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Journal articles on the topic 'Pnicogen bond'

Author: Grafiati

Published: 6 September 2023

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1

Xu, Hui-Ying, Wei Wang, Jian-Wei Zou, and Xiao-Lu Xu. "Theoretical calculations of π-type pnicogen bonds in the triad intermolecular complexes." Journal of Theoretical and Computational Chemistry 13, no. 08 (December 2014): 1450068. http://dx.doi.org/10.1142/s0219633614500680.

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The pnicogen bonding interactions of PCl3and π-electron systems (acetylene, ethylene, benzene) were calculated by using MP2/aug-cc-pVDZ method and the effect of hydrogen bond on pnicogen bond systems were investigated. It has been indicated that the hydrogen bonding and the pnicogen bonding interactions have influence on each other and the positively cooperative effect has been detected. The interaction energies of pnicogen bonded supramolecular system were also calculated by using DFT method (M06-2X) and some simple comparisons with those by using MP2 method were made. It has been disclosed from natural bond orbitals (NBO) analysis that more the amount of charge transfer of pnicogen bonding interaction, the greater the stability of the corresponding complex. Through AIM topological analysis, it has been revealed that the electron density of pnicogen bond BCP point is positively correlated with the stability of trimeric complex. Electron localization function (ELF) was also adopted to analyze the nature of pnicogen bonding interactions. Furthermore, density difference function (DDF) method was adopted to analyze the variation of electron density of pnicogen bond system because of hydrogen bond.

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2

Esrafili, Mehdi D., and Fariba Mohammadian-Sabet. "Cooperative effects in hydrogen bond and pnicogen bond: a comparative study." Canadian Journal of Chemistry 92, no. 12 (December 2014): 1151–56. http://dx.doi.org/10.1139/cjc-2014-0379.

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A comparative study of the cooperative effects of hydrogen and pnicogen bonding on open-chain clusters of (PH2CN)n=2–7 and (HCN)n=2–7 is performed at the MP2/6-311++G(d,p) level of theory. These effects are studied in terms of geometric and energetic properties, electron density analysis, and 15N chemical shielding parameters of the clusters at the MP2/6-311++G** level. The intermolecular distances observed in the (HCN)n clusters exhibit quite larger bond contractions than those found in the (PH2CN)n clusters. Our results strongly suggest that cooperative effects induced by pnicogen and hydrogen bonds are significant in both linear PH2CN and HCN clusters, respectively. They also provide some evidence that these effects seem to reach a limit for a relatively small number of monomers. The n-dependent variation in the 15N chemical shielding tensor should serve as a useful signature of cooperativity effects in the PH2CN and HCN clusters.

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3

Chandra, Swaroop, B. Suryaprasad, N. Ramanathan, and K. Sundararajan. "Nitrogen as a pnicogen?: evidence for π-hole driven novel pnicogen bonding interactions in nitromethane–ammonia aggregates using matrix isolation infrared spectroscopy and ab initio computations." Physical Chemistry Chemical Physics 23, no. 10 (2021): 6286–97. http://dx.doi.org/10.1039/d0cp06273a.

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4

Alkorta, Ibon, Cristina Trujillo, Goar Sánchez-Sanz, and José Elguero. "Solvent and Substituent Effects on the Phosphine + CO2 Reaction." Inorganics 6, no. 4 (October 10, 2018): 110. http://dx.doi.org/10.3390/inorganics6040110.

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A theoretical study of the substituent and solvent effects on the reaction of phosphines with CO2 has been carried out by means of Møller-Plesset (MP2) computational level calculations and continuum polarizable method (PCM) solvent models. Three stationary points along the reaction coordinate have been characterized, a pre-transition state (TS) assembly in which a pnicogen bond or tetrel bond is established between the phosphine and the CO2 molecule, followed by a transition state, and leading finally to the adduct in which the P–C bond has been formed. The solvent effects on the stability and geometry of the stationary points are different. Thus, the pnicogen bonded complexes are destabilized as the dielectric constant of the solvent increases while the opposite happens within the adducts with the P–C bond and the TSs trend. A combination of the substituents and solvents can be used to control the most stable minimum.

