SAT化学真题：Electron Configurations-SAT - SAT资讯-出国外语考试-出国留学网

标题

SAT化学真题：Electron Configurations

内容

Now let’s discuss how to determine the electron configuration for an atom—in other words, how electrons are arranged in an atom. The first and most important rule to remember when attempting to determine how electrons will be arranged in the atom is Hund’s rule, which states that the most stable arrangement of electrons is that which allows the maximum number of unpaired electrons. This arrangement minimizes electron-electron repulsions. Here’s an analogy. In large families with several children, it is a luxury for each child to have his or her own room. There is far less fussing and fighting if siblings are not forced to share living quarters: the entire household experiences a lower-intensity, less-frazzled energy state. Likewise, electrons will go into available orbitals singly before beginning to pair up. All the single–occupant electrons of orbitals have parallel spins, are designated with an upward-pointing arrow, and have a magnetic spin quantum number of +1/2.　　As we mentioned earlier, each principal energy level, n, has n sublevels. This means the first has one sublevel, the second has two, the third has three, etc. The sublevels are named s, p, d, and f.Energy level principal quantum number, nNumber of sublevelsNames of sublevels

11s

22s, p

33s, p, d

44s, p, d, f

At each additional sublevel, the number of available orbitals is increased by two: s = 1, p = 3, d = 5, f = 7, and as we stated above, each orbital can hold only two electrons, which must be of opposite spin. So s holds 2, p holds 6 (2 electrons times the number of orbitals, which for the p sublevel is equal to 3), d holds 10, and f holds 14.Sublevelspdf

Number of orbitals1357

Maximum number of electrons261014

Quantum number, l0123

We can use the periodic table to make this task easier.

更多sat考试个性化问题欢迎咨询新航道官网

随便看

出国留学网出国外语考试提供雅思、托福、GRE等外语考试复习资料，是出国外语考试复习及应试的有利工具。