1. Bonding and Nomenclature Ionic and Covalent Bonds

2. What is a chemical bond? A force that holds 2 atoms together.

3. Why do atoms bond? To have 8 valence electrons.

4. What are the 8 valence electrons called? An octet.

5. What attracts two atoms together? Positive and negative forces attract.

6. What is an ion called that has lost electrons? A cation

7. Why does it lose electrons? In order to have a full valence shell.

8. When an atom gain or loses electrons what does it resemble? A noble gas.

9. What do metals do to have full valence shells? Form cations.

10. How predictable are metals cations? Very! Use the periodic table.

11. How do I use the periodic table? Group 1 +1 Group 2 +2 Group13 +3 Group 14 +4

12. How do you name a cation? Its just the element name with ion at the end

13. What is an example? Al +3 Na +

14. What about transition metals? They lose different numbers of electrons, depending on the situation they are in.

15. How do you know how many they lost? The metal will have a roman numeral after the element name.

16. What is an example? Cu +2 Iron (III) ion

17. What is the charge called? An oxidation number

18. What is an ion that has gained electron called? An anion

19. What are most nonmetals? Anions

20. What about the metalloids? Above the stair step, they act more like nonmetals (anions) Under the stair step, they act more like metals (cations)

21. What kinds of charges do the anions have? Group 14 -4 Group 15 -3 Group 16 -2 Group 17 -1

22. How do you name anions? Drop the last part of the name and add -ide.

23. What is an example? O 2- F -

24. Here are all the PT anions … Hydride Carbide Nitride Oxide Fluoride Silicide Phosphide Sulfide Chloride Arsenide Selenide Bromide Telluride Iodide

25. What is a polyatomic ion? They are groups of ions that gain or lose electrons as a whole Don’t EVER change their name or formula. EVER!

26. Can you split up polyatomic ions? No!

27. What are some examples? Sulfate (SO 4 ) -2 Sulfite (SO 3 ) -2

28. Where can I find the polyatomic ions? On the back of my periodic table FOR THE TEST YOU MUST KNOW THE 12 PAI WE LEARNED BEFORE!

29. NamePolyatomic IonNamePolyatomic Ion AcetateC 2 H 3 O 2 -1 HydroxideOH -1 AmmoniumNH 4 +1 HypobromiteBrO -1 BromateBrO 3 -1 HypochloriteClO -1 BromiteBrO 2 -1 NitrateNO 3 -1 CarbonateCO 3 -2 NitriteNO 2 -1 ChlorateClO 3 -1 OxalateC 2 O 4 -2 ChloriteClO 2 -1 PerbromateBrO 4 -1 ChromateCrO 4 -2 PerchlorateClO 4 -1 CyanateOCN -1 PermanganateMnO 4 -1 CyanideCN -1 PhosphatePO 4 -3 DichromateCr 2 O 7 -2 PhosphitePO 3 -3 Dihydrogen PhosphiteH 2 PO 4 -1 SelenateSeO 4 -2 BicarbonateHCO 3 -1 SulfateSO 4 -2 Hydrogen PhosphateHPO 4 -2 SulfiteSO 3 -2 Hydrogen SulfateHSO 4 -1 ThiocyanateSCN -1 Hydrogen SulfiteHSO 3 -1 ThiosulfateS 2 O 3 -2

30. What does an ionic bond contain? A cation and an anion.

32. How do I write an ionic chemical formula? Find the charge of the cation Find the charge of the anion Swap and drop the charges Reduce charges if possible

34. The Compound end up NEUTRAL!!! The charges cancel each other out!

35. Examples K and Br Ca and PO 4 -3 Rb and P Mg and S Sr and Si

36. How do you name ionic formulas? Name the cation Name the anion NaCl is Sodium Chloride

37. Examples Calcium Oxide Aluminum chloride Cs 2 Se InBr 3

38. How do I name it if there is a PAI in the formula? Do NOT EVER change the NAME of the PAI! NEVER! Ca(OH) 2 is calcium hydroxide

39. Differences in: Nitrate Nitrite Nitride

40. What is special about the transition metals? You HAVE to write the oxidation number as a roman numeral between the cation and anion.

41. What 2 elements are transition metal wannabes? Tin and Lead They get roman numerals too!

42. Example FeCl 3 SnO Chromium (III) Telluride Molybdenum (VI) Sulfide

43. Example problem Write all of the correct formulas between sulfur, sodium, chlorate, iron (II), and nitrogen.

44. What happens in ionic bonds? Electrons are transferred from the cation to the anion.

45. What is one property of ionic compounds? The compounds are packed into repeating patterns.

46. What are these repeating patterns called? Crystal lattices.

47. What is the smallest part of a crystal lattice? A formula unit Basically one of your formulas you wrote

48. What else can be said about ionic bonds? They have high melting points and high boiling points compared to other bonds

