用户:Zhantongz/沙盒1

现在正在的进行的沙盒1项目：分子理论史

“ 此项目在完成后将会立即移至分子理论史条目 ”

水分子(H₂O)的CPK模型

现代分子的概念可以追溯到古希腊哲学家留基伯时代，他认为宇宙是由原子和空洞组成。早在战国时期，儒家经典《尚书‧洪范》曰：“五行，一曰水、二曰火、三曰木、四曰金、五曰土”，即五行。五行是中国最早的元素概念。在公元前约450年，古希腊人恩培多克勒想象出构成世界的是基本元素（火()、地()、风()和水()）以及这些元素间的相互作用力。在此之前，赫拉克利特曾声称我们生存的根本是由相反属性结合成的火。在《蒂迈欧篇》中，受毕达哥拉斯影响的柏拉图认为数学实体（例如数、点、线和三角形）是世界的基本构成元素，并认为火、地、风和水四种元素是由数学原理或元素能通过的东西组成的物质。 第五种元素，以太，被认为是天体的基本构成物质。恩培多克勒和留基伯的观点，与以太一起，被亚里士多德接受并传递到中世纪和文艺复兴时期的欧洲。

随着实验证明了纯化学元素（单质）的存在，并又有实验发现了不同的单个原子形成化学性质稳定的分子（如氢气和氧气的单个原子可以结合起来形成水分子）的过程，现代概念上的分子在19世纪开始发展。

17世纪

The earliest views on the shapes and connectivity of atoms was that proposed by Leucippus, Democritus, and Epicurus who reasoned that the solidness of the material corresponded to the shape of the atoms involved. Thus, iron atoms are solid and strong with hooks that lock them into a solid; water atoms are smooth and slippery; salt atoms, because of their taste, are sharp and pointed; and air atoms are light and whirling, pervading all other materials. It was Democritus that was the main proponent of this view. Using analogies from our sense experiences, he gave a picture or an image of an atom in which atoms were distinguished from each other by their shape, their size, and the arrangement of their parts. Moreover, connections were explained by material links in which single atoms were supplied with attachments: some with hooks and eyes others with balls and sockets.

A water molecule as Descartes' hook-and-eye model might have represented it. Note that at the time (c.1625) the composition of water was not known.

With the rise of Christianity and the decline of the Roman Empire, the atomic theory was abandoned for nearly two millennia in favor of the various four element theories and later alchemical theories. The 17th century, however, saw a resurgence in the atomic theory primarily through the works of Descartes, Gassendi, and Newton. Using earlier Greek atomic theories to explain how the tiniest particles of matter bonded together, Descartes visualized that atoms were held together by microscopic hooks and barbs. He held that two atoms combined when the hook of one got caught in the eye of the other (see diagram):

By the mid 1770s, it was generally believed that any theory involving particles endowed with physical hooks was considered “Cartesian chemistry”. Similar to Descartes, Gassendi, who had recently written a book on the life of Epicurus, reasoned that to account for the size and shape of atoms moving in a void could account for the properties of matter. Heat was due to small, round atoms; cold, to pyramidal atoms with sharp points, which accounted for the pricking sensation of severe cold; and solids were held together by interlacing hooks.

Newton, though he acknowledged the various atom attachment theories in vogue at the time, i.e. “hooked atoms”, “glued atoms” (bodies at rest), and the “stick together by conspiring motions” theory, rather believed, as famously stated in "Query 31" of his 1704 Opticks, that particles attract one another by some force, which “in immediate contact is extremely strong, at small distances performs the chemical operations, and reaches not far from particles with any sensible effect.”

In a more concrete manner, however, the concept of aggregates or units of bonded atoms, i.e. "molecules", traces its origins to Robert Boyle's 1661 hypothesis, in his famous treatise The Sceptical Chymist, that matter is composed of clusters of particles and that chemical change results from the rearrangement of the clusters. Boyle argued that matter's basic elements consisted of various sorts and sizes of particles, called "corpuscles", which were capable of arranging themselves into groups.

In 1680, using the corpuscular theory as a basis, French chemist Nicolas Lemery stipulated that the acidity of any substance consisted in its pointed particles, while alkalis were endowed with pores of various sizes. A molecule, according to this view, consisted of corpuscles united through a geometric locking of points and pores.

