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统编高一化学教材中讨论了电子在原子核外的排布规律即电子填入原子轨道的先后次序是在不违背保里不相容原理的前提下,遵循能量最低原理,按原子轨道的能量高低:1s、2s、2p、3s、3p、4s、3d、4p、5s、4d…依次填入的。这里,能量为什么有这样的次序?3d能量为什么会高于4s?如果3d能量高于4s,那么又为什么当铁原子变成正离子时,先失去的是4s电子?本文想就电子云钻穿效应来讨论这些问题。
In the textbook of the high school chemistry, we discussed the arrangement of electrons outside the atomic nucleus, that is, the order in which the electrons fill in atomic orbitals is to follow the energy minimum principle and the energy in the atomic orbit without violating the incompatible principle of Pauli. Levels: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d... sequentially. Here, why does energy have this order? Why does 3d energy be higher than 4s? If 3d energy is higher than 4s, then why would the first 4s electrons be lost when the iron atoms become positive ions? Effects to discuss these issues.