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5

Grabowski, Sławomir J. "Classification of So-Called Non-Covalent Interactions Based on VSEPR Model." Molecules 26, no. 16 (August 15, 2021): 4939. http://dx.doi.org/10.3390/molecules26164939.

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The variety of interactions have been analyzed in numerous studies. They are often compared with the hydrogen bond that is crucial in numerous chemical and biological processes. One can mention such interactions as the halogen bond, pnicogen bond, and others that may be classified as σ-hole bonds. However, not only σ-holes may act as Lewis acid centers. Numerous species are characterized by the occurrence of π-holes, which also may play a role of the electron acceptor. The situation is complicated since numerous interactions, such as the pnicogen bond or the chalcogen bond, for example, may be classified as a σ-hole bond or π-hole bond; it ultimately depends on the configuration at the Lewis acid centre. The disadvantage of classifications of interactions is also connected with their names, derived from the names of groups such as halogen and tetrel bonds or from single elements such as hydrogen and carbon bonds. The chaos is aggravated by the properties of elements. For example, a hydrogen atom can act as the Lewis acid or as the Lewis base site if it is positively or negatively charged, respectively. Hence names of the corresponding interactions occur in literature, namely hydrogen bonds and hydride bonds. There are other numerous disadvantages connected with classifications and names of interactions; these are discussed in this study. Several studies show that the majority of interactions are ruled by the same mechanisms related to the electron charge shifts, and that the occurrence of numerous interactions leads to specific changes in geometries of interacting species. These changes follow the rules of the valence-shell electron-pair repulsion model (VSEPR). That is why the simple classification of interactions based on VSEPR is proposed here. This classification is still open since numerous processes and interactions not discussed in this study may be included within it.

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6

Alkorta, Ibon, Goar Sánchez-Sanz, José Elguero, and Janet E. Del Bene. "Influence of Hydrogen Bonds on the P···P Pnicogen Bond." Journal of Chemical Theory and Computation 8, no. 7 (June 22, 2012): 2320–27. http://dx.doi.org/10.1021/ct300399y.

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7

Lo, Rabindranath, Petr Švec, Zdeňka Růžičková, Aleš Růžička, and Pavel Hobza. "On the nature of the stabilisation of the E⋯π pnicogen bond in the SbCl3⋯toluene complex." Chemical Communications 52, no. 17 (2016): 3500–3503. http://dx.doi.org/10.1039/c5cc10363k.

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8

Sánchez-Sanz, Goar, Cristina Trujillo, Ibon Alkorta, and José Elguero. "Intramolecular pnicogen interactions in phosphorus and arsenic analogues of proton sponges." Phys. Chem. Chem. Phys. 16, no. 30 (2014): 15900–15909. http://dx.doi.org/10.1039/c4cp01072h.

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A computational study of the intramolecular pnicogen bond in 1,8-bis-substituted naphthalene derivatives (ZXH and ZX₂ with Z = P, As and X = H, F, Cl, and Br), structurally related to proton sponges, has been carried out.

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9

Zhu, Jian-Qing, Sheng-Wei Cao, Wei Wang, Xiao-Lu Xu, and Hui-Ying Xu. "The Substituent Effects on π-type Pnicogen Bond Interaction." IOP Conference Series: Earth and Environmental Science 63 (May 2017): 012027. http://dx.doi.org/10.1088/1755-1315/63/1/012027.

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10

Scheiner, Steve. "The Pnicogen Bond: Its Relation to Hydrogen, Halogen, and Other Noncovalent Bonds." Accounts of Chemical Research 46, no. 2 (November 7, 2012): 280–88. http://dx.doi.org/10.1021/ar3001316.

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11

Scheiner, Steve. "Detailed comparison of the pnicogen bond with chalcogen, halogen, and hydrogen bonds." International Journal of Quantum Chemistry 113, no. 11 (October 29, 2012): 1609–20. http://dx.doi.org/10.1002/qua.24357.

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12

Li, Qingzhong, Hongjie Zhu, Hongying Zhuo, Xin Yang, Wenzuo Li, and Jianbo Cheng. "Complexes between hypohalous acids and phosphine derivatives. Pnicogen bond versus halogen bond versus hydrogen bond." Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy 132 (November 2014): 271–77. http://dx.doi.org/10.1016/j.saa.2014.05.001.

