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Journal articles on the topic 'Chemical bonding'

Author: Grafiati

Published: 4 June 2021

Last updated: 1 February 2025

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1

Breugst, Martin, Daniel von der Heiden, and Julie Schmauck. "Novel Noncovalent Interactions in Catalysis: A Focus on Halogen, Chalcogen, and Anion-π Bonding." Synthesis 49, no. 15 (May 23, 2017): 3224–36. http://dx.doi.org/10.1055/s-0036-1588838.

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Noncovalent interactions play an important role in many biological and chemical processes. Among these, hydrogen bonding is very well studied and is already routinely used in organocatalysis. This Short Review focuses on three other types of promising noncovalent interactions. Halogen bonding, chalcogen bonding, and anion-π bonding have been introduced into organocatalysis in the last few years and could become important alternate modes of activation to hydrogen bonding in the future.1 Introduction2 Halogen Bonding3 Chalcogen Bonding4 Anion-π Bonding5 Conclusions

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2

Putz, Mihai V. "Chemical Bonding by the Chemical Orthogonal Space of Reactivity." International Journal of Molecular Sciences 22, no. 1 (December 28, 2020): 223. http://dx.doi.org/10.3390/ijms22010223.

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The fashionable Parr–Pearson (PP) atoms-in-molecule/bonding (AIM/AIB) approach for determining the exchanged charge necessary for acquiring an equalized electronegativity within a chemical bond is refined and generalized here by introducing the concepts of chemical power within the chemical orthogonal space (COS) in terms of electronegativity and chemical hardness. Electronegativity and chemical hardness are conceptually orthogonal, since there are opposite tendencies in bonding, i.e., reactivity vs. stability or the HOMO-LUMO middy level vs. the HOMO-LUMO interval (gap). Thus, atoms-in-molecule/bond electronegativity and chemical hardness are provided for in orthogonal space (COS), along with a generalized analytical expression of the exchanged electrons in bonding. Moreover, the present formalism surpasses the earlier Parr–Pearson limitation to the context of hetero-bonding molecules so as to also include the important case of covalent homo-bonding. The connections of the present COS analysis with PP formalism is analytically revealed, while a numerical illustration regarding the patterning and fragmentation of chemical benchmarking bondings is also presented and fundamental open questions are critically discussed.

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3

BOERNER, LEIGH KRIETSCH. "CHEMICAL BONDING." Chemical & Engineering News 88, no. 42 (October 18, 2010): 39–41. http://dx.doi.org/10.1021/cen-v088n042.p039.

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4

Yokura, Miyoshi, Kenichi Uehara, Guo Xiang, Kazuya Hanada, Yoshinobu Nakamura, Lakshmi Sanapa Reddy, Kazuhiro Endo, and Tamio Endo. "Ultralong Lifetime of Active Surface of Oxygenated PET Films by Plasma-irradiation and Bonding Elements." MRS Proceedings 1454 (2012): 201–6. http://dx.doi.org/10.1557/opl.2012.1128.

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ABSTRACTBiaxially oriented polyethylene terephthalate (PET) films can be bonded directly by oxygen plasma irradiation and low temperature heat press around 100°C. The irradiated films were kept in the atmosphere for six years, yet they can be bonded tightly as well. Dry- and wet-peel tests indicate that two bonding elements can be suggested, hydrogen bonding and chemical bonding. The films are bonded by these two elements at lower temperatures, but by the pure chemical bonding at higher temperatures. FTIR results on the non-irradiated, irradiated and bonded samples indicate that OH and COOH groups are created at the surface, they are responsible for the hydrogen and chemical bondings. Dehydrated condensation reaction is proposed for the chemical bonding. It is briefly mentioned on two origins for the long lifetime of irradiated active surface.

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5

Putz, Mihai V. "Chemical action and chemical bonding." Journal of Molecular Structure: THEOCHEM 900, no. 1-3 (April 2009): 64–70. http://dx.doi.org/10.1016/j.theochem.2008.12.026.

