Table of Contents
Elements and Their Properties
Section 1 • Metals
Section 2 • Nonmetals
Section 3 • Mixed Groups
Section
Metals
1
Properties of Metals
• In the periodic
table, metals
are elements
found to the
left of the stairstep line.
Section
Metals
1
Properties of Metals
• Metals usually have
common
propertiesthey are
good conductors of
heat and electricity,
and all but one are
solid at room
temperature.
Section
1
Metals
Properties of Metals
• Metals also reflect light. This is a property called
luster.
• Metals are malleable (MAL ee uh bul), which means
they can be hammered or rolled into sheets.
• Metals are also ductile, which means they can be
drawn into wires.
Section
1
Metals
Ionic Bonding in Metals
• The atoms of metals generally have one to three
electrons in their outer energy levels.
• In chemical reactions, metals tend to give up electrons
easily because of the strength of charge of the protons
in the nucleus.
Section
1
Metals
Ionic Bonding in Metals
• When metals combine with nonmetals,
the atoms of the metals tend to lose
electrons to the atoms of nonmetals,
forming ionic bonds.
• Both metals and nonmetals become more chemically
stable when they form ions.
Section
Metals
1
Metallic Bonding
• In metallic bonding, positively charged metallic
ions are surrounded by a sea of electrons.
• Outer-level electrons are not
held tightly to the nucleus of an
atom. Rather, the electrons
move freely among many
positively charged ions.
Section
Metals
1
Metallic Bonding
• The idea of metallic bonding explains many of the
properties of metals.
• When a metal is hammered into a sheet or drawn into
a wire, it does not break because the ions are in
layers that slide past one another without losing their
attraction to the electron sea.
• Metals are also good conductors of electricity because
the outer-level electrons are weakly held and can move
relatively feely.
Section
Metals
1
The Alkali Metals
• The elements in Group 1 of the periodic table are the
alkali (AL kuh li) metals.
• Group 1 metals are shiny,
malleable, and ductile.
• They are also good conductors
of heat and electricity.
However, they are softer than
most other metals.
Section
Metals
1
The Alkali Metals
• The alkali metals are the most
reactive of all the metals. They
react rapidly, sometimes violently,
with oxygen and water.
• Alkali metals don’t occur in nature
in their elemental form and are
stored in substances that are
unreactive, such as an oil.
Section
Metals
1
The Alkali Metals
• Each atom of an alkali metal has one electron in its
outer energy level.
• This electron is given up when an alkali metal combines
with another atom.
• As a result, the alkali metal becomes a positively
charged ion in a compound such as sodium chloride.
Section
Metals
1
The Alkali Metals
• Alkali metals and their compounds have many uses.
• Doctors use lithium compounds to treat bipolar
depression.
• Living organisms need sodium and potassium in their
diets to remain healthy.
Section
Metals
1
The Alkali Metals
• The operation of some photocells depends upon
rubidium or cesium compounds.
• Francium, the last element in Group 1, is extremely
rare and radioactive.
• A radioactive element is one in which the nucleus
breaks down and gives off particles and energy.
Section
1
Metals
The Alkaline Earth Metals
• The alkaline earth metals
make up Group 2 of the
periodic table.
• Each atom of an alkaline
earth metal has two electrons
in its outer energy level.
Section
1
Metals
The Alkaline Earth Metals
• These electrons are given up when an alkaline earth
metal combines with a nonmetal.
• As a result, the alkaline earth metal becomes a
positively charged ion in a compound such as calcium
fluoride, CaF2.
Section
1
Metals
Coloring Fireworks
• Magnesium metal is one of the metals used to produce
the brilliant white color in fireworks.
• Compounds of strontium produce the bright red flashes.
Section
Metals
1
Magnesium
• Magnesium’s lightness and strength account for its
use in cars, planes, and spacecraft.
• Magnesium also is used in compounds to make such
things as household ladders, and baseball and softball
bats.
Section
Metals
1
Calcium
• Calcium is seldom used
as a free metal, but its
compounds are needed
for life.
• Calcium phosphate in
your bones helps make
them strong.
Section
1
Metals
Other Alkaline Earth Metals
• The barium compound BaSO4 is used to diagnose
some digestive disorders because it absorbs X-ray
radiation well.
• Radium, the last element in Group 2, is radioactive
and is found associated with uranium. It was once
used to treat cancers.
Section
1
Metals
Transition Elements
• Transition elements are those elements in Groups 3
through 12 in the periodic table.
