What are the possible values of n and ml for an electron in a 5d orbital ? A) n = 5 and ml = -2, -1, 0, +1, or +2 B) n = 1, 2, 3, 4, or 5 and ml = 2 C) n = 5 and ml = 2 D) n = 1, 2, 3, 4, or 5 and ml = -2, -1, 0, +1, or +2

1 Answer
Apr 16, 2015

The answer is A).

The principal quantum number, or #n#, describes the energy lelvel in which the electron can be found, Since you're interested in an electron located in a 5d-orbital, #n=5#.

The angular momentum quantum number, or #l#, describes the subshell, or orbital type, in which your electron is located. Since you have a d-orbital, #l=2#.

The value of #l# will give you the value of the magnetic quantum number, or #m_l#, which describes the orientation of the orbital.

The accepted values for #m_l# range from #-l# to #+l#, which means that you can have 5 d-orbitals in the fifth energy level, #d_(xy)#, #d_(xz)#, #d_(yz)#, #d_(z^2)#, and #d_(x^2-y^2)#, each described by a magnetic quantum number

#m_l = -2#
#m_l = -1#
#m_l = 0#
#m_l = +1#
#m_l = +2#

As an example, here's how these orbitals would look for the 3d subshell

http://catalog.flatworldknowledge.com/bookhub/4309?e=averill_1.0-ch06_s05