49. What about their strength? They are very strong compounds. They take a lot of energy to break apart.

50. What else do ionic bonds do? They conduct electricity in aqueous solutions.

51. What is another term for that? Electrolytes

52. How else do atoms find an octet? They make covalent bonds.

53. What is a covalent bond? When atoms share electrons to make an octet.

54. What makes up a covalent bond? Two nonmetals.

55. Can two metals ever make a bond? No

56. Why not? They form an alloy instead of a chemical bond.

57. What is an alloy? A mixture of 2 or more metals.

58. What is formed when you have a covalent bond? A molecule

59. What are the most common covalent bonds? Diatomic elements.

60. What is a diatomic element? One that bonds to itself.

61. What are the diatomic elements? BrINClHOF Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, Fluorine

62. How are they always written? Br 2, I 2, N 2, Cl 2, H 2, O 2, F 2

63. How are they named? Just by their names, even though there are 2 of them.

64. Examples of diatomic compounds: Hydrogen Br 2 Iodine

65. How are covalent bonds named? By using prefixes.

66. What are the prefixes? Mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

67. What is the first rule? The first element stays the same, the second ends in –ide.

68. What is the second rule? Add the prefixes to tell how many of each element are present.

69. What is the third rule? Never begin a molecule name with mono-.

70. Do I reduce a covalent compound? No! Never!

71. What is an example? C 5 H 7 NO PO 4 difluorine monosulfide

72. What if the compound begins with H? The compound is an acid. HCl HClO 3 H 2 S

73. How are acids named? It depends on their ending or what is bonding.

74. What is an –ide acid? One that contains hydrogen and an anion that ends in -ide

75. How are –ide acids named? Start with hydro- Write the “root” of the anion End with –ic Acid HCl is Hydrochloric acid

76. What are some odd roots for anions? P becomes phosphoric S becomes sulfuric C becomes carbonic For the rest, where you would write –ide put –ic instead.

77. Examples H 2 S H 3 P hydronitric acid hydrobromic acid Hydrocyanic acid

78. What about naming –ate and –ite acids? Do not start with hydro- If it ends in –ate, substitute –ic Acid If it ends in –ite, substitute –ous Acid H 2 CO 3 is Carbonic Acid HClO 2 is Chlorous Acid

79. What are the 2 odd polyatomic ions? Phosphate/ite and sulfate/ite. Becomes: phosphoric or phosphorous Sulfuric or sulfurous H 2 SO 4 is Sulfuric Acid H 3 PO 3 is Phosphorous Acid

80. Examples HClO 4 HClO 3 Bromic acid Cyanic acid

81. What are some characteristics of covalent bonds? They are relatively weak bonds. They are not strong as solids.

82. What else? They have low melting and boiling points

83. Are they electrolytes? No

84. Molecular Shape

85. What is an electron dot structure? It is a way of showing the valence electrons bonding and lone pairs of electrons.

86. What is a lone pair? A pair of electrons in the valence shell that are not bonded.

87. How many bonds can be in between covalent compounds? One, two or three

88. What is a single bond? Two bonded elements sharing one pair of electrons

89. What is a double bond? Two bonded elements sharing 2 pair of electrons.

90. What is a triple bond? Two bonded elements sharing three pairs of electrons.

91. What is VSEPR? Valence Shell Electron Pair Repulsion It helps us to know the shape of compounds, as electrons try to spread as far away from one another as possible.

92. What are the shapes we will study? Linear Tetrahedral Trigonal Planar Bent Pyramidal

93. What is the first shape? Linear

94. What is a linear molecule made of? Contain two atoms, but even some with three atoms can be linear

95. What is another shape? Trigonal Planar A shape that is flat and triangular in shape, on a single plane in space

96. What is a trigonal planar molecule made up of? Molecules with three atoms, or two atoms and a lone pair, surrounding a central atom on one plane

97. What is another shape? Tetrahedral A shape that has four surfaces, such as a pyramid, 3-D in space

98. What makes up a tetrahedral molecule? Molecules contain four atoms that surround a central atom

99. What is yet another shape? Pyramidal Similar to tetrahedral

100. What is a pyramidal molecule made up of? Three atoms around a central atom and ONE lone pair

101. What is the last molecular shape? Bent Similar to tetrahedral

102. What makes up a bent molecule? Two atoms around a central atom and TWO lone pairs

103. LinearHas only 2 bonds Has only 2 atoms Number of Bonds Around Central Atom Number of Lone Pairs on Central Atom Trigonal Planar3232 0101 Tetrahedral40 Pyramidal31 Bent22

104. What is polarity? When one atom is more electronegative, so it does not share electrons fairly.

105. What is a polar molecule? They do not share equally When one atom has a difference of EN of 0.4-1.7

106. What is a non polar molecule? One in which the atoms share equally. EN is less than 0.4

107. What is an ionic bond? A molecule that does not share, it steals electrons. EN is more than 1.7

108. Where do I find these electronegativities? In a chart.

109. Electronegativities

110. What happens with molecular shape and polarity? If the shape is symmetrical, the molecule is NON POLAR

111. What do we do with polarity? It helps us to figure out if things will dissolve into one another.

112. What is the rule? The “ like dissolves like ” rule.

113. What polarity is water? Polar