1. Chapter 6 Ionic Compounds Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Have your i-clickers ready Silence cell phones and pagers.

2. Chapter 06 – Slide 2 of 91 An octet Contains 8 valence electrons. Is associated with the stability of the noble gases. Exception is He that is stable with 2 valence electrons (duet). valence electrons He 22 Ne 2, 88 Ar 2, 8, 8 8 Kr 2, 8, 18, 88 Octet Rule

3. Chapter 06 – Slide 3 of 91 Review: Valence Electrons The valence electrons Are the electrons in the s and p sublevels in the highest energy level. Are related to the Group number of the element. Determine the chemical properties of the elements. Elements with similar properties have the same number of ___________________ !

4. Chapter 06 – Slide 4 of 91 Forming Octets Atoms acquire octets By losing, gaining, or sharing valence electrons. To form compounds. To become more stable.

5. Chapter 06 – Slide 5 of 91 Atomic Size Atomic radius Is the distance from the nucleus to the valence electrons. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

6. Chapter 06 – Slide 6 of 91 Sizes of Metal Atoms and Ions A positive ion Has lost its valence electrons. Is smaller (about half the size) than its corresponding metal atom. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

7. Chapter 06 – Slide 7 of 91 Size of Sodium Ion The sodium ion Na + Forms when the Na atom loses one electron from the 3 rd energy level, its valence electron. Is smaller than a Na atom. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Octet

8. Chapter 06 – Slide 8 of 91 Sizes of Nonmetal Atoms and Ions A negative ion Has a complete octet. Increases the number of valence electrons. Is larger (about twice the size) than its corresponding metal atom. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

9. Chapter 06 – Slide 9 of 91 Size of Fluoride Ion The fluoride ion F - Forms when a valence electron is added. Has increased repulsions due to the added valence electron. Is larger than F atom Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Octet

10. Chapter 06 – Slide 10 of 91 Ionic and Covalent Bonds Ionic bonds involve Loss of electrons by a metal. Gain of electrons by a nonmetal. Covalent bonds involve A sharing of electrons. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

11. Chapter 06 – Slide 11 of 91 Metals Form Positive Ions Metals form Octets by losing all of their valence electrons. Positive ions with the electron configuration of the nearest noble gas. Positive ions with fewer electrons than protons. Group 1A(1) metals  ion 1+ Group 2A(2) metals  ion 2+ Group 3A(13) metals  ion 3+ Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

12. Chapter 06 – Slide 12 of 91 Formation of a Sodium Ion, Na + Sodium achieves an octet by losing its one valence electron. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings 2, 8, 1 2, 8

13. Chapter 06 – Slide 13 of 91 Charge of Sodium Ion, Na + With the loss of its valence electron, the sodium ion has a 1+ charge. Sodium atom Sodium ion 11p + 11p + 11e - 10e - 0 1+ Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings 2, 8

14. Chapter 06 – Slide 14 of 91 Formation of Mg 2+ Magnesium achieves an octet by losing its two valence electrons. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings 2, 8, 2 2, 8

15. Chapter 06 – Slide 15 of 91 Charge of Magnesium Ion Mg 2+ With the loss of two valence electrons, magnesium forms a positive ion with a 2+ charge. Mg atomMg 2+ ion 12p + 12p + 12e- 10e - 0 2+ Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings 2, 8

16. Chapter 06 – Slide 16 of 91 Formation of Negative Ions In ionic compounds, nonmetals Achieve an octet arrangement. Gain electrons. Form negatively charged ions with 3-, 2-, or 1- charges.

17. Chapter 06 – Slide 17 of 91 Formation of Chloride Ion, Cl - Chlorine achieves an octet by adding an electron to its valence electrons. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings 2, 8, 7 2, 8, 8

18. Chapter 06 – Slide 18 of 91 Charge of a Chloride Ion, Cl - A chlorine ion forms When Cl gains one electron With a 1- charge. Chlorine atom Chloride ion 17p + 17p + 17e - 18e - 0 1 – Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

19. Chapter 06 – Slide 19 of 91 Some Ionic Charges Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

20. Chapter 06 – Slide 20 of 91 Ionic Charge from Group Numbers The charge of a positive ion is equal to its Group number. Group 1A(1) = 1+ Group 2A(2) = 2+ Group 3A(13) = 3+ The charge of a negative ion is obtained by subtracting 8 or 18 from its Group number. Group 6A(16) = 6 - 8 = 2- or 16 - 18= 2-

21. Chapter 06 – Slide 21 of 91 Upon loss or gain of electons, the electronic arrangement of the ion is “isoelectronic” with its nearest noble gas.

