aufbau principle

简明释义

构造原理

英英释义

例句

1.Understanding the aufbau principle Aufbau原理 helps students grasp the concept of electron configurations more easily.

理解aufbau principle Aufbau原理可以帮助学生更容易掌握电子排布的概念。

2.The aufbau principle Aufbau原理 is essential for predicting the electron configuration of elements in the periodic table.

理解aufbau principle Aufbau原理 对于预测元素在周期表中的电子排布至关重要。

3.In chemistry class, we learned about the aufbau principle Aufbau原理 to explain how electrons fill atomic orbitals.

在化学课上，我们学习了aufbau principle Aufbau原理，以解释电子如何填充原子轨道。

4.When studying the aufbau principle Aufbau原理, remember that lower energy orbitals fill before higher energy ones.

在学习aufbau principle Aufbau原理时，请记住低能量轨道会先于高能量轨道填充。

5.The teacher explained the aufbau principle Aufbau原理 using diagrams of atomic orbitals.

老师使用原子轨道的图示来解释aufbau principle Aufbau原理。

作文

The aufbau principle is a fundamental concept in chemistry that describes how electrons are arranged in atoms. According to this principle, electrons fill atomic orbitals in order of increasing energy levels. This means that the lowest energy orbitals are filled first before moving on to higher energy levels. Understanding the aufbau principle is essential for predicting the electronic configuration of elements, which in turn influences their chemical properties and reactivity.To illustrate the aufbau principle, consider the case of hydrogen, the simplest element. Hydrogen has one electron, which occupies the 1s orbital, the lowest energy level. As we move to helium, which has two electrons, both electrons also occupy the 1s orbital. It is only when we reach lithium, with three electrons, that we start filling the next available orbital, which is the 2s orbital. This pattern continues for all elements in the periodic table.The aufbau principle is often summarized by the acronym 'Aufbau,' which means 'building up' in German. This building-up process reflects how electrons are added one at a time to the atomic orbitals as we move across the periodic table. The sequence in which these orbitals are filled is determined by their energy levels, which can be understood through the use of the diagonal rule. This rule helps predict the order in which orbitals are filled based on their increasing energy levels.In addition to the aufbau principle, there are other important principles that govern electron configuration, including the Pauli Exclusion Principle and Hund's Rule. The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of quantum numbers, meaning that an orbital can hold a maximum of two electrons with opposite spins. Hund's Rule, on the other hand, states that electrons will occupy degenerate orbitals singly before pairing up. Together, these principles help chemists understand and predict the behavior of atoms and molecules.The implications of the aufbau principle extend beyond simple electron configuration. For instance, the arrangement of electrons determines how an element will interact with others in chemical reactions. Elements with similar electron configurations tend to exhibit similar chemical behaviors. This is why groups of elements in the periodic table, such as the alkali metals or noble gases, display similar properties; they have similar valence electron arrangements due to the aufbau principle.In practical applications, the aufbau principle is crucial in fields such as material science, pharmacology, and nanotechnology. By understanding how electrons are arranged in various materials, scientists can design new compounds with specific properties. For example, knowing the electronic structure of a semiconductor can lead to innovations in electronics and solar energy technologies.In conclusion, the aufbau principle is a key concept in understanding atomic structure and electron configuration. It not only provides insight into the arrangement of electrons within an atom but also helps explain the chemical behavior of elements. Mastery of the aufbau principle and its associated rules is essential for anyone studying chemistry, as it lays the groundwork for more advanced topics in the field. As we continue to explore the complexities of atomic interactions, the aufbau principle remains a cornerstone of our understanding of matter at the most fundamental level.

“aufbau原则”是化学中的一个基本概念，描述了电子在原子中的排列方式。根据这一原则，电子按照能量级的递增顺序填充原子轨道。这意味着最低能量的轨道首先被填充，然后才会移动到更高的能量级。理解“aufbau原则”对于预测元素的电子配置至关重要，而这又影响着它们的化学性质和反应性。为了说明“aufbau原则”，考虑氢的例子，这是最简单的元素。氢有一个电子，它占据1s轨道，即最低的能量级。当我们进入氦时，氦有两个电子，这两个电子也占据1s轨道。只有当我们达到锂时，锂有三个电子，我们才开始填充下一个可用的轨道，即2s轨道。这一模式在周期表中的所有元素中持续进行。“aufbau原则”通常用德语单词“Aufbau”来总结，意思是“构建”。这种构建过程反映了当我们在周期表中逐个添加电子时，电子是如何被逐步填充的。这些轨道被填充的顺序取决于它们的能量级，可以通过使用对角线规则来理解。这个规则帮助预测轨道的填充顺序，基于其递增的能量级。除了“aufbau原则”之外，还有其他重要的原则支配电子配置，包括泡利不相容原理和洪德规则。泡利不相容原理规定，原子中的两个电子不能具有相同的量子数，这意味着一个轨道最多可以容纳两个自旋相反的电子。另一方面，洪德规则则规定，电子将在简并轨道中单独占据，随后再成对填充。这些原则共同帮助化学家理解和预测原子和分子的行为。“aufbau原则”的影响超越了简单的电子配置。例如，电子的排列决定了元素在化学反应中的相互作用方式。具有相似电子配置的元素往往表现出相似的化学行为。这就是为什么周期表中的元素组，例如碱金属或惰性气体，显示出类似的性质；由于“aufbau原则”，它们具有相似的价电子排列。在实际应用中，“aufbau原则”在材料科学、药理学和纳米技术等领域至关重要。通过理解各种材料中电子的排列，科学家可以设计出具有特定性质的新化合物。例如，了解半导体的电子结构可以推动电子和太阳能技术的创新。总之，“aufbau原则”是理解原子结构和电子配置的关键概念。它不仅提供了原子内电子排列的见解，还帮助解释元素的化学行为。掌握“aufbau原则”及其相关规则对于任何学习化学的人来说都是必不可少的，因为它为该领域的更高级主题奠定了基础。随着我们继续探索原子相互作用的复杂性，“aufbau原则”仍然是我们理解物质最基本层面的基石。