Answer:
5p 5, 1, -1, +1/2
6d 6, 2, -2, +1/2
Explanation:
Give a combination of four quantum numbers that could be assigned to an electron occupying a 5p orbital.
The electron is in the energy level 5 so the principal quantum number (n) is 5.
The p orbital is associated with the angular quantum number (l) 1. l indicates the type of orbital.
The magnetic quantum number (ml) can take values from -l to +l. In this case, the possible values are -1, 0, +1.
The spin quantum number (ms) can take the values +1/2 or -1/2.
One possible combination for n, l, ml, ms is 5, 1, -1, +1/2.
Do the same for an electron occupying a 6d orbital.
The electron is in the energy level 6 so the principal quantum number (n) is 6.
The d orbital is associated with the angular quantum number (l) 2. l indicates the type of orbital.
The magnetic quantum number (ml) can take values from -l to +l. In this case, the possible values are -2, -1, 0, +1, +2.
The spin quantum number (ms) can take the values +1/2 or -1/2.
One possible combination for n, l, ml, ms is 6, 2, -2, +1/2.
