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  • 博赫尔原子模型

    Rutherford'S Gold Foil Experiment Setup, Including Alpha Particle Source And Detector.

    The gold foil experiment was conducted under the supervision of Ernest Rutherford at the University of Manchester in 1909 by Hans Geiger and Ernest Marsden. The popular theory of atomic structure at the time of Rutherford’s experiment was the “plum pudding model.” This theory held that the negatively charged electrons in an atom were floating in a sea of positive charge (the electrons playing the role of plums in a bowl of plum pudding). Rutherford’s gold foil experiment demonstrated that almost all of the mass of an atom is in a tiny volume in the center of the atom which Rutherford called the nucleus . This positively charged mass was responsible for deflecting alpha particles propelled through the gold foil. Rutherford’s “nuclear model” of the atom replaced the plum pudding model in 1911.
    ::1909年,在曼彻斯特大学欧内斯特·卢瑟福(Ernest Rutherford)的监督下,汉斯·盖格和欧内斯特·马尔斯登(Ernest Rutherford)在曼彻斯特大学进行了金发实验。 卢瑟福实验时流行的原子结构理论是“布丁模型 ” 。 这一理论认为原子内负电电流漂浮在正充电的海洋中(在梅子布丁碗里发挥梅子作用的电子 ) 。 鲁瑟福的金粉实验表明,几乎所有原子的重量都在卢瑟福(Rutherford)称之为核的原子中心一个微小的体积中。 这一正电量的原子是导致通过金块驱动的α粒子转移的。 卢瑟福(Lutherford)的“核模型”取代了1911年的梅布丁模型。

    The Bohr Model of the Atom
    ::原子的布尔模型

    Early History of the Atom
    ::原子早期历史

    Hypotheses concerning the existence of atoms as indivisible particles were known as early as the ancient Greek philosophers Democritus and Epicurus. The concepts of atoms that prevailed in the 17 th and 18 th centuries were poorly defined. Some scientists supposed that atoms could combine into more complex particles but specific chemical and physical properties were not attributed to atoms. In the period 1780-1803, Lavoisier made careful quantitative measurements which allowed the compositions of compounds to be determined accurately, Proust established the Law of Definite Proportions (each compound always contained the same proportions of elements), and John Dalton had developed the Law of Simple Proportions (compounds composed of the same elements contained simple multiples of component elements). These laws provided a solid foundation for a more thorough atomic theory.
    ::早在古希腊哲学家民主党和埃皮古鲁斯时代就已经知道关于原子存在是不可分割粒子的假设,17世纪和18世纪盛行的原子概念定义不清,有些科学家认为原子可以结合成更复杂的粒子,但具体的化学和物理特性并不归结于原子。在1780年至1803年期间,Lavoisier进行了谨慎的定量测量,使化合物的构成得以准确确定,Prust制定了《确定定界比例法》(每个化合物总是包含相同比例的要素),John Dalton制定了《简单比例法》(由相同元素组成的复合体包含简单的元素的多重元素 ) 这些法律为更彻底的原子理论提供了坚实的基础。

    Dalton’s Atomic Theory
    ::道尔顿的原子理论

    John Dalton developed his atomic theory in 1803. Dalton’s theory was different from previous discussions of atoms because it had the of careful chemical measurements behind it. Dalton’s theory went beyond just a philosophical statement that there are atoms. Dalton’s theory proposed a number of basic ideas: 1) All matter is composed of indivisible, tiny particles called atoms, 2) atoms can neither be created nor destroyed, 3) all atoms of the same element are identical (have the same mass), 4) elements differ from one another because they have different types of atoms (different mass), 5) compounds are composed of combinations of different elements because the atoms of different elements are bonded to one another, and 6) chemical reactions occur when atoms in compounds are rearranged.
    ::约翰·道尔顿在1803年发展了他的原子理论。 道尔顿的理论与先前对原子的讨论不同,因为它背后有谨慎的化学测量方法。 道尔顿的理论超出了关于原子存在的哲学理论的范畴。 道尔顿的理论提出了一些基本想法sad1) 所有物质都由不可分割的微粒组成,这些微粒被称为原子,(2)原子不能创造或摧毁,(3) 同一元素的所有原子都是一样的(质量相同 ) ,(4) 元素不同,因为它们有不同种类的原子(质量不同 ) , (5) 化合物由不同元素的组合组成,因为不同元素的原子相互捆绑,(6) 当原子在化合物中重新组合时,化学反应会发生。

