2. Table of Contents Elements and Their Properties Section 1 • Metals
Section 2 • Nonmetals
Section 3 • Mixed Groups

3. Properties of Metals
In the periodic table, metals are elements found to the left of the stair-step line.

4. 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.

5. 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.

6. 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.

7. 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.

8. 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.

9. 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.

10. 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.

11. 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.

12. 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.

13. 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.

14. 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.

15. 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.

16. 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.

17. 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.

18. 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.

19. 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.

20. 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.

21. 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.

22. 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.

23. 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.

24. 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.
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25. 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.

26. 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.

27. 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.

28. 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.

29. 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.

30. 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.

31. 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.

32. 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.

33. 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.

34. 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.

35. 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.

36. 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.

37. Section Check Question 2
Which of these best describes electrons in metallic bonding?
A. electron acceptor
B. electron sea
C. electron donor
D. electrons in fixed orbits

38. Section Check
Answer
The answer is B. In metallic bonding, positively charged metallic ions are surrounded by a sea of electrons.

39. Section Check Question 3
How do alkaline earth metals differ from alkali metals?

40. 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.

41. 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.

42. 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.

43. 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.

44. 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.

45. 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.

46. 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.

47. 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.

48. Hydrogen
A diatomic molecule consists of two atoms of the same element in a covalent bond.

49. 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.

50. 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.

51. The Halogens
They are very reactive and their compounds have many uses.

52. 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.

53. 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.
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54. 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.

55. Chlorine Chlorine compounds are used to disinfect water.
Chlorine, the most abundant halogen, is obtained from seawater at ocean-salt recovery sites.

56. Chlorine
Household and industrial bleaches used to whiten flour, clothing, and paper also contain chlorine compounds.

57. 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.

58. 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.

59. 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.

60. 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.

61. The Noble Gases
The stability of noble gases is what makes them useful.
The light weight of helium makes it useful in lighter-than-air blimps and balloons.
Neon and argon are used in neon lights for advertising.

62. Section Check Question 1
Which elements exist primarily as gases or brittle solids at room temperature?
A. metals
B. metalloids
C. nonmetals
D. synthetics

63. Section Check
Answer
The answer is C. Solid nonmetals are brittle or powdery and not malleable or ductile.

64. Section Check Question 2
A(n) __________ molecule consists of two atoms of the same element in a covalent bond.
A. actinide
B. allotropic
C. diatomic
D. lanthanide

65. Section Check
Answer
The answer is C. When water is broken down into its elements, hydrogen becomes a gas made up of diatomic molecules.

66. Section Check Question 3
Which of the following accounts for 90 percent of the atoms in the universe?
A. carbon
B. hydrogen
C. nitrogen
D. oxygen

67. 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.

68. Properties of Metalloids
Metalloids share unusual characteristics.
Metalloids can form ionic and covalent bonds with other elements and can have metallic and nonmetallic properties.

69. 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.

70. 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.

71. 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.

72. 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.

73. The Boron Group Gallium is a metal use in electronic components.
Indium and thallium are rare metals.

74. 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.

75. The Carbon Group
Carbon is a nonmetal, silicon and germanium are metalloids, and tin and lead are metals.

76. 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.

77. 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.

78. 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.

79. 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.

80. 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.

81. Allotropes of Carbon
In the mid-1980s, a new allotrope of carbon called buckminsterfullerene was discovered. This soccer-ball-shaped molecule, informally called a buckyball, was named after the architect-engineer R. Buckminster Fuller, who designed structures with similar shapes.

82. 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.

83. 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.

84. 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.

85. 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.

86. 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.

87. 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.

88. 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.

89. The Oxygen Group Group 16 on the periodic table is the oxygen group.
Oxygen, a nonmetal, exists in the air as diatomic molecules, O2.

90. 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.

91. 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.

92. 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.

93. 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.

94. 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.

95. 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.

