QUANTUM NUMBERS AND LEWIS DOTS FOR ATOMS (and more)!
Quantum Numbers: another way to describe the location of electrons in atoms!
n
l
ml
1
s (0)
0
s (0)
0
2
p (1)
-1 0 1
s (0)
0
3
p (1)
-1 0 1
d (2)
-2 -1 0 1 2
s (0)
0
4
p (1)
-1 0 1
(and beyond)
d (2)
-2 -1 0 1 2
f (3)
-3 -2 -1 0 1 2 3
1.
ms
+1/2 , -1/2
Using the numerical notations above, give the ending electrons configuration that represents that element, the
orbital diagram for the ending configuration, and the set of quantum numbers for each electron specified. The
first one is done for you!
n = 2, l = 0, ml = 0, ms = -½
th
4
50th
2s2
2, 0, 0, -½
17th
77th
19th
81st
27th
59th
36th
80th
39th
98th
2. Using the pattern of sublevels from low energy to high energy (1s to 7p), give the ending configuration of the
last electron of the following elements:
Sn
_____
Li
_____
I
_____
Ba
_____
Fm
_____
Ru
_____
Hg
_____
Pr
_____
3. Using the method discussed in class, give the ABBREVIATED electron configuration for each of the following
elements:
(a) Cobalt
(e) Cerium (Ce)
(b) Hafnium (Hf)
(f) Vanadium
(c) Curium (Cm)
(g) Chlorine
(d) Tin
QUANTUM NUMBERS AND LEWIS DOTS FOR ATOMS (and more)!
4. Tell whether the following are in GROUND state (GS), EXCITED state (ES) or IMPOSSIBLE (I) electron
configurations.
(a) 1s22s22p4____
(e) 1s22s22p10____
(b) 1s22s22p63p1
____
(f) [Ar]3s2____
(c) 1s22s22p63s23p64s23d84p1____
(g) 1s22s22p63s33p64s23d104p65s1 ____
1
(d) [Xe]7s ____
5.
List the maximum number of electrons possible in each of these “spaces”:
a. a p sublevel __________
b. a 3d orbital _________
c. the 4th energy level _________
d. the 1st energy level _________
e. the 5f sublevel ___________
f. a 7s orbital ___________
g. the 7th energy level ___________
h. the 5d sublevel ____________
6. List the number of valence electrons in each element, and draw the Lewis dot diagram that represents
them around the symbol for the element:
a)
Si
i)
Ra
b)
Kr
j)
P
c)
Sr
k)
Rn
d)
Co
l)
H
e)
Na
m) W
f)
Al
n)
Sn
g)
Te
o)
Cl
h)
Cd
p)
Fr