22. Chapter 06 – Slide 22 of 91 An octet Is ___ valence electrons Is associated with the stability of the noble gases He is stable with ___ valence electrons (duet). valence electrons He 1s 2 __ Ne 1s 2 2s 2 2p 6 __ Ar 1s 2 2s 2 2p 6 3s 2 3p 6 __ Kr 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 __ Octet Rule - What is special about “8” ?

23. Chapter 06 – Slide 23 of 91 Compounds - Compounds result from the formation of chemical bonds between two or more different elements.

24. Chapter 06 – Slide 24 of 91 Chemical bond: attractive force holding two or more atoms together.

25. Chapter 06 – Slide 25 of 91 Ionic Bonds - electron transfer process. Typically between a metal and a nonmetals Covalent Bonds - electrons shared. Typically involving nonmetals.

26. Chapter 06 – Slide 26 of 91 Ionic compounds Consist of positive and negative ions. Have ionic bonds between positively and negatively charged ions. Have high melting and boiling points. Are solid at room temperature. Ionic Compounds

27. Chapter 06 – Slide 27 of 91 Salt is An Ionic Compound Sodium chloride (table salt) is an example of an ionic compound. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

28. Chapter 06 – Slide 28 of 91 An ionic formula Consists of positively and negatively charged ions. Is neutral. Has charge balance. total positive charge = total negative charge Uses subscripts to indicate the number of ions needed to give charge balance. Ionic Formulas

29. Chapter 06 – Slide 29 of 91 Ionic Formula of NaCl In an ionic formula The symbol of the metal is written first followed by the symbol of the nonmetal. The charges of the ions in the compound are not shown. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

30. Chapter 06 – Slide 30 of 91 The formulas of ionic compounds are determined from the charges on the ions. atoms ions     – Na  +  F :  Na + : F :  NaF     sodium fluorine sodium fluoride The overall charge of NaF is zero (0). Na + F - = NaF (1+ ) + (1-) = 0 Charge Balance in NaF

31. Chapter 06 – Slide 31 of 91 Charge Balance In MgCl 2 In forming MgCl 2 A Mg atom loses two valence electrons. Two Cl atoms each gain one electron. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

32. Chapter 06 – Slide 32 of 91 Using Lewis Electron Dot Symbols Br Ca + → Br

33. Chapter 06 – Slide 33 of 91 Using Lewis Electron Dot Symbols Al + N →

34. Chapter 06 – Slide 34 of 91 Writing Ionic Formulas from Charges Charge balance is used to write the formula for sodium nitride, a compound containing Na + and N 3−. Na + 3Na + +N 3− = Na 3 N Na + 3(+1) + 1(3-) = 0 Note: the subscript 3 for three sodium ions.

35. Chapter 06 – Slide 35 of 91 Write the ionic formula of the compound with Ba 2+ and Cl . Write the symbols of the ions. Ba 2+ Cl  Balance the charges. Ba 2+ Cl  two Cl - needed Cl  Write the ionic formula using a subscript 2 for two chloride ions. BaCl 2 Formula from Ionic Charges

36. Chapter 06 – Slide 36 of 91 Write the correct formula for the ionic compounds formed by the following ions: 1. 2. 3. Learning Check

37. Chapter 06 – Slide 37 of 91 Naming and Writing Ionic Formulas Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

38. Chapter 06 – Slide 38 of 91 Naming of Ionic Compounds In the name of an ionic compound The positive ion (first ion) is named as the element. The negative ion (second ion) is named by changing the end of the element name to –ide.

