![]() One way you can look at it is that l is the number of nodes (points of zero density) in the. l is the angular momentum quantum number. Fortunately, it is given to you: 3d tells you that n 3 for this set of orbitals. and ml goes from l to -l in unit increments. You now have all the information that you need to write the sets of quantum numbers that can describe an electron located on the #"4th"# energy level, in the #4d# subshell. It is the number that governs all the other quantum numbers. ![]() Now, the #d# subshell can hold a maximum of five #d# orbitals, which are denoted by the values of the magnetic quantum number, #m_l#.įinally, the spin quantum number, #m_s#, which denotes the spin of the electron, can take two possible values The last energy sublevel to fill was the p orbital. The angular momentum quantum number, #l#, tells you the energy subshell in which the electron is located. To do this, we look at the valence or differential electron, that is, the last electron that has filled the orbital. Give all the possible values of the four quantum numbers of an electron in the 3d orbital. Give all the possible values of the four quantum numbers of an electron in the 3s orbital. In your case, the electron is said to occupy the #"4th"# energy level, which is equivalent to saying that it is located in the #"4th"# energy shell, so Give all the possible values of the four quantum numbers of an electron in the 4p orbital. As you know, the principal quantum number, #n#, tells you the energy shell in which the electron is located.
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