Name: __________________
Honors Chemistry
Chapter 2 Review
1. What are the four major points in Dalton’s atomic theory?
2. Why did Rutherford conclude that an atom’s nucleus has a positive charge instead of a negative charge?
Summarize the conclusions that Rutherford’s team made about the structure of an atom. Draw and label
his apparatus.
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3. (7pts) From the information below, calculate the weighted average atomic mass of the element X. Show
work and round your answer to the tenth
Isotope
% Abundance
Mass
221
X
74.22
220.9
220
X
12.78
220.0
218
X
13.00
218.1
4. (39pts) Complete the following table:
Symbol
Name
Atomic
Mass
Number
Number
Number
Number
Number
of protons
of
of electrons
neutrons
238
92U
Co-58
28
58
33
85
40
37Rb
84
60
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2
True/False (14pts)
1. ____Group VIIIA of the periodic table contains elements that are gaseous
nonmetals
2. ____The conservation of mass law states that matter can neither be created nor
destroyed during a chemical reaction.
3. ____Two isotopes of the same element differ only in the number of neutrons
found in the nucleus
4. ____All the isotopes of the nonmetal series elements are radioactive
5. ___Most of the elements on the periodic table are metals
Part B Matching (16pts): Each answer is used only once
Column A
Column B
1. _____The number of protons in the nucleus of an element
a. Germanium
2. _____Exists in all three states of matter at room temperature
b. mass number
3. _____The total number of protons and neutrons in the
c. atomic number
nucleus of an atom.
4. _____A semi conductor
d. non-metals
5. _____Atoms with the same number of protons but
e. nucleus
different numbers of neutrons.
6.____A positively charged atomic particle
f. halogens
7. ____The central core of an atom, composed of
g. proton
Protons and neutrons.
8.____Exists as diatomic molecules
h. isotopes
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1.
Which two of Dalton’s postulates aren’t exactly true? Explain why.
2. (3pts) Explain the significance of Thomson’s experiment. Draw and label
Thomson’s experiment
3. Name the following elements and tell which family they belong too:
a. V______________________
Family__________________
b. Pb______________________
Family__________________
c. I_______________________
Family__________________
d. F_______________________
Family__________________
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e. Au______________________
Family__________________
f. Mo______________________
Family__________________
g. Al_______________________
Family__________________
h. H_______________________
Family__________________
i. Cr______________________
Family__________________
j. Fe_______________________
Family__________________
k. Na_______________________
Family__________________
4. (18 pts) Write the symbols for the following elements and tell which families they
belong too.
l. Co_______________________
Family____________________
m. K_________________________
Family_____________________
n. Arsenic_____________________
Family______________________
o. Magnesium__________________________
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Family_____________________________
p. Germanium_________________________
Family_______________________
q. Fluorine___________________________
Family______________________________
r. Iron_______________________________
Family_____________________________
s. Carbon____________________________
Family_____________________________
t. Lithium____________________________
Family_____________________________
5. Why do elements in the same family generally have similar properties?
6. Write the names of the following compounds:
a. SnS2 _____________________________
b. Pb3(PO4)2_________________________
c. NaNO3___________________________
d. H2S(aq)____________________________
e. CuI2______________________________
f. N2O7_____________________________
g. PCl5______________________________
h. Al5O7 ____________________________
i. S5Br6 ____________________________
j. CCl4 _____________________________
7. Write the formulas for the following compounds:
a. Beryllium oxide____________________
b. Dinitrogen tetraoxide________________
c. Potassium sulfide___________________
d. Sulfuric acid____________________
e. Calcium hydroxide________________
f. Hydroiodic acid_________________
g. Sodium acetate_________________
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h. Carbon dioxide_________________
i. Sulfur diiodide_________________
j. Iron (III) oxide_________________
1. Which one of the following does not occur as diatomic molecules in elemental
form?
a. Oxygen
b. Nitrogen
c. Sulfur
d. Hydrogen
e. Bromine
2. Which one of the following is most likely to lose electrons when forming an ion?
a. F
b. P
c. Rh
d. S
3. Which one of the following is not an ionic compound?
a. PCl5
b. MoCl6
c. RbCl
d. PbCl2
4. What is the correct name for PCl3:
a.
b.
c.
d.
Potassium chloride
Phosphorus trichloride
Phosphorus (III) chloride
Monophosphorus trichloride
5. What is the formula for the salt formed from Ca+2 and PO43- is
a.
b.
c.
d.
e.
CaPO4
Ca2PO12
Ca2(PO4)3
Ca2PO4
Ca3(PO4)2
6. Which one of the following is hydrochloric acid?
a.
b.
c.
d.
HCl
HClO4
HClO
HClO2
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7. The atomic number indicates ___________.
a. the number of neutrons in a nucleus
b. the total number of neutrons and protons in a nucleus
c. the number protons or electrons in a neutral atom
d. the number of atoms in 1 g of an element
8. Elements in Group 8A are known as the ___________.
a. Chalcogens
b. alkali metals
c. noble gases
d. alkaline earth metals
9. When a metal and a nonmetal react, the _______ tends to lose electrons and
the_____________ tends to gain electrons.
a. metal, metal
b. metal, nonmetal
c. nonmetal, metal
d. None of the above, these elements share electrons.
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