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6

Senn, Peter. "On chemical bonding." American Journal of Physics 54, no. 7 (July 1986): 587. http://dx.doi.org/10.1119/1.14535.

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7

Balasubramanian, K. "Relativity and chemical bonding." Journal of Physical Chemistry 93, no. 18 (September 1989): 6585–96. http://dx.doi.org/10.1021/j100355a005.

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8

Ashcheulov, A. A., O. N. Manyk, T. O. Manyk, S. F. Marenkin, and V. R. Bilynskiy-Slotylo. "Chemical bonding in cadmium." Inorganic Materials 47, no. 9 (August 25, 2011): 952–56. http://dx.doi.org/10.1134/s0020168511090019.

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9

MORRISSEY, SUSAN R. "NSF'S CHEMICAL BONDING CENTERS." Chemical & Engineering News Archive 82, no. 41 (October 11, 2004): 33–34. http://dx.doi.org/10.1021/cen-v082n041.p033.

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10

JACOBY, MITCH. "CHEMICAL BONDING FORCES MEASURED." Chemical & Engineering News Archive 79, no. 14 (April 2, 2001): 12. http://dx.doi.org/10.1021/cen-v079n014.p012.

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11

Finzel, Kati. "Chemical bonding without orbitals." Computational and Theoretical Chemistry 1144 (November 2018): 50–55. http://dx.doi.org/10.1016/j.comptc.2018.10.004.

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12

Calais, Jean-Louis. "Chemical bonding and vibrations." Journal of Molecular Structure: THEOCHEM 261 (July 1992): 121–32. http://dx.doi.org/10.1016/0166-1280(92)87071-7.

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13

Jeung, G. H. "Chemical bonding in ScCS." Chemical Physics Letters 176, no. 2 (January 1991): 233–38. http://dx.doi.org/10.1016/0009-2614(91)90159-7.

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14

Ghafouri, Reza, Fatemeh Ektefa, and Mansour Zahedi. "Characterization of Hydrogen Bonds in the End-Functionalized Single-Wall Carbon Nanotubes: A DFT Study." Nano 10, no. 03 (April 2015): 1550036. http://dx.doi.org/10.1142/s1793292015500368.

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A systematic computational study is carried out to shed some light on the structure of semiconducting armchair single-wall carbon nanotubes (n, n) SWCNTs, n = 4, 5 and 6, functionalized at the end with carboxyl (– COOH ) and amide (– CONH 2) from the viewpoint of characterizing the intramolecular hydrogen bondings at the B3LYP/6-31++G(d, p) level. Geometry parameters display different types of intramolecular hydrogen bonding possibilities in the considered functionalized SWCNTs. All of the hydrogen bondings are confirmed by natural bonding orbitals (NBO) analysis as well as nuclear magnetic resonance (NMR) and nuclear quadrupole resonance (NQR) parameters. Based on NBO analysis, the calculated [Formula: see text] delocalization energies E(2), 1.15 kcal/mol to 7.04 kcal/mol, are in direct relation with the hydrogen bonding strengths. Differences in the chemical shielding principal components of 13 C and 17 O nuclei correlate well with the strengths of the hydrogen bondings. Participating in stronger hydrogen bondings, a larger SWCNT has a decreasing effect on 13 C (= O ) and 17 O isotropic chemical shieldings, σiso, consistent with the NBO analysis. The considerable changes of 13 C /17 O σiso can be interpreted as a result of shielding tensor component orientation. The 13 C (= O ) and 17 O quadrupole coupling constants C Q decrease under the effect of hydrogen bonding while asymmetry parameters ηQ significantly increase, indicating that 17 O ηQ is more sensitive to hydrogen bondings.

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15

Zhao, Lili, Sudip Pan, Nicole Holzmann, Peter Schwerdtfeger, and Gernot Frenking. "Chemical Bonding and Bonding Models of Main-Group Compounds." Chemical Reviews 119, no. 14 (June 28, 2019): 8781–845. http://dx.doi.org/10.1021/acs.chemrev.8b00722.

