α-溴代羰基化合物脱溴的一种简便方法

卤代物的脱卤反应是有机合成中重要反应之一,应用有机碲试剂使某些邻二溴代物脱溴反应及α-卤代羰基化合物的脱卤反应已有文献报道。我们在研究碲 Ylide 反应过程中发现二丁基碲能使某些单取代的α-溴代酮发生脱溴反应,这是一种未见文献报道的新的脱溴反应。为了考察二丁基碲作为一种新的脱溴试剂应用的可能性,我们对二丁基碲的脱     

α—溴代芳基酮还原脱溴的新方法

α—溴代芳基酮的还原脱溴是有机化学中一种非常重要的官能团相互转换，通常有机合成中经常采用的是由芳基酮来制备α—溴代芳基酮，而反过来由α—溴代芳基酮来制备芳基酮的研究甚少，现在对碲使α—溴代芳基酮的还原脱溴反应进行研究，不仅拓宽了碲的应用范围，而且对将...     

二级胺与羰基化合物的一步还原烷基化

碲试剂作为还原剂已得到较广泛的应用,Yamashita、周洵钧将NaHTe用于羰基化合物还原胺化为二级胺,Kambe等近期用H_2Te还原烯胺、亚胺到相应的胺,我们曾用NaHTe将二级胺与羰基化合物还原烷基化。本文采用不同二级胺进一步研究发现,脂肪环胺与醛的反应效果较好,同一条件下烯胺也可被还原,反应条件温和,脯氨酸酯还原烷基化的产物不发生明显消旋化(表1,3),可应用于氨基酸类反应。     

E -型α, β-不饱和酰胺的立体选择合成

本文报道了在钯及二丁基碲存在下, 溴代乙酰胺与醛的亲卤缩合反应, 提供了E型α, β-不饱和酰胺的立体选择合成。     

大孔型聚合物氧化三甲胺的制备及其氧化卤代烃成醛的研究

本文以D301大孔弱碱性阴离子交换树脂为原料制备了一种稳定的氧化树脂——大孔型聚合物氧化三甲胺,并研究了其氧化各类卤代烃成醛的反应。实验结果表明:该氧化树脂能在温和条件下将伯碘代物、伯溴代物、烯丙基型卤代物及苄基卤代物高产率地氧化成醛;用该氧化树脂氧化双溴代物可得到良好产率的单醛;当同一化合物中卤原子和其它官能团共存时,该氧化树脂可对其中的卤原子进行选择性氧化。反应后的树脂可完全再生,重复使用三次后树脂的活性没有明显的降低。     

2-甲基-6-溴苯并碲唑及其衍生菁染料的合成

以对溴苯胺为原料,经汞化、酰化,再与四氯化碲发生亲电取代反应生成2-乙酰氨基-5-溴苯基三氯化碲(内盐);后者以硼氢化钠还原、浓盐酸关环,用碳酸氢钠中和后即得关键中间体2-甲基-6-溴苯并碲唑。苯并碲唑经碘甲烷或碘乙烷季铵化后,用原甲酸三乙酯缩合制得相应的对称染料2,2'-二甲基-5,5'-二溴碲碳菁碘盐和2,2'-二乙基-5,5'-二溴碲碳菁碘盐。测定了它们的可见吸收光谱。     

(Z)-1-三苯基锡基-3-对氯苯基-1-丁烯-3-醇及其卤代物的合成、表征和晶体结构

在氮气保护下,3-对氯苯基-1-丁炔-3-醇与三苯基氢化锡进行游离基加成反应,获得加成物(Z)-1-三苯基锡基-3-对氯苯基-1-丁烯-3-醇(1).加成物(1)与卤素反应后,与锡原子相连的苯基被取代,得到一卤代、二卤代和混合二卤代物(2-8).通过元素分析、¹HNMR和IR表征了化合物1～8的结构,并测定了加成物(1)、一溴代物(3)和二溴代物(5)的晶体结构.在加成物(1)的晶体结构中存在一对对映体,由于分子内存在较弱的O→Sn配位作用,构成以锡原子为中心的扭曲四面体构型.在化合物3和5分子中,存在分子内O→Sn配位键,构成以锡为中心的扭曲三角双锥构型.该系列化合物分子内的O→Sn配位能力和Lewis酸性强弱的顺序为:二卤化物>一卤化物>加成物;氯代物>溴代物>碘代物.     

