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Chemistry - Ch 3 Prep-Test

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

 1. 
Who was the schoolmaster who studied chemistry and proposed an atomic theory?
a.
John Dalton
c.
Robert Brown
b.
Jons Berzelius
d.
Dmitri Mendeleev
 

 2. 
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
 

 3. 
According to Dalton's atomic theory, atoms
a.
of different elements combine in simple whole-number ratios to form compounds.
b.
can be divided into protons, neutrons, and electrons.
c.
of all elements are identical in size and mass.
d.
can be destroyed in chemical reactions.
 

 4. 
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.
 

 5. 
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.
 

 6. 
A positively charged particle with mass 1.673 ´ 10–24 g is a(n)
a.
proton.
c.
electron.
b.
neutron.
d.
positron.
 

 7. 
Which part of an atom has a mass approximately equal to 1/2000 of the mass of a common hydrogen atom?
a.
nucleus
c.
proton
b.
electron
d.
electron cloud
 

 8. 
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.
 

 9. 
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.
 

 10. 
Protons have
a.
negative charges.
c.
no charges.
b.
an attraction for neutrons.
d.
no mass.
 

 11. 
Most of the volume of an atom is occupied by the
a.
nucleus.
c.
electron cloud.
b.
nuclides.
d.
protons.
 

 12. 
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.
 

 13. 
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.
 

 14. 
Atoms of the same element that have different masses are called
a.
moles.
c.
nuclides.
b.
isotopes.
d.
neutrons.
 

 15. 
Isotopes of an element contain different numbers of
a.
electrons.
c.
neutrons.
b.
protons.
d.
nuclides.
 

 16. 
All isotopes of hydrogen contain
a.
one neutron.
c.
one proton.
b.
two electrons.
d.
two nuclei.
 

 17. 
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.
 

 18. 
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.
 

 19. 
Atoms of the same element can differ in
a.
chemical properties.
c.
atomic number.
b.
mass number.
d.
number of protons and electrons.
 

 20. 
The abbreviation for atomic mass unit is
a.
amu.
c.
a.
b.
mu.
d.
m.
 

 21. 
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.
 

 22. 
A single atom of an isotope does not have a(n)
a.
relative atomic mass.
c.
mass number.
b.
atomic number.
d.
average atomic mass.
 
 
nar001-1.jpg
 

 23. 
What is the atomic number for aluminum from the figure above?
a.
13
c.
26.98
b.
14
d.
26.9815
 

 24. 
In the figure above, a neutral atom of silicon contains
a.
14 electrons.
c.
16 electrons.
b.
28.09 electrons.
d.
38 electrons.
 

 25. 
An atom of potassium has 19 protons and 20 neutrons. What is its mass number?
a.
19
c.
39
b.
20
d.
10
 

 26. 
Ag-109 has 62 neutrons. The neutral atom has
a.
40 electrons.
c.
53 electrons.
b.
47 electrons.
d.
62 electrons.
 

 27. 
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.
 

 28. 
Silicon-30 contains 14 protons. It also contains
a.
16 electrons.
c.
30 neutrons.
b.
16 neutrons.
d.
44 neutrons.
 

 29. 
Neon-22 contains 12 neutrons. It also contains
a.
12 protons.
c.
22 electrons.
b.
22 protons.
d.
10 protons.
 

 30. 
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.
 

 31. 
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
 

 32. 
Argon, krypton, and xenon are
a.
alkaline earth metals.
c.
actinides.
b.
noble gases.
d.
lanthanides.
 

 33. 
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.
 

 34. 
The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in this group is
a.
4.
c.
11.
b.
10.
d.
18.
 
 
nar002-1.jpg
 

 35. 
To which group do lithium and potassium belong? Refer to the figure above.
a.
alkali metals
c.
halogens
b.
transition metals
d.
noble gases
 

 36. 
Refer to the figure above. To which group do fluorine and chlorine belong?
a.
alkaline-earth metals
c.
halogens
b.
transition elements
d.
actinides
 

 37. 
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
 

 38. 
How many valence electrons are in an atom of phosphorus?
a.
2
c.
4
b.
3
d.
5
 

 39. 
How many valence electrons are in an atom of magnesium?
a.
2
c.
4
b.
3
d.
5
 

 40. 
What is the charge on the strontium ion?
a.
2–
c.
1mc040-1.jpg
b.
1–
d.
2mc040-2.jpg
 

 41. 
Which of the following elements does NOT form an ion with a charge of 1mc041-1.jpg?
a.
fluorine
c.
potassium
b.
hydrogen
d.
sodium
 

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

 42. 

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

 43. 

 a positively charged subatomic particle
 

 44. 

 a negatively charged subatomic particle
 

 45. 

 a subatomic particle with no charge
 

 46. 

 the central part of an atom, containing protons and neutrons
 
 
Match each item with the correct statement below.
a.
mass number
d.
atomic mass
b.
atomic mass unit
e.
isotope
c.
atomic number
 

 47. 

 atoms with the same number of protons, but different numbers of neutrons in the nucleus of an atom
 

 48. 

 the total number of protons and neutrons in the nucleus of an atom
 

 49. 

 the number of protons in the nucleus of an element
 

 50. 

 the weighted average of the masses of the isotopes of an element
 

 51. 

 one-twelfth the mass of a carbon atom having six protons and six neutrons
 



 
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