• They are called transition elements because they are
considered to be elements in transition between
Groups 1 and 2 and Groups 13 through 18.
Section
1
Metals
Transition Elements
• Transition elements are
familiar because they often
occur in nature as uncombined
elements.
• Transition elements often
form colored compounds.
• Gems show brightly
colored compounds
containing chromium.
Section
1
Metals
Iron, Cobalt, and Nickel
• The first elements in
Groups 8, 9, and 10iron,
cobalt, and nickelform a
unique cluster of transition
elements.
• These three sometimes
are called the iron triad.
• All three elements are used in
the process to create steel and
other metal mixtures.
Section
1
Metals
Iron, Cobalt, and Nickel
• Ironthe main component
of steelis the most widely
used of all metals.
• Nickel is added to some
metals to give them
strength.
Click image to play movie
Section
1
Metals
Copper, Silver, and Gold
• Copper, silver, and goldthe three elements in Group
11are so stable that they can be found as free
elements in nature.
• These metals were once
used widely to make coins,
so they are known as the
coinage metals.
• Today, only copper is used
in coins.
Section
1
Metals
Copper, Silver, and Gold
• Copper often is used in electrical wiring because of its
superior ability to conduct electricity and its relatively low
cost.
• Silver iodide and silver bromide break down when
exposed to light and are used to make photographic film
and paper.
• Gold is used in jewelry because of its softness, color,
and rarity.
Section
1
Metals
Zinc, Cadmium, and Mercury
• Zinc, cadmium, and mercury are found in Group 12 of
the periodic table.
• Zinc combines with oxygen in
the air to form a thin,
protective coating of zinc
oxide on its surface.
• Zinc and cadmium often are
used to coat, or plate, other
metals such as iron because
of this protective quality.
Section
1
Metals
Zinc, Cadmium, and Mercury
• Mercury is a silvery, liquid metalthe only metal that
is a liquid at room temperature.
• It is used in thermostats, switches, and batteries.
• Mercury is poisonous and can accumulate in the
body.
• Therefore, mercury is not longer used in thermometers.
Section
1
Metals
The Inner Transition Metals
• The two rows of elements that seem to be disconnected
from the rest on the periodic table are called the inner
transition elements.
Section
1
Metals
The Inner Transition Metals
• They are called this because like the transition
elements, they fit in the periodic table between Groups
3 and 4 in periods 6 and 7, as shown.
Section
Metals
1
The Lanthanides
• The first row includes a series of elements with atomic
numbers of 58 to 71.
• These elements are called the lanthanide series
because they follow the element lanthanum.
Section
Metals
1
The Actinides
• The second row of inner transition metals includes
elements with atomic numbers ranging from 90 to
103.
• These elements are called the actinide series because
they follow the element actinium.
• All of the actinides are radioactive and unstable.
• Thorium and uranium are the actinides found in the
Earth’s crust in usable quantities.
Section
1
Metals
Metals in the Crust
• Earth’s hardened outer layer, called the crust,
contains many compounds and a few uncombined
metals such as gold and copper.
• Most of the world’s platinum is found in South Africa.
• The United States imports most of its chromium from
South Africa, the Philippines, and Turkey.
Section
1
Metals
Ores: Minerals and Mixtures
• Metals in Earth’s crust that combined with other
elements are found as ores.
• Most ores consist of a metal compound, or mineral,
within a mixture of clay or rock.
Section
1
Metals
Ores: Minerals and Mixtures
• After an ore is mined from Earth’s crust, the rock is
separated from the mineral.
• Then the mineral often is converted to another physical
form.
• This step usually involves heat and is called roasting.
Section
1
Section Check
Question 1
What are common properties of metals?
Answer
Metals are good conductors of heat and electricity, reflect
light, are malleable and ductile, and, except for mercury,
are solid at room temperature.
Section
Section Check
1
Question 2
Which of these best describes electrons in metallic
bonding?
A.
B.
C.
D.
electron acceptor
electron sea
electron donor
electrons in fixed orbits
Section
1
Section Check
Answer
The answer is B. In metallic bonding, positively charged
metallic ions are surrounded by a sea of electrons.
Section
1
Section Check
Question 3
How do alkaline earth metals differ from alkali metals?
Section
1
Section Check
Answer
Alkali metals have one
electron in the outer energy
level of each atom. Each
atom of alkaline earth metals
has two electrons in its outer
energy level.
Section
2
Nonmetals
Properties of Nonmetals
• Most of your body’s
mass is made of
oxygen, carbon,
hydrogen, nitrogen and
phosphorus.