新型含氮三齿钯(II)配合物的合成及其催化性能研究

以白屈氨酸为原料, 经酯化、还原、溴化、胺化等反应合成了4位带活性基团的新型含氮(NN'N)三齿配体, 配体进一步与氯化钯反应制得了Pd(II)的配合物, 并用红外、核磁、元素分析等手段进行了表征. 考察了这种钳形配合物的催化性能, 结果表明该配合物对卤代苯与乙烯基化合物的Heck芳基化反应具有较高的催化活性.     

多溴联苯醚的光催化还原脱溴

多溴联苯醚(PBDEs)在生态环境中是普遍存在的并已证实具有潜在的毒性,因此PBDEs引起了环境化学领域的广泛关注。光催化技术具有可利用太阳能、反应选择性高且反应条件温和等优点,其在降解PBDEs这类污染物方面具有独特的优势。近年来光催化在降解含卤有机污染物的研究中取得长足进展。本文就多卤代芳烃类化合物中最为典型的PBDEs的光催化还原研究现状进行介绍,并着重阐述TiO_2催化剂对PBDEs的光催化还原脱溴反应的基本过程、提高光催化还原效率的途径以及光催化还原脱溴机理等。除此之外,本文也对PBDEs未来光催化还原脱溴的前景进行了简单的展望。     

2—甲基—6—溴苯并碲唑及其衍生菁染料的合成

以对溴苯胺为原料，经汞化、酰化，再与四氯化碲发生亲电取代反应生成２－乙酰氨基－５－溴苯基三氯化碲（内盐）；后者以硼氢化钠还原、浓盐酸关环，用碳酸氢钠中和后即得关键中间体２－甲基－６－溴苯并碲唑，苯并碲唑经碘甲烷或碘乙烷季铵化后，用原甲酸三乙酯缩合制得相应的对称染料２，２’－二甲基－５，５’－二溴碲碳菁碘盐和２，２’－二乙基－５，５’－二溴碲碳菁磺盐，屯它们的可见吸收光谱。     

Hydrogen bond and halogen bond inside the carbon nanotube

The hydrogen bond and halogen bond inside the open-ended single-walled carbon nanotubes have been investigated theoretically employing the newly developed density functional M06 with the suitable basis set and the natural bond orbital analysis. Comparing with the hydrogen or halogen bond in the gas phase, we find that the strength of the hydrogen or halogen bond inside the carbon nanotube will become weaker if there is a larger intramolecular electron-density transfer from the electron-rich region of the hydrogen or halogen atom donor to the antibonding orbital of the X-H or X-Hal bond involved in the formation of the hydrogen or halogen bond and will become stronger if there is a larger intermolecular electron-density transfer from the electron-rich region of the hydrogen or halogen atom acceptor to the antibonding orbital of the X-H or X-Hal bond. According to the analysis of the molecular electrostatic potential of the carbon nanotube, the driving force for the electron-density transfer is found to be the negative electric field formed in the carbon nanotube inner phase. Our results also show that the X-H bond involved in the formation of the hydrogen bond and the X-Hal bond involved in the formation of the halogen bond are all elongated when encapsulating the hydrogen bond and halogen bond within the carbon nanotube, so the carbon nanotube confinement may change the blue-shifting hydrogen bond and the blue-shifting halogen bond into the red-shifting hydrogen bond and the red-shifting halogen bond. The possibility to replace the all electron nanotube-confined calculation by the simple polarizable continuum model is also evaluated.     

