electron pair

简明释义

电子偶

英英释义

例句

1.When drawing Lewis structures, you must account for all electron pairs 电子对 around the central atom.

在绘制路易斯结构时，必须考虑中心原子周围的所有电子对 电子对。

2.In water molecules, the oxygen atom has two lone electron pairs 电子对 that affect its shape.

在水分子中，氧原子有两个孤立的电子对 电子对，这影响了其形状。

3.A lone electron pair 电子对 on a nitrogen atom can influence molecular geometry.

氮原子上的孤立电子对 电子对可以影响分子几何形状。

4.In a covalent bond, two atoms share an electron pair 电子对 to achieve stability.

在共价键中，两个原子共享一个电子对 电子对以达到稳定。

5.The formation of a double bond involves two electron pairs 电子对 between the same two atoms.

双键的形成涉及同两个原子之间的两个电子对 电子对。

作文

In the realm of chemistry, understanding the fundamental concepts that govern molecular interactions is crucial. One such concept is the idea of an electron pair, which plays a significant role in chemical bonding and molecular geometry. An electron pair refers to a pair of electrons that are either shared between two atoms in a covalent bond or are found in the outer shells of individual atoms. This pairing of electrons is essential for the formation of stable molecules and the overall behavior of substances.When two atoms approach each other, their outermost electron shells interact. If they are nonmetals, they may share electrons to achieve a full outer shell, which leads to the formation of a covalent bond. In this scenario, the shared electrons constitute an electron pair. For instance, in a water molecule (H₂O), the oxygen atom shares its electrons with two hydrogen atoms, resulting in two electron pairs that help stabilize the molecule.Furthermore, the concept of electron pairs extends beyond simple covalent bonding. In addition to bonding pairs of electrons, there are also lone pairs, which are pairs of electrons that are not involved in bonding. These lone pairs can influence the shape of a molecule significantly. For example, in ammonia (NH₃), the nitrogen atom has one lone pair and three bonding pairs. The presence of the lone pair pushes the hydrogen atoms closer together, resulting in a trigonal pyramidal shape rather than a flat tetrahedral shape that would occur if there were no lone pairs.The arrangement of electron pairs around a central atom is described by the Valence Shell Electron Pair Repulsion (VSEPR) theory. This theory posits that electron pairs, whether bonding or lone pairs, will arrange themselves as far apart as possible to minimize repulsion. By applying VSEPR theory, chemists can predict the geometry of molecules based on the number of electron pairs present. For instance, if there are four electron pairs around a central atom, the molecule will adopt a tetrahedral shape, whereas three electron pairs will lead to a trigonal planar arrangement.Understanding electron pairs is vital not only for predicting molecular shapes but also for grasping reactivity and properties of different substances. The way that electron pairs are arranged can affect how molecules interact with one another. For example, the polarity of a molecule is influenced by the distribution of electron pairs. Molecules with uneven distributions of electron pairs can create dipoles, leading to polar characteristics that affect solubility and boiling points.In conclusion, the concept of electron pairs is fundamental in the study of chemistry. From their role in bonding to their influence on molecular shape and properties, electron pairs are key players in the interactions that define chemical behavior. A thorough understanding of electron pairs allows chemists to predict and explain the characteristics of various compounds, making it an indispensable part of chemical education and research.

在化学领域，理解支配分子相互作用的基本概念至关重要。一个这样的概念是电子对的概念，它在化学键和分子几何中发挥着重要作用。电子对指的是一对电子，这对电子要么在共价键中被两个原子共享，要么位于单个原子的外壳中。这种电子的配对对于形成稳定的分子和物质的整体行为是必不可少的。当两个原子彼此靠近时，它们最外层的电子壳会相互作用。如果它们是非金属元素，它们可能会共享电子以实现完整的外壳，这导致了共价键的形成。在这种情况下，共享的电子构成了一个电子对。例如，在水分子（H₂O）中，氧原子与两个氢原子共享其电子，从而产生两个电子对，帮助稳定该分子。此外，电子对的概念不仅限于简单的共价键合。除了参与键合的电子对，还有孤对，即不参与键合的电子对。这些孤对可以显著影响分子的形状。例如，在氨分子（NH₃）中，氮原子有一个孤对和三个键合对。孤对的存在使氢原子更靠近，从而导致三角锥形状，而不是如果没有孤对则会出现的平面四面体形状。围绕中心原子的电子对的排列由价壳电子对排斥（VSEPR）理论描述。该理论认为，无论是键合对还是孤对，电子对都会尽可能远离，以最小化排斥力。通过应用VSEPR理论，化学家可以根据存在的电子对的数量预测分子的几何形状。例如，如果中心原子周围有四个电子对，则分子将采用四面体形状，而三个电子对将导致三角平面排列。理解电子对不仅对于预测分子形状至关重要，而且对于掌握不同物质的反应性和性质也至关重要。电子对的排列方式会影响分子之间的相互作用。例如，分子的极性受电子对分布的影响。不均匀分布的电子对可以产生偶极，导致极性特征，从而影响溶解度和沸点。总之，电子对的概念在化学研究中是基础。从它们在键合中的作用到它们对分子形状和性质的影响，电子对都是定义化学行为的相互作用中的关键角色。透彻理解电子对使化学家能够预测和解释各种化合物的特性，使其成为化学教育和研究中不可或缺的一部分。