Theoretical determination of the hydrogen-bond system in the α-d-galactopyranose crystal

1982 ◽  
Vol 88 (3-4) ◽  
pp. 383-385 ◽  
Author(s):  
V.N. Gritsan ◽  
V.G. Kachur ◽  
R.G. Zhbankov
Keyword(s):  
Hydrogen Bond ◽  
Theoretical Determination ◽  
Hydrogen Bond System ◽  
Bond System

Pyridine 1:1 adducts of urea (Z′ = 1) and thiourea (Z′ = 8)

2018 ◽  
Vol 74 (4) ◽  
pp. 406-410 ◽  
Author(s):  
Mark Strey ◽  
Peter G. Jones
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonds ◽  
Layer Structure ◽  
Urea Adduct ◽  
Standard Type ◽  
Space Group ◽  
Hydrogen Bond System ◽  
Bond System ◽  
Bifurcated Hydrogen Bond ◽  
Urea Adducts

During our studies of urea and thiourea adducts, we noticed that no adducts with unsubstituted pyridine had been structurally investigated. The 1:1 adduct of pyridine and urea, C5H5N·CH4N2O, crystallizes in the P21/c space group with Z = 4. The structure is of a standard type for urea adducts, whereby the urea molecules form a ribbon, parallel to the a axis, consisting of linked R 2 2(8) rings, and the pyridine molecules are attached to the periphery of the ribbon by bifurcated (N—H...)2N hydrogen bonds. The 1:1 adduct of pyridine and thiourea, C5H5N·CH4N2S, crystallizes in the P21/n space group, with Z = 32 (Z′ = 8). The structure displays similar ribbons to those of the urea adduct. There are two independent ribbons parallel to the b axis at z ≃ 0 and 1 \over 2, and three at z ≃ 1 \over 4 and 3 \over 4; the latter are crosslinked to form a layer structure by additional long N—H...S interactions, which each formally replace one branch of a bifurcated hydrogen-bond system.

scholarly journals Studies of the the Hydrogen Bond. IV. Theoretical Determination of Electronic Polarization Energies.

1958 ◽  
Vol 12 ◽  
pp. 584-585 ◽  
Author(s):  
Inga Fischer-Hjalmars ◽  
Ragnar Grahn ◽  
Klaus Mosbach ◽  
Per Fritzson ◽  
B. Zaar ◽  
...  
Keyword(s):  
Hydrogen Bond ◽  
Electronic Polarization ◽  
Theoretical Determination

{Bis[2-(3,5-dimethylpyrazol-1-yl)ethyl]amine-κ2 N,N′}dichloridozinc(II) methanol solvate

2007 ◽  
Vol 63 (11) ◽  
pp. m2679-m2679 ◽  
Author(s):  
Rae Eun Lee ◽  
Yeon Do Park ◽  
Jong Hwa Jeong
Keyword(s):  
Hydrogen Bond ◽  
Dihedral Angle ◽  
Title Compound ◽  
Solvent Molecule ◽  
Hydrogen Bond System ◽  
Bond System ◽  
Cl Atoms ◽  
Ethyl Amine

In the title compound, [ZnCl2(C14H23N5)]·CH3OH, the Zn atom is coordinated by two N atoms and two Cl atoms in an approximately tetrahedral arrangement. The dihedral angle between the N—Zn—N and Cl—Zn—Cl planes is 89.69 (5)°. The methanol solvent molecule takes part in the formation of the hydrogen-bond system.

scholarly journals Nickel alendronate

2012 ◽  
Vol 68 (6) ◽  
pp. m820-m821 ◽  
Author(s):  
Małgorzata Sikorska ◽  
Maria Gazda ◽  
Jaroslaw Chojnacki
Keyword(s):  
Crystal Structure ◽  
Hydrogen Bond ◽  
Hydrogen Bonds ◽  
Water Molecule ◽  
Title Compound ◽  
Intermolecular Hydrogen Bond ◽  
Hydrothermal Conditions ◽  
Complex Molecules ◽  
Hydrogen Bond System ◽  
Bond System

The title compound {systematic name: bis(μ2-dihydrogen 4-azaniumyl-1-hydroxybutane-1,1-diphosphonato)bis[aqua(dihydrogen 4-azaniumyl-1-hydroxybutane-1,1-diphosphonato)nickel(II)] dihydrate}, [Ni2(C4H12NO7P2)4(H2O)2]·2H2O, was synthesiized under hydrothermal conditions. Its structure is isotypic with the CoII analogue. The crystal structure is built up from centrosymmetric dinuclear complex molecules and the structure is reinforced by a net of intermolecular O—H...O and N—H...O hydrogen bonds. One water molecule is bound to the NiII atom in the octahedral coordination sphere, while the second is part of the intermolecular hydrogen-bond system.

Hydrogen bond system generated by nitroamino rearrangement: new character for designing next generation energetic materials

2021 ◽  
Author(s):  
Lu Hu ◽  
Richard J. Staples ◽  
Jean’ne M. Shreeve
Keyword(s):  
Hydrogen Bond ◽  
Energetic Materials ◽  
Lower Sensitivity ◽  
Next Generation ◽  
Hydrogen Bond System ◽  
Bond System ◽  
Intermolecular Distances

Hydrogen bond systems stabilize molecules and shorten intermolecular distances to give higher density and lower sensitivity.

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