Name
Date
Period
TEST REVIEW - UNIT 2
Test Review: Atomic Theory, Atomic Structure, Isotopes, and Atomic Mass
1.
2.
3.
4.
5.
6.
Determine number of protons, neutrons, and electrons given charge, atomic number, and mass
number
Describe early models of the atom and how the theory has changed over time (focus on the
contributions of Dalton, Thomson, Rutherford, and Bohr).
Describe the two major experiments that contributed to the development of atomic theory
(Rutherford’s gold foil, Thomson’s cathode ray tube)
Calculate atomic mass using relative abundance and mass of isotopes
Determine which is the most abundant isotope from average atomic mass
Isotopic Notation
a. Calcium - 40
b.
40
20
Ca ion have
Practice Questions and Problems:
40
20
1.
How many protons does a dipositive
Ca ion have?
2.
How many electrons does a uninegative
3.
4.
How many neutrons does a Ca - 42 atom have? ____
Write the chemical configuration for an isotope with 10 neutrons, 10 electrons and a mass number of 12.
______
5.
What is the charge of a particle having 9 protons and 10 electrons?_____
6.
Explain in detail how a neutral atom becomes a cation or an anion?
______________________________________________________________________________________
______________________________________________________________________________________
7.
What is the definition of an atom?
______________________________________________________________________________________
______________________________________________________________________________________
8.
Fill in the following table:
Subatomic Particle
Mass (amu)
Proton
80
35
____
Br ion have? ____
Charge
Location
Symbol
Neutron
Electron
9. Atoms of the same element have the same number of ________________.
10. The modern periodic table is arranged in order of increasing ________________ _________________.
11. What three things determine the atomic mass of an element?
a. __________________________________________________________
b. __________________________________________________________
c. __________________________________________________________
12. Thomson is famous for his ________ ________ ______ experiment.
13. What is the significance of Thomson’s above experiment?
______________________________________________________________________________________
______________________________________________________________________________________
Name
Date
Period
14. Rutherford is famous for his ________ ________ experiment.
15. What is the significance of Rutherford’s above experiment?
______________________________________________________________________________________
______________________________________________________________________________________
______________________________________________________________________________________
16. Describe Bohr’s atomic model _____________________________________________________________
_____________________________________________________________________________________
17. What do isotopes of the same element have in common?
______________________________________________________________________________________
18. What do isotopes of the same element NOT have in common?
______________________________________________________________________________________
19. Write the chemical configuration for a particle with 19 protons and 18 electrons _______
20. An atom of neon has a mass number of 21. How many neutrons does it have? ________
21. What is the overall charge of an atom? ____
22. What kind of charge does the nucleus of an atom have? ____
23. In what way/s has Dalton’s Atomic Theory been disproved by modern day Atomic Theory?
______________________________________________________________________________________
______________________________________________________________________________________
24. According to the chemical configuration of this mercury atom determine:
a.
b.
c.
# of Protons _______
# of Neutrons ______
# of Electrons ______
201
Hg
80
Calculating Average Atomic Mass
Round to 3 decimal places.
25.
10B
(19.78%), 11B (80.22%)
Average Atomic weight =___________
26. Naturally occurring copper exists in two isotopic forms: Cu-63 and Cu-65. Which of them is the more
abundant isotope? Justify your answer.