    Dalton’s theory did not convince everyone immediately. It did convince a number of chemists right away but several decades were required for all opposition to cease. Dalton’s theory underwent a number of modifications in the next 150 years but many of its ideas are still part of the modern atomic theory. In 1869, Dmitri Mendeleev ascertained that there were groups of elements which had the same (or very similar) chemical properties, the same valence, and similar physical properties and showed that the chemical and physical properties of the elements were periodically repeated. His periodic table remains a major idea in chemistry today.
    ::道尔顿的理论并没有立即说服所有人。 它确实立刻说服了许多化学家,但所有反对者都必须停止几十年才能停止。 道尔顿的理论在未来150年中经历了许多修改,但其中的许多想法仍然是现代原子理论的一部分。 1869年,德米特里·门捷列夫确定,有些元素的化学特性相同(或非常相似 ) , 价值相同,物理特性相似,并表明元素的化学和物理特性定期重复。 他的定期表今天仍然是化学学方面的一个主要想法。

    Discovery of Electrons and Radioactivity
    ::发现电子和放射性

    During the investigation of the flow of electric current through gases, scientists discovered rays that were emitted from a cathode discharge tube and had the property of being deflected in electric and magnetic fields. It was determined that these rays consisted of rapidly moving, negatively charged particles called electrons. It was also determined that upon heating or illumination by light, metals emitted electrons. Logically, neutral atoms containing electrons must also contain positively charged particles. Thus, the indivisibility of the atom was disproved. This was further emphasized by Marie Curie’s discoveries that through alpha and beta decay, atoms of one element could transmute into other elements. Curie’s discoveries also determined that atoms of the same element may have different masses (isotopes) and thus the idea that all the atoms of the same element are identical was also lost.
    ::在对气流电流流动进行调查的过程中,科学家们发现了从阴极排放管中排放的射线,这些射线在电磁场中具有被偏转的特性,确定这些射线包括迅速移动的负电荷粒子,这些微粒被称为电子,还确定在光线加热或发光时,金属排放电子,逻辑上,含有电子的中性原子也必须包含有正电荷粒子。因此,原子的不可分割性被推翻了。Marie Curie发现,一个元素的原子通过阿尔法和贝塔衰变可以转化成其他元素,进一步强调了这一点。Curie的发现还确定,同一元素的原子可能具有不同的质量(同位素),因此,同一元素的所有原子都是一样的想法也消失了。

    Rutherford’s Planetary Model of the Atom
    ::卢瑟福的原子行星模型

    Now that it was known that the atom had component parts, a new model was needed. In the model proposed by J. J. Thomson in 1903, the atom was represented as a positively charged sphere with the negatively charged electrons distributed around the exterior. This was the so-called “plum-pudding” model with the positive charge playing the role of the pudding and the electrons playing the role of the plums. The next big step in the development of the model of the atom occurred in 1911 with Rutherford’s gold foil experiment. In the Thomson model of the atom, the density of the atom was necessarily small. The mass of the atom divided by the volume of the atom and assuming an even distribution of mass resulted in a low density for the atom.
    ::现在人们知道原子有组成部分,需要一个新的模型。在1903年J.J.Thomson提出的模型中,原子代表着一个在外部分布的负电荷负电球的正电球。这就是所谓的“铺路机”模型,以正面电荷发挥布丁的作用,而电子则发挥梅子的作用。原子模型开发的下一个重大步骤发生在1911年,鲁瑟福德的金金发实验。在原子的汤姆森模型中,原子的密度必然很小。原子的质量除以原子的体积,假设质量的均衡分布导致原子的低密度。