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13

Jiao, Yinchun, and Frank Weinhold. "What Is the Nature of Supramolecular Bonding? Comprehensive NBO/NRT Picture of Halogen and Pnicogen Bonding in RPH2···IF/FI Complexes (R = CH3, OH, CF3, CN, NO2)." Molecules 24, no. 11 (May 31, 2019): 2090. http://dx.doi.org/10.3390/molecules24112090.

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We employ a variety of natural bond orbital (NBO) and natural resonance theory (NRT) tools to comprehensively investigate the nature of halogen and pnicogen bonding interactions in RPH2···IF/FI binary complexes (R = CH3, OH, CF3, CN, and NO2) and the tuning effects of R-substituents. Though such interactions are commonly attributed to “sigma-hole”-type electrostatic effects, we show that they exhibit profound similarities and analogies to the resonance-type 3-center, 4-electron (3c/4e) donor-acceptor interactions of hydrogen bonding, where classical-type “electrostatics” are known to play only a secondary modulating role. The general 3c/4e resonance perspective corresponds to a continuous range of interatomic A···B bond orders (bAB), spanning both the stronger “covalent” interactions of the molecular domain (say, bAB ≥ ½) and the weaker interactions (bAB ˂ ½, often misleadingly termed “noncovalent”) that underlie supramolecular complexation phenomena. We show how a unified NBO/NRT-based description of hydrogen, halogen, pnicogen, and related bonding yields an improved predictive utility and intuitive understanding of empirical trends in binding energies, structural geometry, and other measurable properties that are expected to be manifested in all such supramolecular interaction phenomena.

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14

Grabowski, Sławomir J. "σ-Hole Bonds and the VSEPR Model—From the Tetrahedral Structure to the Trigonal Bipyramid." Sci 4, no. 2 (April 19, 2022): 17. http://dx.doi.org/10.3390/sci4020017.

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Complexes linked by various interactions are analysed in this study. They are characterized by the tetrahedral configuration of the Lewis acid centre. Interactions, being a subject of this study, are classified as σ-hole bonds, such as the halogen, chalcogen, pnicogen, and tetrel bonds. In the case of strong interactions, the tetrahedral configuration of the Lewis acid centre changes into the trigonal bipyramid configuration. This change is in line with the Valence-Shell Electron-Pair Repulsion model, VSEPR, and this is supported here by the results of high-level ab initio calculations. The theoretical results concerning the geometries are supported mainly by the Natural Bond Orbital, NBO, method.

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15

Scheiner, Steve. "New ideas from an old concept: the hydrogen bond." Biochemist 41, no. 4 (August 1, 2019): 6–9. http://dx.doi.org/10.1042/bio04104006.

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Ongoing studies of the hydrogen bond (HB), in which a hydrogen (H) atom acts as a bridge between a pair of chemical groups, continues to offer new ideas about this interaction that have applications to biochemical processes. The ability of a proton to transfer within a HB can be controlled by conformational changes that cause small alterations to the HB geometry. The CH group, widely prevalent in biological systems, participates in HBs and contributes to the structure and stability of commonly occurring protein secondary structures such as the β-sheet. The concept of the HB has been extended to systems where the bridging proton is replaced by any of a large variety of electronegative atoms, in the form of halogen, chalcogen, pnicogen and tetrel bonds, with no loss of strength.

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16

Zhuo, Hongying, Qingzhong Li, Wenzuo Li, and Jianbo Cheng. "The dual role of pnicogen as Lewis acid and base and the unexpected interplay between the pnicogen bond and coordination interaction in H3N⋯FH2X⋯MCN (X = P and As; M = Cu, Ag, and Au)." New Journal of Chemistry 39, no. 3 (2015): 2067–74. http://dx.doi.org/10.1039/c4nj02051k.

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17

Lu, Jia, and Steve Scheiner. "Effects of Halogen, Chalcogen, Pnicogen, and Tetrel Bonds on IR and NMR Spectra." Molecules 24, no. 15 (August 2, 2019): 2822. http://dx.doi.org/10.3390/molecules24152822.

