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Period 1 Chemistry - Chapter 3 Prep-Test

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 
Who first recognized that the ratio of the number of atoms that combine is the same as the ratio of the masses that combine?
a.
Jons Berzelius
c.
John Dalton
b.
Edward Morley
d.
Jon Newlands
 

 2. 
Because most particles fired at metal foil passed straight through, Rutherford concluded that
a.
atoms were mostly empty space.
c.
electrons formed the nucleus.
b.
atoms contained no charged particles.
d.
atoms were indivisible.
 

 3. 
Rutherford fired positively charged particles at metal foil and concluded that most of the mass of an atom was
a.
in the electrons.
c.
evenly spread throughout the atom.
b.
concentrated in the nucleus.
d.
in rings around the atom.
 

 4. 
The mass of a neutron is
a.
about the same as that of a proton.
c.
double that of a proton.
b.
about the same as that of an electron.
d.
double that of an electron.
 

 5. 
The nucleus of most atoms is composed of
a.
tightly packed protons.
c.
tightly packed protons and neutrons.
b.
tightly packed neutrons.
d.
loosely connected protons and electrons.
 

 6. 
Protons have
a.
negative charges.
c.
no charges.
b.
an attraction for neutrons.
d.
no mass.
 

 7. 
The charge on the electron cloud
a.
prevents compounds from forming.
b.
balances the charge on the nucleus.
c.
attracts electron clouds in other atoms to form compounds.
d.
does not exist.
 

 8. 
The smallest unit of an element that can exist either alone or in combination with other such particles of the same or different elements is the
a.
electron.
c.
neutron.
b.
proton.
d.
atom.
 

 9. 
Atoms of the same element that have different masses are called
a.
moles.
c.
nuclides.
b.
isotopes.
d.
neutrons.
 

 10. 
Isotopes of an element contain different numbers of
a.
electrons.
c.
neutrons.
b.
protons.
d.
nuclides.
 

 11. 
The total number of protons and neutrons in the nucleus of an atom is its
a.
atomic number.
c.
mass number.
b.
Avogadro constant.
d.
number of neutrons.
 

 12. 
As the mass number of the isotopes of an element increases, the number of protons
a.
decreases.
b.
increases.
c.
remains the same.
d.
doubles each time the mass number increases.
 

 13. 
The average atomic mass of an element depends on both the masses of its isotopes and each isotope's
a.
atomic number.
c.
relative abundance.
b.
radioactivity.
d.
mass number.
 

 14. 
What is the atomic number for aluminum?
a.
13
c.
26.98
b.
14
d.
26.9815
 

 15. 
A neutral atom of silicon contains___________ .
a.
14 electrons.
c.
16 electrons.
b.
28.09 electrons.
d.
38 electrons.
 

 16. 
An atom of potassium has 19 protons and 20 neutrons. What is its mass number?
a.
19
c.
39
b.
20
d.
10
 

 17. 
Ag-109 has 62 neutrons. The neutral atom has
a.
40 electrons.
c.
53 electrons.
b.
47 electrons.
d.
62 electrons.
 

 18. 
Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils, has
a.
6 neutrons.
c.
10 neutrons.
b.
8 neutrons.
d.
14 neutrons.
 

 19. 
Silicon-30 contains 14 protons. It also contains
a.
16 electrons.
c.
30 neutrons.
b.
16 neutrons.
d.
44 neutrons.
 

 20. 
Mendeleev's table was called periodic because the properties of the elements
a.
showed no pattern.
b.
occurred at repeated intervals called periods.
c.
occurred at regular time intervals called periods.
d.
were identical.
 

 21. 
What are the elements with atomic numbers from 58 to 71 in the periodic table called?
a.
the lanthanide elements
c.
the actinide elements
b.
the noble gases
d.
the alkali metals
 

 22. 
Argon, krypton, and xenon are
a.
alkaline earth metals.
c.
actinides.
b.
noble gases.
d.
lanthanides.
 

 23. 
In the modern periodic table, elements are ordered according to
a.
decreasing atomic mass.
c.
increasing atomic number.
b.
Mendeleev's original design.
d.
the date of their discovery.
 

 24. 
To which group do lithium and potassium belong? Refer to your periodic table.
a.
alkali metals
c.
halogens
b.
transition metals
d.
noble gases
 

 25. 
Refer to your periodic table. To which group do fluorine and chlorine belong?
a.
alkaline-earth metals
c.
halogens
b.
transition elements
d.
actinides
 

 26. 
What does the number 84 in the name krypton-84 represent?
a.
the atomic number
c.
the sum of the protons and electrons
b.
the mass number
d.
twice the number of protons
 

 27. 
mc027-1.jpg

How many neutrons are found in this isotope of Carbon?
a.
6
c.
14
b.
12
d.
8
 

 28. 
Two isotopes of a new element, Dontpanicium (Dpg), was discovered in the back hills of Whittier.  One isotope had a mass of 255 and the other as mass of 261.  Dpg-255 has a relative abundance of 35% and Dpg-261 has a relative abundance of 65%.  What is the average atomic mass of Dpg?
a.
256.9
c.
258.9
b.
257.9
d.
259.9
 

 29. 
The following data was collected from a student’s Isotopes of Pennium Lab.

Number of Pre-‘82 Pennies (relative abundance)
12 (60%)
Number of Post-‘82 Pennies (relative abundance)
8 (40%)
Ave. Atomic Mass of Pre-‘82 Pennies
3.00
Ave. Atomic Mass of Post-‘82 Pennies
2.50

Calculate the Ave. Atomic Mass of this sample of Pennium using the following equation:

Ave. Atomic Mass of Pe =
(relative abundance of pre-‘82 pennies x Ave. At. Mass Pre-‘82 Pennies) + (relative abundance of post-‘82 pennies x Ave. At. Mass of post-‘82 pennies)
a.
2.50
c.
2.80
b.
3.00
d.
2.60
 

 30. 
Two isotopes of a new element (Ma) recovered from Mars have mass numbers of 130 and 132. Ma-130 has a relative abundance of 20% while Ma-132 has a relative abundance of 80%. What is the Average Atomic Mass of Ma?
a.
130.6
c.
131.6
b.
129.6
d.
132.6
 

Matching
 
 
Match each item with the correct statement below.
a.
proton
d.
electron
b.
nucleus
e.
neutron
c.
atom
 

 31. 

 the smallest particle of an element that retains the properties of that element
 

 32. 

 a positively charged subatomic particle
 

 33. 

 a negatively charged subatomic particle
 

 34. 

 a subatomic particle with no charge
 

 35. 

 the central part of an atom, containing protons and neutrons
 



 
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