1. Bell Work 1 / Atomic Particles Table
Symbol
Charge
Relative Mass
Actual Mass
Location
Protons
1.67 x10-24 N0
9.11 x 10-28

2. Bell Work 1 / Atomic Particles Table
Key
Particle
Symbol
Charge
Relative Mass
Actual Mass
Location
Protons P+ +1 1
1.67 x10-24
Nucleus
Neutron N0
Electron e- -1
1/2000
9.11 x 10-28
Energy Levels

3. Bell Work 2 / Atomic Particles
1. What are the three parts of an atom and what are their charges?
N -3
Use the nucleic symbol for Nitrogen above to determine:
Number of protons
Number of electrons
Number of neutrons
3. Is the nucleic symbol considered an Atom, an Ion, or an isotope? Explain your answer

4. Bell Work 2 / Atomic Particles
1. What are the three parts of an atom and what are their charges?
 Protons = Positive, Electrons = negative Neutrons = neutral
N -3
Use the nucleic symbol for Nitrogen above to determine:
Number of protons = 7
Number of electrons = 10
Number of neutrons = 8 
3. Is the nucleic symbol considered an Atom, an Ion, or an isotope? Explain your answer. Ion, are defined by having a charge. In this example nitrogen has 10 electrons and 7 protons, therefore it contains a Negative 3 charge

5. Bell Work 3 / Table of Sub-Atomic Particles
Fill in the following table:
Substance
Symbol
Atomic
Number
Mass
Number of
Protons
Neutrons
Electrons
Helium He 2 4
Magnesium
Ion
Mg+2 12
Zinc Zn 30 65
Bromine
Br-1 80 36
Aluminum
Al+3 13 14
Uranium U
146 92

6. Bell Work 3 / Table of Sub-Atomic Particles
Fill in the following table: KEY
Substance
Symbol
Atomic
Number
Mass
Number of
Protons
Neutrons
Electrons
Helium He 2 4
Magnesium
Ion
Mg+2 12 24 10
Zinc Zn 30 65 35
Bromine
Br-1 80 45 36
Aluminum
Al+3
13  27 13 14
Uranium U 92
238 
146

7. Bell Work Day 4 / Nucleic Exprssion
1. Write the Nucleic Expression and PEN number for the following elements.
2. Then draw the Bohr’s diagram
Lithium b. Oxygen
c. Sodium d. Sulfur

8. Bell Work Day 4 / Nucleic Exprssion
1. Write the Nucleic Expression and PEN number for the following elements.
2. Then draw the Bohr’s diagram
Lithium b. Oxygen
c. Sodium d. Sulfur

9. Bell Work 5 / Borh’s Hydrogen Model
A. An electron transitions from n=5 to n=2. What is considered the electrons excited state and its ground state? What is the wavelength?
B. An electron transitions from n=4 to n=1. What wavelength of EM radiation. What is the series of the wavelength?
C. Which transition (A or B) released a wave with more energy? Defend your answer by comparing the wavelength and frequency of the 2 waves released.

10. Bell Work 6/ Average Atomic Mass
1. In a sample of 400 lithium atoms, it is found that 30 atoms are lithium-6 (6.015 g/mol) and 370 atoms are lithium-7 (7.016 g/mol). Calculate the average atomic mass of lithium.

11. Bell Work 7 / Average Atomic Mass
Magnesium has three isotopes: Mg-24, Mg-25, and Mg-26. They occur naturally with percentage abundance of 78.6 %, 10.1 % and 11.3 % respectively. The exact masses of these isotopes are , , and What is the average atomic mass of the three isotopes?

12. Bell Work 9 / Mass Defect
1. Find the mass defect of a copper-63 nucleus if the actual mass of a copper-63 nucleus is amu. Then determine the nuclear binding energy.

13. Bell Work 9 / Atomic Models
Place the following men in order that they contributed to the modern atomic model and then match the term that goes with each.
1. JJ Thomson a. atom is indivisible
2. John Dalton b. Cathode Ray Tube
3. Democritus c. Solar System Model
4. Neils Bohr d. Plum Pudding Model
5. Earnest Rutherford e. First Atomic Model

14. Bell Work 8 / Flame Test
What supplied the energy to excite the electrons?
2. Do you think more than one electron was being excited in the metal ions? Explain?

15. Bell Work 10 / Mass Defect
1. If you calculate the mass of an atom based on the number of protons, electrons, and neutrons you will get an number slightly larger than what the actual mass is. Why is there a slight difference in the calculated mass and actual mass of an atom?

16. Bell Work 10 / Mass Defect
1. If you calculate the mass of an atom based on the number of protons, electrons, and neutrons you will get an number slightly larger than what the actual mass is. Why is there a slight difference in the calculated mass and actual mass of an atom?

17. Bell Work 10 / Balancing Nuclear Equations
Balance the following nuclear equations: 3719K → _____ + 0+1e 24195Am + 42He → 210n + _____ 23592U + 10n → ____10n Ba Kr 4219K → 0-1e + _____ _____ → 42He Tl 2713Al + _____ → 2411Na + 42He 23994Pu → 42He + _____

18. Bell Work 11 / ½ Life Problem
1. Phosphorus-32 is a commonly used radioactive nuclide in biochemical research, particularly in studies of nucleic acids. The half-life of P-32 is 14.3 days. If you start with a sample of P-32 with a mass of 175mg. What mass of P-32 will remain after 57.2 days? 2. The half-life of molybdenum – 99 is 2.4 days. How much of a 2.50 mg sample of will remain after hours?

19. Bell Work 12 / Nuclear Fusion and Fission
1. What are the 6 Nuclear Emissions? 2. What are the two types of nuclear reactions? 3. Which type of reaction do we use in our Nuclear Power plants? 4. What are some of the major problems with using nuclear power plants to generate electricity?

20. Bell Work 12 / Nuclear Fusion and Fission
1. What are the 6 Nuclear Emissions?
1. Alpha 2. Beta 3. Gamma
4. Positron 5. Neutron 6. Proton
2. What are the two types of nuclear reactions?
1. Fission Reaction 2. Fusion Reaction
3. Which type of reaction do we use in our Nuclear Power plants?
Fission Reaction
4. What are some of the major problems with using nuclear power plants to generate electricity?
Fission reactions produce dirty energy which means it produces a lot of gamma radiation. Then you must store this radiation for 100’s of years.

21. Bell Work 13 / Atomic Structure Review
What happens to the atom if you change the number of protons?
2. What happens to the atom if you gain or lose electrons?
3. What happens to the atom if the number of neutrons change?
4. Chlorine- 36 has how many neutrons?

22. Bell Work Extra / Nuclear Chemistry
Particle
Symbol
Charge
Relative Mass
Penetrating Power
Alpha
Beta
Gamma