion is free to precipitate with Ag⁺ ions.

Werner assumed that transition-metal complexes had definite shapes. According to his theory, the ligands in six-coordinate cobalt(III) complexes are oriented toward the corners of an octahedron, as shown in the figure below.

Any ion or molecule with a pair of nonbonding electrons can be a ligand. Many ligands are described as monodentate (literally, 'one-toothed') because they 'bite' the metal in only one place. Typical monodentate ligands are given in the figure below.

Other ligands can attach to the metal more than once. Ethylenediamine (en) is a typical bidentate ligand.

Each end of this molecule contains a pair of nonbonding electrons that can form a covalent bond to a metal ion. Ethylenediamine is also an example of a chelating ligand. The term chelate comes from a Greek stem meaning 'claw.' It is used to describe ligands that can grab the metal in two or more places, the way a claw would.

Linking ethylene- diamine fragments gives tridentate ligands and tetradentate ligands, such as diethylenetriamine (dien) and triethylenetetramine (trien). Adding four -CH₂CO₂^- groups to an ethylenediamine framework gives a hexadentate ligand, which can single-handedly satisfy the secondary valence of a transition-metal ion.

Typical Coordination Numbers

Transition-metal complexes have been characterized with coordination numbers that range from 1 to 12, but the most common coordination numbers are 2, 4, and 6. Examples of complexes with these coordination numbers are given in the table below.

Examples of Common Coordination Numbers

Note that the charge on the complex is always the sum of the charges on the ions or molecules that form the complex.

Cu²⁺ + 4 NH₃ Cu(NH₃)₄²⁺

Pb²⁺ + 2 OAc^- Pb(OAc)₂

Fe²⁺ + 6 CN^- Fe(CN)₆^4-

Note also that the coordination number of a complex often increases as the charge on the metal ion becomes larger.

Cu⁺ + 2 NH₃ Cu(NH₃)₂⁺

Cu²⁺ + 4 NH₃ Cu(NH₃)₄²⁺

Dmg Ligand

G. N. Lewis was the first to recognize that the reaction between a transition-metal ion and ligands to form a coordination complex was analogous to the reaction between the H⁺ and OH^- ions to form water. The reaction between H⁺ and OH^- ions involves the donation of a pair of electrons from the OH^- ion to the H⁺ ion to form a covalent bond.

The H⁺ ion can be described as an electron-pair acceptor. The OH^- ion, on the other hand, is an electron-pair donor. Lewis argued that any ion or molecule that behaves like the H⁺ ion should be an acid. Conversely, any ion or molecule that behaves like the OH^- ion should be a base. A Lewis acid is therefore any ion or molecule that can accept a pair of electrons. A Lewis base is an ion or molecule that can donate a pair of electrons.

When Co³⁺ ions react with ammonia, the Co³⁺ ion accepts pairs of nonbonding electrons from six NH₃ ligands to form covalent cobalt-nitrogen bonds as shown in the figure below.

The metal ion is therefore a Lewis acid, and the ligands coordinated to this metal ion are Lewis bases.

Dmg Ligand Denticity

The Co³⁺ ion is an electron-pair acceptor, or Lewis acid, because it has empty valence-shell orbitals that can be used to hold pairs of electrons. To emphasize these empty valence orbitals we can write the configuration of the Co³⁺ ion as follows.

Co³⁺: [Ar] 3d⁶ 4s⁰ 4p⁰

There is room in the valence shell of this ion for 12 more electrons. (Four electrons can be added to the 3d subshell, two to the 4s orbital, and six to the 4p subshell.) The NH₃ molecule is an electron-pair donor, or Lewis base, because it has a pair of nonbonding electrons on the nitrogen atom.

According to this model, transition-metal ions form coordination complexes because they have empty valence-shell orbitals that can accept pairs of electrons from a Lewis base. Ligands must therefore be Lewis bases: They must contain at least one pair of nonbonding electrons that can be donated to a metal ion.