Name _______________________________
Spectral Lines
Directions:
Date ________________
Mrs. Hutchinson 
Bright-Line Spectra differ for each element and are used to identify which
elements are involved in creating a mixture.
1. Given the bright-line spectra of the three elements and the spectrum of a mixture formed
from at least two of these elements:
Identify which elements are present in this mixture.
2. The diagram below represents the bright-line spectra of four elements and a bright-line
spectrum produced by a mixture of two of these elements.
Which two elements are in this mixture?
3. The Bright-Line Spectra for three different elements and a mixture are shown below.
A. Identify all the elements in the mixture.
B. Explain, in terms of both electrons and energy, how the bright-line spectrum of an
element is produced.
Name _______________________________
Quantum Numbers
Date ________________
Mrs. Hutchinson 
Directions: Use your notes to help answer these questions.
1. Define what the n quantum number stands for and calculate the number of electrons that
n = 11 can hold.
2. When identifying sublevels using the principle quantum number what is the general rule that
you abide by to determine what your ℓ quantum number is equal to.
3. Identify the ℓ quantum number that corresponds to each sublevel.
Sublevel
s
p
d
f
ℓ quantum number
4. When n = 4, what sublevel(s) is/are possible?
5. The m quantum number states how many orbitals are present in each sublevel. What is the
general rule in determining the number of orbitals that are present in each sublevel.
6.
p = ___ ___ ___
-1
0 +1
Using the example above, draw and correctly label orbitals present in an f-subshell.
7. Identify the four quantum numbers for the following electrons
___
1s
___ ___ ___ ___
2s
2p
___
3s
___ ___ ___
3p
8. Each orbital can hold a maximum number of how many electrons? Create an equation for
determining the number of electrons each orbital can hold.
Name _______________________________
Orbital Filling
Date ________________
Mrs. Hutchinson 
Directions: Draw the electron configurations for the elements in question like the example
below.
Be = 1s22s2
1. Nitrogen (N)
2. Cobalt (Co)
3. Potassium (K)
4. Rubidium (Rb)
5. Manganese (Mn)
6. Selenium (Se)
7. Neon (Ne)
8. Krypton (Kr)
9. Zinc (Zn)
10. Carbon (C)
Name _______________________________
Ground state vs. Excited state
Date ________________
Mrs. Hutchinson 
Directions: Determine whether the following configurations indicate an atom in a ground state
or an excited state and identify the element.
1. 2 – 8 – 4
2. 1s22s22p63s23p54s1
3. 1s22s22p6
4. 2 – 8 – 17 – 2
5. 1s22s22p63s23p4
6. 1s
2s
2p
2s
2p
7. 2 – 7 – 1
8. 1s22s12p4
9. 1s
10. 2 – 8 – 18 – 8
3s
Name _______________________________
Atom or ion
Date ________________
Mrs. Hutchinson 
Directions: Identify whether the electron configuration is an atom or an ion.
1. Oxygen: 2 – 8
2. Phosphorus: 1s22s22p63s23p3
3. Sodium:
1s
2s
2p
3s
2p
3s
4. Magnesium: 2 – 8
5. Potassium: 1s22s22p63s23p6
6. Sulfur:
1s
2s
7. Germanium: 2 – 8 – 18 – 4
8. Boron: 1s22s22p1
9. Beryllium:
1s
10. Iron: 2 – 8 – 14 – 2
2s
3p