    In 1896, Henri Becquerel discovered that uranium compounds emitted penetrating rays, some of which were massive, high , positively charged particles which were later named alpha particles (α). These alpha particles would be detected by a zinc sulfide coated screen (scintillation counter) that emitted a small flash of light every time an alpha particle hit it. Rutherford used these alpha particles and the zinc sulfide coated screen in his gold foil experiment. The alpha particles were fired at a very thin sheet of gold foil. It was thought that all of the alpha particles would pass straight through the gold foil with no deflection. This was because the alpha particles were known to be very dense and, due to the “plum pudding” model of the atom where the mass of the atom was spread out evenly over the volume of the atom, the atoms of gold were thought to have very low density.
    ::1896年,Henri Becquerel发现,铀化合物释放了穿透性射线,其中有些是巨大的、高的、有正电的粒子,后来称为α粒子(α)。这些α粒子将通过一个硫化锌涂层屏幕(闪烁反射器)检测出来,每当一个α粒子击中它时,就释放出一小束光亮。Lutherford在其金宝石实验中使用了这些α粒子和硫化锌涂层。这些α粒子是射向一块非常薄的金宝石。人们认为,所有α粒子将直接通过金封,没有偏移。这是因为,已知的α粒子非常稠密,而且由于原子的“颗粒布”模型,原子质量在原子的体积上均匀地分布,黄金原子被认为密度非常低。

    While the great majority of the alpha particles did pass straight through the foil with no deflection, to everyone’s surprise, some alpha particles were deflected. In fact, some alpha were bounced almost straight backward by the foil. Rutherford, using Coulomb’s law and Newton’s laws found that the results could be explained only if all the positive charge of the atom were concentrated in a tiny, central core, now called the nucleus . Rutherford’s model of the atom is therefore, called the nuclear model of the atom. All of the positive charge and essentially all of the mass of the atom are in its nucleus. The atom is 10,000 times as large as the nucleus and is mostly empty space. It was known that electrons are outside the nucleus but how the electrons were arranged in an atom was still a mystery.
    ::尽管绝大多数的阿尔法粒子没有偏转,而是直接穿过浮宫,令每个人都感到惊讶,但有些阿尔法粒子被偏转了。 事实上,有些阿尔法粒子几乎被浮宫直向后反弹。 卢瑟福(Lutherford)利用库伦姆(Coulomb)的法律和牛顿(Newton)的法律发现,只有原子的所有正电荷集中在一个微小的中心核心(现在称为核核 ) , 才能解释结果。 因此,卢瑟福的原子模型被称为原子的核模型。 所有的正电荷和原子质量都在其核核中。 原子的原子体积是其核的一万倍之大,而且大部分是空空的。 众所周知,电子在核外,但原子中是如何安排的,这仍然是个谜。

    Problems with the Planetary Model
    ::行星模型的问题

    The planetary model had two major problems immediately. According to classical mechanics, a charged particle being accelerated (speeding up, slowing down, or turning a corner) would always emit electromagnetic radiation . That means that an orbiting electron would constantly emit and thus move closer to the nucleus until eventually it would collapse into the nucleus. Clearly this doesn’t happen and thus it opposes the idea that electrons move like planets. The second problem was that atoms gain energy (in the form of or light) and re-emit the energy in an exact set of light frequencies. The magnitude of the energy involved in this light emission is too small to be involved with nuclear changes and therefore, the electron configuration must be responsible for the light emission by atoms. The planetary model offered no explanation for the light spectrum of atoms.
    ::行星模型立即出现了两大问题。 根据古典机械学,充电粒子加速(加速、减速或转角 ) 总是会释放电磁辐射。 这意味着轨道电子会不断发射,从而更接近核核,直到最终崩溃到核核中。 显然这不会发生,因此它反对电子像行星一样移动的想法。 第二个问题是原子获得能量(以光或光的形式)和以精确的光频率再浓缩能量。 光排放的能量规模太小,不能涉及核变化,因此电子配置必须负责原子的光排放。 行星模型没有解释原子的光谱。

    The Emission Spectrum Of Hydrogen Light Through A Prism, Revealing Specific Frequencies.

