3. Chapter Menu Section 5.1Section 5.1Ionic Compounds Section 5.2 Section 5.2 Covalent Compounds Click a hyperlink to view the corresponding slides.

4. Section 5.1 Ionic Compounds Apply ionic charge to writing formulas for ionic compounds. Apply formulas to name ionic compounds. Interpret the information in a chemical formula.

5. Section 5.1 Ionic Compounds ion: an atom or group of combined atoms that has a charge because of loss or gain of electrons

6. Section 5.1 Ionic Compounds binary compound formula unit oxidation number polyatomic ion hydrate hygroscopic deliquescent anhydrous The attraction of oppositely charged ions holds atoms in ionic compounds together.

7. Section 5.1 Binary Ionic Compounds Ionic compounds are made up of oppositely charged ions held together strongly in well-organized units.

8. Section 5.1 Binary Ionic Compounds (cont.) A binary compound is a compound that contains only two elements, such as sodium chloride (NaCl).binary compound In naming a binary ionic compound, the element with the positively charged ion, usually a metal, is named first with the negatively charged ion, usually a nonmetal, named next, modified to end in –ide.

9. Name the following binary compounds: Li 2 O MgS Ca 3 N 2

10. Section 5.1 Binary Ionic Compounds (cont.) When writing a formula, you add subscripts to the symbols for the ions until the algebraic sum of the ions’ charge is zero. If more than one ion of a given element is present in a compound, the subscript indicates how many ions are present.

11. Section 5.1 Binary Ionic Compounds (cont.) The simplest ratio of ions in a compound is called a formula unit.formula unit

12. Section 5.1 Binary Ionic Compounds (cont.) Metals tend to lose electrons and become positively charged while nonmetals tend to gain electrons and become negatively charged.

13. Section 5.1 Binary Ionic Compounds (cont.) The charge on the ion is known as the oxidation number of the atom. oxidation number

14. Write formulas for the following binary compounds: sodium chloride strontium fluoride beryllium oxide

15. Section 5.1 Binary Ionic Compounds (cont.) In a polyatomic ion, an ion that has two or more different elements, a group of elements is covalently bonded together when the atoms share electrons.polyatomic ion

16. Section 5.1 Binary Ionic Compounds (cont.) In naming a compound with a polyatomic ion, the molecule with the positive charge is named first, followed by the negative ion. The ending of the negative polyatomic ion name does not change.

17. Section 5.1 Binary Ionic Compounds (cont.)

18. Practice Problems #3-4 page 160 3) a) ammonium and sulfate ions b) calcium and monohydrogen phosphate ions c) ammonium and dichromate ions d) barium and nitrate ions

19. Practice Problems #3-4 page 160 4) a) sodium phosphate b) magnesium hydroxide c) ammonium phosphate d) potassium dichromate

20. Section 5.1 Compounds of transition elements Transition elements can form more than one type of positive ion and have more than one oxidation number. To distinguish the names of compounds formed from the different ions of a transition element, scientists use a Roman numeral to indicate the oxidation number of a transition element ion.

21. Practice Problems #5-6 page 163 5) a) copper(I) and sulfite b) tin(IV) and fluoride c) gold(III) and cyanide d) lead(II) and sulfide

22. Practice Problems #5-6 page 163 6) a) Pb(NO 3 ) 2 b) Mn 2 O 3 c) Ni(C 2 H 3 O 2 ) 2 d) HgF 2

23. Section 5.1 Compounds of transition elements (cont.)

24. Section 5.1 Compounds of transition elements (cont.)

25. Section 5.1 Hydrates A compound in which there is a specific ratio of water to ionic compound is a hydrate. In a hydrate, the water molecules are chemically bonded to the ionic compound.

26. Section 5.1 Hydrates (cont.) A hygroscopic substance is a substance that absorbs water molecules from the air to become a hydrate. Compounds that form hydrates often are used as drying agents, also called desiccants, because they absorb so much water from the air when they become hydrated.

27. Section 5.1 Hydrates (cont.) Heating hydrates can result in an anhydrous compound, or a compound in which all the water has been removed. anhydrous To name hydrates, follow the regular name for the compound with the word hydrate, to which a prefix has been added to indicate the number of water molecules present.

