What is the ml quantum number for an electron in the 5d orbital?

1 Answer
Dec 25, 2015

Answer:

#m_l = {-2,-1,0,1,2}#

Explanation:

As you know, the position and spin of an electron in an atom are determined by a set of four quantum numbers

figures.boundless.com

In your case, you're interested about figuring out what value of the magnetic quantum number, #m_l#, would correspond to an electron located in a 5d-orbital.

The magnetic quantum number gives you the exact orbital in which the electron is located. The subshell that holds that orbital is determined by the angular momentum quantum number, #l#.

As you can see, the values of #m_l# depend on the value of #l#, which can be

  • #l=0 -># characterizes the s-subshell
  • #l=1 -># characterizes the p-subshell
  • #l=2 -># characterizes the d-subshell

In your case, #l=2#, since you're dealing with a d-subshell. This means that #m_l# can take any of the following values

#m_l = {-2, -1, color(white)(-)0, color(white)(-)1, color(white)(-)2}#

Each d-subshell contains a total of five orbitals. In the case of a 5d-subshell, these orbitals correspond to the following #m_l# values

  • #m_l = -2 -># the #5d_(xy)# orbital
  • #m_l = -1 -># the #5d_(xz)# orbital
  • #m_l = color(white)(-)0 -># the #5d_(yz)# orbital
  • #m_l = color(white)(-)1 -># the #5d_(x^2-y^2)# orbital
  • #m_l = color(white)(-)2 -># the #5d_(z^2)# orbital

http://2012books.lardbucket.org/books/principles-of-general-chemistry-v1.0/s10-05-atomic-orbitals-and-their-ener.html