• Calcium, a metal, and
other elements make
up the remaining four
percent of your body’s
mass.
Section
2
Nonmetals
Properties of Nonmetals
• Sulfur, and chlorine are among these other elements
found in your body.
• These elements are classified as nonmetals.
• Nonmetals are elements that usually are gases or
brittle solids at room temperature.
Section
2
Nonmetals
Properties of Nonmetals
• Most nonmetals do not conduct heat or electricity well,
and generally they are not shiny.
• In the periodic table, all nonmetals except hydrogen are
found at the right of the stair-step line.
Section
2
Nonmetals
Properties of Nonmetals
• The noble gases, Group 18, make up the only group of
elements that are all nonmetals.
• Group 17 elements, except for astatine, are also
nonmetals.
Section
2
Nonmetals
Bonding in Nonmetals
• The electrons in most nonmetals cannot move freely.
So, as a group, nonmetals are poor conductors of heat
and electricity.
• Most nonmetals can form ionic and covalent
compounds.
Section
2
Nonmetals
Bonding in Nonmetals
• When nonmetals gain electrons from metals, the
nonmetals become negative ions in ionic
compounds.
• When bonded with other nonmetals, atoms of
nonmetals usually share electrons to form covalent
compounds.
Section
Nonmetals
2
Hydrogen
• If you could count all the atoms in the universe, you
would find that about 90 percent of them are hydrogen.
• When water is broken down
into its elements, hydrogen
becomes a gas made up of
diatomic molecules.
Section
Nonmetals
2
Hydrogen
• A diatomic molecule consists of two atoms of the
same element in a covalent bond.
Section
Nonmetals
2
Hydrogen
• Hydrogen is highly reactive.
• A hydrogen atom has a single electron, which the
atom shares when it combines with other nonmetals.
• Hydrogen can gain an electron when it combines with
alkali and alkaline earth metals.
• The compounds formed are hydrides.
Section
Nonmetals
2
The Halogens
• Halogen lights contain
small amounts of bromine
or iodine vapor.
• These elements, as well as
fluorine, chlorine, and
astatine, are called
halogens and are in Group
17.
Section
Nonmetals
2
The Halogens
• They are very reactive
and their compounds
have many uses.
Section
Nonmetals
2
The Halogens
• Because an atom of a halogen has seven electrons
in its outer energy level, only one electron is
needed to complete this energy level.
• If a halogen gains an electron from a metal, an ionic
compound, called a salt is formed.
Section
Nonmetals
2
The Halogens
• In the gaseous state,
the halogens form
reactive diatomic
covalent molecules and
can be identified by
their distinctive colors.
• Chlorine is greenish yellow,
bromine is reddish orange,
and iodine is violet.
Click image to play movie
Section
Nonmetals
2
The Halogens
• Fluorine is the most chemically active of all
elements.
• Hydrofluoric acid, a mixture of hydrogen fluoride and
water, is used to etch glass and to frost the inner
surfaces of lightbulbs and is also used in the fabrication
of semiconductors.
Section
Nonmetals
2
Chlorine
• Chlorine compounds are
used to disinfect water.
• Chlorine, the most
abundant halogen, is
obtained from seawater
at ocean-salt recovery
sites.
Section
Nonmetals
2
Chlorine
• Household and industrial
bleaches used to whiten
flour, clothing, and paper
also contain chlorine
compounds.
Section
Nonmetals
2
Bromine
• Bromine, the only nonmetal that is a liquid at room
temperature, also is extracted from compounds in
seawater.
• The bromine compound ethidium bromide fluoresces
and is used to stain DNA so that scientists can follow
parts of the genetic code.
Section
Nonmetals
2
Iodine
• Iodine, a shiny purple-gray solid at room temperature,
is obtained from seawater.
• When heated, iodine changes directly to a purple vapor.
• The process of a solid changing directly to a vapor
without forming a liquid is called sublimation.
Section
2
Nonmetals
Uses of Halogens
• Astatine is the last member of Group 17. It is
radioactive and rare, but has many properties similar to
those of the other halogens.
• Because astatine is so rare, it is usually used in
research.
Section
2
Nonmetals
The Noble Gases
• The noble gases exist as
isolated atoms.
• They are stable because
their outermost energy
levels are full.
• No naturally occurring
noble gas compounds
are known.
Section
2
Nonmetals
The Noble Gases
• The stability of noble gases is what makes them useful.
