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Alfa Aesar is a leading manufacturer and supplier of research chemicals, pure metals and materials for a wide span of applications. Dioxime and pyridine-2-aldoxime complexes of Re (CO) 3 + can be readily generated by reaction of the ligands with Re (CO) 5 X or Re (CO) 3 (H 2 O 3) Br. These compounds represent a significant addition to the oxime coordination chemistry of d 6 metal complexes. In all cases, the resultant complexes are typical Re(I) compounds with a facial. The CAS register number of 2,6-Dichloropyridine is 2402-78-0. It also can be called as Pyridine, 2,6-dichloro- and the IUPAC name about this chemical is 2,6-dichloropyridine. Balance the reaction of NaCl + Mg(C2H3O2)2 = NaC2H3O2 + MgCl2 using this chemical equation balancer! Periodic Table. Chemical Equation Balancer NaCl + Mg(C2H3O2)2 = NaC2H3O2 + MgCl2. Balanced Chemical Equation. 2 NaCl + Mg(C 2 H 3 O 2) 2 = 2 NaC 2 H 3 O 2 + MgCl 2. Reaction Information. Sodium Chloride + Magnesium. Hello Everybody! I have been doing the D3/K2 combination for the last 4 months (40k D3) and one Life extension super K taken with coconut oil and it has cleared me at least 60-70% I have just started using the Magnesium oil last 2 weeks and it is also helping me clear more!

Incubated into 6 mL 10 mM aqueous solution of Co(DMG)2Cl2. The 2-((pyridine-4-ylmethyl)amino)ethane-1-thiol was functionalized onto the TNPs’ surface using Au-S bond leaving the pyridine group free onto the surface which further attached to Co(DMG)2Cl2. 2,6-Dimethylanilinium chloride monohydrate Wajda Smirani, Olfa Amri and Mohamed Rzaigui S1. Comment As part of our ongoing studies of organic-inorganic hybrid networks containing the 2,6-xylidinium cation (Mrad et al., 2006; Abid et al., 2007) we now report the synthesis and structure of the title compound, (I).

Associated Data

Crystal structure: contains datablocks I, global. DOI: 10.1107/S1600536810020568/pv2285sup1.cif

Structure factors: contains datablocks I. DOI: 10.1107/S1600536810020568/pv2285Isup2.hkl

Additional supplementary materials: crystallographic information; 3D view; checkCIF report

Abstract

In the crystal structure of the title compound, C₈H₁₂N⁺·Cl⁻, all H atoms bonded to the ammonium N atom are hydrogen bonded to the chloride ions, with N⋯Cl distances in the range 3.080 (2)–3.136 (2) Å, resulting in 16-membered macrocyclic rings involving four formula units of the title compound.

Related literature

For background to phase transition materials see: Li et al. (2008 ▶); Zhang et al. (2009).

Experimental

Crystal data

• C₈H₁₂N⁺·Cl⁻

• M_r = 157.64

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• Monoclinic,

• a = 9.4739 (19) Å

• b = 9.894 (2) Å

• c = 9.6709 (19) Å

• β = 96.31 (3)°

• V = 901.0 (3) ų

• Z = 4

• Mo Kα radiation

• μ = 0.35 mm⁻¹

• T = 293 K

• 0.4 × 0.3 × 0.2 mm

Data collection

• Rigaku Mercury2 diffractometer

• Absorption correction: multi-scan (CrystalClear; Rigaku, 2005 ▶) T_min = 0.880, T_max = 0.932

• 9081 measured reflections

• 2068 independent reflections

• 1585 reflections with I > 2σ(I)

• R_int = 0.038

Refinement

• R[F² > 2σ(F²)] = 0.047

• wR(F²) = 0.150

• S = 1.01

• 2068 reflections

• 91 parameters

• H-atom parameters constrained

• Δρ_max = 0.38 e Å⁻³

• Δρ_min = −0.28 e Å⁻³

Data collection: CrystalClear (Rigaku, 2005 ▶); cell refinement: CrystalClear; data reduction: CrystalClear; program(s) used to solve structure: SHELXS97 (Sheldrick, 2008); program(s) used to refine structure: SHELXL97 (Sheldrick, 2008); molecular graphics: SHELXTL (Sheldrick, 2008); software used to prepare material for publication: PRPKAPPA (Ferguson, 1999 ▶).