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Complexes were formed pairing FX, FHY, FH2Z, and FH3T (X = Cl, Br, I; Y = S, Se, Te; Z = P, As, Sb; T = Si, Ge, Sn) with NH3 in order to form an A⋯N noncovalent bond, where A refers to the central atom. Geometries, energetics, atomic charges, and spectroscopic characteristics of these complexes were evaluated via DFT calculations. In all cases, the A–F bond, which is located opposite the base and is responsible for the σ-hole on the A atom, elongates and its stretching frequency undergoes a shift to the red. This shift varies from 42 to 175 cm−1 and is largest for the halogen bonds, followed by chalcogen, tetrel, and then pnicogen. The shift also decreases as the central A atom is enlarged. The NMR chemical shielding of the A atom is increased while that of the F and electron donor N atom are lowered. Unlike the IR frequency shifts, it is the third-row A atoms that undergo the largest change in NMR shielding. The change in shielding of A is highly variable, ranging from negligible for FSnH3 all the way up to 1675 ppm for FBr, while those of the F atom lie in the 55–422 ppm range. Although smaller in magnitude, the changes in the N shielding are still easily detectable, between 7 and 27 ppm.

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18

Grabowski, Sławomir J. "Hydrogen Bond and Other Lewis Acid–Lewis Base Interactions as Preliminary Stages of Chemical Reactions." Molecules 25, no. 20 (October 13, 2020): 4668. http://dx.doi.org/10.3390/molecules25204668.

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Various Lewis acid–Lewis base interactions are discussed as initiating chemical reactions and processes. For example, the hydrogen bond is often a preliminary stage of the proton transfer process or the tetrel and pnicogen bonds lead sometimes to the SN2 reactions. There are numerous characteristics of interactions being first stages of reactions; one can observe a meaningful electron charge transfer from the Lewis base unit to the Lewis acid; such interactions possess at least partly covalent character, one can mention other features. The results of different methods and approaches that are applied in numerous studies to describe the character of interactions are presented here. These are, for example, the results of the Quantum Theory of Atoms in Molecules, of the decomposition of the energy of interaction or of the structure-correlation method.

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19

Michalczyk, Zierkiewicz, Wysokiński, and Scheiner. "Theoretical Studies of IR and NMR Spectral Changes Induced by Sigma-Hole Hydrogen, Halogen, Chalcogen, Pnicogen, and Tetrel Bonds in a Model Protein Environment." Molecules 24, no. 18 (September 12, 2019): 3329. http://dx.doi.org/10.3390/molecules24183329.

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Various types of σ-hole bond complexes were formed with FX, HFY, H2FZ, and H3FT (X = Cl, Br, I; Y = S, Se, Te; Z = P, As, Sb; T = Si, Ge, Sn) as Lewis acid. In order to examine their interactions with a protein, N-methylacetamide (NMA), a model of the peptide linkage was used as the base. These noncovalent bonds were compared by computational means with H-bonds formed by NMA with XH molecules (X = F, Cl, Br, I). In all cases, the A–F bond, which lies opposite the base and is responsible for the σ-hole on the A atom (A refers to the bridging atom), elongates and its stretching frequency undergoes a shift to the red with a band intensification, much as what occurs for the X–H bond in a H-bond (HB). Unlike the NMR shielding decrease seen in the bridging proton of a H-bond, the shielding of the bridging A atom is increased. The spectroscopic changes within NMA are similar for H-bonds and the other noncovalent bonds. The C=O bond of the amide is lengthened and its stretching frequency red-shifted and intensified. The amide II band shifts to higher frequency and undergoes a small band weakening. The NMR shielding of the O atom directly involved in the bond rises, whereas the C and N atoms both undergo a shielding decrease. The frequency shifts of the amide I and II bands of the base as well as the shielding changes of the three pertinent NMA atoms correlate well with the strength of the noncovalent bond.

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20

Lu, Jia, and Steve Scheiner. "Relationships between Bond Strength and Spectroscopic Quantities in H-Bonds and Related Halogen, Chalcogen, and Pnicogen Bonds." Journal of Physical Chemistry A 124, no. 38 (September 8, 2020): 7716–25. http://dx.doi.org/10.1021/acs.jpca.0c05936.