18世纪

Étienne François Geoffroy’s 1718 Affinity Table: at the head of the column is a substance with which all the substances below can combine.

An early precursor to the idea of bonded "combinations of atoms", was the theory of "combination via chemical affinity". For example, in 1718, building on Boyle’s conception of combinations of clusters, the French chemist Étienne François Geoffroy developed theories of chemical affinity to explain combinations of particles, reasoning that a certain alchemical “force” draws certain alchemical components together. Geoffroy's name is best known in connection with his tables of "affinities" (tables des rapports), which he presented to the French Academy in 1718 and 1720.

These were lists, prepared by collating observations on the actions of substances one upon another, showing the varying degrees of affinity exhibited by analogous bodies for different reagents. These tables retained their vogue for the rest of the century, until displaced by the profounder conceptions introduced by CL Berthollet.

In 1738, Swiss physicist and mathematician Daniel Bernoulli published Hydrodynamica, which laid the basis for the kinetic theory of gases. In this work, Bernoulli positioned the argument, still used to this day, that gases consist of great numbers of molecules moving in all directions, that their impact on a surface causes the gas pressure that we feel, and that what we experience as heat is simply the kinetic energy of their motion. The theory was not immediately accepted, in part because conservation of energy had not yet been established, and it was not obvious to physicists how the collisions between molecules could be perfectly elastic.

In 1789, William Higgins published views on what he called combinations of "ultimate" particles, which foreshadowed the concept of valency bonds. If, for example, according to Higgins, the force between the ultimate particle of oxygen and the ultimate particle of nitrogen were 6, then the strength of the force would be divided accordingly, and similarly for the other combinations of ultimate particles:

William Higgins' combinations of ultimate particles (1789)

19世纪

约翰·道尔顿

1803年，约翰·道尔顿以最轻的原子 - 氢原子的原子质量为单位，用比例来描述化合物。例如，亚硝酸酐的原子个数比为2:3给出的化学式为 N₂O₃。有趣的是，道尔顿错误地想象原子互相“钩住”形成分子。

阿莫迪欧·阿伏伽德罗

后来，1808年，道尔顿发表了著名的原子组合图：

约翰·道尔顿的化合物中原子的比例图（由于某些错误的原子量，比例并不一定正确） (1808)

在阿莫迪欧·阿伏伽德罗1811年发表的 "Essay on Determining the Relative Masses of the Elementary Molecules of Bodies"论文中，他本质上指出：

气体的最小粒子是不一定是单个的原子，而是一些原子以一定的吸引力结合在一起形成的一个分子。

注意这句话并非直译。阿伏伽德罗把原子和分子都称为”分子“ 。具体来说，他使用”初级分子“来表述原子，并使用”复合分子“和”超复合分子“来表达物质的聚合。

During his stay in Vercelli, Avogadro wrote a concise note (memoria) in which he declared the hypothesis of what we now call Avogadro's law: equal volumes of gases, at the same temperature and pressure, contain the same number of molecules. This law implies that the relationship occurring between the weights of same volumes of different gases, at the same temperature and pressure, corresponds to the relationship between respective molecular weights. Hence, relative molecular masses could now be calculated from the masses of gas samples.

Avogadro developed this hypothesis in order to reconcile Joseph Louis Gay-Lussac's 1808 law on volumes and combining gases with Dalton's 1803 atomic theory. The greatest difficulty Avogadro had to resolve was the huge confusion at that time regarding atoms and molecules—one of the most important contributions of Avogadro's work was clearly distinguishing one from the other, admitting that simple particles too could be composed of molecules, and that these are composed of atoms. Dalton, by contrast, did not consider this possibility. Curiously, Avogadro considers only molecules containing even numbers of atoms; he does not say why odd numbers are left out.

In 1826, building on the work of Avogadro, the French chemist Jean-Baptiste Dumas states:

Gases in similar circumstances are composed of molecules or atoms placed at the same distance, which is the same as saying that they contain the same number in the same volume.

In coordination with these concepts, in 1833 the French chemist Marc Antoine Auguste Gaudin presented a clear account of Avogadro's hypothesis, regarding atomic weights, by making use of “volume diagrams”, which clearly show both semi-correct molecular geometries, such as a linear water molecule, and correct molecular formulas, such as H₂O:

Marc Antoine Auguste Gaudin's volume diagrams of molecules in the gas phase (1833)

In two papers outlining his "theory of atomicity of the elements" (1857–58), Friedrich August Kekulé was the first to offer a theory of how every atom in an organic molecule was bonded to every other atom. He proposed that carbon atoms were tetravalent, and could bond to themselves to form the carbon skeletons of organic molecules.