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16

Cassiday, Laura. "The bonding of chemical giants." INFORM: International News on Fats, Oils, and Related Materials 27, no. 3 (March 1, 2016): 26–27. http://dx.doi.org/10.21748/inform.03.2016.26.

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17

Gonçalves, A. M., and Ana M. Segadães. "Unshaped Refractories with Chemical Bonding." Materials Science Forum 34-36 (January 1991): 705–9. http://dx.doi.org/10.4028/www.scientific.net/msf.34-36.705.

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18

Bag, Sampad, Sankhabrata Chandra, Jayanta Ghosh, Anupam Bera, Elliot R. Bernstein, and Atanu Bhattacharya. "The attochemistry of chemical bonding." International Reviews in Physical Chemistry 40, no. 3 (July 3, 2021): 405–55. http://dx.doi.org/10.1080/0144235x.2021.1976499.

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19

Putz, Mihai. "Density Functionals of Chemical Bonding." International Journal of Molecular Sciences 9, no. 6 (June 26, 2008): 1050–95. http://dx.doi.org/10.3390/ijms9061050.

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20

Vaughan, D. J. "Chemical Bonding in Sulfide Minerals." Reviews in Mineralogy and Geochemistry 61, no. 1 (January 1, 2006): 231–64. http://dx.doi.org/10.2138/rmg.2006.61.5.

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21

Castro, Abril C., Mikael P. Johansson, Gabriel Merino, and Marcel Swart. "Chemical bonding in supermolecular flowers." Physical Chemistry Chemical Physics 14, no. 43 (2012): 14905. http://dx.doi.org/10.1039/c2cp42045g.

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22

Nishitani, Shigeto R., Shunsuke Fujii, Masataka Mizuno, Isao Tanaka, and Hirohiko Adachi. "Chemical bonding of3dtransition-metal disilicides." Physical Review B 58, no. 15 (October 15, 1998): 9741–45. http://dx.doi.org/10.1103/physrevb.58.9741.

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23

Lee, Chengteh, Han Chen, and George Fitzgerald. "Chemical bonding in water clusters." Journal of Chemical Physics 102, no. 3 (January 15, 1995): 1266–69. http://dx.doi.org/10.1063/1.468914.

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24

Sacks, Lawrence J. "Coulombic Models in Chemical Bonding." Journal of Chemical Education 77, no. 4 (April 2000): 445. http://dx.doi.org/10.1021/ed077p445.1.

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25

Marghussian, V. K., and R. Naghizadeh. "Chemical bonding of silicon carbide." Journal of the European Ceramic Society 19, no. 16 (December 1999): 2815–21. http://dx.doi.org/10.1016/s0955-2219(99)00068-0.

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26

Hagenmuller, Paul. "Intercalation chemistry and chemical bonding." Journal of Physics and Chemistry of Solids 59, no. 4 (April 1998): 503–6. http://dx.doi.org/10.1016/s0022-3697(97)90189-x.

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27

Harris, Mary. "Chemical Bonding Makes a Difference!" Journal of Chemical Education 83, no. 10 (October 2006): 1435. http://dx.doi.org/10.1021/ed083p1435.

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28

Hoffmann, P., O. Baake, B. Beckhoff, W. Ensinger, N. Fainer, A. Klein, M. Kosinova, et al. "Chemical bonding in carbonitride nanolayers." Nuclear Instruments and Methods in Physics Research Section A: Accelerators, Spectrometers, Detectors and Associated Equipment 575, no. 1-2 (May 2007): 78–84. http://dx.doi.org/10.1016/j.nima.2007.01.030.

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29

Harcourt, Richard D. "Kinetic energy and chemical bonding." American Journal of Physics 56, no. 7 (July 1988): 660–61. http://dx.doi.org/10.1119/1.15535.

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30

Hagenmuller, Paul. "Intercalation chemistry and chemical bonding." Journal of Power Sources 90, no. 1 (September 2000): 9–12. http://dx.doi.org/10.1016/s0378-7753(00)00437-7.

