Name: 
 

Chemistry -- Chapters 4/5:  Atoms & the Periodic Table


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

 1. 
Atoms have no electric charge because they
a.
have an equal number of charged and noncharged particles.
b.
have neutrons in their nuclei.
c.
have an equal number of electrons and protons.
d.
have an equal number of neutrons and protons.
 

 2. 
Valence electrons determine an atom’s
a.
mass.
c.
electric charge.
b.
chemical properties.
d.
period.
 

 3. 
A mole is an SI base unit that describes the
a.
mass of a substance.
c.
volume of a substance.
b.
amount of a substance.
d.
electric charge of a substance.
 

 4. 
If the atomic mass of carbon is 12 u, 1 mole of pure carbon will have a mass of
a.
6 g.
c.
12 g.
b.
6 mol.
d.
12 mol.
 

 5. 
You have 85.5 g of fluorine, which has a molar mass of approximately 19 g/mol. How many moles of fluorine do you have?
a.
4.5 mol
c.
45 mol
b.
19 mol
d.
85 mol
 

 6. 
A subatomic particle that has a negative charge is called a(n)
a.
molecule.
c.
element.
b.
electron.
d.
compound.
 

 7. 
Which of the following statements not true?
a.
Protons have a positive charge.
b.
A nucleus has a positive charge.
c.
Neutrons have no charge.
d.
Neutrons have a negative charge.
 

 8. 
What is an atom’s nucleus made of?
a.
protons and neutrons
c.
only neutrons
b.
only protons
d.
anodes
 

 9. 
Avogadro’s number is useful for
a.
counting atoms.
c.
locating an atom’s electrons.
b.
counting large objects.
d.
None of the above
 

 10. 
The charge of an atom is
a.
positive.
c.
negative.
b.
neutral.
d.
unbalanced.
 

 11. 
An iron atom has an atomic mass of 56. Its atomic number is 26. How many neutrons does the iron atom have?
a.
30
c.
26
b.
56
d.
82
 

 12. 
How much effect do commonly found isotopes have on the average atomic mass of an element?
a.
less than rarely found isotopes
c.
same as rarely found isotopes
b.
no effect on atomic mass
d.
more than rarely found isotopes
 

 13. 
An element’s atomic number is equal to its number of
a.
protons.
c.
valence electrons
b.
neutrons.
d.
protons and neutrons.
 

 14. 
Two different isotopes of an element have different
a.
numbers of neutrons.
c.
atomic numbers.
b.
numbers of protons.
d.
numbers of electrons.
 

 15. 
A sodium atom, which has 11 electrons, has _____ electron(s) in its third energy level.
a.
0
c.
2
b.
1
d.
8
 

 16. 
Which of the following is not a type of orbital?
a.
s
c.
p
b.
d
d.
x
 

 17. 
An electron jumps to a new energy level when
a.
the atom becomes charged.
b.
the atom becomes unstable.
c.
the electron’s location is pinpointed.
d.
the atom gains or loses energy.
 

 18. 
The number of energy levels filled in an atom is determined by
a.
protons.
c.
neutrons.
b.
electrons.
d.
photons.
 

 19. 
Which statement about the atom’s nucleus is correct?
a.
The nucleus is made of protons and neutrons and has a negative charge.
b.
The nucleus is made of protons and neutrons and has a positive charge.
c.
The nucleus is made of electrons and has a positive charge.
d.
The nucleus is made of electrons and has a negative charge.
 

 20. 
Oxygen’s atomic number is 8. This means that an oxygen atom has
a.
eight neutrons in its nucleus.
b.
a total of eight protons and neutrons.
c.
eight protons in its nucleus.
d.
a total of eight neutrons and electrons.
 

 21. 
Which statement about an element’s average atomic mass is correct?
a.
It is determined by counting the number of isotopes in a sample of the element.
b.
It is equal to one-twelfth the mass of the most common isotope.
c.
It is a weighted average, so common isotopes have a greater effect than uncommon ones.
d.
It is based on an isotope’s charge, so negatively charged isotopes have a greater effect than positive ones.
 

 22. 
An atom’s mass number equals the number of
a.
protons plus the number of electrons.
b.
protons plus the number of neutrons.
c.
protons.
d.
neutrons.
 

