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所在平台: Udemy |
课程主页: https://www.udemy.com/course/the-p-block-elements-part-ii/
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**课程名称：** p-区元素 part-II **课程概述：** 本课程深入探讨了元素周期表中第13至18族（p-区元素）的性质。这些元素的通式电子构型为ns²np¹⁻⁶，其中s轨道已满，p轨道则逐渐填充。p-区元素的性质与其p轨道的电子密切相关。 课程总结了p-区元素的一些关键特征，方便快速回顾： 1. **原子半径和离子半径：** * 原子半径在同一周期内从左到右递减。 * 原子半径在同一族内从上到下递增。 2. **电离焓：** * 电离焓在同一周期内从左到右递增。 * 电离焓在同一族内从上到下递减。 * 值得注意的是，第13族元素的电离焓通常小于第2族（碱土金属）元素。 3. **电子增益焓：** * 电子增益焓在同一周期内从左到右递增。 * 电子增益焓在同一族内从上到下递减。 4. **电负性：** * 电负性是指原子在分子中吸引共享电子对的能力。 * 电负性受原子大小和填满价电子层所需电子数量的影响。 * 总的来说，电负性在同一周期内从左到右递增。 * 电负性在同一族内从上到下递减。 * 两原子间的电负性差值可以用于判断它们之间形成的化学键类型。 **教学大纲：** 无
The p-block ElementsElements belonging to groups 13 to 18 of the periodic table are called p-block elements.Their general electronic configuration is ns 2 np 1 - 6. The s-orbitalsof these elements are complete whereas the p-orbitals are progressively filled. The properties of these elements are dependent upon the electrons present in p-orbitals.Some characteristics of p-block elements summarized for a quick reference:1.Atomic and Ionic Radii. The size of an atom is expressed in terms of atomic radius, van der Waal's radius or covalent radius. The atomic radii of p-block elements decrease on moving from left to right in a given period and increases from top to bottom in any group.2. Ionization Enthalpy. The ionization enthalpy of p-block elements increases from left to right in a period and decreases on descending a group. However, the ionization energy of group 13 elements is found to be smaller than the group 2 elements (Alkaline earths).3. Electron Gain Enthalpy. Electron gain enthalpy increases from left to right along a period amongst the p-block elements. It value decreases from top to bottom in a particular group.4. Electronegativity. It is the property of an atom in a molecule. It refers to the tendency of an atom to pull the shared pair of electrons towards itself. It depends upon(i)size of atom and(ii) electrons needed complete the valency shell.In general, the electronegativity increases from left to right along the period and decreases from top to bottom in a group. The difference of electronegativities between the two atoms gives us an idea about the kind of bond set up between two atoms.