39. Chapter 06 – Slide 39 of 91 Names of Some Common Ions 3A (13) Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Table 6.3

40. Chapter 06 – Slide 40 of 91 Complete the names of the following ions: Ba 2+ Al 3+ K + _________ __________ _________ N 3  O 2  F  _________ ___________________ P 3  S 2  Cl  _________ __________ _________ Learning Check

41. Chapter 06 – Slide 41 of 91 To name a compound that contains two elements Identify the cation and anion. Name the positive metal ion (cation) as the element. Name the anion by changing the ending to ide. Name the cation first followed by the name of the anion. Naming Ionic Compounds with Two Elements

42. Chapter 06 – Slide 42 of 91 Charges of Representative Elements Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

43. Chapter 06 – Slide 43 of 91 Formula IonsName NaClNa + Cl - sodium chloride K 2 SK + S 2- potassium sulfide MgOMg 2+ O 2- magnesium oxide CaI 2 Ca 2+ I - calcium iodide Al 2 O 3 Al 3+ O 2- aluminum oxide Some Ionic Compounds with Two Elements

44. Chapter 06 – Slide 44 of 91 More Ionic Compounds Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

45. Chapter 06 – Slide 45 of 91 Homework Assignment: Your Name:________________________ Write the formulas and names for compounds of the following ions: N 3− Br − S 2− Na + Al 3+

46. Chapter 06 – Slide 46 of 91 Write the names of the following compounds: 1) CaO___________ 2) KBr___________ 3) Al 2 O 3 ___________ 4) MgCl 2 ___________ Homework Assignment: Your Name:________________________

47. Chapter 06 – Slide 47 of 91 Most Transition Metals form Two or More Positive Ions Most of the transition metals Form 2 or more positive ions. For example, Copper forms Cu + and Cu 2+ Iron forms Fe 2+ and Fe 3+ Gold form Au + and Au 3+

48. Chapter 06 – Slide 48 of 91 Metals that form more than One Cation Table 6.4 Some Metals That Form More Than One Positive Ion Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Lead Pb 2+ lead(II) Pb 4+ lead(IV)

49. Chapter 06 – Slide 49 of 91 Periodic Table and Some Ions Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

50. Chapter 06 – Slide 50 of 91 Naming Variable Charge Metals Transition metals With two different ions use a Roman numeral after the name of the metal to indicate ionic charge. Only zinc, silver, and cadmium form one ion (Zn 2+, Ag +, and Cd 2+ ) Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

51. Chapter 06 – Slide 51 of 91 Naming FeCl 2 To name FeCl 2 [ 1 Iron ion + 2 chloride ions ] 1. Determine the charge of the cation using the charge of the anion (Cl - ). Fe ion + 2 Cl - = 1(?) + 2(1-) = 0 Fe ion = 2+ Fe 2+ 2. Name the cation by the element name and a Roman numeral in parenthesis to show charge. Fe 2+ = iron(II) 3. Write the name of the anion with an ide ending. iron(II) chloride = FeCl 2

52. Chapter 06 – Slide 52 of 91 Naming Cr 2 O 3 To name Cr 2 O 3 1. Determine the charge of cation from the anion (O 2- ). 2Cr ions + 3 O 2- = ? + 3(2-) = ? - 6 = 0 ? = +6 +6/ 2Cr ions = +3 Cr ion = 3+ Cr 3+ 2. Name the cation by the element name and use a Roman numeral in parenthesis to show its charge. Cr 3+ = chromium(III) 3. Write the name of the anion with -ide ending. chromium (III) oxide = Cr 2 O 3

53. Chapter 06 – Slide 53 of 91 Learning Check Select the correct name for each. 1. 2. P - 1

54. Chapter 06 – Slide 54 of 91 Writing Formulas Write the formula of potassium sulfide. STEP 1Identify the cation and anion. potassium = K + sulfide = S 2− STEP 2. Balance the charges. K + S 2− K + 2(1+) + 2(1-) = 0 STEP 3. 2 K + and 1 S 2− = K 2 S

55. Chapter 06 – Slide 55 of 91 Writing Formulas Write the formula of cobalt(III) chloride. STEP1. Identify the cation and anion. cobalt (III) = Co 3+ (III = charge of 3+) chloride = Cl − STEP 2. Balance the charges. Co 3+ Cl − Cl − = (3+) + 3(1-) = 0 Cl − STEP 3. 1 Co 3+ and 3 Cl − = CoCl 3