 23. 
A unified atomic mass unit is equal to
a.
one-half the mass of a hydrogen atom.
b.
one-fourth the mass of a lithium atom.
c.
one-twelfth the mass of a carbon-12 atom.
d.
one-fifteenth the mass of a nitrogen-15 atom.
 

 24. 
Avogadro’s number is defined as the number of particles in
a.
one mole of a substance.
c.
one gram of a substance.
b.
one liter of a substance.
d.
one kilogram of a substance.
 

 25. 
Molar mass is defined as
a.
the number of particles in one mole of a substance.
b.
the SI base unit that describes the amount of a substance.
c.
the amount of a substance necessary to have a positive charge.
d.
the mass in grams of one mole of a substance.
 

 26. 
The order of elements in the periodic table is based on
a.
the number of protons in the nucleus.
b.
the electric charge of the nucleus.
c.
the number of neutrons in the nucleus.
d.
atomic mass.
 

 27. 
Atoms of elements that are in the same group have the same number of
a.
protons.
c.
valence electrons.
b.
neutrons.
d.
protons and neutrons.
 

 28. 
Which of the following elements is an alkali metal?
a.
calcium
c.
mercury
b.
magnesium
d.
sodium
 

 29. 
Semiconductors are elements that
a.
have large atomic masses but small atomic numbers.
b.
do not form compounds.
c.
can conduct heat and electricity under certain conditions.
d.
are extremely hard.
 

 30. 
Carbon and other nonmetals are found in which area of the periodic table?
a.
on the left-most side
b.
on the right side
c.
in the middle column of the periodic table
d.
in the bottom rows
 

 31. 
In Mendeleev’s periodic table, elements in each column had similar
a.
atomic masses.
c.
atomic numbers
b.
properties.
d.
symbols.
 

 32. 
Magnesium (Mg) is located to the right of sodium (Na) because Mg has
a.
fewer protons.
c.
no protons.
b.
no neutrons.
d.
more protons.
 

 33. 
As you move from left to right across the periodic table, elements
a.
become less metallic.
c.
have a lower atomic weight.
b.
have a lower atomic number.
d.
become more metallic.
 

 34. 
How was Mendeleev’s periodic table arranged?
a.
by increasing atomic mass
c.
by increasing atomic number
b.
by decreasing atomic mass
d.
by decreasing atomic number
 

 35. 
What is Mendeleev is known for?
a.
creating today’s atomic model
c.
publishing the first periodic table
b.
discovering protons
d.
discovering Mendelevium
 

 36. 
Mendeleev left gaps in his periodic table because
a.
the table was too small.
c.
the table was too full.
b.
protons belonged there.
d.
no known elements fit there.
 

 37. 
Each column of the periodic table is
a.
an element.
c.
an isotope.
b.
a group.
d.
a period.
 

 38. 
The periodic law states that elements that have similar properties appear
a.
to the left of each other.
c.
at every tenth element.
b.
to the right of each other.
d.
at regular intervals.
 

 39. 
As you move from up to down in a column of the periodic table, elements have
a.
fewer protons.
c.
a higher atomic number.
b.
a lower atomic number.
d.
a higher group number.
 

 40. 
What is the location of elements in the periodic table related to?
a.
color
c.
atomic weight
b.
number of neutrons
d.
electron arrangement
 

 41. 
Elements that belong to the same group have the same number of
a.
valence electrons.
c.
inner electrons.
b.
neutral electrons.
d.
total electrons.
 

 42. 
Because they differ in numbers of protons in their nuclei and in numbers of electrons in their filled inner energy levels, elements in a group
a.
have different charges.
c.
are very interactive.
b.
are not exactly the same.
d.
are inert.
 

 43. 
Atoms that gain or lose electrons are called
a.
metals.
c.
ions.
b.
nonmetals.
d.
isotopes.
 

 44. 
Elements that have one valence electron tend to
a.
be highly reactive.
c.
become charged.
b.
form ions.
d.
All of the above
 

 45. 
The three main groups of elements are metals, nonmetals, and
a.
inert gases.
c.
radioactive isotopes.
b.
alkali metals.
d.
semiconductors.
 