    A major clue to the electron arrangement in an atom came from studying the light emitted by atoms. When electricity is passed through gaseous atoms, the atoms emit a spectrum of light that is specific for that element. The hydrogen atom, for example, emits a pinkish light but when that light is passed through a prism, we see a very few frequencies of light that are quite specific for hydrogen. The energies of these light frequencies is much too small to be involved in the nucleus of atoms, therefore, any explanation of these would have to involve the electron arrangement in atoms.
    ::原子电子安排的主要线索来自研究原子释放的光。当电力通过气体原子时,原子会释放出与该元素具体相关的光谱。例如,氢原子释放出粉色光线,但当光线通过棱镜时,我们看到的光频非常少,对氢非常特殊。因此,这些光频的能量太小,无法进入原子核,因此,任何解释都必须涉及原子中的电子安排。

    The Bohr Model of the Atom
    ::原子的布尔模型

    Niels Bohr attempted to join the nuclear model of the atom with Einstein’s quantum theory of light and with his own idea of electron energy levels to explain the electron arrangement within the atom. Bohr started with the planetary model of electron arrangement but postulated that electrons in stable orbits would not radiate energy even though the electrons were being accelerated by traveling in circular paths. Bohr hypothesized that the electrons were organized into stepwise energy levels within the electron cloud and only radiated energy when the electrons moved from one energy level to another. Bohr’s hypothesis suggested that the energy of atomic electrons came in packages and only whole packages could be absorbed or emitted. This quantization of energy allowed electrons to only absorb or emit exact amounts of energy to move from one energy level to another.
    ::尼尔斯·伯赫尔试图将原子的核模型与爱因斯坦的量子光理论以及他自己的电子能源水平理念结合到原子的核模型中来解释原子内的电子安排。 伯尔从电子安排的行星模型开始,但假设稳定轨道上的电子不会辐射能源,即使电子通过环状路径加速。 伯尔假设电子在电子云中被组织成分级能量水平,只有在电子从一个能源水平移动到另一个能源水平时才有辐射能量。 伯尔的假设表明原子电子的能量是包装的,只有整个包件才能被吸收或排放。 这种能源的量化只能让电子吸收或将确切数量的能量从一个能源水平转移到另一个能源水平。

    The quantization of energy is not apparent in everyday experience. If we could observe molecular sized automobiles traveling down miniature roads, we would see cars traveling at 7 miles per hour, or 14 miles per hour, or 21 miles per hour, but never at 9 or 17 miles per hour. The quantization of energy means that energy comes in packages and when energy is added to an object, whole packets of energy must be added. This is the explanation for why atomic electrons are only allowed to have certain amounts of energy and therefore, occupy certain energy levels. The lowest energy level for an electron is near the nucleus and each quanta of energy added moves the electron to the next distant energy level. Einstein’s theory says that each light photon has an energy of @$\begin{align*}hf\end{align*}@$ , where  @$\begin{align*}h\end{align*}@$ is Planck’s constant, and @$\begin{align*}f\end{align*}@$ is the frequency. The emission of a photon of light from an atom indicates a change in energy level for an electron such that
    ::能源的定量化在日常经验中并不明显。 如果我们可以看到分子规模的汽车在迷你公路下行, 我们可以看到汽车每小时行驶7英里, 或每小时14英里, 或每小时21英里, 但从来不是每小时9或17英里。 能源的量化化意味着能源是用包装的, 当能量被添加到一个物体时, 必须加上整包能源。 这就是为什么原子电子只允许拥有一定数量的能量, 因此占据一定的能量水平。 电子的最低能量水平接近核心, 并且每增加的能量的量将电子移动到下一个遥远的能源水平。 爱因斯坦的理论指出, 每张光的能量为 @ $\ begin{ align\\\\\\\\ end\ $, 在那里, @ $\ begin { h\ end{ { leign} $ 是Planck 的常数, 和 @ $\ begin{ align\\\\\\\\\\\\ reign{ lex n$ 频率是频率。 。 从电子的光的输出显示这种能量水平的变化。

    @$\begin{align*}hf = E_{higher} - E_{lower}\end{align*}@$ .
    ::@ $\ begin{ align} hf = Ehigher} - Elower{end{ align}$。