In 1856, Scottish chemist Archibald Couper began research on the bromination of benzene at the laboratory of Charles Wurtz in Paris. One month after Kekulé's second paper appeared, Couper's independent and largely identical theory of molecular structure was published. He offered a very concrete idea of molecular structure, proposing that atoms joined to each other like modern-day Tinkertoys in specific three-dimensional structures. Couper was the first to use lines between atoms, in conjunction with the older method of using brackets, to represent bonds, and also postulated straight chains of atoms as the structures of some molecules, ring-shaped molecules of others, such as in tartaric acid and cyanuric acid In later publications, Couper’s bonds were represented using straight dotted lines (although it is not known if this is the typesetter’s preference) such as with alcohol and oxalic acid below:

Archibald Couper's molecular structures, for alcohol and oxalic acid, using elemental symbols for atoms and lines for bonds (1858)

In 1861, an unknown Vienna high-school teacher named Joseph Loschmidt published, at his own expense, a booklet entitled Chemische Studien I, containing pioneering molecular images which showed both "ringed" structures as well as double-bonded structures, such as:

Joseph Loschmidt's molecule drawings of ethylene H₂C=CH₂ and acetylene HC≡CH (1861)

Loschmidt also suggested a possible formula for benzene, but left the issue open. The first proposal of the modern structure for benzene was due to Kekulé, in 1865. The cyclic nature of benzene was finally confirmed by the crystallographer Kathleen Lonsdale. Benzene presents a special problem in that, to account for all the bonds, there must be alternating double carbon bonds:

Benzene molecule with alternating double bonds

In 1865, German chemist August Wilhelm von Hofmann was the first to make stick-and-ball molecular models, which he used in lecture at the Royal Institution of Great Britain, such as methane shown below:

Hofmann's 1865 stick-and-ball model of methane CH₄.

The basis of this model followed the earlier 1855 suggestion by his colleague William Odling that carbon is tetravalent. Hofmann's color scheme, to note, is still used to this day: nitrogen = blue, oxygen = red, chlorine = green, sulfur = yellow, hydrogen = white. The deficiencies in Hofmann's model were essentially geometric: carbon bonding was shown as planar, rather than tetrahedral, and the atoms were out of proportion, e.g. carbon was smaller in size than the hydrogen.

In 1864, Scottish organic chemist Alexander Crum Brown began to draw pictures of molecules, in which he enclosed the symbols for atoms in circles, and used broken lines to connect the atoms together in a way that satisfied each atom's valence.

The year 1873, by many accounts, was a seminal point in the history of the development of the concept of the "molecule". In this year, the renowned Scottish physicist James Clerk Maxwell published his famous thirteen page article 'Molecules' in the September issue of Nature. In the opening section to this article, Maxwell clearly states:

An atom is a body which cannot be cut in two; a molecule is the smallest possible portion of a particular substance.

After speaking about the atomic theory of Democritus, Maxwell goes on to tell us that the word 'molecule' is a modern word. He states, "it does not occur in Johnson's Dictionary. The ideas it embodies are those belonging to modern chemistry." We are told that an 'atom' is a material point, invested and surrounded by 'potential forces' and that when 'flying molecules' strike against a solid body in constant succession it causes what is called pressure of air and other gases. At this point, however, Maxwell notes that no one has ever seen or handled a molecule.

In 1874, Jacobus Henricus van 't Hoff and Joseph Achille Le Bel independently proposed that the phenomenon of optical activity could be explained by assuming that the chemical bonds between carbon atoms and their neighbors were directed towards the corners of a regular tetrahedron. This led to a better understanding of the three-dimensional nature of molecules.

Emil Fischer developed the Fischer projection technique for viewing 3-D molecules on a 2-D sheet of paper:

In 1898, Ludwig Boltzmann, in his Lectures on Gas Theory, used the theory of valence to explain the phenomenon of gas phase molecular dissociation, and in doing so drew one of the first rudimentary yet detailed atomic orbital overlap drawings. Noting first the known fact that molecular iodine vapor dissociates into atoms at higher temperatures, Boltzmann states that we must explain the existence of molecules composed of two atoms, the “double atom” as Boltzmann calls it, by an attractive force acting between the two atoms. Boltzmann states that this chemical attraction, owing to certain facts of chemical valence, must be associated with a relatively small region on the surface of the atom called the sensitive region.

