The lattice energies of the alkali halides

Morris, D.F.C.

doi:10.1107/s0365110x56000498

Cited by 33 publications

(20 citation statements)

References 1 publication

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“…This points to a BF 4 -anion directly bound to the Li + ion with fast exchange between bridging and terminal fluoride atoms. Contrary to what is found for 1‚LiBF 4 , the 7 Li and the 19 F spectra of the complexes 2‚LiBF 4 and 3‚LiBF 4 show simple singlets, indicating solvent-separated BF 4 -ions. Apparently, the sterically demanding Cp* ligands disfavor The structures of 1‚LiBF 4 and 2‚LiBF 4 were determined by single-crystal X-ray crystallography (Figure 1).…”

Section: Stabilization Of Molecular Lif and Lifhfcontrasting

confidence: 84%

“…Absorption correction was applied to all data sets but one (2‚1.5C 6 H 6 ‚H 2 O‚LiF). For 2‚toluene‚LiBF 4 and 1‚1.25C 6 H 6 ‚H 2 O‚LiF, a semiempirical method (MULTI-SCAN) 22 was employed, whereas an empirical method (DIFABS) 23 was used for the remaining structures. Structure solutions were determined with ab initio direct methods.…”

Section: Methodsmentioning

confidence: 99%

“…The solution was heated under reflux for 1 h. Evaporation of the solvent under reduced pressure gave an orange powder (yield: 55 mg, 100%). Red crystals were obtained by slow diffusion of pentane into a solution of 1‚LiBF 4 6 Hz, 3H, CH, cymene), 5.85 (dd, 3 J ) 6 Hz, 3 J ) 7 Hz, 3H, CH, pyridone), 6.32 (d, 3 J ) 5 Hz, 3H, CH, cymene), 6.52 (dd, 3 J ) 7 Hz, 4 J ) 2 Hz, 3H, CH, pyridone), 6.89 (dd, 3 J ) 6 Hz, 4 J ) 2 Hz, 3H, CH, pyridone). 13 [Cp*Rh(C 5 H 3 NO 2 )] 3 ‚LiBF 4 (2‚LiBF 4 ).…”

Section: Methodsmentioning

confidence: 99%

“…3 The difficulty in stabilizing complexes of molecular LiF is due to the very high lattice energy of this salt. 4 Consequently, the crystalline form represents a thermodynamic trap. A similar situation is found for the less common but theoretically interesting salt LiFHF.…”

Section: Introductionmentioning

confidence: 99%

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Stabilization of Molecular LiF and LiFHF inside Metallamacrocyclic Hosts

2002

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Complexes of molecular LiF and LiFHF were synthesized using the metallamacrocyclic receptors [(cymene)Ru(C(5)H(3)NO(2))](3) (1), [CpRh(C(5)H(3)NO(2))](3) (2), and [CpIr(C(5)H(3)NO(2))](3) (3). LiBF(4) complexes of 1-3 were prepared and subsequently treated with F(-) or FHF(-) to give the desired products in an anion-exchange reaction. All complexes were characterized by multinuclear NMR spectroscopy ((1)H, (13)C, (19)F, (7)Li). Strong scalar coupling between (7)Li and (19)F is observed for the LiF and the LiFHF complexes ((1)J(LiF) = 91-103 Hz). The LiFHF adduct of 1 displays fluxional behavior with fast exchange of the two fluorine atoms. The structures of the complexes 1.LiBF(4), 2.LiBF(4), 1.LiF, 2.LiF, 1.LiFHF, and 3.LiFHF were determined by single-crystal X-ray analysis. Li-F bond lengths between 1.77 and 1.81 A were found. The LiFHF complexes show a hydrogen difluoride anion coordinated in a bent fashion via one fluorine atom to the lithium ion.

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Section: Stabilization Of Molecular Lif and Lifhfcontrasting

confidence: 84%

Section: Methodsmentioning

confidence: 99%

Section: Methodsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

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Stabilization of Molecular LiF and LiFHF inside Metallamacrocyclic Hosts

2002

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“…This equation is given as follow: the viscosity (Pa s) of molten alkali halides is related to enthalpy of sublimation (taken from literature) [16][17][18][19][20][21] and can be calculated as follows: The viscosity values obtained from Eq. (10), at the melting points, are tabulated in Table 2.…”

Section: Viscositymentioning

confidence: 99%

Correlations of the surface tension and some thermodynamic and transport properties of the alkali metal halides at their melting temperatures based on their corresponding molar volumes

Aqra

Ayyad

2015

Fluid Phase Equilibria

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Lithium and Lithium Compounds

Kamienski¹,

McDonald

Stark

et al. 2004

Kirk-Othmer Encyclopedia of Chemical Technology

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Lithium, an element of unique physical and chemical properties, is useful in a wide range of applications as the metal, as the lithium ion in inorganic salts, and as the more covalent species in inorganic compounds. The largest uses of lithium compounds are in traditional areas such as the preparation of glass, glass‐ceramics, and enamels; in aluminum cell broth; in the preparation of lithium greases; and as polymerization initiators. Lithium compounds are also employed as psychopharmacological agents and in organic synthesis, catalysis, absorption, air conditioning, photographic processing, and in batteries. The use of organic lithium compounds as industrial catalysts and the consumption of various lithium compounds in batteries are the most rapidly expanding markets. The various lithium mineral and brine resources are reviewed along with the processes for lithium extraction and recovery. Manufacturing processes, properties, health and safety factors, and applications for lithium metal and lithium compounds are discussed.

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The lattice energies of the alkali halides

Cited by 33 publications

References 1 publication

Stabilization of Molecular LiF and LiFHF inside Metallamacrocyclic Hosts

Stabilization of Molecular LiF and LiFHF inside Metallamacrocyclic Hosts

Correlations of the surface tension and some thermodynamic and transport properties of the alkali metal halides at their melting temperatures based on their corresponding molar volumes

Lithium and Lithium Compounds

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