96. Transuranium Elements
All of the transuranium elements are synthetic and unstable, and many of them disintegrate quickly.

97. Seeking Stability
By studying how the synthesized elements form and disintegrate, you can gain an understanding of the forces holding the nucleus together.

98. 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.

99. Section Check Question 1
Which of these compounds is not an allotrope of carbon?
A. buckminsterfullerene
B. diamond
C. graphite
D. quartz

100. Section Check
Answer
The answer is D. Quartz is a mineral composed of silicon dioxide.
Graphite
Diamond
Buckyball

101. 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

102. Section Check
Answer
The answer is D. 90 percent of the 360º in a circle is equal to 324º.

103. 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.

104. Help
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106. Chapter Resources
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Image Bank
Video Clips and Animations
Chapter Summary
Chapter Review Questions
Standardized Test Practice

107. Image Bank
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108. Image Bank
Calcium Supplement

109. Image Bank
Gems

110. Image Bank
Bleach

111. Image Bank
Ionic Bonding

112. Image Bank
Metallic Bonding

113. Image Bank
Alkali Metals

114. Image Bank
Alkali Earth Metals

115. Image Bank
Elements

116. Image Bank
Coinage Metals

117. Image Bank
Zinc, Cadmium, Mercury

118. Image Bank
Lanthanide & Actinide Series

119. Image Bank
Elements in the Human Body

120. Image Bank
Hydrogen

121. Image Bank
Halogens

122. Image Bank
Noble Gases

123. Image Bank
The Boron Group

124. Image Bank
The Carbon Group

125. Image Bank
Diamond

126. Image Bank
Graphite

127. Image Bank
Buckminsterfullerene

128. Image Bank
The Nitrogen Group

129. Image Bank
The Oxygen Group

130. Image Bank
The Transuranium Elements

131. Image Bank
Elements in the Human Body

132. Video Clips and Animations
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133. Video Clips and Animations
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134. Video Clips and Animations

135. 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.

136. 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.

137. 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.

138. 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.

139. 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.

140. 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.

141. Chapter Review Question 1
Which metal is not solid at room temperature?
A. copper
B. lead
C. mercury
D. zinc

142. Chapter Review
Answer
The answer is C. Mercury is liquid at room temperature.

143. Chapter Review Question 2
Which property of metals allows them to be drawn into wires?
A. bondable
B. conductile
C. ductile
D. malleable

144. Chapter Review
Answer
The answer is C. Metals are ductile; they can be drawn out into wires.

145. Chapter Review Question 3
Why are nonmetals poor conductors of heat and electricity?
Answer
The outer level electrons in most nonmetals cannot move freely.

146. 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.

147. Standardized Test Practice
Question 1
Materials from which of these groups would be best for connecting a battery to a light bulb?
A. Group 11
B. Group 16
C. Group 17
D. Group 18

148. Standardized Test Practice
Answer
The answer is A. Group 11 elements are metals, which are good conductors of electricity.

149. Standardized Test Practice
Question 2
Which group is represented by the diagram?
A. actinides
B. alkali metals
C. alkaline earth metals
D. nonmetals

150. Standardized Test Practice
Answer
The answer is B. The elements in Group 1 except hydrogen of the periodic table are the alkali metals.

151. Standardized Test Practice
Question 2
Which of these is not highly reactive?
A. fluorine
B. helium
C. hydrogen
D. sodium

152. Standardized Test Practice
Answer
The answer is B. Helium is a noble gas.

153. Standardized Test Practice
Question 4
Which group is represented in the diagram?
A. alkali metals
B. alkaline earth metals
C. halogens
D. noble gases

154. Standardized Test Practice
Answer
The answer is C. The elements in Group 17 are halogens and are highly reactive in their elemental form.

155. 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. 112
B. 285
C. 173
D. 61

156. Standardized Test Practice
Answer
The answer is B protons neutrons = 285 particles in the nucleus.

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