Basics
Writing Configurations
Valence Electrons
Writing Short Configurations
100
What is Hund’s rule?
A rule stating that when filling orbitals of equal energy, electrons will occupy empty orbitals singly before pairing with other electrons
100
What is the full electron configuration for Li.
1s2 2s1
100
How many valence electrons are in the following configuration: 1s2 2s2. What element is this?
2 valence electrons, Beryllium
100
Write the short electron configuration for Oxygen.
[He] 2s2 2p4
200
Identify the blocks in the periodic table for electron configurations
Blue=s, Yellow=d, Pink=p, Green=f
200
What is the full electron configuration for Ar.
1s2 2s2 2p6 3s2 3p6
200
How many valence electrons are in the following configuration: 1s2 2s2 2p5. What element is this?
7 valence electrons, Fluorine
200
Write the short electron configuration for Chlorine.
[Ne] 3s2 3p5
300
What is the Pauli exclusion principle?
A principle stating that no more than 2 electrons can occupy an orbital and that the 2 electrons must have opposite spins
300
What is the full electron configuration for Ge?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
300
Write the electron configuration for the valence electrons of Bromine.
4s2 4p5
300
Write the short electron configuration for Calcium.
[Ar] 4s2
400
How many electrons can the s, p, d, and f subshells hold?
The s subshell can hold 2 electrons, the p subshell can hold 6 electrons, the d subshell can hold 10 electrons, and the f subshell can hold 14 electrons
400
What is the full electron configuration for Ca?
1s2 2s2 2p6 3s2 3p6 4s2
400
Write the electron configuration for the valence electrons of Indium.
5s2 5p1
400
Write the short electron configuration for Gallium.
[Ar] 4s2 3d10 4p1
500
What is the order of filling out orbitals? (use a diagram)
Down in a diagonal order
500
What is the full electron configuration for Sb?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p3
500
Write the electron configuration for the valence electrons of Phosphorus.
3s2 3p3
500
Write the short electron configuration for Tin.
[Kr] 5s2 4d10 5p2