Electron Configuration Practice Worksheet II

Name: ____________________________
When is this due? __________________
Date: ______
Period: _______
Electron Configuration Practice Worksheet II
1. Write the ground state electron configuration for each neutral atom. Remember ground state means that all
of the lowest possible energy levels (up to the proper number of electrons for the element) are filled.
a) Na
b) Pb
c) Sr
d) N
2. Write the ground state electron configuration for each neutral atom in Nobel Gas Notation. Remember
ground state means that all of the lowest possible energy levels (up to the proper number of electrons for
the element) are filled.
a) Na
b) Pb
c) Sr
d) N
Name: ____________________________
When is this due? __________________
Date: ______
Period: _______
3. Write the ground state electron configuration for the following ions. Remember ions have a change in total
number of electrons (positive ions, cations, have lost an electron and negative ions, anions, have gained an
ion). [Example: N-3 is 1s22s23p6 and has 3 extra electrons]
a)
O-2
b) Fe+2
c) Cl-1
d) K+
4. Use the Pauli Exclusion Principle and Hund’s Rule to identify how many unpaired electrons are present in the
following atomic structures :
The Pauli Exclusion Principle states that a maximum of two electrons can occupy a single atomic orbital to
form paired electrons, but only if the two electrons have opposite spins.
Hund’s Rule states that single electrons with the same spin must occupy each equal-energy orbital before
additional electrons with opposite spins can occupy the same orbital.
a) Si
b) Cl
c) Mn
d) Ru
Name: ____________________________
When is this due? __________________
Date: ______
Period: _______
5. When writing the electron configuration of an element, why would we fill the 4s orbital before we fill the 3d
orbital?
6. The elements silicon, gallium, arsenic, germanium, aluminum, cadmium, sulfur, and selenium
are all used in the manufacture of various semiconductor devises. Write the ground state
electron configuration for germanium.
7. Identify which element would have the following electron configuration as a ground state atom?
[Ne]3s2 3p3
8. Fill out the information below?
s-orbital
Draw the general
shape of the orbital
How many electrons
can it hold?
What is the lowest
energy level in which it
can exist?
p-orbital
d-orbital
f-orbital
Name: ____________________________
When is this due? __________________
Date: ______
Period: _______
9. Draw the Electron Configuration for Ru.
Energy Level
sorbitals
p-orbitals
d-orbitals
f-orbitals
n=5
____
5s
____ ____ ____
5p
____ ____ ____ ____
____
5d
____ ____ ____ ____ ____
____ ____
5f
n=4
____
4s
____ ____ ____
4p
____ ____ ____ ____
____
4d
____ ____ ____ ____ ____
____ ____
4f
n=3
____
3s
____ ____ ____
3p
____ ____ ____ ____
____
3d
n=2
____
2s
____ ____ ____
2p
n=1
____
1s
10. Fill out the chart below:
Element
Atomic
Number
Na
11
S
16
K
Number of electrons
in each level
1st
2nd
3rd
4th
2
8
1
1st
2nd
3rd
2
8
6
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
1st
2nd
3rd
4th
5th
4th
5th
5th
Al
Cl
Xe
Ca
Electron Configuration
Number of ethat can be lost
or gained
Number of
electrons left
after ionization
Charge on
the ion
1s22s22p63s1
Lose 1
10
+1
1s22s22p63s23p4
Gain 2
18
-2