Table 1

Symmetry codes: (i) ; (ii) .

Supplementary Material

Crystal structure: contains datablocks I, global. DOI: 10.1107/S1600536810020568/pv2285sup1.cif

Structure factors: contains datablocks I. DOI: 10.1107/S1600536810020568/pv2285Isup2.hkl

Additional supplementary materials: crystallographic information; 3D view; checkCIF report

Acknowledgments

The author is grateful to the starter fund of Southeast University for financial support to purchase the diffractometer.

supplementary crystallographic information

Comment

There has been interest in the study of phase transition materials, includingorganic ligands, metal-organic coordination compounds, organic-inorganichybrids, etc. (Li et al., 2008; Zhang et al.,2009).Exploring the phase transition materials, the dielectric properties of thetitle compound, have been investigated in my laboratory. Unfortunately, therewas no distinct anomaly observed from 93 K to 380 K, (m.p. 408 K-410 K).In this article, the crystal structure of the title compound has beenpresented.

The asymmetric unit of the title compound containsa 2,4-dimethylanilinium cation and a chloride anion (Fig. 1).The non-H atoms of the 2,4-dimethylanilinium cation are essentially coplanar.In the crystal structure, all hydrogen atoms bonded to the ammoniumnitrogen (N1) are hydrogen bonded to the chloride ions with N···Cl distancesin the range 3.080 (2) - 3.136 (2) Å; four formula units of the titlecompound are hydrogen bonded to form sixteen membered macrocyclic rings inthe bc-plane (Tab. 1, Fig. 2).

Experimental

The title compound was prepared by the reaction of2,4-dimethylbenzenamine (1.21 g, 10 mmol) and hydrochloric acid solution(1.01 g, 10 mmol) in 30 ml methanol. The reaction mixture was filtered andleft at room temperature for 4 days. Colorlesscrystals were obtained by slow evaporation.

Refinement

Positional parameters of all H atoms were calculated geometrically and wereallowed to ride on the atoms to which they are bonded, with N—H = 0.89 Åand C—H = 0.93 and 0.96 Å, for aryl and methyl type H-atoms, respectively,U_iso(H) = 1.2 to 1.5U_eq(C/N).

Figures

The molecular structure of the title compound, showing the atomic numbering scheme. Displacement ellipsoids are drawn at the 30% probability level.

A view of the packing of the title compound, showing H-bonded bands along the c-axis; dashed lines indicate hydrogen bonds.

Crystal data

Data collection

Refinement

Special details

Fractional atomic coordinates and isotropic or equivalent isotropic displacement parameters (Ų)

Atomic displacement parameters (Ų)

Geometric parameters (Å, °)

Hydrogen-bond geometry (Å, °)

Co Dmg 2 Pyridine Chloride Bf2 10

Symmetry codes: (i) −x+1, y+1/2, −z+3/2; (ii) x, −y+1/2, z+1/2.

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Footnotes

Supplementary data and figures for this paper are available from the IUCr electronic archives (Reference: PV2285).

References

• Ferguson, G. (1999). PRPKAPPA University of Guelph, Canada.
• Li, X. Z., Qu, Z. R. & Xiong, R. G. (2008). Chin. J. Chem.11, 1959–1962.
• Rigaku (2005). CrystalClear Rigaku Corporation, Tokyo, Japan.
• Sheldrick, G. M. (2008). Acta Cryst. A64, 112–122. [PubMed]
• Zhang, W., Chen, L. Z., Xiong, R. G., Nakamura, T. & Huang, S. D. (2009). J. Am. Chem. Soc.131, 12544–12545. [PubMed]

A spectrochemical series is a list of ligands ordered on ligand strength and a list of metal ions based on oxidation number, group and its identity. In crystal field theory, ligands modify the difference in energy between the d orbitals (Δ) called the ligand-field splitting parameter for ligands or the crystal-field splitting parameter, which is mainly reflected in differences in color of similar metal-ligand complexes.

Spectrochemical series of ligands[edit]

The spectrochemical series was first proposed in 1938 based on the results of absorption spectra of cobalt complexes.^[1]

A partial spectrochemical series listing of ligands from small Δ to large Δ is given below. (For a table, see the ligand page.)

