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Volumn 10, Issue 1, 2008, Pages 96-105

The hydration of glucose: The local configurations in sugar-water hydrogen bonds

Author keywords

[No Author keywords available]

Indexed keywords

CARBOHYDRATE; GLUCOSE; HYDROXIDE; HYDROXIDE ION; UNCLASSIFIED DRUG; WATER;

EID: 37249067197     PISSN: 14639076     EISSN: None     Source Type: Journal    
DOI: 10.1039/b708719e     Document Type: Article
Times cited : (82)

References (57)
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  • 2
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    • The local structure of the first coordination shell of a water molecule in the liquid has been under intense scrutiny for the past three years. For reasons discussed later in this paper, however, I traditionally classify water as a locally tetrahedral liquid
    • D. Prendergast G. Galli Phys. Rev. Lett. 2006 96 215502
    • (2006) Phys. Rev. Lett. , vol.96 , pp. 215502
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    • Prentice Hall, Upper Saddle River, NJ, 5th edn
    • P. Y. Bruice, Organic Chemistry, Prentice Hall, Upper Saddle River, NJ, 5th edn, 2007, ch. 2
    • (2007) Organic Chemistry
    • Bruice, P.Y.1
  • 13
    • 37249021038 scopus 로고    scopus 로고
    • J. Grotendorst, John von Neumann Institute for Computing, Forschungszentrum Julich, Germany, 2nd edn, pp. 329-477
    • D. Marx and J. Hutter, in Modern Methods and Algorithms of Quantum Chemistry Proceedings, ed., J. Grotendorst,, John von Neumann Institute for Computing, Forschungszentrum Julich, Germany, 2nd edn, 2000, NIC series, vol. 3, pp. 329-477
    • (2000) Modern Methods and Algorithms of Quantum Chemistry Proceedings, Ed.
    • Marx, D.1    Hutter In, J.2
  • 14
  • 29
    • 0003516749 scopus 로고    scopus 로고
    • LP leads to an increase in the lone pair angle because the two lone pairs tend to exert more electron repulsion between each other. In general, the wider the lone pair angle, the more s character the lone pair has
    • P. Atkins and J. Paula, Physical Chemistry, Oxford University Press, New York, 8th edn, 2006, ch. 18
    • (2006) Physical Chemistry
    • Atkins, P.1    Paula, J.2
  • 37
    • 0001477338 scopus 로고    scopus 로고
    • The shift of the centres of the covalent OH1 and OH6 bond orbitals toward their oxygen nuclei (Fig. 3) indicates that their electronic charge densities shifted toward the oxygen nuclei along the bonds. This probably reduces the repulsive overlap interactions between the bond orbitals and lone pairs of water molecules, leading to an enhancement of the H-bonding (ref. 34). Further, strong charge-transfer interactions tend to lengthen the O-H bond distance and to reduce the overall oxygen-oxygen distance (ref. 33). Actually, this tendency was observed for the OH1 and OH6 bonds (Tables 1 and 2)
    • J. J. Dannenberg L. Haskamp A. Masunov J. Phys. Chem. A 1999 103 7083
    • (1999) J. Phys. Chem. a , vol.103 , pp. 7083
    • Dannenberg, J.J.1    Haskamp, L.2    Masunov, A.3
  • 53
    • 33947678371 scopus 로고    scopus 로고
    • In B. Lewin, L. Cassimeris, V. R. Lingappa and G. Plopper, Jones & Bartlett, Sudbury, MA, pp. 63-70
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    • (2007) Cells, Ed.


* 이 정보는 Elsevier사의 SCOPUS DB에서 KISTI가 분석하여 추출한 것입니다.