aufbau principle

简明释义

电子充填原理;

英英释义

例句

1.In quantum mechanics, the aufbau principle (构建原则) helps determine the ground state electron configuration of an atom.

在量子力学中，aufbau principle（构建原则）有助于确定原子的基态电子排布。

2.To predict the chemical properties of elements, understanding the aufbau principle (构建原则) is essential.

为了预测元素的化学性质，理解aufbau principle（构建原则）是必不可少的。

3.When drawing Lewis structures, we apply the aufbau principle (构建原则) to ensure accurate electron placement.

在绘制路易斯结构时，我们应用aufbau principle（构建原则）以确保电子的准确放置。

4.The electron configuration of an atom follows the aufbau principle (构建原则), filling lower energy orbitals before higher ones.

原子的电子排布遵循aufbau principle（构建原则），先填充低能量轨道，再填充高能量轨道。

5.In chemistry classes, we often discuss the aufbau principle (构建原则) to explain how electrons are arranged in atoms.

在化学课上，我们常常讨论aufbau principle（构建原则）来解释电子在原子中的排列方式。

作文

The aufbau principle is a fundamental concept in quantum chemistry and atomic physics that describes the process of electron configuration in atoms. According to this principle, electrons fill atomic orbitals in a specific order, starting from the lowest energy levels and moving to higher ones. This systematic arrangement not only helps us understand the structure of atoms but also provides insights into the chemical properties of elements. To illustrate the aufbau principle, consider the example of the hydrogen atom. Hydrogen has one electron, which occupies the 1s orbital, the lowest energy level available. As we progress through the periodic table, we encounter helium, which has two electrons. These two electrons also fill the 1s orbital, adhering to the aufbau principle. As we continue to add more electrons, we move to lithium, which has three electrons. The first two electrons fill the 1s orbital, while the third electron occupies the next available energy level, the 2s orbital. This pattern continues with each subsequent element, where electrons fill the orbitals in accordance with the aufbau principle. For instance, carbon has six electrons: two in the 1s, two in the 2s, and two in the 2p orbitals. The significance of the aufbau principle extends beyond merely filling up orbitals; it lays the groundwork for understanding the periodic trends observed in elements. For example, the arrangement of electrons influences an element's reactivity, ionization energy, and electronegativity. Elements in the same group of the periodic table have similar electron configurations in their outer shells, leading to comparable chemical behaviors. Furthermore, the aufbau principle is essential when discussing molecular bonding and the formation of compounds. When atoms bond, they do so based on the availability of electrons in their outermost orbitals. Understanding how these orbitals are filled allows chemists to predict the types of bonds that will form between different elements. In addition to its applications in chemistry, the aufbau principle also serves as a cornerstone for advanced studies in fields like material science and nanotechnology. By manipulating the electron configurations of materials, scientists can design substances with specific properties for various applications, such as semiconductors and superconductors. In conclusion, the aufbau principle is a crucial concept that underpins our understanding of atomic structure and behavior. It elucidates how electrons occupy orbitals in a systematic manner, providing a framework for predicting the chemical properties of elements and their interactions. Whether in basic chemistry or advanced scientific research, the aufbau principle remains an indispensable tool for scientists and students alike, highlighting the intricate relationship between electron configuration and the behavior of matter.

“ Aufbau 原则”是量子化学和原子物理学中的一个基本概念，描述了原子中电子配置的过程。根据这一原则，电子以特定的顺序填充原子轨道，从最低能级开始，逐渐移动到更高的能级。这种系统的排列不仅有助于我们理解原子的结构，还提供了对元素化学性质的深入了解。 以氢原子为例来说明“ Aufbau 原则”。氢只有一个电子，它占据了1s轨道，这是可用的最低能级。随着我们在周期表中继续前进，我们会遇到氦，氦有两个电子。这两个电子也填满了1s轨道，遵循“ Aufbau 原则”。 当我们继续添加更多电子时，我们会进入锂，它有三个电子。前两个电子填充1s轨道，而第三个电子占据下一个可用的能级，即2s轨道。这个模式随着每个后续元素的增加而继续，其中电子根据“ Aufbau 原则”填充轨道。例如，碳有六个电子：两个在1s轨道上，两个在2s轨道上，两个在2p轨道上。 “ Aufbau 原则”的重要性不仅仅在于填充轨道；它为理解元素观察到的周期趋势奠定了基础。例如，电子的排列影响元素的反应性、离子化能和电负性。周期表中同一组的元素在其外层的电子配置相似，导致化学行为相似。 此外，“ Aufbau 原则”在讨论分子键合和化合物形成时也是必不可少的。当原子结合时，它们是基于外层轨道中电子的可用性进行结合的。理解这些轨道是如何填充的使化学家能够预测不同元素之间将形成的键的类型。 除了在化学中的应用外，“ Aufbau 原则”还作为材料科学和纳米技术等领域高级研究的基石。通过操纵材料的电子配置，科学家可以设计具有特定性质的物质，用于各种应用，如半导体和超导体。 总之，“ Aufbau 原则”是支撑我们理解原子结构和行为的关键概念。它阐明了电子如何以系统的方式占据轨道，为预测元素的化学性质及其相互作用提供了框架。无论是在基础化学还是高级科学研究中，“ Aufbau 原则”仍然是科学家和学生不可或缺的工具，突显了电子配置与物质行为之间的复杂关系。