 46. 
Most elements are
a.
metals.
c.
metalloids.
b.
nonmetals.
d.
semiconductors.
 

 47. 
Most elements on the left side of the periodic table are
a.
semiconductors.
c.
nonmetals.
b.
metals.
d.
metalloids.
 

 48. 
Most nonmetals are
a.
brittle.
c.
metalloids.
b.
good conductors.
d.
shiny.
 

 49. 
Each element in an element family shares the same
a.
average atomic mass.
c.
number of valence electrons.
b.
number of protons.
d.
atomic number
 

 50. 
Elements in an element family have similar
a.
atomic symbols.
c.
atomic weights.
b.
atomic sizes.
d.
chemical properties.
 

 51. 
How do you know that potassium, an alkali metal, is highly reactive?
a.
It conducts heat.
c.
It is a soft and shiny metal.
b.
It conducts electricity.
d.
It has one valence electron.
 

 52. 
Which of the following is not true of noble gases?
a.
They are highly reactive.
c.
They belong to Group 18.
b.
They exist as single atoms.
d.
They are nonmetals.
 

 53. 
When can semiconductors conduct heat and electricity?
a.
under all conditions
c.
under some conditions
b.
under almost all conditions
d.
under no conditions
 

 54. 
The order of elements in the modern periodic table is based on an element’s
a.
atomic number.
c.
chemical symbol.
b.
name.
d.
atomic mass.
 

 55. 
Elements within the same group in the periodic table have similar properties because they have the same number of
a.
protons.
c.
ions.
b.
neutrons.
d.
valence electrons.
 

 56. 
Ionization refers to the process of
a.
changing from one period to another.
c.
turning lithium into fluorine.
b.
losing or gaining protons.
d.
losing or gaining electrons.
 

 57. 
Elements that share properties of both metals and nonmetals are called
a.
ions.
c.
semiconductors.
b.
periods.
d.
valences.
 

 58. 
Elements in a family often have a similar
a.
appearance.
c.
number of total electrons.
b.
atomic mass.
d.
number of total protons.
 

 59. 
Which statement about the alkali metals is correct?
a.
They are located in the left-most column of the periodic table.
b.
They are extremely nonreactive.
c.
They are usually gases.
d.
They form negative ions with a 1– charge.
 

 60. 
Which statement about noble gases is correct?
a.
They form compounds with very bright colors.
b.
They exist as single atoms rather than as molecules.
c.
They are highly reactive with both metals and nonmetals.
d.
They are extremely rare in nature.
 

 61. 
Group 18 noble gases are relatively inert because
a.
they readily form positive ions.
b.
they can have either a positive or a negative charge.
c.
their outermost energy level is missing one electron.
d.
their s and p orbitals are filled.
 

 62. 
Which element is a semiconductor?
a.
carbon
c.
sodium
b.
silicon
d.
uranium
 

 63. 
Mendeleev studied the properties of the elements and looked for
a.
electrons.
c.
patterns.
b.
ions.
d.
protons.
 

 64. 
As one moves from left to right across a period in the modern periodic table, elements become
a.
smaller.
c.
less metallic.
b.
lighter.
d.
more unlike each other.
 

 65. 
Elements that are found in the same group have the same number of
a.
protons.
c.
valence electrons.
b.
neutrons.
d.
protons and neutrons.
 

 66. 
A lithium ion is much less reactive than a lithium atom because it
a.
is much more massive.
c.
has a negative electric charge.
b.
has a filled outer s orbital
d.
has no charge.
 

 67. 
Metals tend to be
a.
gases.
c.
dull.
b.
good conductors of heat.
d.
brittle.
 

 68. 
Which is not a family of the periodic table?
a.
alkaline-earth metals
c.
halogens
b.
anions
d.
noble gases
 

 69. 
Alkali metals are extremely reactive because they
a.
have very small atomic masses.
b.
are not solid at room temperature.
c.
have one valence electron that is easily removed to form a positive ion.
d.
have two valence electrons that form compounds with calcium and magnesium.
 

 70. 
Most halogens form compounds by
a.
gaining an electron to form a negative ion
b.
losing an electron to form a positive ion.
c.
losing protons.
d.
joining with both calcium and carbon.
 

 71. 
Transition metals such as copper or tungsten form compounds by
a.
gaining electrons to form negative ions
b.
losing electrons to form positive ions.
c.
losing neutrons.
d.
changing shape and color.
 

 72. 
Silicon, a semiconductor, is often found in
a.
air.
c.
steel.
b.
computers.
d.
wood.