28. Section 5.1 Hydrates (cont.)

29. Name the hydrates. MgBr 2 ●6H 2 O CaSO 4 ●2H 2 O

30. Section 5.1 Interpreting Formulas A formula summarizes how many atoms of each element are present. If more than one formula unit of a compound is present, a coefficient is placed before the formula. How many formula units are present? 2 NaCl 3 H 3 PO 4 6 CO 2

31. Section 5.1 Section Assessment The simplest ratio of ions in a compound is called a(n) ___. A.oxidation unit B.formula unit C.binary compound D.binary ionic compound

32. Section 5.1 Section Assessment Which compound is a binary compound? A.Potassium iodide B.Lithium copper C.Iron magneside D.Sulfur hydrogen

33. End of Section 5.1

34. Section 5.2 Covalent Compounds Compare the properties of molecular and ionic substances. Distinguish among allotropes of an element. Apply formulas to name molecular compounds.

35. Section 5.2 Covalent Compounds anhydrous: a compound in which all of the water has been removed, usually by heating

36. Section 5.2 Covalent Compounds distillation molecular element allotrope organic compound inorganic compound hydrocarbon Covalent bonds hold atoms in covalent compounds together.

37. Section 5.2 Properties of Covalent Compounds The properties of most ionic and covalent compounds are different enough that their differences can be used to classify and separate them from one another.

38. Section 5.2 Properties of Covalent Compounds (cont.) Distillation is the method of separating substances in a mixture by the evaporation of a liquid and subsequent condensation of its vapor. Most covalent compounds are not electrolytes because they do not easily form ions.

39. Section 5.2 A molecule that forms when atoms of the same element bond together is called a molecular element. molecular element Molecular Elements

40. Section 5.2 Seven nonmetal elements are found naturally as diatomic elements, or molecular elements of two identical atoms. –hydrogen –nitrogen –oxygen –fluorine Molecular Elements (cont.) –chlorine –bromine –iodine

41. Section 5.2 Molecules of a single element that differ in crystalline or molecular structure are called allotropes. allotropes The properties of allotropes are usually different even though they contain the same element. Molecular Elements (cont.)

42. Section 5.2 Phosphorous has three common allotropes formed from P 4 molecules that are joined in different ways. –Each allotrope of phosphorous has a unique structure and set of properties. Molecular Elements (cont.)

43. Section 5.2 Carbon occurs as several important allotropes with different properties. –Diamonds are crystals in which the atoms of carbon are held rigidly in place in a three-dimensional network. –In graphite, carbon atoms are held together closely in flat layers that can slide over each other. Molecular Elements (cont.)

44. Section 5.2 Allotropes of oxygen –Ozone consists of three atoms of oxygen, occurs naturally, and is harmful to living things. Molecular Elements (cont.)

45. Section 5.2 Substances are either organic or inorganic. Compounds that contain carbon, with a few exceptions, are classified as organic compounds.organic compounds Formulas and Names of Covalent Compounds

46. Section 5.2 Compounds that do not contain carbon are called inorganic compounds.inorganic compounds If inorganic compounds contain only two nonmetal elements, they are bonded covalently and are referred to as molecular binary compounds. Formulas and Names of Covalent Compounds (cont.)

47. Section 5.2 Naming the compound –Name of the first nonmetal farthest left on the periodic table is listed first, followed by name of second nonmetal with its ending changed to –ide. –Add a prefix to the name of each element to indicate how many atoms of each element are present. Formulas and Names of Covalent Compounds (cont.)

48. Section 5.2 Formulas and Names of Covalent Compounds (cont.)

49. Practice Problems page 179 13) Name the following covalent compounds. a) S 2 Cl 2 b) CS 2 c) SO 3 d) P 4 O 10 14) Write the formula for the following compounds. a) carbon tetrachloride b) iodine heptafluoride c) dinitrogen monoxide d) sulfur dioxide

50. Section 5.2 Some scientists use the more common names for certain compounds, such as water, ammonia, and sulfuric acid. Formulas and Names of Covalent Compounds (cont.)

51. Section 5.2 Formulas and Names of Covalent Compounds (cont.)

52. Naming Acids Binary Acids The first word has the prefix hydro- followed by the root of the element plus the suffix –ic. The second word is always acid. Oxyacids An oxyacid is an acid that contains both a hydrogen atom and an ion containing oxygen.oxyacid Identify the oxygen-containing ion present. The first word is the root of the ion plus the suffix -ic if the anion ends in -ate or -ous if the oxyanion ends in -ite. The second word is always acid.

