aufbau principle

简明释义

构造原理

英英释义

例句

1.Understanding the aufbau principle is essential for predicting the behavior of elements.

理解 Aufbau 原则 对于预测元素的行为是至关重要的。

2.In chemistry class, we learned about the aufbau principle and how it applies to electron configuration.

在化学课上，我们学习了 Aufbau 原则 以及它如何应用于电子排布。

3.The aufbau principle states that electrons fill the lowest energy orbitals first.

Aufbau 原则 指的是电子首先填充最低能量的轨道。

4.According to the aufbau principle, the electron configuration of oxygen is 1s² 2s² 2p⁴.

根据 Aufbau 原则，氧的电子排布为 1s² 2s² 2p⁴。

5.The aufbau principle helps explain why certain elements are more stable than others.

Aufbau 原则 有助于解释为什么某些元素比其他元素更稳定。

作文

The aufbau principle is a fundamental concept in quantum chemistry and atomic physics that describes how electrons are arranged in an atom. According to this principle, electrons occupy the lowest energy orbitals available before filling higher energy levels. This idea is crucial for understanding the electronic structure of atoms, which in turn influences their chemical behavior and reactivity. The term 'aufbau' comes from the German word meaning 'building up', which is a fitting description of how electrons fill atomic orbitals in a systematic manner.To illustrate the aufbau principle, consider the simplest atom, hydrogen, which has one electron. This electron occupies the 1s orbital, the lowest energy state available. As we move to helium, the second element, it has two electrons that also fill the 1s orbital. When we reach lithium, the third element, it has three electrons. The first two electrons fill the 1s orbital, while the third electron begins to fill the next available orbital, the 2s orbital.As we continue to add more electrons and move through the periodic table, we see that the aufbau principle governs the order in which these electrons fill the various orbitals: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on. This order is often represented by the Aufbau diagram or the Madelung rule, which helps predict the electron configuration of elements based on their atomic number.Understanding the aufbau principle is essential not only for predicting the arrangement of electrons but also for explaining the properties of different elements. For instance, the valence electrons, which are the outermost electrons, determine how an atom interacts with others to form chemical bonds. Elements with similar electron configurations often exhibit similar chemical properties, a concept that is foundational to the study of chemistry.Moreover, the aufbau principle has implications beyond simple electron configurations. It also plays a role in understanding phenomena such as ionization energy, electronegativity, and the formation of ions. For example, elements that have nearly full or nearly empty outer shells tend to be more reactive than those with a stable configuration. This insight is invaluable when predicting how different elements will behave in chemical reactions.In summary, the aufbau principle is a cornerstone of atomic theory that describes how electrons are arranged within an atom. By following this principle, scientists can predict the electronic structure of elements and understand their chemical properties. This principle not only enhances our comprehension of individual atoms but also provides a framework for exploring the interactions between different elements in the vast field of chemistry. The aufbau principle serves as a reminder of the intricate order that underlies the seemingly chaotic nature of the chemical world, allowing us to make sense of the relationships between different substances and their behaviors.

“aufbau原则”是量子化学和原子物理学中的一个基本概念，它描述了电子在原子中的排列方式。根据这一原则，电子先占据可用的最低能量轨道，然后再填充更高能级的轨道。这个观点对于理解原子的电子结构至关重要，而电子结构又影响着原子的化学行为和反应性。“aufbau”一词源自德语，意为“建立”，这恰如其分地描述了电子如何以系统的方式填充原子轨道。为了说明“aufbau原则”，我们可以考虑最简单的原子——氢，它只有一个电子。这个电子占据1s轨道，这是可用的最低能量状态。当我们移动到氦，第二个元素时，它有两个电子，也填充1s轨道。到锂，第三个元素时，它有三个电子。前两个电子填充1s轨道，而第三个电子开始填充下一个可用的轨道，即2s轨道。随着我们继续增加电子并穿过周期表，我们看到“aufbau原则”支配着这些电子填充各种轨道的顺序：1s、2s、2p、3s、3p、4s、3d、4p，等等。这一顺序通常用Aufbau图或Madelung规则表示，帮助预测元素的电子配置，基于它们的原子序数。理解“aufbau原则”不仅对预测电子排列至关重要，还对解释不同元素的性质也很重要。例如，价电子，即最外层的电子，决定了原子如何与其他原子相互作用形成化学键。具有相似电子配置的元素往往表现出相似的化学性质，这一概念是化学研究的基础。此外，“aufbau原则”还超越了简单的电子配置，涉及到理解电离能、电负性和离子的形成等现象。例如，外壳几乎满或几乎空的元素往往比那些具有稳定配置的元素更具反应性。这一见解在预测不同元素在化学反应中的行为时是非常宝贵的。总之，“aufbau原则”是原子理论的基石，描述了电子在原子内的排列方式。通过遵循这一原则，科学家可以预测元素的电子结构，并理解它们的化学性质。这个原则不仅增强了我们对单个原子的理解，还为探索不同元素之间的相互作用提供了框架，在广阔的化学领域中至关重要。“aufbau原则”提醒我们，尽管化学世界看似混乱，但其背后却有着复杂的秩序，使我们能够理解不同物质之间的关系及其行为。