1. What is the azimuthal quantum number l, for this orbital? (Integer answer)
2. Compare the orbital from 1 to the orbital shown here in size, shape, and orientation. Which
quantum number(s) would be different for these two orbitals?
None of this is in my textbook, so Any help is greatly appreciated! Thanks
1. its dxy orbital …one of the five orbitals of d-subshell so l = 2
2.its d(x^2-y^2) orbital …..difference is :- The dxy orbital points its lobes between the x and y axes. The d(x^2-y^2) orbital points its lobes directly along the x and y axes.
feel free to ask any questions
Quantum numbers are used to label the state of a quantum procedure. On your case, it’s concerning the state of an electron round a nucleus. 4 quantum numbers are used. Most important quantum quantity, n = 1, 2, 3, four, … ================================ Enumerates the shells in which the electron can go. Shell 1 is closest to the nucleus, and has room for 2 electrons. Shell 2 has room for eight electrons. In general, shell n has room for two * n^2 electrons. Azimuthal quantum quantity, L = 0, 1, …, n =============================== shows absolutely the worth of the angular momentum. This defines the specific “orbitals” within a shell. For illustration, in shell 1 we have now L = 0: s-orbital, two electrons L = 1: p-orbital, six electrons L = 2: d-orbital, ten electrons most likely, orbital L can have 4n – 2 electrons. Magnetic quantum quantity m = -L, …, zero, …, L ================================= indicates the magnitude of the angular momentum of an electron in a constant course (regularly, along the z-axis). For example, the 2p orbital (n = 2, L = 1) can condominium three pairs of electrons, with m = -1, 0 or 1. They are customarily written as 2px, 2py, 2pz. Spin quantum number s = -half of, +1/2 =========================== Electron spin is either “up” or “down”. For each blend n, L, m there are two viable spin states.