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Percoski
College Chemistry I
Name: __________________________________
MLC
Block: _____________Date: _______________________
Elements, Atoms and the Periodic Table – Test Review
1.
What effect did Democritus have on the theory of the atom? Was his theory consistent with modern atomic theories? How
did it differ?
2.
How did the Greek theories (Democritus and Aristotle) of matter compare to today’s? How do they contrast?
3.
Summarize the contributions of all historical figures that contributed to the modern structure of the atom.
4.
What are the rules that are used when writing symbols for elements? Write the symbols for Oxygen, Cobalt, Chromium,
Zirconium and Fluorine.
5.
Why do some symbols for atoms not represent or indicate the letters that are in its name. For example, why is gold’s symbol
Au?
6.
Define the following terms:
a. Electron
b. Neutron
c. Proton
d. Isotopes
e. Mass number
f. Atomic number
g. Nucleus
Percoski
7.
College Chemistry I
MLC
Are the following statements true or false? If the statement is false, rewrite it correctly.
a.
b.
c.
In his cathode ray tube experiments, J.J. Thompson obtained beams of different types of particles which bended
away from a positively charged piece of metal placed outside of the tube.
Thompson assumed that there must be negatively charged particles present because an isolated atom has no overall
charge.
In the chocolate chip cookie model of the atom, Thomson believed that atoms were composed of a mass of negative
charge with positively charged particles spread throughout the atom.
8.
What is Dalton’s atomic theory? Summarize each component of the theory.
9.
The three subatomic particles are protons, neutrons and electrons. Where do each fit into each other in relation to the rest of
an atom. Draw an example of an atom of Carbon.
10. Do the proton and neutron have exactly the same mass? How do the masses of the proton and neutron compare to an
electron? How do they identify an atom?
11. What is the notation of an atom that has 51 protons and a mass number of 108? What is this atom’s identity?
12. Are all atoms of the same element identical? If not, how are they different?
Percoski
College Chemistry I
MLC
13. Explain how Mendeleev contributed to the modern periodic table.
14. What are the three main sections of the periodic table? What is the separation of the sections?
15. What is the property that the periodic table uses to organize the elements? What happens to this property as elements change
across the periodic table?
16. Where are the metallic elements located on the periodic table? Are there more elements which are considered metallic or
non-metallic?
17. Explain what is meant by the periodic table of elements being “periodic.” What is the periodic change which is reported on
the table?
18. Calculate the average atomic mass of the following element: Show all of your work for credit.
Isotope
50
V
51
V
Mass Number
49.9472
50.9440
Natural Abundance (%)
0.250
99.750
Percoski
College Chemistry I
MLC
19. What is the average atomic mass of the elements, Chevroletium: Show all of your work for credit.
Isotope
132
Ch
135
Ch
137
Ch
Mass Number (amu)
131.86
134.92
136.28
Natural Abundance (%)
27.31%
61.35%
11.34%
20. How many protons and neutrons are contained in the nucleus of each of the following atoms? In an atom of each element,
how many electrons are present?
a.
41
22
Ti
b.
64
30
Zn
c.
76
32
Ge
21. When moving across the periodic table, all elements in a particular row have something in common. What is this row called?
What is the common characteristic of a row as it goes across the periodic table?