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31

Needham, Paul. "The source of chemical bonding." Studies in History and Philosophy of Science Part A 45 (March 2014): 1–13. http://dx.doi.org/10.1016/j.shpsa.2013.10.011.

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32

Greenspan, D. "Electron attraction and chemical bonding." Computers & Mathematics with Applications 38, no. 11-12 (December 1999): 217–27. http://dx.doi.org/10.1016/s0898-1221(99)00300-4.

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33

HAGENMULLER, P. "Chemical bonding and intercalation processes." Solid State Ionics 40-41 (August 1990): 3–9. http://dx.doi.org/10.1016/0167-2738(90)90275-v.

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34

Kematick, R. J., H. F. Franzen, and D. K. Misemer. "Chemical bonding interactions in Zr2Al." Journal of Solid State Chemistry 60, no. 3 (December 1985): 297–304. http://dx.doi.org/10.1016/0022-4596(85)90280-4.

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35

King, R. B. "Chemical bonding topology of superconductors." Journal of Solid State Chemistry 71, no. 1 (November 1987): 224–32. http://dx.doi.org/10.1016/0022-4596(87)90162-9.

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36

King, R. B. "Chemical bonding topology of superconductors." Journal of Solid State Chemistry 71, no. 1 (November 1987): 233–36. http://dx.doi.org/10.1016/0022-4596(87)90163-0.

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37

Weyrich, W. "Chemical bonding as electronic coherence." Acta Crystallographica Section A Foundations of Crystallography 58, s1 (August 6, 2002): c191. http://dx.doi.org/10.1107/s0108767302092668.

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38

Ghatikar, M. N. "Phase shifts and chemical bonding." Physica B: Condensed Matter 158, no. 1-3 (June 1989): 383–85. http://dx.doi.org/10.1016/0921-4526(89)90318-9.

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39

Cundari, Thomas R. "Chemical bonding involving d-orbitals." Chemical Communications 49, no. 83 (2013): 9521. http://dx.doi.org/10.1039/c3cc45204b.

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40

Batsanov, Stepan S. "Energy Electronegativity and Chemical Bonding." Molecules 27, no. 23 (November 25, 2022): 8215. http://dx.doi.org/10.3390/molecules27238215.

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Historical development of the concept of electronegativity (EN) and its significance and prospects for physical and structural chemistry are discussed. The current cutting-edge results are reviewed: new methods of determining the ENs of atoms in solid metals and of bond polarities and effective atomic charges in molecules and crystals. The ENs of nanosized elements are calculated for the first time, enabling us to understand their unusual reactivity, particularly the fixation of N2 by nanodiamond. Bond polarities in fluorides are also determined for the first time, taking into account the peculiarities of the fluorine atom’s electronic structure and its electron affinity.

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41

Herbst‐Irmer, Regine, and Erhard Irmer. "Experimental Visualisation of Chemical Bonding." CHEMKON 27, no. 6 (October 2020): 275–81. http://dx.doi.org/10.1002/ckon.202000015.

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42

King, R. B. "Chemical Bonding Topology of Superconductors." Journal of Solid State Chemistry 124, no. 2 (July 1996): 329–32. http://dx.doi.org/10.1006/jssc.1996.0245.

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43

King, R. B. "Chemical Bonding Topology of Superconductors." Journal of Solid State Chemistry 131, no. 2 (July 1997): 394–98. http://dx.doi.org/10.1006/jssc.1997.7415.

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44

Krapp, Andreas, F. Matthias Bickelhaupt, and Gernot Frenking. "Orbital Overlap and Chemical Bonding." Chemistry - A European Journal 12, no. 36 (December 13, 2006): 9196–216. http://dx.doi.org/10.1002/chem.200600564.

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45

Yun, Yong Sup, Takanori Yoshida, Norifumi Shimazu, Yasushi Inoue, Nagahiro Saito, and Osamu Takai. "Behavior of Various Organosilicon Molecules in PECVD Processes for Hydrocarbon-Doped Silicon Oxide Films." Solid State Phenomena 124-126 (June 2007): 347–50. http://dx.doi.org/10.4028/www.scientific.net/ssp.124-126.347.

