2. Elements and Their Properties Chapter 12 Chem. Apps 2013 Mr. Gilbertson

3. Chapter 12: Elements and Their Properties Unit 5: Diversity of Matter Table of Contents 12 12.4: Mixed GroupsMixed Groups 12.1: Metals 12.3: NonmetalsNonmetals 12.2: New Elements, New Properties

4. Properties of Metals Metals - good conductors of heat and electricity, 12.1 Metals All but one are solid at room temperature.

5. Properties of Metals Metals also reflect light (Luster) shiny when smooth and clean Malleable- Can be hammered or rolled into sheets. 12.1 Metals Ductile- Can be drawn into wires.

6. Generally have 3 or less valence electrons Tend to lose electrons when bonding (“metals are losers”) Bond only with nonmetals (ionically) Metals bond with each other in metallic bonds Properties of Metals 12.1

7. Metallic Bonding In metallic bonding, positively charged metallic ions are surrounded by a cloud 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. 12.1 Metals

8. Metallic Bonding Explains Properties Metal does not break because the ions are in layers that slide past one another without losing their attraction to the electron cloud. Makes metals malleable and ductile. 12.1 Metals Metals are good conductors because the outer-level electrons are weakly held. This allows electrons to flow freely through the metal.

9. The Alkali Metals Group 1 metals are shiny, malleable, and ductile. 12.1 Metals They are also good conductors of heat and electricity. They are softer than most other metals.

10. The Alkali Metals Group 1- Alkali metals- most reactive of all the metals. They react violently - with oxygen and water. (stored in oil) 19.1 Metals Alkali metals don’t occur in nature in their elemental form and are stored in substances that are unreactive, such as an oil.

11. The Alkali Metals Each atom of an alkali metal has one electron in its outer energy level. 12.1 Metals This electron is given up when an alkali metal combines with another atom. They react violently with water to form H 2 gas and an alkaline solution (hence the name).

12. The Alkali Metals - Uses 12.1 Metals Doctors use Lithium compounds to treat bipolar depression. Biologically important for muscle an nerve function K and Na must be available for normal cell function.

13. The Alkali Metals - Uses The operation of some photocells depends upon rubidium or cesium compounds. 12.1 Metals Francium, the last element in Group 1, is extremely rare and radioactive (most reactive element of all). A radioactive element is one in which the nucleus breaks down and gives off particles and energy.

14. The Alkaline Earth Metals Group 2 Alkaline earth metal- Not as reactive as Alkali Metals. Oxides form alkaline solutions in water. Have 2 valence electrons form +2 ions. 12.1 Metals

15. The Alkaline Earth Metals 12.1 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, CaF 2.

16. Fireworks and Other Uses Magnesium- used to produce the brilliant white color in fireworks. 12.1 Metals strontium produce the bright red flashes.

17. Fireworks and Other Uses Magnesium’s lightness and strength account for its use in cars, planes, and spacecraft. 12.1 Metals Magnesium also is used in compounds to make such things as household ladders, and baseball and softball bats.

18. The Alkaline Earth Metals and Your Body Calcium is seldom used as a free metal, but its compounds are needed for life. 12.1 Metals Calcium phosphate in your bones helps make them strong.

19. The Alkaline Earth Metals Excessive amounts of Calcium and Magnesium compounds make hard water. 12.1 Hard water interferes with the action of soaps making it difficult to remove oils and grease.

20. The Alkaline Earth Metals and Your Body The barium compound BaSO 4 is used to diagnose some digestive disorders because it absorbs X-ray radiation well. 12.1 Metals 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. (Transition between the other groups) d-block elements 12.1 Metals 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. 12.1 Metals Transition elements often form colored compounds. Gems show brightly colored compounds containing chromium.

23. Iron, Cobalt, and Nickel Iron, cobalt, and nickel (Iron Triad) 12.1 Metals Elements are used in the process to create various types of steel (alloys). Alloys - Mixtures of metals with new properties.

24. Iron, Cobalt, and Nickel Iron  the main component of steel  is the most widely used of all metals. 12.1 Metals Nickel is added to some metals to give them strength. Click image to play movie

25. Copper, Silver, and Gold Coinage metals - Copper, Silver, and Gold - stable metal elements that were used widely to make coins. More recently Nickel, Zinc, and Platinum 12.1 Metals

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. 12.1 Metals Silver iodide and silver bromide break down when exposed to light, producing an image on photographic paper. Consequently, these compounds are used to make photographic film and paper.

