Name: _____________________________________________ Date: ___________________________ Period: ________
Unit 5 Test Study Guide
Nuclear & Quantum Chemistry
Nuclear Equations
Write nuclear equations for the following scenarios:
1. Alpha emission by plutonium-239, one of the substances formed in nuclear power plants.
2.
Beta decay by sodium-24, used to detect blood clots
3. Oxygen-15 undergoes positron emission, used to assess the efficiency of the lungs.
4. Copper-64 goes through electron capture, used to diagnose lung disease.
5. A radioactive isotope is bombarded with an alpha particle to produce Polonium-84.
6. A silver-117 undergoes three beta emissions before it reaches a stable nuclide. What is the final product?
Complete the following nuclear equations and identify which type of nuclear decay it is.
90
7.
Sr  90
Y + ____
This is ___________________________________.
38
39
17
8.
F  17
O + ____
This is ___________________________________.
9
8
9.
222
Rn
86
 218
Po + ____
84
10.
18
F + _____
9
11.
235
U
92
12.
118
Xe
54
 _______ + _____
13.
204
Sr
84
+
 18
O
8
 42He + ____
0
e
−1
 ____
This is ___________________________________.
This is ___________________________________.
This is ___________________________________.
This is positron emission.
This is ___________________________________.
Radioactivity & Half-Lives
14. One of the radioactive nuclides formed in nuclear power plants is hydrogen-3, called tritium, which has a halflife of 12.26 years. How long before a sample decreases to 1/8 of its original amount?
15. Uranium-238 is one of the radioactive nuclides sometimes found in soil. It has a half-life of 454 years. What
percentage of a sample is left after 2270 years?
16. Cesium-133, which is used in radiation therapy, has a half-life of 30 years. What was the size of the original
sample if after 120 years you now have 16.0 grams?
17. Phosphorus-32, which is used for leukemia therapy, has decayed to 1/16th of its original amount in 42.9 days.
What is the half-life of phosphorous-32?
18. Iodine has a half-life of 8.07 days. Assuming you start with 90.5 grams, how much of the sample (in mg) would
you have left after 24.21 days?
Bohr Model Diagrams
In the Bohr model diagrams show below, indicate the number of protons (p) and neutrons (n) in the nucleus of each atom.
Write the number of electrons (e) on each energy level. Not all energy levels will be used for every element.
19.
(a.)
silicon-30
(b.)
calcium-41
Electromagnetic Spectrum
20.
List the seven colors of the visible spectrum from shortest to longest wavelength.
__________________________________________________________________________________________
21.
What is the wavelength range of visible light? _____________ nm to ______________ nm.
22.
Draw your interpretation of a long wavelength (above the time frame) and a short wavelength (below the time
frame). Indicate which has higher frequency and higher energy.

23.
10 second time frame

(a) Which has a longer wavelength, orange or blue? _____________________________
(b) Which has a lower frequency, green or red? _________________________________
(c) Which has more energy, indigo or yellow? __________________________________
Quantum Mechanics
Explain each of the following rules or terms associated with quantum mechanics.
24.
Hund’s Rule
__________________________________________________________
25.
Aufbau Principle
__________________________________________________________
26.
Pauli Exclusion Principle
__________________________________________________________
27.
Heisenberg’s Uncertainty Principle
__________________________________________________________
28.
orbital
__________________________________________________________
29.
identify the three (of the four) quantum numbers
_____________________________________________
Orbital Diagrams
Draw the orbital diagrams (boxes and arrows) for each of the following elements.
30.
silicon
31.
zinc
Electron Configuration
32.
Identify the element described by each electron configuration.
(a.)
1s22s22p63s2
_________________
(b.)
1s22s22p63s23p64s23d104p65s24d3
_________________
(c.)
1s22s22p63s23p64s23d8
_________________
(d.)
[Kr] 5s24d6
_________________
(e.)
[Ar]4s23d104p4
_________________
Electron Configuration Continued
33.
Write the full electron configuration for the following atoms/ions (do NOT use the Noble Gas shortcut method).
(a.)
P
____________________________________________________________________________
34.
(b.)
Y
____________________________________________________________________________
(c.)
Ca+2
____________________________________________________________________________
(d.)
Br-
____________________________________________________________________________
Write the Noble Gas (shortcut) electron configuration for each of the following.
(a.)
Te
______________________________________________________________________________
(b.)
Sb
______________________________________________________________________________
(c.)
Bi
______________________________________________________________________________
Relating Bohr’s Diagram and Electron Configurations to the Quantum Numbers
35.
Which quantum number tells you the main energy level? _______
36.
In the atom, 1s22s22p4 – what is the highest every level that holds an electron? _______
37.
How many orbitals are in the p-sublevel? ________ How many electrons? ________
38.
How many orbitals are in the d-sublevel? ________ How many electrons? ________
39.
Which quantum mechanical principle states that (choose from Pauli Exclusion Principle, Aufbau Principle, and
Hund’s Rule):
(a) electrons will fill orbitals from lowest to highest energy? _________________________
(b) no two electrons can have the same set of quantum numbers? __________________________
(c) electrons will avoid pairing in an orbital if an orbital of equal energy is available? (the sharing rule) _________
40.
How many electrons can be accommodated in each of the following:
(a) one d orbital _______
(b) a set of f orbitals _______
(d) the 7s orbital ______
(c) the n = 4 shell _______
(e) one p orbital ______
Important Vocabulary & Concepts to review
Define the following words
Trajectory
______________________________________________________________________________
quantum
______________________________________________________________________________
entail
______________________________________________________________________________
valence electrons
________________________________________________________________________
frequency
______________________________________________________________________________
Wavelength
______________________________________________________________________________
Explain the following concepts (you can use words and pictures)
1. Nuclear decay
2. Radioactivity
3. Radioactive particle
4. Half-Life
5. Fission
6. Fusion
7. Electron orbital diagram
8. Electron configuration
9. Bohr model of the atom
10. The relationship between wavelength, frequency and energy
11. The relationship between energy levels, sublevels and orbitals
12. The relationship between an element’s electron configuration & its position on the periodic table