53. Section 5.2 The name of even the most complex organic compound is based on the name of a hydrocarbon, an organic compound that contains only the elements hydrogen and carbon.hydrocarbon Formulas and Names of Covalent Compounds (cont.) Compounds containing the noble gases helium, neon, and argon have never been found.

54. Section 5.2 Formulas and Names of Covalent Compounds (cont.)

55. Section 5.2 Section Assessment Which of the following is not a hydrocarbon? A.hexane B.nonane C.heptane D.lexane

56. Section 5.2 Section Assessment What is the correct formula for dinitrogen trioxide? A.N 2 O 3 B.N 2 O 2 C.N 3 O 2 D.N 2 O

57. End of Section 5.2

58. Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion

59. Study Guide 1 Key Concepts The position of an element in the periodic table indicates what charge its ions will have. Binary ionic compounds are named by first naming the metal element and then the nonmetal element, with its ending changed to –ide. Subscripts are used in formulas to indicate how many atoms of each element are present in the compound. Polyatomic ions can combine with ions of opposite charge to form ionic compounds which are named by writing the name of the positive ion first and then the name of the negative ion. Most transition elements can form two or more positively charged ions. The oxidation number of the transition element is indicated by a Roman numeral in parentheses. Hydrates are ionic compounds bonded to water molecules.

60. Study Guide 2 Key Concepts Covalent compounds generally have low melting points, low water solubility, and little or no ability to act as electrolytes. Seven elements occur naturally as diatomic molecules. They are hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine. Some elements exist in different structural forms called allotropes. Binary covalent compounds are named by writing the two elements in the order they are found in the formula, changing the ending of the second element to –ide, and adding Greek prefixes to the element names to indicate how many atoms of each are present.

61. Chapter Assessment 1 Which compound is not a polyatomic ion? A.sulfate B.potassium chloride C.ammonium D.hydrogen carbonate

62. Chapter Assessment 2 What kind of substance absorbs water molecules from the air to become a hydrate? A.oxidation compound B.anhydrous compound C.desiccant D.hygroscopic substance

63. Chapter Assessment 3 A formula summarizes how many ___ are present. A.electrons B.atoms C.elements D.compounds

64. Chapter Assessment 4 To create an anhydrous compound, what must be added to the hydrates? A.water B.air C.heat D.light

65. Chapter Assessment 5 What is the method of separating substances in a mixture by the evaporation of a liquid and subsequent condensation of its vapor? A.distillation B.hydration C.oxidation D.molecular division

66. STP 1 How many nonmetal elements are found naturally as molecular elements of two identical atoms? A.six B.seven C.eight D.twelve

67. STP 2 Which of the following is not a diatomic element? A.nitrogen B.bromine C.chlorine D.sulfur

68. STP 3 Which is an allotrope of oxygen? A.graphite B.diamond C.fullerene D.ozone

69. STP 4 Which is the most versatile element in forming allotropes? A.phosphorous B.carbon C.oxygen

70. STP 5 What is the chemical name for water? A.dihydroxide oxygen B.dioxide monohydride C.dihydrogen monoxide D.dioxygen hydroxide

71. IB Menu Click on an image to enlarge.

72. IB 1

73. IB 2

74. IB 3

75. IB 4

76. IB 5

77. IB 6

78. IB 7

79. IB 8

80. IB 9

81. IB 10

82. IB 11

83. IB 12

84. IB 13

85. CIM Table 5.5 Naming Prefixes Table 5.7Names of Common Acids and Bases

86. Help Click the Forward button to go to the next slide. Click the Previous button to return to the previous slide. Click the Home button to return to the Chapter Menu. Click the Return button in a feature to return to the main presentation. Click the Exit button or press the Escape key [Esc] to end the slide show. Click the Help button to access this screen. Click the Chapter Resources button to view available resources for the chapter. These resources include Chemistry Online, Study Guide, Chapter Assessment, Standardized Test Practice, Image Bank, and Concepts in Motion. Concepts in Motion pieces can also be accessed on relevant lecture note slides. To use this Interactive Chalkboard product:

87. End of Custom Shows This slide is intentionally blank.