27. Zinc, Cadmium, and Mercury 12.1 Metals Zinc combines with oxygen in the air to form a thin, protective coating of zinc oxide on its surface (galvanized metals). 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. 12.1 Metals It is used in thermometers, thermostats, switches, and batteries. Mercury is poisonous and can accumulate in the body.

29. The Inner Transition Metals Inner transition elements- Elements that are disconnected from the periodic table 12.1 Metals

30. The Inner Transition Metals 12.1 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 12.1 Metals Lanthanide- Upper row of inner transition elements Actinide- Lower row of inner transition elements (all are radioactive) Thorium and uranium are the actinides found in the Earth’s crust in usable quantities. The Actinides

32. Ores, Minerals, and Mixtures Ores – metal compounds in the earths crust which can be mined at a profit. Mineral – naturally occurring, solid, inorganic, compound with a definite composition and crystal form. Mixtures – rocks are natural mixtures of minerals. Alloys – mixture of metals with new and useful properties.

33. Synthetic Elements By smashing existing elements with particles accelerated in a heavy ion accelerator, scientists have been successful in creating elements not typically found on Earth. 12.2 Mixed Groups Except for technetium-43 and promethium- 61, each synthetic element has more than 92 protons.

34. Transuranium Elements transuranium elements- Man made synthetic elements that are radioactive. (After Uranium) 12.2 Mixed Groups These elements do not belong exclusively to the metal, nonmetal, or metalloid group.

35. Synthetic Elements Plutonium also can be changed to americium, element 95. This element is used in home smoke detectors. 12.2 Mixed Groups

36. Why make elements? The most recently discovered elements are synthetic. 12.2 Mixed Groups By studying how the synthesized elements form and disintegrate, you can gain an understanding of the forces holding the nucleus together.

37. Properties of Nonmetals Most of your body’s mass is made of oxygen, carbon, hydrogen, and nitrogen. Calcium, a metal, and other elements make up the remaining four percent of your body’s mass. 12.3 Nonmetals

38. Properties of Nonmetals Phosphorus, sulfur, and chlorine are among these other elements found in your body. 12.3 Nonmetals Nonmetals are elements that usually are gases or brittle solids at room temperature. Poor conductors and not shiny (dull and brittle as solids) most are gases at room temperature.

39. Properties of Nonmetals 12.3 Nonmetals In the periodic table, all nonmetals are found at the right of the stair-step line. Hydrogen is an unusual element.

40. Bonding in Nonmetals The electrons in nonmetals are strongly held. So, nonmetals are poor conductors Prefer to gain or share electrons, rarely lose electrons. Tend to form ionic bonds when bonding with metals Tend to form covalent bonds with each other. 12.3 Nonmetals

41. Hydrogen 90% of Universe is Hydrogen Hydrogen is highly reactive. 12.3 Nonmetals When water is broken down into its elements, hydrogen becomes a gas made up of diatomic molecules.

42. The Hindenburg A hydrogen filled Zeppelin Which caught fire and burned while docking. video

43. Diatomic Molecules Always found in pairs in nature Elements Hydrogen - H 2 Nitrogen - N 2 Oxygen - O 2 Fluorine - F 2 Chlorine - Cl 2 Bromine - Br 2 Iodine - I 2 Location of Diatomic Elements

44. The Halogens 12.3 Nonmetals Group 17 Halogens- react and form salts

45. The Halogens 12.3 Nonmetals They are very reactive in their elemental form, and their compounds have many uses.

46. 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. 12.3 Nonmetals salt - when a halogen gains an electron from a metal

47. Uses of Halogens 12.3 Nonmetals Household and industrial bleaches used to whiten flour, clothing, and paper also contain chlorine compounds.

48. Uses of Halogens Chlorine compounds are used to disinfect water. 12.3 Nonmetals Chlorine, the most abundant halogen, is obtained from seawater at ocean- salt recovery sites.

49. The Halogens In the gaseous state, the halogens form reactive diatomic covalent molecules and can be identified by their distinctive colors. 12.3 Nonmetals Chlorine is greenish yellow, bromine is reddish orange, and iodine is violet. Click image to play movie

50. Uses of Halogens Bromine, the only nonmetal that is a liquid at room temperature, also is extracted from compounds in seawater. 12.3 Nonmetals Bromine compounds are used as dyes in cosmetics.