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21

Scheiner, Steve. "On the Ability of Nitrogen to Serve as an Electron Acceptor in a Pnicogen Bond." Journal of Physical Chemistry A 125, no. 48 (November 30, 2021): 10419–27. http://dx.doi.org/10.1021/acs.jpca.1c09213.

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22

Setiawan, Dani, Elfi Kraka, and Dieter Cremer. "Strength of the Pnicogen Bond in Complexes Involving Group Va Elements N, P, and As." Journal of Physical Chemistry A 119, no. 9 (November 7, 2014): 1642–56. http://dx.doi.org/10.1021/jp508270g.

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23

Esrafili, Mehdi D., Parvin Fatehi, and Mohammad Solimannejad. "Mutual interplay between pnicogen bond and dihydrogen bond in HMH⋯HCN⋯PH2X complexes (M=Be, Mg, Zn; X=H, F, Cl)." Computational and Theoretical Chemistry 1034 (April 2014): 1–6. http://dx.doi.org/10.1016/j.comptc.2014.02.003.

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24

Dong, Wenbo, Yu Wang, Jianbo Cheng, Xin Yang, and Qingzhong Li. "Competition between σ-hole pnicogen bond and π-hole tetrel bond in complexes of CF2=CFZH2 (Z = P, As, and Sb)." Molecular Physics 117, no. 3 (August 12, 2018): 251–59. http://dx.doi.org/10.1080/00268976.2018.1508782.

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25

Scheiner, Steve. "Relative Strengths of a Pnicogen and a Tetrel Bond and Their Mutual Effects upon One Another." Journal of Physical Chemistry A 125, no. 12 (March 18, 2021): 2631–41. http://dx.doi.org/10.1021/acs.jpca.1c01211.

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26

Michalczyk, Mariusz, Magdalena Malik, Wiktor Zierkiewicz, and Steve Scheiner. "Experimental and Theoretical Studies of Dimers Stabilized by Two Chalcogen Bonds in the Presence of a N···N Pnicogen Bond." Journal of Physical Chemistry A 125, no. 2 (January 11, 2021): 657–68. http://dx.doi.org/10.1021/acs.jpca.0c10814.

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27

Esrafili, Mehdi D., Fariba Mohammadian-Sabet, and Mohammad Solimannejad. "Mutual influence between anion–π and pnicogen bond interactions: The enhancement of P⋯N and P⋯O interactions by an anion–π bond." Journal of Molecular Graphics and Modelling 57 (April 2015): 99–105. http://dx.doi.org/10.1016/j.jmgm.2015.01.010.

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28

Zabardasti, Abedien, Saeed Farhadi, and Aliyar Mahdizadeh. "Cooperative effect between pnicogen bond and hydrogen bond interactions in typical X…AsH2F…HF complexes (X = NR3, PR3 and OR2; R = CH3, H, F)." Phosphorus, Sulfur, and Silicon and the Related Elements 193, no. 11 (November 2, 2018): 759–65. http://dx.doi.org/10.1080/10426507.2018.1513514.

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29

Abroushan, Eslam, Abedien Zabaradsti, Saeed Farhadi, and Ahmad Abodolmaleki. "Pnicogen bond interaction between PF2Y (Y = –C☰N, –N☰C) with NH3, CH3OH, H2O, and HF molecules." Structural Chemistry 28, no. 6 (May 25, 2017): 1843–51. http://dx.doi.org/10.1007/s11224-017-0968-1.

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30

LIU, YAN-ZHI, KUN YUAN, ZHAO YUAN, YUAN-CHENG ZHU, and XIANG ZHAO. "Theoretical exploration of pnicogen bond noncovalent interactions in HCHO⋯PH2X (X=CH3, H, C6H5, F, Cl, Br, and NO2) complexes." Journal of Chemical Sciences 127, no. 10 (October 2015): 1729–38. http://dx.doi.org/10.1007/s12039-015-0933-8.

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31

Gholipour, Alireza. "Mutual interplay between pnicogen–π and tetrel bond in PF3⊥X–Pyr…SiH3CN complexes: NMR, SAPT, AIM, NBO, and MEP analysis." Structural Chemistry 29, no. 5 (April 4, 2018): 1255–63. http://dx.doi.org/10.1007/s11224-018-1106-4.