56. Chapter 06 – Slide 56 of 91 Learning Check The correct formula for each of the following is: 1. 2.

57. Chapter 06 – Slide 57 of 91 Polyatomic Ions Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

58. Chapter 06 – Slide 58 of 91 A polyatomic ion Is a group of atoms. Has an overall ionic charge. Some examples of polyatomic ions are NH 4 + ammoniumOH − hydroxide NO 3 − nitrateNO 2 − nitrite CO 3 2− carbonatePO 4 3− phosphate HCO 3 − hydrogen carbonate (bicarbonate) Polyatomic Ions

59. Chapter 06 – Slide 59 of 91 Some Compounds with Polyatomic Ions Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

60. Chapter 06 – Slide 60 of 91 The names of common polyatomic anions End in ate. NO 3 − nitratePO 4 3− phosphate With one oxygen less end in ite. NO 2 − nitritePO 3 3− phosphite With hydrogen attached use prefix hydrogen (or bi). HCO 3 − hydrogen carbonate (bicarbonate) HSO 3 − hydrogen sulfite (bisulfite) More Names of Polyatomic Ions

61. Chapter 06 – Slide 61 of 91 Names and Formulas of Common Polyatomic Ions Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

62. Chapter 06 – Slide 62 of 91 Names and Formulas of Common Polyatomic Ions Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

63. Chapter 06 – Slide 63 of 91 Polyatomic ions of the halogens require prefixes. ClO 4 − perchlorateone oxygen more ClO 3 − chlorate most common form ClO 2 − chloriteone oxygen less ClO − hypochlorite two oxygens less Prefixes for Names of Polyatomic Ions of Halogens

64. Chapter 06 – Slide 64 of 91 The positive ion is named first followed by the name of the polyatomic ion. NaNO 3 sodium nitrate K 2 SO 4 potassium sulfate Fe(HCO 3 ) 3 iron(III) bicarbonate or iron(III) hydrogen carbonate (NH 4 ) 3 PO 3 ammonium phosphite Naming Compounds with Polyatomic Ions

65. Chapter 06 – Slide 65 of 91 Some Compounds with Polyatomic Ions Table 5.7 Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

66. Chapter 06 – Slide 66 of 91 Select the correct formula for each: 1. 2. 3. 4. Learning Check P - 2

67. Chapter 06 – Slide 67 of 91 Match each formula with the correct name: 1. MgSA) magnesium sulfite B) magnesium sulfate C) magnesium sulfide D) calcium chlorate E) calcium chlorite F) calcium hypochlorite Learning Check 2. MgSO 3 3. MgSO 4 4. Ca(ClO 3 ) 2 5. Ca(ClO) 2 6. Ca(ClO 2 ) 2

68. Chapter 06 – Slide 68 of 91 Learning Check Name each of the following compounds: 1. Mg(NO 3 ) 2 2.Cu(ClO 3 ) 2 3.PbO 2 4.Fe 2 (SO 4 ) 3 5.Ba 3 (PO 3 ) 2

69. Chapter 06 – Slide 69 of 91 Writing Formulas with Polyatomic Ions The formula of an ionic compound Containing a polyatomic ion must have a charge balance that equals zero(0). Na + and NO 3 − →NaNO 3 With two or more polyatomic ions encloses the polyatomic ions in parentheses. Mg 2+ and 2NO 3 − → Mg(NO 3 ) 2 subscript 2 for charge balance

70. Chapter 06 – Slide 70 of 91 Learning Check Write the correct formula for each: 1.potassium bromate 2.calcium carbonate 3.sodium phosphate 4.iron(III) oxide 5.iron (II) nitrite

71. Chapter 06 – Slide 71 of 91 Naming Ionic Compounds Review: Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Table 5.8

72. Chapter 06 – Slide 72 of 91 Flowchart for Naming Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

73. Chapter 06 – Slide 73 of 91 Learning Check Name the following compounds: A. Ca 3 (PO 4 ) 2 B. FeBr 3 C. Al 2 S 3 D. Mn(NO 2 ) 2 E. NaHCO 3