51. Uses of Halogens 12.3 Nonmetals When heated, iodine changes directly to a purple vapor. Sublimation- solid changes directly to a vapor without forming a liquid is called

52. The Halogens Fluorine is the most chemically active of all elements. 12.3 Nonmetals Hydrofluoric acid, a mixture of hydrogen fluoride and water, is used to etch glass and to frost the inner surfaces of light bulbs and is also used in the fabrication of semiconductors.

53. The Noble Gases 12.3 Nonmetals Group 18 Noble Gases – Un-reactive because their outermost energy levels are full.

54. The Noble Gases The stability of noble gases is what makes them useful. 12.3 Nonmetals 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.

55. 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. 12.3 Mixed Groups

56. The Boron Group 12.4 Mixed Groups One of these is borax, which is used in some laundry products to soften water. The other is boric acid, a mild antiseptic.

57. The Boron Group Aluminum- is the most abundant metal in Earth’s crust. It is used in soft-drink cans, foil wrap, cooking pans, and as siding. 12.4 Mixed Groups Aluminum is strong and light and is used in the construction of airplanes.

58. 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. 12.4 Mixed Groups

59. The Carbon Group Carbon is a nonmetal, silicon and germanium are metalloids, and tin and lead are metals. 12.4 Mixed Groups

60. The Carbon Group 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. 12.4 Mixed Groups

61. The Nitrogen Group The nitrogen family makes up Group 15. 12.4 Mixed Groups Each element has five electrons in its outer energy level. These elements tend to share electrons and to form covalent compounds with other elements.

62. The Nitrogen Group Nitrogen is the fourth most abundant element in your body. 12.4 Mixed Groups Each breath you take is about 80 percent gaseous nitrogen in the form of diatomic molecules, N 2.

63. Uses of the Nitrogen Group Phosphorus is a nonmetal that has three allotropes. 12.4 Mixed Groups Antimony is a metalloid, and bismuth is a metal. Both elements are used with other metals to lower their melting points.

64. The Oxygen Group - Chalcogen Group 16 on the periodic table is the oxygen group. 12.4 Mixed Groups Oxygen, a nonmetal, exists in the air as diatomic molecules, O 2.

65. The Oxygen Group Group 16 on the periodic table is the oxygen group. 12.4 Mixed Groups Oxygen, a nonmetal, exists in the air as diatomic molecules, O 2. During electrical storms, some oxygen molecules, O 2, change into ozone molecules, O 3.

66. The Oxygen Group The second element in the oxygen group is sulfur. 12.4 Mixed Groups Sulfur is a nonmetal that exists in ten allotropic forms. It exists as different-shaped crystals and as a noncrystalline solid.

67. The Oxygen Group The nonmetal selenium and two metalloids  tellurium and polonium  are the other Group 16 elements. 12.4 Mixed Groups 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.

68. Properties of Metalloids Metalloids have metallic and nonmetallic properties. 12.4 Mixed Groups

69. Properties of Metalloids Some metalloids are semiconductors- conduct electricity better than most nonmetals, but not as well as some metals With the exception of aluminum, the metalloids are the elements in the periodic table that are located along the stair-step line. 12.4 Mixed Groups

70. The Carbon Group Silicon is second only to oxygen in abundance in Earth’s crust. 12.4 Mixed Groups Allotropes - different forms of the same element.

71. Allotropes of Carbon Carbon Allotropes- diamond and graphite, In a diamond, each carbon atom is bonded to four other carbon atoms at the vertices, or corner points, of a tetrahedron. 12.4 Mixed Groups

72. Allotropes of Carbon 12.4 Mixed Groups In turn, many tetrahedrons join together to form a giant molecule in which the atoms are held tightly in a strong crystalline structure.

73. 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. 12.4 Mixed Groups

74. The Carbon Group 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. 12.4 Mixed Groups

75. The Carbon Group Tin is used to coat other metals to prevent corrosion. Tin also is combined with other metals to produce bronze and pewter. 12.4 Mixed Groups Lead was used widely in paint at one time, but because it is toxic, lead no longer is used.

76. Element Groups to remember: Alkali metals Alkali earth metals Chalcogens Halogens Noble gases Transition Metals Inner Transition Metals

77. 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.

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

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

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

81. 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.

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

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

84. 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

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

86. 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

87. 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.

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

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

90. 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

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

92. 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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