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32

Esrafili, Mehdi D., and Hossein Akhgarpour. "Anab initiostudy on competition between pnicogen and chalcogen bond interactions in binary XHS:PH2X complexes (X = F, Cl, CCH, COH, CH3, OH, OCH3and NH2)." Molecular Physics 114, no. 12 (March 11, 2016): 1847–55. http://dx.doi.org/10.1080/00268976.2016.1158421.

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33

Ghafari Nikoo Jooneghani, Saber, and Alireza Gholipour. "Mutual cooperation of π-π stacking and pnicogen bond interactions of substituted monomeric Lawesson’s reagent and pyridine rings: Theoretical insight into Pyr||X-PhPS2⊥pyr complexes." Chemical Physics Letters 721 (April 2019): 91–98. http://dx.doi.org/10.1016/j.cplett.2019.02.027.

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34

Shukla, Rahul, and Deepak Chopra. "“Pnicogen bonds” or “chalcogen bonds”: exploiting the effect of substitution on the formation of P⋯Se noncovalent bonds." Physical Chemistry Chemical Physics 18, no. 20 (2016): 13820–29. http://dx.doi.org/10.1039/c6cp01703g.

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35

Jing, Xinyue, Yanli Zeng, Xueying Zhang, Lingpeng Meng, and Xiaoyan Li. "Competition and conversion between pnicogen bonds and hydrogen bonds involving prototype organophosphorus compounds." Physical Chemistry Chemical Physics 23, no. 34 (2021): 18794–805. http://dx.doi.org/10.1039/d1cp00474c.

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36

Shukla, Rahul, and Deepak Chopra. "Characterization of N⋯O non-covalent interactions involving σ-holes: “electrostatics” or “dispersion”." Physical Chemistry Chemical Physics 18, no. 43 (2016): 29946–54. http://dx.doi.org/10.1039/c6cp05899j.

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37

Guan, Liangyu, and Yirong Mo. "Electron Transfer in Pnicogen Bonds." Journal of Physical Chemistry A 118, no. 39 (March 11, 2014): 8911–21. http://dx.doi.org/10.1021/jp500775m.

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38

Alkorta, Ibon, José Elguero, and Sławomir J. Grabowski. "Pnicogen and hydrogen bonds: complexes between PH3X+ and PH2X systems." Physical Chemistry Chemical Physics 17, no. 5 (2015): 3261–72. http://dx.doi.org/10.1039/c4cp04840g.

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39

Roohi, Hossein, and Tahereh Tondro. "Exploring the pnicogen bond non-covalent interactions in 4-XPhNH 2 :PF n H 3-n complexes (n = 1–3, X = H, F, CN, CHO, NH 2 , CH 3 , NO 2 and OCH 3 )." Journal of Fluorine Chemistry 202 (October 2017): 19–33. http://dx.doi.org/10.1016/j.jfluchem.2017.08.009.

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40

Alkorta, Ibon, Janet Del Bene, and Jose Elguero. "H2XP:OH2 Complexes: Hydrogen vs. Pnicogen Bonds." Crystals 6, no. 2 (February 2, 2016): 19. http://dx.doi.org/10.3390/cryst6020019.

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41

Zahn, Stefan, René Frank, Eva Hey‐Hawkins, and Barbara Kirchner. "Pnicogen Bonds: A New Molecular Linker?" Chemistry – A European Journal 17, no. 22 (April 18, 2011): 6034–38. http://dx.doi.org/10.1002/chem.201002146.

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42

Del Bene, Janet E., Ibon Alkorta, and José Elguero. "Can HNNH, FNNH, or HNCHOH bridge the σ-hole and the lone pair at P in binary complexes with H2XP, for X = F, Cl, NC, OH, CN, CCH, CH3, and H?" Physical Chemistry Chemical Physics 17, no. 45 (2015): 30729–35. http://dx.doi.org/10.1039/c5cp05832e.

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43

Mohajeri, Afshan, K. Eskandari, and Saeedeh Amin Safaee. "Endohedral pnicogen and triel bonds in doped C60 fullerenes." New Journal of Chemistry 41, no. 19 (2017): 10619–26. http://dx.doi.org/10.1039/c7nj01477e.

