Question

Describe all 4 quantum numbers for last electron of 3d^5?

Answer 1

see below

Explanation:

it is Mn (manganese)
N= 3 third energetic level
l= 3 shape of orbitals of type d : (quatrefoil)
5 = the 5 orbitals d are all full means with only one electron in every orbitals (M,magnetic orbitatals = -2,-1, 0 +1 +2 what is the last, you don't know because are isoenergetic)
s =intrinsic magnetic moment `= +- h/(2 xx pi)`(what is the last, you don't know, for convention the negative one)

Answer 2

The four quantum numbers are 3, 2, +2, +½.

Explanation:

The four quantum numbers are

• `n color(white)(ll)=` principal quantum number; determines energy and size of orbital
• `l color(white)(m)=` secondary quantum number; determines shape of orbital
• `m_text(l) =`magnetic quantum number; determines orientation of orbital in magnetic field
• `m_text(s) =` spin quantum number; determines direction of electron spin

The rules for quantum numbers are:

• `n color(white)(ll)=` integers from 1 to ∞.
• `lcolor(white)(m)=` integers from 0 to `n - 1`
• `m_text(l) =` integers from `-l` to `+l`
• `m_text(s) =` +½ or -½

Here is a table of quantum numbers for the first five `"3d"` electrons. The quantum numbers for the fifth electron are red.

`ulbb(ncolor(white)(m)lcolor(white)(ml)m_text(l)color(white)(ml)m_text(s))`
`3color(white)(m)2color(white)(mll)"-2"color(white)(m)"+½`
`3color(white)(m)2color(white)(mll)"-1"color(white)(m)"+½`
`3color(white)(m)2color(white)(mm)"0"color(white)(m)"+½`
`3color(white)(m)2color(white)(m)"+1"color(white)(m)"+½`
`color(red)(3color(white)(m)2color(white)(m)"+2"color(white)(m)"+½)`

Here's how the quantum numbers fit in the Periodic Table