• The light weight of helium makes it useful in lighter-thanair blimps and balloons.
• Neon and argon are used in neon lights for advertising.
Section
Section Check
2
Question 1
Which elements exist primarily as gases or brittle solids
at room temperature?
A.
B.
C.
D.
metals
metalloids
nonmetals
synthetics
Section
2
Section Check
Answer
The answer is C. Solid nonmetals are brittle or powdery
and not malleable or ductile.
Section
Section Check
2
Question 2
A(n) __________ molecule consists of two atoms of the
same element in a covalent bond.
A.
B.
C.
D.
actinide
allotropic
diatomic
lanthanide
Section
2
Section Check
Answer
The answer is C. When water is broken down into its
elements, hydrogen becomes a gas made up of diatomic
molecules.
Section
Section Check
2
Question 3
Which of the following accounts for 90 percent of the
atoms in the universe?
A.
B.
C.
D.
carbon
hydrogen
nitrogen
oxygen
Section
2
Section Check
Answer
The answer is B. Hydrogen makes up 90 percent of the
atoms in the universe. On Earth, most hydrogen is found
in the compound water.
Section
3
Mixed Groups
Properties of Metalloids
• Metalloids share unusual characteristics.
• Metalloids can form ionic and covalent bonds with
other elements and can have metallic and nonmetallic
properties.
Section
3
Mixed Groups
Properties of Metalloids
• Some metalloids can conduct electricity better than
most nonmetals, but not as well as some metals, giving
them the name semiconductor.
• With the exception of aluminum, the metalloids are the
elements in the periodic table that are located along
the stair-step line.
Section
3
Mixed Groups
The Boron Group
• Boron, a metalloid, is
the first element in
Group 13.
• If you look around your
home, you might find
two compounds of
boron.
Section
Mixed Groups
3
Boron
• One of these is borax, which is used in some laundry
products to soften water.
• The other is boric acid, a mild antiseptic.
• Boron is also used to make heat-resistant glassware.
Section
Mixed Groups
3
Aluminum
• Aluminum, a metal in Group 13, is the most abundant
metal in Earth’s crust.
• It is used in soft-drink cans, foil wrap, cooking pans, and
as siding.
• Aluminum is strong and light and is used in the
construction of airplanes.
Section
3
Mixed Groups
The Boron Group
• Gallium is a metal
use in electronic
components.
• Indium and thallium
are rare metals.
Section
3
Mixed Groups
The Carbon Group
• Each element in Group
14, the carbon family,
has four electrons in its
outer energy level, but
this is where much of
the similarity ends.
Section
3
Mixed Groups
The Carbon Group
• Carbon is a nonmetal,
silicon and germanium
are metalloids, and tin
and lead are metals.
Section
Mixed Groups
3
Carbon
• Carbon occurs as an element in coal and as a
compound in oil, natural gas, and foods.
• Carbon compounds, many of which are essential to life,
can be found in you and all around you.
Section
Mixed Groups
3
Allotropes
• Carbon can form different molecular structures.
• Different molecular structures of the same element are
called allotropes.
• Diamond, graphite, and buckminsterfullerene are
allotropes of carbon.
Section
Mixed Groups
3
Graphite
• Graphite is a black powder
made up of layers of
hexagonal structures of
carbon atoms.
• The layers of hexagons are
weakly bonded and can slide
easily over each other.
• This structure makes
graphite a good lubricant.
Section
3
Mixed Groups
Allotropes of Carbon
• Diamond, graphite, and
buckminsterfullerene are
allotropes of an element.
• In a diamond, each carbon
atom is bonded to four other
carbon atoms at the
vertices, or corner points, of
a tetrahedron.
Section
3
Mixed Groups
Allotropes of Carbon
• In turn, many tetrahedrons
join together to form a giant
molecule in which the
atoms are held tightly in a
strong crystalline structure.
Section
3
Mixed Groups
Allotropes of Carbon
• In the mid-1980s, a new
allotrope of carbon called
buckminsterfullerene was
discovered. This soccer-ballshaped molecule, informally
called a buckyball, was named
after the architect-engineer R.
Buckminster Fuller, who
designed structures with similar
shapes.
Section
3
Mixed Groups
Allotropes of Carbon
• In 1991, scientists were able to use the buckyballs to
synthesize extremely thin, graphitelike tubes.
• These tubes, called nanotubes, are about 1 billionth of a
meter in diameter.
• Nanotubes might be used someday to make computers
that are smaller and faster and to make strong building
materials.
