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Date: ___________________

Unit 3 Review Packet

Subatomic Particles and the Nuclear Atom

1. Know the scientists and their contributions to atomic theory.

|Scientist’s Name |Contribution |Experiment |

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2. What particles make up the mass of an atom? __________________________

3. What are the results and conclusions of the gold foil experiment?

a. Result 1: _________________________________________________

Conclusion 1: _____________________________________________

b. Result 2:__________________________________________________

Conclusion 2: _____________________________________________

4. Draw and label a diagram of each atomic model below:

a) Plum Pudding Model

b) Nuclear Atomic Model

5. Complete the following table of proton, electron, and neutron characteristics:

|Particle |Symbol |Location |Charges |Mass |

|Proton | | | | |

| |n0 | | | |

| | | | |0amu |

How Atoms Differ

For each statement below, write true or false:

_________ 1. The number of neutrons in an atom is referred to as its atomic number

_________ 2. The periodic table is arranged by increasing atomic number

_________ 3. The number of protons in an atom identifies it as an atom of a particular element

_________ 4. In a neutral atom, the atomic number is equal to the number of electrons

_________ 5. The number of neutrons comes from subtracting the mass number from the atomic number

Answer the following questions:

6. Lead has an atomic number of 82. How many protons and electrons does lead have? _______________

7. Oxygen has 8 electrons. How many protons does oxygen have? __________

8. Zinc has 30 protons. What is its atomic number? ____________

9. Complete the following chart:

|Symbol |Protons |Neutrons |Electrons |Mass Number |Atomic Number |

|Ca | | | | | |

|Sr | | | | | |

|As | | | | | |

Determine the number of protons, electrons, and neutrons for each isotope described below:

10. As isotope has an atomic number of 19 and a mass number of 39:

a. Protons: _________

b. Electrons: ________

c. Neutrons: ________

11. An isotope has 14 electrons and a mass number of 28:

a. Protons: _________

b. Electrons: ________

c. Neutrons: ________

Write each isotope below in symbolic notation. Use the periodic table to determine the atomic number of each isotope:

12. Neon-22 _______________

13. Cesium-133 _____________

Circle the letter of the choice that best completes the statement:

14. The mass of an electron is:

a) Smaller than the mass of a proton

b) Smaller than the mass of a neutron

c) A tiny fraction of the mass of an atom

d) All of the above

15. The atomic mass of an atom is usually not a whole number because it accounts for:

a) Only the relative abundance of the atom’s isotopes

b) Only the mass of each of the atom’s isotopes

c) The mass of the atom’s electrons

d) Both the relative abundance and the mass of each of the atom’s isotopes

Isotopes:

1. Calculate the average atomic mass of the element described below. Then, use the periodic table to identify the unknown (X) element.

|Isotope |Mass (amu) |Percent Abundance |

|63X |62.930 |69.17 |

|65X |64.928 |30.83 |

2. Element Y exists in three isotopic forms. The isotopic mixture consists of 15.0% 21X, 65.0% 22X, and 20.0% 23X. What is the average mass of this element?

3. Element X exists in three isotopic forms. The isotopic mixture consists of 10.0% 10X, 20% 11X, and 70% 12X. What is the average atomic mass of this element?

Alpha and Beta Decay:

1. What is the symbol for alpha decay? ________

2. What is the symbol for beta decay? ________

3. 23090Th ( 22688Ra + _________

4. 21484Po ( 21082Pb + _________

5. 22286Rn ( ________ + 42He

Unstable Nuclei and Radioactive Decay

Complete the following table of the characteristics of alpha, beta, and gamma radiation:

|Radiation Type |How does the nucleus change? |Symbol |Charge |

|Alpha | | | |

| | | | |

| | | | |

1. What is is the difference between fission and fusion?

Unit 2 Review:

Convert the following numbers into scientific notation:

1. 132,000,000 ___________________

2. 565.45 ___________________

3. 0.000481 ___________________

4. 0.0167 ___________________

5. 1.00865 ___________________

Convert the following into standard notation:

1. 1.56 x 104 ___________________

2. 7.86 x 10-6 ___________________

3. 3.4211 x 100 ___________________

4. 8.003 x 10-3 ___________________

5. 2.15 x 103 ___________________

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