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在无机化学和结构化学的教学中,当讲授核外电子排布的问题时,常采用L.Pauling提出的原子轨道近似能级图(图1)。这个图简单明确,便于掌握,易于教学。它可以解释为什么19、20号两种元素的最外层电子是4s而不是3d;37、38号两元素的最外层电子为什么是5s而不是4d;55、56号两元素是6s而不是5d;为什么会出现镧系和锕系元素:为什么元素周期系会出现2、8、8、18、18、32、32的元素性质的周期性递变规律等等。但是这个图不能解释21号及其后的各元素为什么首先失去4s电子而不是
In the teaching of inorganic chemistry and structural chemistry, when teaching the problem of extranuclear electron arrangement, the atomic orbital approximate energy level diagram proposed by L. Pauling is often used (Fig. 1). This diagram is simple and clear, easy to grasp, and easy to teach. It can explain why the outermost electrons of the two elements 19 and 20 are 4s instead of 3d; the outermost electrons of the two elements 37 and 38 are 5s instead of 4d; the 55 and 56 two elements are 6s instead of 5d; Why are there lanthanides and lanthanides: why the periodicity of the elements in the elemental cycle will occur in the periodical law of the elemental nature of 2,8,8,18,18,32,32, and so on. However, this figure cannot explain why the 21st and subsequent elements first lose 4s electrons instead of