A Halogen‐Bond Donor Catalyst for Templated Macrocyclization

A halogen‐bond templated 1:1 macrocyclization in solution is reported. Tetra(iodoperfluorophenyl) ethers were used as halogen‐bonded exotemplates in a substoichiometric amount (5 mol %). Pyridine‐containing macrocyclic architectures were formed by ruthenium‐catalyzed tandem metathesis/transfer hydrogenation sequence using sodium borohydride and methanol as non‐dihydrogen hydrogen source. The halogen‐bonded stabilization energies were analyzed relying on density functional theory.     

Theoretical study on the bromomethane-water 1:2 complexes

Bromomethane-water 1:2 complexes have been theoretically studied to reveal the role of hydrogen bond and halogen bond in the formation of different aggregations. Four stable structures exist on the potential energy surface of the CH3Br(H2O)2 complex. The bromine atom acts mainly as proton acceptor in the four studied structures. It is also capable of participating in the formation of the halogen bond. The properties and characteristics of the hydrogen bond and the halogen bond are investigated employing several different quantum chemical analysis methods. Cooperative effects for the pure hydrogen bonds or the mixed hydrogen bonds with halogen bonds and the possibility of describing cooperative effects in terms of the topological analysis of the electronic density or the charge-transfer stabilization energy are discussed in detail. An atoms-in-molecules study of the hydrogen bond or the halogen bond in the bromomethane-water 1:2 complexes suggests that the electronic density topology of the hydrogen bond or the halogen bond is insensitive to the cooperative effect. The charge-transfer stabilization energy is proportional to the cooperative effect, which indicates the donor-acceptor electron density transfer to be mainly responsible for the trimer nonadditive effect.     

Competition between hydrogen and halogen bonding in halogenated 1‐methyluracil: Water systems

The competition between hydrogen‐ and halogen‐bonding interactions in complexes of 5‐halogenated 1‐methyluracil (XmU; X = F, Cl, Br, I, or At) with one or two water molecules in the binding region between C5‐X and C4?O4 is investigated with M06‐2X/6‐31+G(d). In the singly‐hydrated systems, the water molecule forms a hydrogen bond with C4?O4 for all halogens, whereas structures with a halogen bond between the water oxygen and C5‐X exist only for X = Br, I, and At. Structures with two waters forming a bridge between C4?O and C5‐X (through hydrogen‐ and halogen‐bonding interactions) exist for all halogens except F. The absence of a halogen‐bonded structure in singly‐hydrated ClmU is therefore attributed to the competing hydrogen‐bonding interaction with C4?O4. The halogen‐bond angle in the doubly‐hydrated structures (150–160°) is far from the expected linearity of halogen bonds, indicating that significantly non‐linear halogen bonds may exist in complex environments with competing interactions. © 2016 Wiley Periodicals, Inc.     

A Convenient Method of Synthesis of Dialkyltellurides and Dialkylditellurides

Elemental tellurium is reduced by thioureadioxide in alkaline medium, leading to disodium telluride or ditelluride, depending on the amount of thioureadioxide used. The intermediate disodium telluride or ditelluride reacts “in situ” with alkyl halides to give dialkyltellurides or dialkylditellurides in high yield.     

Some measures for making halogen bonds stronger than hydrogen bonds in H2CS-HOX (X = F, Cl, and Br) complexes

The properties and applications of halogen bonds are dependent greatly on their strength. In this paper, we suggested some measures for enhancing the strength of the halogen bond relative to the hydrogen bond in the H(2)CS-HOX (X = F, Cl, and Br) system by means of quantum chemical calculations. It has been shown that with comparison to H(2)CO, the S electron donor in H(2)CS results in a smaller difference in strength for the Cl halogen bond and the corresponding hydrogen bond, and the Br halogen bond is even stronger than the hydrogen bond. The Li atom in LiHCS and methyl group in MeHCS cause an increase in the strength of halogen bonding and hydrogen bonding, but the former makes the halogen bond stronger and the latter makes the hydrogen bond stronger. In solvents, the halogen bond in the Br system is strong enough to compete with the hydrogen bond. The interaction nature and properties in these complexes have been analyzed with the natural bond orbital theory.     

