Orbital magnetic quantum

Ml total (resultant) orbital magnetic quantum number... 

The orbital magnetic quantum number m gives the orientation of the electron s angular motion. The values of M, /, and mi specify an orbital. 

The third quantum number m is called the magnetic quantum number for it is only in an applied magnetic field that it is possible to define a direction within the atom with respect to which the orbital can be directed. In general, the magnetic quantum number can take up 2/ + 1 values (i.e. 0, 1,. .., /) thus an s electron (which is spherically symmetrical and has zero orbital angular momentum) can have only one orientation, but a p electron can have three (frequently chosen to be the jc, y, and z directions in Cartesian coordinates). Likewise there are five possibilities for d orbitals and seven for f orbitals. 

The third quantum number required to specify an orbital is mh the magnetic quantum number, which distinguishes the individual orbitals within a subshell. This quantum number can take the values... 

The spins of two electrons are said to be paired if one is T and the other 1 (Fig. 1.43). Paired spins are denoted Tl, and electrons with paired spins have spin magnetic quantum numbers of opposite sign. Because an atomic orbital is designated by three quantum numbers (n, /, and mt) and the two spin states are specified by a fourth quantum number, ms, another way of expressing the Pauli exclusion principle for atoms is... 

For each orbital listed in Exercise 1.51, give the possible values for the magnetic quantum number. 

Among atomic orbitals, s orbitals are spherical and have no directionality. Other orbitals are nonspherical, so, in addition to having shape, every orbital points in some direction. Like energy and orbital shape, orbital direction is quantized. Unlike footballs, p, d, and f orbitals have restricted numbers of possible orientations. The magnetic quantum number (fflj) indexes these restrictions. 

The magnetic quantum number derives its name from the fact that different orbital orientations generate different behaviors in... 

Magnetic quantum number One solution to Schrodinger s wave equation produces the magnetic quantum number. It specifies how the s, p, d, and/orbitals are oriented in space. 

In addition to the magnetism due to the electron spin, the magnetism of the orbital motion has to be considered. For this purpose the magnetic quantum numbers of the electrons are added to a resultant orbital quantum number L = beginning with the highest magnetic quantum number. For example ... 

Depending on the permitted values of the magnetic quantum number m, each subshell is further broken down into units called orbitals. The number of orbitals per subshell depends on the type of subshell but not on the value of n. Each orbital can hold a maximum of two electrons hence, the maximum number of electrons that can occupy a given subshell is determined by the number of orbitals available. These relationships are presented in Table 17-5. The maximum number of electrons in any given energy level is thus determined by the subshells it contains. The first shell can contain 2 electrons the second, 8 electrons the third, 18 electrons the fourth, 32 electrons and so on. 

From the mathematical restrictions on the solution of the equations comes a set of constraints known as quantum numbers. The first of these is n, the principal quantum number, which is restricted to integer values (1, 2, 3,. ..). The second quantum number is 1, the orbital angular momentum quantum number, and it must also be an integer such that it can be at most (n — 1). The third quantum number is m, the magnetic quantum number, which gives the projection of the 1 vector on the z axis as shown in Figure 2.2. 

A The magnetic quantum number, m, is not reflected in the orbital designation. 

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