    The energy of an orbit is related to the inverse of the square of the orbit number. The energy of an electron in a given energy level of hydrogen is calculated by
    ::轨道的能量与轨道号正方的反方的能量有关。

    @$\begin{align*}E_n=(-2.17\times 10^{-18} \ J)\left(\frac{1}{n^2}\right)\end{align*}@$ .
    ::@ $\ begin{ align} E_ n= (-2.17\times 10\\\\ 18}\ J)\ left (\ frac{ 1\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\

    The radius of an orbit is related to the square of the orbit number.
    ::轨道的半径与轨道号的方形有关。

    Bohr calculated allowed electron energy levels for the hydrogen atom and found the emission spectrum of hydrogen to match perfectly with particular electron transitions between his suggested energy levels. Other electron transitions predicted electromagnetic frequencies outside the visible range and when those were looked for, they were present and also matched precisely with theoretical calculations.
    ::博赫尔计算出氢原子的电子能量水平,发现氢的排放频谱与其建议的能量水平之间的特定电子转换完全吻合。其他电子转换预测了可见范围以外的电磁频率,当寻找这些频率时,它们就存在并且与理论计算完全吻合。

    Examples
    ::实例

    Example  1
    ::例1

    For the hydrogen atom, determine
    ::氢原子,确定

    1. the energy of the innermost energy level @$\begin{align*}(n=1)\end{align*}@$ .
      ::最核心能量水平的能量@$\ begin{ aliign} (n=1)\ end{ aliign}$。
    2. the energy of the second energy level.
      ::第二能量水平的能量。
    3. the difference between the first and second energy levels.
      ::一级和二级能源水平的差别。

     

    1. @$\begin{align*}E_n=(-2.17\times 10^{-18} \ J)\left(\frac{1}{n^2}\right) \qquad E_1=(-2.17\times 10^{-18} \ J)\left(\frac{1}{1^2}\right)=-2.17 \times 10^{-18} \ J\end{align*}@$
      ::@ $\ begin{ align} E_ n= (-2.17\times 10\ 18}\ J)\ left (\ frac{ 1\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\
    2. @$\begin{align*}E_n=(-2.17\times 10^{-18} \ J)\left(\frac{1}{n^2}\right) \qquad E_2=(-2.17\times 10^{-18} \ J)\left(\frac{1}{2^2}\right)=-5.43 \times 10^{-19} \ J\end{align*}@$
      ::@ $\ begin{ align} E_ n= (-2.17\times 10\ 18}\ J)\ left (\ frac{ 1\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\
    3. @$\begin{align*}E_{2-1}=(-5.43 \times 10^{-19} \ J)-(-2.17 \times 10^{-18} \ J)=1.63 \times 10^{-18} \ J\end{align*}@$
      ::@ $\ begin{ align} E2-1 (-5.43\ times 10\\ - 19} \ J- 2- 2- 17\ times 10\\ - 18}\ J)= 1. 63\ times 10\ - 18} \ J\ end{ align $

    This is the amount of energy that would need to be added to a 1 st energy level electron to raise it to the second energy level.
    ::这是需要添加到第一级能源水平电子中的能量量, 才能将其提高到第二级能源水平。

    Example 2  
    ::例2

    According to the Bohr model, how many times larger is the second level hydrogen orbit compared to the first level hydrogen orbit?
    ::根据Bohr模型,与第一级氢轨道相比,第二级氢轨道比第二级氢轨道大多少倍?

    4 times
    ::4 次 4 次

    Launch the PLIX Interactive below to observe Bohr’s Atomic Model. You can excite the red electron and drag it to a higher orbital to model what would happen if the electron gained energy. Then, use the table to determine the wavelength of radiation emitted when the electron releases this energy and returns to its lowest orbital:
    ::启动下面的 PLIX 交互式互动以观察 Bohr 的原子模型。 您可以刺激红色电子, 将其拖到更高的轨道上, 模拟如果电子获得能量会发生什么。 然后, 使用这个表格来确定当电子释放出这种能量并返回到最低轨道时所释放的辐射波长 :