Boltzmann states that this "sensitive region" will lie on the surface of the atom, or may partially lie inside the atom, and will firmly be connected to it. Specifically, he states “only when two atoms are situated so that their sensitive regions are in contact, or partly overlap, will there be a chemical attraction between them. We then say that they are chemically bound to each other.” This picture is detailed below, showing the α-sensitive region of atom-A overlapping with the β-sensitive region of atom-B:

Boltzmann’s 1898 I₂ molecule diagram showing atomic “sensitive region” (α, β) overlap.

20世纪

In the early 20th century, the American chemist Gilbert N. Lewis began to use dots in lecture, while teaching undergraduates at Harvard, to represent the electrons around atoms. His students favored these drawings, which stimulated him in this direction. From these lectures, Lewis noted that elements with a certain number of electrons seemed to have a special stability. This phenomenon was pointed out by the German chemist Richard Abegg in 1904, to which Lewis referred to as "Abegg's law of valence" (now generally known as Abegg's rule). To Lewis it appeared that once a core of eight electrons has formed around a nucleus, the layer is filled, and a new layer is started. Lewis also noted that various ions with eight electrons also seemed to have a special stability. On these views, he proposed the rule of eight or octet rule: Ions or atoms with a filled layer of eight electrons have a special stability.

Moreover, noting that a cube has eight corners Lewis envisioned an atom as having eight sides available for electrons, like the corner of a cube. Subsequently, in 1902 he devised a conception in which cubic atoms can bond on their sides to form cubic-structured molecules.

In other words, electron-pair bonds are formed when two atoms share an edge, as in structure C below. This results in the sharing of two electrons. Similarly, charged ionic-bonds are formed by the transfer of an electron from one cube to another, without sharing an edge A. An intermediate state B where only one corner is shared was also postulated by Lewis.

Lewis cubic-atoms bonding to form cubic-molecules

Hence, double bonds are formed by sharing a face between two cubic atoms. This results in the sharing of four electrons.

In 1913, while working as the chair of the department of chemistry at the University of California, Berkeley, Lewis read a preliminary outline of paper by an English graduate student, Alfred Lauck Parson, who was visiting Berkeley for a year. In this paper, Parson suggested that the electron is not merely an electric charge but is also a small magnet (or "magneton" as he called it) and furthermore that a chemical bond results from two electrons being shared between two atoms. This, according to Lewis, meant that bonding occurred when two electrons formed a shared edge between two complete cubes.

On these views, in his famous 1916 article The Atom and the Molecule, Lewis introduced the “Lewis structure” to represent atoms and molecules, where dots represent electrons and lines represent covalent bonds. In this article, he developed the concept of the electron-pair bond, in which two atoms may share one to six electrons, thus forming the single electron bond, a single bond, a double bond, or a triple bond.

路易斯认为的化学键

路易斯认为：一个电子可能会属于两个不同原子，且不能说这个电子是任何一个原子独占的。

Moreover, he proposed that an atom tended to form an ion by gaining or losing the number of electrons needed to complete a cube. Thus, Lewis structures show each atom in the structure of the molecule using its chemical symbol. Lines are drawn between atoms that are bonded to one another; occasionally, pairs of dots are used instead of lines. Excess electrons that form lone pairs are represented as pair of dots, and are placed next to the atoms on which they reside:

亚硝酸根离子的路易斯结构式

To summarize his views on his new bonding model, Lewis states:

Two atoms may conform to the rule of eight, or the octet rule, not only by the transfer of electrons from one atom to another, but also by sharing one or more pairs of electrons...Two electrons thus coupled together, when lying between two atomic centers, and held jointly in the shells of the two atoms, I have considered to be the chemical bond. We thus have a concrete picture of that physical entity, that "hook and eye" which is part of the creed of the organic chemist.

The following year, in 1917, an unknown American undergraduate chemical engineer named Linus Pauling was learning the Dalton hook-and-eye bonding method at the Oregon Agricultural College, which was the vogue description of bonds between atoms at the time. Each atom had a certain number of hooks that allowed it to attach to other atoms, and a certain number of eyes that allowed other atoms to attach to it. A chemical bond resulted when a hook and eye connected. Pauling, however, wasn't satisfied with this archaic method and looked to the newly-emerging field of quantum physics for a new method.

