Download Quantum Numbers Chart

Values of Quantum Numbers
n
1
2
0
0
1
0
1
2
0
1
2
3
3
4
l
(s-orbital)
(s-orbital)
(p-orbital)
(s-orbital)
(p-orbital)
(d-orbital)
(s-orbital)
(p-orbital)
(d-orbital)
(f-orbital)
Ml
0
0
+1, 0, -1
0
+1, 0, -1
+2, +1, 0, -1, -2
0
+1, 0, -1
+2, +1, 0, -1, -2
+-3,+2, +1, 0, -1, -2, -3
ms
+1/2, -1/2
+1/2, -1/2
± ½ for each value of ml
+1/2, -1/2
± ½ for each value of ml
± ½ for each value of ml
+1/2, -1/2
± ½ for each value of ml
± ½ for each value of ml
± ½ for each value of ml
Atomic Orbital – a region of space in which the probability of finding an electron is high.
1.
Principal quantum number – n, describes the main energy level, or shell, that an electron
occupies. N equals the period number that an element is in.
i.
Chlorine = period 3, thus n = 3
2.
Angular Momentum quantum number – l, designates the sublevel, or specific shape of
atomic orbaital that an electron may occupy.
i.
(0) S-orbital – spherical shaped
ii.
(1) P- orbital
iii.
(2) D- orbital
iv.
(3) F- orbital
Magnetic Quantum number, ml, designates a specific orbital w/I a subshell
3.
Block
S- block
P-block
D-block
F- block
Orbitals
1 orbital
3 orbitals
5 orbitals
7 orbitals
Magnetic Quantum Number
0
+1, 0, -1
+2, +1, 0, -1, -2
+3,+2, +1, 0, -1, -2, -3
Fluorine = 9 electrons
F = 1s ___ 2s ___ 2p ___ ___ ___
ml
0
0
+1, 0, -1
4.
Spin Quantum number, ms, refers to the spin of an electron and the orientation of the magnetic field
produced by this spin. For every set of n, l, and ml values, ms can take the value +1/2 or -1/2.
Argon = 18 electrons
Electron
N
L
Ml
Ms
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
1
1
2
2
2
2
2
2
2
2
3
3
3
3
3
3
3
3
0
0
0
0
1
1
1
1
1
1
0
0
1
1
1
1
1
1
0
0
0
0
+1
0
-1
+1
0
-1
0
0
+1
0
-1
+1
0
-1
+
+
+
+
+
+
+
+
+
-
Write the electron configuration for Argon…
a) Label Magnetic quantum number for each orbital
b) Label the Spin quantum number for each electron