Section
Mixed Groups
3
Silicon
• Silicon is second only to oxygen in abundance in Earth’s
crust.
• The crystal structure of silicon dioxide is similar to the
structure of diamond.
• Silicon occurs as two allotropes.
Section
3
Mixed Groups
Silicon and Germanium
• Silicon is the main component in
semiconductorselements that conduct an electric
current under certain conditions.
• Germanium, the other metalloid in the carbon group, is
used along with silicon in making semiconductors.
Section
3
Mixed Groups
Tin and Lead
• Tin is used to coat other metals to prevent corrosion.
• Tin also is combined with other metals to produce
bronze and pewter.
• Lead was used widely in paint at one time, but because
it is toxic, lead no longer is used.
Section
3
Mixed Groups
The Nitrogen Group
• The nitrogen family makes up
Group 15.
• Each element has five
electrons in its outer
energy level.
• These elements tend to
share electrons and to form
covalent compounds with
other elements.
Section
Mixed Groups
3
Nitrogen
• Nitrogen is the fourth most abundant element in your
body.
• Each breath you take is about 80 percent gaseous
nitrogen in the form of diatomic molecules, N2.
Section
3
Mixed Groups
Uses of the Nitrogen Group
• Phosphorus is a nonmetal that has three allotropes.
• Phosphorus is used in match heads, fertilizers, and
fine china.
• Antimony is a metalloid, and bismuth is a metal.
• Both antimony and bismuth are used with other metals
to lower their melting points.
Section
3
Mixed Groups
The Oxygen Group
• Group 16 on the periodic
table is the oxygen group.
• Oxygen, a nonmetal,
exists in the air as
diatomic molecules, O2.
Section
Mixed Groups
3
Oxygen
• During electrical storms, some
oxygen molecules, O2, change
into ozone molecules, O3.
• Water (H2O) is an oxygen
compound needed by living
organisms.
• The compound hydrogen
peroxide (H2O2) is used as a
disinfectant.
Section
Mixed Groups
3
Sulfur
• The second element in the oxygen group is sulfur.
• Sulfur is a nonmetal that exists in several allotropic
forms.
• It exists as different-shaped crystals and as a
noncrystalline solid.
Section
3
Mixed Groups
The Oxygen Group
• The nonmetal selenium and two metalloidstellurium
and poloniumare the other Group 16 elements.
• Selenium is the most common of these three.
• This element is one of several that you need in trace
amounts in your diet.
• But selenium is toxic if too much of it gets into your
system.
Section
3
Mixed Groups
Synthetic Elements
• The most recently discovered elements are synthetic.
• By smashing existing elements with particles
accelerated in a heavy ion accelerator, scientists have
been successful in creating elements not typically
found on Earth.
• Except for technetium-43 and promethium-61, each
synthetic element has more than 92 protons.
Section
3
Mixed Groups
Why make elements?
• When these atoms disintegrate, they are said to be
radioactive.
• Radioactive elements can be useful. For example,
technetium’s radioactivity makes it ideal for many
medical applications.
Section
3
Mixed Groups
Transuranium Elements
• Elements having more
than 92 protons, the
atomic number of uranium,
are called transuranium
elements.
• These elements do not
belong exclusively to the
metal, nonmetal, or
metalloid group.
Section
3
Mixed Groups
Transuranium Elements
• All of the transuranium elements are synthetic and
unstable, and many of them disintegrate quickly.
Section
3
Mixed Groups
Seeking Stability
• By studying how the synthesized elements form and
disintegrate, you can gain an understanding of the
forces holding the nucleus together.
Section
3
Mixed Groups
Seeking Stability
• In the 1960s, scientists theorized that stable synthetic
elements exist.
• Finding one might help scientists understand how the
forces inside the atom work.
Section
Section Check
3
Question 1
Which of these compounds is not an allotrope of carbon?
A.
B.
C.
D.
buckminsterfullerene
diamond
graphite
quartz
Section
Section Check
3
Answer
The answer is D. Quartz is a mineral composed of silicon
dioxide.
Graphite
Diamond
Buckyball
Section
3
Section Check
Question 2
If you want to use a circle graph to represent the amount
of hydrogen in the universe relative to other elements,
how many degrees will be used to represent hydrogen?
A. 36º
B. 90º
C. 186º
D. 324º
Section
3
Section Check
Answer
The answer is D. 90 percent of the 360º in a circle is
equal to 324º.