In 1927, the physicists Fritz London and Walter Heitler applied the new quantum mechanics to the deal with the saturable, nondynamic forces of attraction and repulsion, i.e., exchange forces, of the hydrogen molecule. Their valence bond treatment of this problem, in their joint paper, was a landmark in that it brought chemistry under quantum mechanics. Their work was an influence on Pauling, who had just received his doctorate and visited Heitler and London in Zürich on a Guggenheim Fellowship.

Subsequently, in 1931, building on the work of Heitler and London and on theories found in Lewis' famous article, Pauling published his ground-breaking article "The Nature of the Chemical Bond" (see: manuscript) in which he used quantum mechanics to calculate properties and structures of molecules, such as angles between bonds and rotation about bonds. On these concepts, Pauling developed hybridization theory to account for bonds in molecules such as CH₄, in which four sp³ hybridised orbitals are overlapped by hydrogen's 1s orbital, yielding four sigma (σ) bonds. The four bonds are of the same length and strength, which yields a molecular structure as shown below:

甲烷中碳原子的杂化轨道和氢原子的轨道重叠的示意图

莱纳斯·鲍林

由于提出这些理论，鲍林荣获1954年诺贝尔化学奖。值得一提的是，他是唯一一个赢得两个非共享诺贝尔奖的人，他还在1962年因反对核武器的使用赢得诺贝尔和平奖。

1926年，法国物理学家让·佩兰因最终证明分子的存在而获得诺贝尔物理学奖。他通过用包括液相的三种方法计算了阿伏伽德罗常数。第一他使用了一个藤黄肥皂样乳液计算，然后通过做布朗运动的实验计算，最后通过确认爱因斯坦提出的在液相中的粒子旋转计算。

1937年，化学家K.L. 沃尔夫引进了超分子的概念以描述通过氢键形成的乙酸二聚体。这个概念最后形成了研究由非共价键聚合分子的超分子化学学科。

1951年，物理学家欧文威廉·米勒发明了场离子显微镜并用它第一次看到原子。

在1999年，维也纳大学的研究人员报告了对C₆₀分子的波粒二象性研究的实验结果。塞林格等发布的数据与C₆₀分子的德布罗意波干扰是一致的。这个实验大大提高了波粒二象性在宏观上的适用范围。

21世纪

在2009年，IBM的研究人员拍摄了分子的第一张真实照片。 通过原子力显微镜，并五苯的每个原子和化学键都能被看到。

File:IBM Zurich Press Release AFM Image Penacene Aug 2009.jpg

原子力显微镜下并五苯的图象

参见

• 化学史
• 量子力学史
• 热力学史
• 分子生物学史
• 分子动理论
• 原子理论

扩展阅读

• Partington, J.R. A Short History of Chemistry. Dover Publications, Inc. 1989. ISBN 0-486-65977-1. （英文）
• Atkins, Peter. Atkins' Molecules, 2nd Ed. Cambridge University Press. 2003. ISBN 0-521-53536-0. （英文）
• Sargent, Ted. The Dance of Molecules - How Nanotechnology is Changing our Lives. Thunder's Mouth Press. 2006. ISBN 1-56025-809-8. （英文）

外部链接

• 分子的几何结构（英文） - 米德尔伯里学院
• 原子和分子（英文） - 麦克马斯特大学
• 3D分子模型查看（英文） - The Wileys Family
• 本月分子（英文） - 英国布里斯托尔大学化学学院
• {{http://www.chem.pku.edu.cn/wuji/jiaoan/liuzhongfan/9.pdf 分子理论]（简体中文） - 北京大学化学与分子工程学院

分子种类

• 有害分子（英文） - 国家健康博物馆（美国）
• 15种分子种类（英文） - 由IUPAC（国际纯化学与应用化学联合会）提出的分子分类

分子定义

• 分子的定义（英文） - 弗罗斯特堡州立大学（化学系）
• 分子的定义（英文） - IUPAC提出的定义

文章

• Molecules Used to Make Nano-sized Containers（英文） - Technology Research News (TRN) 通讯社
• Molecular Computer Processors（英文） - 惠普实验室