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44

Scheiner, Steve. "Comparison of halide receptors based on H, halogen, chalcogen, pnicogen, and tetrel bonds." Faraday Discussions 203 (2017): 213–26. http://dx.doi.org/10.1039/c7fd00043j.

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A series of halide receptors are constructed and the geometries and energetics of their binding to F⁻, Cl⁻, and Br⁻assessed by quantum calculations. The dicationic receptors are based on a pair of imidazolium units, connectedviaa benzene spacer. The imidazoliums each donate a proton to a halide in a pair of H-bonds. Replacement of the two bonding protons by Br leads to bindingviaa pair of halogen bonds. Likewise, chalcogen, pnicogen, and tetrel bonds occur when the protons are replaced, respectively, by Se, As, and Ge. Regardless of the binding group considered, F⁻is bound much more strongly than are Cl⁻and Br⁻. With respect to the latter two halides, the binding energy is not very sensitive to the nature of the binding atom, whether H or some other atom. But there is a great deal of differentiation with respect to F⁻, where the order varies as tetrel > H ∼ pnicogen > halogen > chalcogen. The replacement of the various binding atoms by their analogues in the next row of the periodic table enhances the fluoride binding energy by 22–56%. The strongest fluoride binding agents utilize the tetrel bonds of the Sn atom, whereas it is I-halogen bonds that are preferred for Cl⁻and Br⁻. After incorporation of thermal and entropic effects, the halogen, chalcogen, and pnicogen bonding receptors do not represent much of an improvement over H-bonds with regard to this selectivity for F⁻, even I which binds quite strongly. In stark contrast, the tetrel-bonding derivatives, both Ge and Sn, show by far the greatest selectivity for F⁻over the other halides, as much as 10¹³, an enhancement of six orders of magnitude when compared to the H-bonding receptor.

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45

Lin, Hui, Lingpeng Meng, Xiaoyan Li, Yanli Zeng, and Xueying Zhang. "Comparison of pnicogen and tetrel bonds in complexes containing CX2 carbenes (X = F, Cl, Br, OH, OMe, NH2, and NMe2)." New Journal of Chemistry 43, no. 39 (2019): 15596–604. http://dx.doi.org/10.1039/c9nj03397a.

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The similarities and differences of pnicogen and tetrel bonds formed by carbenes CX₂ with H₃AsO and H₃SiCN were investigated by carrying out ab initio calculations in association with topological analysis of electron density.

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Saha, Arijit, Ragima V. P. Veluthaparambath, and Binoy K. Saha. "Directionality of P⋯O pnicogen bonding in light of geometry corrected statistical analysis." New Journal of Chemistry 44, no. 23 (2020): 9607–10. http://dx.doi.org/10.1039/d0nj01683g.

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Cone corrected statistical analysis suggests that the X–P⋯O angle prefers linearity which is more prominent in the case of X₃P⋯O compared to X₄P⋯O pnicogen bonds. This preference also increases with an increase in the electronegativity of X.

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Zahn, Stefan, René Frank, Evamarie Hey-Hawkins, and Barbara Kirchner. "Corrigendum: Pnicogen Bonds: A New Molecular Linker?" Chemistry - A European Journal 19, no. 5 (January 17, 2013): 1526. http://dx.doi.org/10.1002/chem.201204538.

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Avens, Larry R., Leonard V. Cribbs, and Jerry L. Mills. "Exchange reactions of tetrakis(trifluoromethyl)diphosphine with pnicogen-pnicogen, phosphorus-hydrogen, and phosphorus-chlorine bonds." Inorganic Chemistry 28, no. 2 (January 1989): 211–14. http://dx.doi.org/10.1021/ic00301a011.

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Tripathi, Garima, Khalid Badi-uz-zama, and Gurunath Ramanathan. "N…N pnicogen bonds in Boc-DOPA-OMe." Chemical Physics Letters 653 (June 2016): 117–21. http://dx.doi.org/10.1016/j.cplett.2016.04.076.

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Grabowski, Sławomir J. "Pnicogen and tetrel bonds—tetrahedral Lewis acid centres." Structural Chemistry 30, no. 4 (May 25, 2019): 1141–52. http://dx.doi.org/10.1007/s11224-019-01358-1.

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