Halogen Bonding in Organic Synthesis and Organocatalysis

Halogen bonding is a noncovalent interaction similar to hydrogen bonding, which is based on electrophilic halogen substituents. Hydrogen‐bonding‐based organocatalysis is a well‐established strategy which has found numerous applications in recent years. In light of this, halogen bonding has recently been introduced as a key interaction for the design of activators or organocatalysts that is complementary to hydrogen bonding. This Concept features a discussion on the history and electronic origin of halogen bonding, summarizes all relevant examples of its application in organocatalysis, and provides an overview on the use of cationic or polyfluorinated halogen‐bond donors in halide abstraction reactions or in the activation of neutral organic substrates.     

Nature of the Hydrogen Bond Enhanced Halogen Bond

The factors responsible for the enhancement of the halogen bond by an adjacent hydrogen bond have been quantitatively explored by means of state-of-the-art computational methods. It is found that the strength of a halogen bond is enhanced by ca. 3 kcal/mol when the halogen donor simultaneously operates as a halogen bond donor and a hydrogen bond acceptor. This enhancement is the result of both stronger electrostatic and orbital interactions between the XB donor and the XB acceptor, which indicates a significant degree of covalency in these halogen bonds. In addition, the halogen bond strength can be easily tuned by modifying the electron density of the aryl group of the XB donor as well as the acidity of the hydrogen atoms responsible for the hydrogen bond.     

Vicarious nucleophilic substitution of hydrogen versus vinylic substitution of halogen in the reactions of carbanions of halomethyl aryl sulfones with dialkyl halofumarates and halomaleates

Reaction of halomethyl aryl sulfone carbanions with dialkyl halofumarates and halomaleates results in nucleophilic substitution of hydrogen and/or of the halogen. The reaction with halofumarates proceeds via addition of the carbanions to the vinylic carbon atom connected with hydrogen, followed by base promoted β-elimination of hydrogen halide in which the halogen originates from the carbanion moiety or from the alkene. In the case of halomaleates the reaction proceeds via an elimination-addition sequence.     

Rational Modification of the Hierarchy of Intermolecular Interactions in Molecular Crystal Structures by Using Tunable Halogen Bonds

A family of 16 isomolecular salts (3‐XpyH)₂[MX′₄] (3‐XpyH=3‐halopyridinium; M=Co, Zn; X=(F), Cl, Br, (I); X′=Cl, Br, I) each containing rigid organic cations and tetrahedral halometallate anions has been prepared and characterized by X‐ray single crystal and/or powder diffraction. Their crystal structures reflect the competition and cooperation between non‐covalent interactions: N? H???X′? M hydrogen bonds, C? X???X′? M halogen bonds and π–π stacking. The latter are essentially unchanged in strength across the series, but both halogen bonds and hydrogen bonds are modified in strength upon changing the halogens involved. Changing the organic halogen (X) from F to I strengthens the C? X???X′? M halogen bonds, whereas an analogous change of the inorganic halogen (X′) weakens both halogen bonds and N? H???X′? M hydrogen bonds. By so tuning the strength of the putative halogen bonds from repulsive to weak to moderately strong attractive interactions, the hierarchy of the interactions has been modified rationally leading to systematic changes in crystal packing. Three classes of crystal structure are obtained. In type A (C? F???X′? M) halogen bonds are absent. The structure is directed by N? H???X′? M hydrogen bonds and π‐stacking interactions. In type B structures, involving small organic halogens (X) and large inorganic halogens (X′), long (weak) C? X???X′? M interactions are observed with type I halogen–halogen interaction geometries (C? X???X′ ≈ X???X′? M ≈155°), but hydrogen bonds still dominate. Thus, minor but quite significant perturbations from the type A structure arise. In type C, involving larger organic halogens (X) and smaller inorganic halogens (X′), stronger halogen bonds are formed with a type II halogen–halogen interaction geometry (C? X???X′ ≈180°; X???X′? M ≈110°) that is electrostatically attractive. The halogen bonds play a major role alongside hydrogen bonds in directing the type C structures, which as a result are quite different from type A and B.