Section
3
Section Check
Question 3
Elements having more than 92 protons are called
__________.
Answer
The atomic number of uranium is 92. Elements having
more than 92 protons are called transuranium elements,
and are synthetic and unstable.
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Calcium Supplement
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Gems
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Bleach
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Ionic Bonding
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Metallic Bonding
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Alkali Metals
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Elements
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Coinage Metals
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Zinc, Cadmium, Mercury
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Lanthanide & Actinide Series
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Elements in the Human Body
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Hydrogen
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Halogens
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Noble Gases
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The Boron Group
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The Carbon Group
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Diamond
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Graphite
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Buckminsterfullerene
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The Nitrogen Group
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The Oxygen Group
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Elements in the Human Body
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Reviewing Main Ideas
Metals
• A typical metal is a hard, shiny solid that, due to metallic
bonding, is malleable, ductile, and a good conductor.
• Groups 1 and 2 are the alkali and alkaline earth
metals, which have some similar and some contrasting
properties.
Reviewing Main Ideas
Metals
• The iron triad, the coinage metals, and the elements in
Group 12 are examples of transition elements.
• The lanthanides and actinides have atomic numbers 58
through 71 and 90 through 103, respectively.
Reviewing Main Ideas
Nonmetals
• Nonmetals can be brittle and dull. They are also poor
conductors of electricity.
• As a typical nonmetal, hydrogen is a gas that forms
compounds by sharing electrons with other nonmetals
and by forming ionic bonds with metals.
Reviewing Main Ideas
Nonmetals
• All the halogens, Group 17, have seven outer
electrons and form covalent and ionic compounds, but
each halogen has some properties that are unlike
each of the others in the group.
• The noble gases, Group 18, are elements whose
properties and uses are related to their chemical
stability.
Reviewing Main Ideas
Mixed Groups
• Groups 13 through 16 include metals, nonmetals, and
metalloids.
• Allotropes are different molecular structures of the
same element.
• The properties of three allotropes of carbongraphite,
diamond, and buckminsterfullerenedepend upon the
differences in their crystal structures.
Reviewing Main Ideas
Mixed Groups
• All synthetic elements are short-lived. Except for
technetium-43 and promethium-61, they have atomic
numbers greater than 92 and are referred to as
transuranium elements. These elements are found
toward the bottom of the periodic table.
Chapter Review
Question 1
Which metal is not solid at room temperature?
A.
B.
C.
D.
copper
lead
mercury
zinc
Chapter Review
Answer
The answer is C. Mercury is liquid at room temperature.
Chapter Review
Question 2
Which property of metals allows them to be drawn into
wires?
A.
B.
C.
D.
bondable
conductile
ductile
malleable
Chapter Review
Answer
The answer is C. Metals are ductile; they can be drawn
out into wires.
Chapter Review
Question 3
Why are nonmetals poor conductors of heat and
electricity?
Answer
The outer level electrons in most nonmetals cannot
move freely.
Chapter Review
Question 4
What is an important use of the element silicon?
Answer
Silicon is the main component in semiconductors. It is
the second most abundant element in Earth’s crust.
Standardized Test Practice
Question 1
Materials from which of these groups would be best for
connecting a battery to a light bulb?
A.
B.
C.
D.
Group 11
Group 16
Group 17
Group 18
Standardized Test Practice
Answer
The answer is A. Group 11 elements are metals, which
are good conductors of electricity.
Standardized Test Practice
Question 2
Which group is
represented by the
diagram?
A.
B.
C.
D.
actinides
alkali metals
alkaline earth metals
nonmetals
Standardized Test Practice
Answer
The answer is B. The elements in Group 1 except
hydrogen of the periodic table are the alkali metals.
Standardized Test Practice
Question 2
Which of these is not highly reactive?
A.
B.
C.
D.
fluorine
helium
hydrogen
sodium
Standardized Test Practice
Answer
The answer is B. Helium is a noble gas.
Standardized Test Practice
Question 4
Which group is
represented in the
diagram?
A.
B.
C.
D.
alkali metals
alkaline earth metals
halogens
noble gases
Standardized Test Practice
Answer
The answer is C. The elements in Group 17 are
halogens and are highly reactive in their elemental
form.
Standardized Test Practice
Question 5
An isotope of Copernicium has 112 protons and 173
neutrons. How many particles are in the nucleus of the
atom?
A.
B.
C.
D.
112
285
173
61
Standardized Test Practice
Answer
The answer is B. 112 protons + 173 neutrons = 285
particles in the nucleus.
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