Electron Configuration Practice Worksheet
In the space below, write the unabbreviated electron configurations of the
following elements:
1)
sodium
________________________________________________
2)
iron
________________________________________________
3)
bromine
________________________________________________
4)
barium
________________________________________________
5)
neptunium
________________________________________________
In the space below, write the abbreviated electron configurations of the following
elements:
6)
cobalt
________________________________________________
7)
silver
________________________________________________
8)
tellurium
________________________________________________
9)
radium
________________________________________________
10)
lawrencium ________________________________________________
Determine what elements are denoted by the following electron configurations:
11)
1s22s22p63s23p4 ____________________
12)
1s22s22p63s23p64s23d104p65s1 ____________________
13)
[Kr] 5s24d105p3 ____________________
14)
[Xe] 6s24f145d6 ____________________
15)
[Rn] 7s25f11 ____________________
Determine which of the following electron configurations are not valid:
16)
1s22s22p63s23p64s24d104p5 ____________________
17)
1s22s22p63s33d5 ____________________
18)
[Ra] 7s25f8 ____________________
19)
[Kr] 5s24d105p5 ____________________
20)
[Xe] ____________________
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Orbital Diagrams
Name ________________
Chem Worksheet 5-5
An orbital diagram uses boxes with arrows to represent the electrons in an atom. Each box in an
orbital diagram represents an orbital. Orbitals have a capacity of two electrons. Arrows are drawn
inside the boxes to represent electrons. Two electrons in the same orbital must have opposite spin so
the arrows are drawn pointing in opposite directions. The following is an orbital diagram for selenium.
Se:
1s
Electrons fill the lowest
available energy levels first.
2s
2p
3s
3p
4s
3d
Two electrons in the same orbital
must have opposite spin.
Each orbital is half-filled
before being completely filled.
In writing an orbital diagram the first step is to determine the
Boxes drawn for various sublevels
number of electrons. Normally this is the same as the number of
s sublevel:
1 orbital
protons, which is known as the atomic number. Next the boxes are
p sublevel:
3 orbitals
drawn for the orbitals. Arrows are drawn in the boxes starting from
the lowest energy sublevel and working up. This is known as the
d sublevel:
5 orbitals
Aufbau rule. The Pauli exclusion principle requires that electrons
f sublevel:
7 orbitals
in the same orbital have opposite spin. Hund’s rule states that
orbitals in a given sublevel are half-filled before they are completely filled.
1s
2s
2p
3s
This violates Hund’s rule. One electron
should be distributed to each of the 3p
orbitals before doubly filling any.
3p
Write the name and symbol for the elements with the following orbital diagrams.
1.
2.
3.
1s
2s
2p
1s
2s
2p
1s
2s
2p
3s
3p
4s
4.
1s
2s
5. [Kr]
3s
5s
6. [Rn]
3p
2p
3s
3p
4d
7s
4s
3d
5p
5f
There is an error with each of the following orbital diagrams. Explain the error.
7. [Ar]
4s
3d
4p
8.
1s
2s
2p
3s
3p
Write orbital diagrams for the following. You may abbreviate using a noble gas.
9.
hydrogen
15.
carbon
10.
boron
16.
cobalt
11.
sodium
17.
platinum
12.
krypton
18.
plutonium
13.
chromium
19.
oxygen
14.
phosphorus
20.
potassium
Chemistry
WS5-5OrbitalDiagrams