74. Chapter 06 – Slide 74 of 91 Learning Check Write the formulas for the following: A. calcium nitrate B. iron(II) hydroxide C. aluminum carbonate D. copper(II) hypobromite E. lithium phosphate

75. Chapter 06 – Slide 75 of 91 Covalent Compounds and Their Names Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

76. Chapter 06 – Slide 76 of 91 Forming a H 2 Molecule Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

77. Chapter 06 – Slide 77 of 91 H 2, A Covalent Molecule In a hydrogen (H 2 ) molecule Two hydrogen atoms share electrons to form a covalent single bond. Each H atom acquires two (2) electrons. Each H becomes stable like helium (He). Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

78. Chapter 06 – Slide 78 of 91 Diatomic Elements These elements share electrons to form diatomic, covalent molecules. Table 6.9 Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

79. Chapter 06 – Slide 79 of 91 Electron-Dot Formulas Electron-dot formulas show The order of bonded atoms in a covalent compound. The bonding pairs of electrons between atoms. The unshared (lone) valence electrons if they exist. A central atom with an octet. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

80. Chapter 06 – Slide 80 of 91 Electron-Dot Formulas and Models of Some Covalent Compounds Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings Table 5.10

81. Chapter 06 – Slide 81 of 91 Names of Covalent Compounds Prefixes are used In the names of covalent compounds. Because typically two nonmetals can form two or more different compounds. Examples of compounds of N and O: NO nitrogen oxide NO 2 nitrogen dioxide N 2 O dinitrogen oxide N 2 O 4 dinitrogen tetroxide N 2 O 5 dinitrogen pentoxide

82. Chapter 06 – Slide 82 of 91 Naming Covalent Compounds STEP 1 Name the first nonmetal as the element. STEP 2 End the name of the second nonmetal with -ide STEP 3 Use prefixes to show the number of atoms (subscripts). Mono is usually omitted. Table 6.11 Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

83. Chapter 06 – Slide 83 of 91 What is the name of SO 3 ? STEP 1 The first nonmetal is S sulfur. STEP 2 The second nonmetal is O named oxide. STEP 3 The subscript 3 of O is shown as the prefix tri. SO 3 → sulfur trioxide The subscript 1(for S) or mono is understood. Naming Covalent Compounds

84. Chapter 06 – Slide 84 of 91 Name P 4 S 3 STEP 1 The first nonmetal P is phosphorus. STEP 2 The second nonmetal S is sulfide. STEP 3 The subscript 4 of P is shown as tetra. The subscript 3 of O is shown as tri. P 4 S 3 → tetraphosphorus trisulfide Naming Covalent Compounds

85. Chapter 06 – Slide 85 of 91 Formulas and Names of Some Covalent Compounds Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings TABLE 6.12

86. Chapter 06 – Slide 86 of 91 Select the correct name for each compound. A.SiCl 4 1) 2) 3) B. P 2 O 5 1) 2) 3) C.Cl 2 O 7 1) 2) 3) Learning Check

87. Chapter 06 – Slide 87 of 91 Write the name of each covalent compound: CO CO 2 PCl 3 CCl 4 N 2 O Learning Check

88. Chapter 06 – Slide 88 of 91 STEP 1 Write the symbols in the order of the elements in the name. STEP 2 Write any prefixes as subscripts. Example: Write the formula for carbon disulfide. STEP 1 Elements are C and S STEP 2 No prefix for carbon means 1 C Prefix di = 2 Formula: CS 2 Guide to Writing Formulas

89. Chapter 06 – Slide 89 of 91 Write the correct formula for each of the following: A. phosphorus pentachloride B. dinitrogen trioxide C. sulfur hexafluoride Learning Check

90. Chapter 06 – Slide 90 of 91 Learning Check Identify each compound as ionic or covalent and give its correct name. 1. SO 3 2. MnCl 2 3. (NH 4 ) 3 PO 3 4. Cu 2 CO 3 5. N 2 O 4

91. Chapter 06 – Slide 91 of 91 Learning Check Identify each compound as ionic or covalent and give its correct name. 1.Ca 3 (PO 4 ) 2 2.FeBr 3 3.SCl 2 4.Cl 2 O