What electron could have quantum numbers #n=2, l=1, m_l = 0, m_s = +1/2#?
1 Answer
Here's what I got.
Explanation:
As you know, four quantum numbers are used to describe the position and spin of an electron in an atom.
The problem provides you with a complete set of quantum numbers and asks you to find an electron that can be described using those quantum numbers.
In your case, the principal quantum number,
The angular momentum quantum number,
#l=0 -># the s-subshell#l=1 -># the p-subshell#l=2 -># the d-subshell#l=3 -># the f-subshell
In your case, the value
The magnetic quantum number,
The p-subshell contains a total of three orbitals, by convention assigned as
#m_l = color(white)(-)0 -># the#2p_z# orbital#m_l = -1 -># the#2p_y# orbital#m_l = +1 -># the#2p_x# orbital
In your case,
Finally, the spin quantum number,
You can thus say that the quantum number set given to you describes an electron
- located on the second energy level
#-> n=2# - located in the 2p-subshell
#-> l=1# - located in the
#2p_z# orbital#-> m_l = 0# - that has spin-up
#-> m_s = +1/2#