    Summary
    ::摘要

    • Rutherford, using Coulomb’s law and Newton’s laws, found that the results of his 'gold foil experiment' could be explained only if all the positive charge of the atom were concentrated in a tiny, central core, now called the nucleus.
      ::卢瑟福利用库伦姆的法律和牛顿的法律发现,他的“古老的化石实验”的结果只有在原子的所有正电荷集中在一个小的核心核心,现在被称为核心时才能解释。
    • The atom is 10,000 times as large as the nucleus and is mostly empty space.
      ::原子的体积是核体的一万倍,而且大部分是空的。
    • The energies of light frequencies in the emission spectrum of atoms is much too small to be involved in the nucleus of atoms, therefore, any explanation of these wavelengths would have to involve the electron arrangement.
      ::原子排放频谱中的光频率能量太小,无法进入原子核,因此,对这些波长的任何解释都必须涉及电子安排。
    • Bohr hypothesized that the electrons were organized into stepwise energy levels within the electron cloud in a planetary model and only radiated energy when the electrons were changing from one energy level to another.
      ::Bohr假设这些电子在行星模型电子云中被组织成分级能量水平,只有当电子从一个能量水平向另一个能量水平变化时,才有辐射能量。
    • Bohr suggested that the energy levels were quantized, that is, the energy held by the atomic electrons came in packages and only whole packages could be absorbed or emitted.
      ::Bohr建议对能量水平进行量化,即原子电子所持有的能量是包装的,只有整包能吸收或排放。
    • Einstein’s theory says that each light photon has an energy of @$\begin{align*}hf\end{align*}@$ , where  @$\begin{align*}h\end{align*}@$ is Planck’s constant, and  @$\begin{align*}f\end{align*}@$ is the frequency. The emission of a photon of light from an atom indicates a change in energy level for an electron such that @$\begin{align*}hf = E_{higher} - E_{lower}\end{align*}@$ .
      ::爱因斯坦的理论指出,每个光光子的能量为 @$\ begin{ align}hf\end{align}$, 其中@$\ begin{align}h\end{align}$是Planck的常数, 而@$\ begin{align}}\ align}f\end{align}$是频率。原子光子的释放表明电子的能量水平有变化,以至于@$\ begin{align}hf = Eghiter} - Elower{end{align} =$。
    • The energy of an electron in a given energy level of hydrogen is calculated by
      ::氢的某一能量水平中电子的能量是按下述方法计算的:

    @$\begin{align*}E_n=(-2.17\times 10^{-18} \ J)\left(\frac{1}{n^2}\right)\end{align*}@$ .
    ::@ $\ begin{ align} E_ n= (-2.17\times 10\\\\ 18}\ J)\ left (\ frac{ 1\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\\

    Review
    ::回顾

    1. Why did Rutherford suggest that the positive charge in an atomic nucleus is concentrated in a tiny region rather than spread evenly throughout the atom?
      ::为什么卢瑟福说原子核的正面电荷集中在一个小地区,而不是平均扩散到整个原子?
    2. The absorption spectrum of an element has the same frequencies as the emission spectrum. How does Bohr’s theory explain this?
      ::元素的吸收频谱与排放频谱的频率相同。 Bohr的理论如何解释这一点?
    3. Why do scientists say the planetary model can’t be correct because the electrons would collapse into the nucleus?
      ::为什么科学家说行星模型不能正确, 因为电子会掉入核?
    4. If you were trying to explain the idea of quantization to younger students, do you think you should use water or money as an example? Why?
      ::如果你试图向年轻学生解释量化的概念,你认为你应该用水或钱作为例子吗?为什么?

    Explore More
    ::探索更多

    Use this resource to answer the questions that follow.
    ::使用此资源回答下面的问题 。

     

    1. Why does the Rutherford planetary model predict that the electron would collapse into the nucleus?
      ::为什么卢瑟福行星模型预测 电子会掉入核?
    2. Bohr used Planck’s suggestion that energy emitted by matter was not emitted in continuous quantities but in _________ bundles.
      ::Bohr使用Planck的建议,即物质排放的能源不是连续排放的,而是在捆包中排放的。
    3. Bohr’s calculations were based on the atoms of which element?
      ::Bohr的计算是基于哪个元素的原子?