主量子数英文

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原子轨道高中不讲的 但是苏教版有一本化学选修叫 物质结构基础，里面有涉及到一点。

谁有化学 物理方面的专业英语词汇 从最基本的到大学6级程度 要求有音标及英语解释 中文解释 人教版？什么教材？人教版不是只出高中的书吗？ 我

Nlm在机械上是应该是机器的一个车床吧，一般这个车上都是用一个英文字母代替的，每个英文字母代表一个环节。

n——主量子数，决定电子能量高低与离核的平均距离主要因素，相同的轨道称为电子层，只能取正整数，n是多少就有几个电子层（主电子层）。

l——角量子数，电子亚层，决定轨道形状，取值为0到n-1 。

m——磁量子数，同一形状的轨道，在空间有不同取向，用m表示，取值为0到正负1。

s——自旋量子数，描述自旋运动状态，只有两个数，为正负1/2。

量子数表征原子、分子、原子核或亚原子粒子状态和性质的数。通常取整数或半整数分立值。量子数是这些粒子系统内部一定相互作用下存在某些守恒量的反映，与这些守恒量相联系的量子数又称为好量子数，它们可表征粒子系统的状态和性质。

在原子物理学中，对于单电子原子（包括碱金属原子）处于一定的状态，有一定的能量、轨道角动量、自旋角动量和总角动量。表征其性质的量子数是主量子数n、角量子数l、自旋量子数s=1/2，和总角动量量子数j。

量子数包括主量子数n、角量子数l、磁量子数m和自旋量子数s四种，前三种是在数学解析薛定谔方程过程中引出的，而最后一种则是为了表述电子的自旋运动提出的。

量子数通常取整数或半整数分立值。

在原子物理学中，对于单电子原子（包括碱金属原子）处于一定的状态，有一定的能量、轨道角动量、自旋角动量和总角动量。表征其性质的量子数是主量子数n、角量子数l、自旋量子数ms=1/2，和总角动量量子数j。

在光谱学上常用大写拉丁字母K，L，M，N，O，P，Q代表电子层数，主量子数n是决定电子能量高低的主要因素。

对单电子原子来说：n值愈大，电子的能量愈高。例如氢原子中电子的能量完全由主量子数n决定。

对多电子原子来说：核外电子的能量除了同主量子数n有关以外还同原子轨道或电子云的形状有关。

因此，n值愈大，电子的能量愈高这句话，只有在原子轨道或电子云的形状相同的条件下，才是正确的。

The principal quantum number（主量子数）The azimuthal quantum number（角量子数）The magnetic quantum number（磁量子数） The spin projection quantum number（自旋量子数） the electron shell, or energy level. The value of ranges from 1 to "n", where "n" is the shell containing the outermost electron of that atom. For example, in cesium (Cs), the outermost valence electron is in the shell with energy level 6, so an electron in cesium can have an value from 1 to 6. the subshell (0 = s orbital, 1 = p orbital, 2 = d orbital, 3 = f orbital, etc.). The value of ranges from 0 to . This is because the first p orbital (l=1) appears in the second electron shell (n=2), the first d orbital (l=2) appears in the third shell (n=3), and so on. A quantum number beginning in 3,0,... describes an electron in the s orbital of the third electron shell of an atom. the specific orbital (or "cloud") within that subshell.* The values of range from to . The s subshell (l=0) contains only one orbital, and therefore the ml of an electron in an s subshell will always be 0. The p subshell (l=1) contains three orbitals (in some systems, depicted as three "dumbbell-shaped" clouds), so the ml of an electron in a p subshell will be -1, 0, or 1. The d subshell (l=2) contains five orbitals, with ml values of -2,-1,0,1, and 2. the spin of the electron within that orbital. since atoms and electrons are in a state of constant motion, there is no universal fixed value for ml and ms values. Therefore, the ml and ms values are defined somewhat arbitrarily. The only requirement is that the naming schematic used within a particular set of calculations or descriptions must be consistent (e.g. the orbital occupied by the first electron in a p subshell could be described as ml=-1 or ml=0, or ml=1, but the ml value of the other electron in that orbital must be the same, and the ml assigned to electrons in other orbitals must be different). The principal quantum number（主量子数） (n = 1, 2, 3, 4 ...) denotes the eigenvalue of H with the J2 part removed. This number therefore has a dependence only on the distance between the electron and the nucleus (i.e., the radial coordinate, r). The average distance increases with n, and hence quantum states with different principal quantum numbers are said to belong to different shells. The azimuthal quantum number（角量子数） (l = 0, 1 ... n�6�11) (also known as the angular quantum number or orbital quantum number) gives the orbital angular momentum through the relation . In chemistry, this quantum number is very important, since it specifies the shape of an atomic orbital and strongly influences chemical bonds and bond angles. In some contexts, l=0 is called an s orbital, l=1 a p orbital, l=2 a d orbital, and l=3 an f orbital. The magnetic quantum number（磁量子数） (ml = �6�1l, �6�1l+1 ... 0 ... l�6�11, l) yields the projection of the orbital angular momentum along a specified axis. . The spin projection quantum number（自旋量子数） (ms = �6�11/2 or +1/2), is the intrinsic angular momentum of the electron or nucleon. This is the projection of the spin s=1/2 along the specified axis. When one takes the spin-orbit interaction into consideration, the l-, m- and s-operators no longer commute with the Hamiltonian, and their eigenvalues therefore change over time. Thus another set of quantum numbers should be used. This set includesThe total angular momentum quantum number (j = 1/2,3/2 ... n�6�11/2) gives the total angular momentum through the relation .The projection of the total angular momentum along a specified axis (mj = -j,-j+1... j), which is analogous to m, and satisfies mj = ml + ms.Parity. This is the eigenvalue under reflection, and is positive (i.e. +1) for states which came from even l and negative (i.e. -1) for states which came from odd l. The former is also known as even parity and the latter as odd parityFor example, consider the following eight states, defined by their quantum numbers:n = 2, l = 1, ml = 1, ms = +1/2n = 2, l = 1, ml = 1, ms = -1/2n = 2, l = 1, ml = 0, ms = +1/2n = 2, l = 1, ml = 0, ms = -1/2n = 2, l = 1, ml = -1, ms = +1/2n = 2, l = 1, ml = -1, ms = -1/2n = 2, l = 0, ml = 0, ms = +1/2n = 2, l = 0, ml = 0, ms = -1/2The quantum states in the system can be described as linear combination of these eight states. However, in the presence of spin-orbit interaction, if one wants to describe the same system by eight states which are eigenvectors of the Hamiltonian (i.e. each represents a state which does not mix with others over time), we should consider the following eight states:j = 3/2, mj = 3/2, odd parity (coming from state (1) above)j = 3/2, mj = 1/2, odd parity (coming from states (2) and (3) above)j = 3/2, mj = -1/2, odd parity (coming from states (4) and (5) above)j = 3/2, mj = -3/2, odd parity (coming from state (6))j = 1/2, mj = 1/2, odd parity (coming from states (2) and (3) above)j = 1/2, mj = -1/2, odd parity (coming from states (4) and (5) above)j = 1/2, mj = 1/2, even parity (coming from state (7) above)j = 1/2, mj = -1/2, even parity (coming from state (8) above)