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Related Concept Videos

Complexation Equilibria: Factors Influencing Stability of Complexes01:09

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In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
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In a radical reaction, the concentration of starting materials governs the selectivity of a radical. For example, the reaction between an alkyl halide and an alkene, in the presence of tin hydride and AIBN, begins with the generation of a tin radical. The generated radical then abstracts halogen from the alkyl halide, producing an alkyl radical. This alkyl radical can either react with tin hydride, yielding an alkane, or add to an alkene, generating a nitrile-stabilized radical, eventually...
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Complexation reactions take place when dative or coordinate covalent bonds form between metal ions and ligands. The compounds formed in these reactions are called coordination compounds. The number of bonds formed between the metal ion and the ligands is called its coordination number. Generally, most metal ions in an aqueous solution are solvated by water molecules and thus exist as aqua complexes.
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The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
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In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
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A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
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Does Metal Ion Complexation Make Radical Clocks Run Fast? An Experimental Perspective.

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The rate constant for cumyloxyl radical β-scission increases with added electrolytes in acetonitrile, influenced by cation size. This effect is weaker in solution than predicted due to solvent interactions.

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Area of Science:

  • Physical Chemistry
  • Organic Chemistry
  • Reaction Kinetics

Background:

  • The β-scission of cumyloxyl radical is a key reaction in radical chemistry.
  • Understanding solvent and electrolyte effects is crucial for controlling reaction rates.

Purpose of the Study:

  • To investigate the influence of various electrolytes on the rate constant (kβ) of cumyloxyl radical β-scission.
  • To elucidate the role of ion-dipole interactions in the reaction mechanism.

Main Methods:

  • Kinetic measurements of β-scission in acetonitrile and DMSO.
  • Addition of various electrolytes (Li+, Mg2+, Na+, nBu4N+) to study their effects.
  • Molecular Orbital (MO) calculations for gas-phase analysis.

Main Results:

  • In acetonitrile, kβ increased with cation size (Li+ > Mg2+ ≈ Na+ > nBu4N+).
  • Ion-dipole interactions in the transition state stabilize the developing carbonyl group.
  • This effect was attenuated in solution compared to gas-phase MO calculations.
  • Electrolytes showed no significant effect in DMSO due to stronger cation-solvent interactions.

Conclusions:

  • Electrolyte effects on β-scission rates are solvent-dependent.
  • Ion-dipole interactions play a role, but are modulated by solvation.
  • The choice of solvent significantly impacts the influence of electrolytes on radical reaction kinetics.