I⁻ < Br⁻ < S²⁻ < SCN⁻ (S–bonded) < Cl⁻ < N₃⁻ < F⁻< NCO⁻ < OH⁻ < C₂O₄²⁻ < O²⁻< H₂O < acac⁻ (acetylacetonate) < NCS⁻ (N–bonded) < CH₃CN < gly (glycine) < py (pyridine) < NH₃ < en (ethylenediamine) < bipy (2,2'-bipyridine) < phen (1,10-phenanthroline) < NO₂⁻ < PPh₃ < CN⁻ < CO

Weak field ligand: H₂O,F-,Cl-,OH-Strong field ligand: CO,CN-,NH₃,PPh₃

Ligands arranged on the left end of this spectrochemical series are generally regarded as weaker ligands and cannot cause forcible pairing of electrons within the 3d level, and thus form outer orbital octahedral complexes that are high spin. On the other hand, ligands lying at the right end are stronger ligands and form inner orbital octahedral complexes after forcible pairing of electrons within 3d level and hence are called low spin ligands.

However, keep in mind that 'the spectrochemical series is essentially backwards from what it should be for a reasonable prediction based on the assumptions of crystal field theory.'^[2] This deviation from crystal field theory highlights the weakness of crystal field theory's assumption of purely ionic bonds between metal and ligand.

The order of the spectrochemical series can be derived from the understanding that ligands are frequently classified by their donor or acceptor abilities. Some, like NH₃, are σ bond donors only, with no orbitals of appropriate symmetry for π bonding interactions. Bonding by these ligands to metals is relatively simple, using only the σ bonds to create relatively weak interactions. Another example of a σ bonding ligand would be ethylenediamine, however ethylenediamine has a stronger effect than ammonia, generating a larger ligand field split, Δ.

Ligands that have occupied p orbitals are potentially π donors. These types of ligands tend to donate these electrons to the metal along with the σ bonding electrons, exhibiting stronger metal-ligand interactions and an effective decrease of Δ. Most halide ligands as well as OH⁻ are primary examples of π donor ligands.

When ligands have vacant π* and d orbitals of suitable energy, there is the possibility of pi backbonding, and the ligands may be π acceptors. This addition to the bonding scheme increases Δ. Ligands that do this very effectively include CN⁻, CO, and many others.^[3]

Spectrochemical series of metals[edit]

The metal ions can also be arranged in order of increasing Δ, and this order is largely independent of the identity of the ligand.^[4]

Mn²⁺ < Ni²⁺ < Co²⁺ < Fe²⁺ < V²⁺ < Fe³⁺ < Cr³⁺ < V³⁺ < Co³⁺

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In general, it is not possible to say whether a given ligand will exert a strong field or a weak field on a given metal ion. However, when we consider the metal ion, the following two useful trends are observed:

• Δ increases with increasing oxidation number, and
• Δ increases down a group.^[4]

See also[edit]

References[edit]

Co Dmg 2 Pyridine Chloride Bf2 1

• Zumdahl, Steven S. Chemical Principles Fifth Edition. Boston: Houghton Mifflin Company, 2005. Pages 550-551 and 957-964.
• D. F. Shriver and P. W. Atkins Inorganic Chemistry 3rd edition, Oxford University Press, 2001. Pages: 227-236.
• James E. Huheey, Ellen A. Keiter, and Richard L. Keiter Inorganic Chemistry: Principles of Structure and Reactivity 4th edition, HarperCollins College Publishers, 1993. Pages 405-408.

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1. ^R. Tsuchida (1938). 'Absorption Spectra of Co-ordination Compounds. I.'Bull. Chem. Soc. Jpn. 13 (5). doi:10.1246/bcsj.13.388.
2. ^7th page of http://science.marshall.edu/castella/chm448/chap11.pdf
3. ^Miessler, Gary; Tarr, Donald (2011). Inorganic Chemistry (4th ed.). Prentice Hall. pp. 395–396. ISBN978-0-13-612866-3.
4. ^ ^abhttp://www.everyscience.com/Chemistry/Inorganic/Crystal_and_Ligand_Field_Theories/b.1013.php

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