The quantum numbers are: n = principal quantum number, describes energy and size of the orbital ℓ = angular momentum quantum number, describes shape and sublevel of the orbital mℓ = magnetic quantum number, describes the orientation of the orbital in space ms = spin quantum number, describes the spin/magnetic properties of the electron Which quantum numbers would be different for the following two orbitals? 3dxy and 3dyz

mℓ

Explanation:

To solve this question one has to have in mind the values the quantum number can assume given a principal quantum number n.

ℓ angular  quantum numbe,can have the values 0, 1, 2,3 to n-1

and they correspond to the shape of the orbital in and have the symbol

0  ⇒   s orbital

1   ⇒   p orbial

2  ⇒   d orbital

for d orbitals ( l= 2 ) we can have five orientations in space  since  mℓ  can have the value which   range from - ℓ to + ℓ:

for l= 2  

mℓ = -2, -1, 0, 1, 2

which corresponds to the five orientations possible for d orbitals:

dz², dxy, dxz, dyz, dx²-y²

Hence it follows the two orbitals in our question differ in their quantum number  mℓ

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer