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Coordination Compounds and Nomenclature02:54

Coordination Compounds and Nomenclature

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In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...
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Metal-Ligand Bonds02:51

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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.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
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Coordination Number and Geometry02:57

Coordination Number and Geometry

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For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
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Ladder Diagrams: Complexation Equilibria01:07

Ladder Diagrams: Complexation Equilibria

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Ladder diagrams are useful for evaluating equilibria involving metal-ligand complexes. The vertical scale of the ladder diagram represents the concentration of unreacted or free ligand, pL. The horizontal lines on the scale depict the log of stepwise formation constants for metal-ligand complexes and indicate the dominant species in all the regions.
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1° Amines to Diazonium or Aryldiazonium Salts: Diazotization with NaNO2 Overview01:26

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Nitrous acid and nitric acids are two types of acids containing nitrogen, among which nitrous acid is weaker than nitric acid. Nitrous acid with a pKa value of 3.37 ionizes in water to give a nitrite ion and the hydronium ion.
The nitrous acid is unstable. Hence, it is formed in situ from a solution of sodium nitrite and cold aqueous acids such as hydrochloric or sulfuric acid. In an acidic solution, the –OH group of nitrous acid undergoes protonation to give oxonium ion, followed by...
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Lewis Structures of Molecular Compounds and Polyatomic Ions02:54

Lewis Structures of Molecular Compounds and Polyatomic Ions

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To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:
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Dinitrogen complexes N2L2 (L = N2, CO, CS, NO+, CN-).

Yahui Li1, Chengxiang Ding1, Lianbin Xie1

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This study investigates the stability and bonding of N2L2 compounds using quantum chemical calculations. The N2(CS)2 adduct shows slight stability, while others are unstable, with dissociation pathways analyzed.

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Area of Science:

  • Computational Chemistry
  • Quantum Chemistry
  • Theoretical Inorganic Chemistry

Background:

  • Investigation of isoelectronic compounds N2L2 (L = N2, CO, CS, NO+, CN-) using ab initio and density functional theory.
  • Analysis of equilibrium structures and vibrational spectra to understand molecular properties.

Purpose of the Study:

  • To determine the thermodynamic stability and dissociation pathways of N2L2 compounds.
  • To elucidate the bonding situations and electronic states involved in these complexes.
  • To identify spectroscopic signatures for experimental characterization.

Main Methods:

  • Quantum chemical calculations, including ab initio methods and density functional theory (DFT).
  • Analysis of equilibrium structures, vibrational spectra, and thermodynamic stability (ΔG298).
  • Energy decomposition analysis with natural orbital for chemical valence (EDA-NOCV) to describe bonding.

Main Results:

  • N2L2 compounds exhibit a trans-periplanar arrangement of L2 ligands.
  • Most complexes are thermodynamically unstable, except for N2(CS)2 which is slightly stable (ΔG298 = 4 kcal mol-1).
  • Heterolytic dissociation (N2L2 → N2 + 2L) is energetically favored over homolytic dissociation.
  • Vibrational spectra show characteristic shifts in ligand stretching frequencies, aiding identification.
  • Bonding analysis reveals charge donation from L to N2, with variations based on the ligand.

Conclusions:

  • The study provides a detailed theoretical understanding of N2L2 compounds' stability and bonding.
  • A donor-acceptor model (N2→(N2)←N2) effectively explains the dissociation mechanisms.
  • Calculated vibrational frequencies offer a route for experimental verification of these novel compounds.