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Plasma diagnosis was performed by means of optical emission spectroscopy in the plasma-enhanced chemical vapor deposition process for preparation of hydrocarbon-doped silicon oxide films. The chemical bonding states were characterized by a fourier-transform infrared spectrometer. Based on the results of the diagnosis in organosilane plasma and the chemical bonding states, a reaction model for the formation process of hydrocarbon-doped silicon oxide films was discussed. From the results of optical emission spectroscopy, we found that the oxygen atoms of methoxy groups in TMMOS molecules can be dissociated easily in the plasma and behave as a kind of oxidizing agent. Siloxane bondings in HMDSO, on the other hand, hardly expel oxygen atoms.

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46

Lusyana Yustin, Dessy, and Antuni Wiyarsi. "Students’ chemical literacy: A study in chemical bonding." Journal of Physics: Conference Series 1397 (December 2019): 012036. http://dx.doi.org/10.1088/1742-6596/1397/1/012036.

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47

de Lange, Jurgens H., Daniël M. E. van Niekerk, and Ignacy Cukrowski. "Quantifying individual (anti)bonding molecular orbitals’ contributions to chemical bonding." Physical Chemistry Chemical Physics 21, no. 37 (2019): 20988–98. http://dx.doi.org/10.1039/c9cp04345d.

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48

Borbora, Angana, and Uttam Manna. "Impact of chemistry on the preparation and post-modification of multilayered hollow microcapsules." Chemical Communications 57, no. 17 (2021): 2110–23. http://dx.doi.org/10.1039/d0cc06917e.

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Different chemical interactions/bonding allowed LbL deposition of selected constituents, and further post-chemical modifications of chemically reactive multilayered microcapsules allowed to associate desired chemical functionalities.

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49

Kim, Yeongjung, Byeong Jo Han, and Jong-Hyun Lee. "Paste Containing 1.5 μm Ag Particles with Enhanced Surface Area: Ultrafast Thermo-Compression Sinter-Bonding and Annealing Effects." Korean Journal of Metals and Materials 60, no. 11 (November 5, 2022): 827–36. http://dx.doi.org/10.3365/kjmm.2022.60.11.827.

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To rapidly sinter a bondline and obtain mechanical stability at high temperature and high thermal conductivity, 1.5 μm Ag particles with enhanced surface area were synthesized by a wet-chemical method, and a sinter-bonding paste containing these Ag particles was obtained. Some particles were present in the form of agglomerates of spike stems and short-branch dendrites, while others existed as spheres with rough nodule surfaces or relatively smooth surfaces. To determine an effective sinter-bonding process, a significantly short thermo-compression bonding (10 s) under 5 MPa in air and subsequent annealing in nitrogen were performed. The thermo-compression bonding at 250 oC resulted in a low shear strength of 8.15 MPa in the formed bondline. Although the annealing at 250 oC increased its strength, it did not reach 20 MPa, which is required for practical applications. Interestingly, the 10 s bonding at 300 oC exhibited sufficient shear strength of 21.96 MPa, and when annealed for 30 min at 300 oC, the excellent strength of 37.75 MPa was obtained. The bondline porosity of 12.16% immediately after the thermo-compression bonding, decreased to 9.13% after annealing for 30 min. The densification in bondline by the annealing also induced a change in the fracture path as well as enhancement in the shear strength. Thus, the suggested subsequent annealing is an effective method for sinter-bonding, similar to the pressureless sinter-bonding process. Consequently, the synthesized Ag particles exhibited superior sintering properties and the suggested combination process shows potential for tremendously improving chip sinter-bonding productivity.

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50

West, Robert, Jefferson D. Cavalieri, James Duchamp, and Kurt W. Zilm. "Chemical Shift Tensors and Chemical Bonding in Cyclic Silanes." Phosphorus, Sulfur, and Silicon and the Related Elements 93, no. 1-4 (August 1994): 213–16. http://dx.doi.org/10.1080/10426509408021819.

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