1. Formulas and Nomenclature

2. Covalent Bonds  Bond between a 2 nonmetals  Polar or nonpolar  Share electrons

3. Ionic Bonds  Transfer of electrons  Bond between a metal and nonmetal Bond between a cation and anion Bond between a cation and anion Cation: positive ion; usually metalCation: positive ion; usually metal Anion: negative ion; usually nonmetalAnion: negative ion; usually nonmetal

4. Metallic Bonds  Between 2 metals Make an alloy Make an alloy

5. Naming Ionic Compunds  Name the cation first and the anion second Cation is always written first in a compound Cation is always written first in a compound  1 st : write the element name for the cation  2 nd : write the root of the anion and attach -ide

6. Example- NaBr  Na + Br -  Cation: Sodium  Anion: Bromine  root: brom Attach ide Attach ide  Name: Sodium Bromide

7. Practice  CaCl 2  MgF 2  Li 2 S

8. Writing the formula for ionic compounds  When given the name, remember 1st element is the cation 1st element is the cation 2 nd element is the anion 2 nd element is the anion

9. Example- Calcium Chloride  Cation first and anion second  Cation: Calcium  Anion: Chloride  Ca 2+ Cl 2 1-  Formula: CaCl 2

10. Practice  Aluminum Bromide  Magnesium Chloride  Potassium Iodide

11. The Criss Cross Method, Polyatomic Ions, and Transition Metals

12. Example- Potassium Oxide  Cation: K +1  Anion: O -2 K +1 O -2  Chemical Formula: K 2 O

13. Criss Cross Practice  Calcium Iodide  Aluminum Selenide  Strontium Nitride  Sodium Oxide

14. Example- FeCl 2  From the criss cross method, you can determine your charges on your cation and anion, which is important when you have transition metals involved Fe Cl 2  Cation: Fe +2  Anion: Cl -1  Name: Iron (II) Chloride Why (II)? Stay tuned… Why (II)? Stay tuned…

15. Monatomic vs. Polyatomic Ions  Monatomic: one atom make up the ion Ex. Cl 1- Ex. Cl 1-  Polyatomic: multiple atoms make up the ion Ex. NH 4 + Ex. NH 4 +

16. Polyatomic Ions  Page 7 of your chemistry reference tables list all the polyatomic ions Blue sheet Blue sheet

17. Naming Ionic Compounds with Polyatomic Ions  1 st : Name the cation with the charge in parentheses if it is a transitional metal Why charge in parentheses for transitional metals? Stay tuned… Why charge in parentheses for transitional metals? Stay tuned…  2 nd : name the polyatomic ion

18. Example- NaOH  Cation: Sodium Na +1 Na +1  Anion: Hydroxide OH -1 OH -1  Name: Sodium Hydroxide

19. Writing the formula for ionic compounds that contain polyatomic ions  When given the name, remember 1st element is the cation 1st element is the cation 2 nd element is the anion or polyatomic ion 2 nd element is the anion or polyatomic ion

20. Example- Hydrogen Chlorate  Cation: Hydrogen H + H +  Anion: Chlorate ClO 3 - ClO 3 -  Formula: HClO 3

21. Practice- Name the following compounds or determine their chemical formulas  PbSO 3  Be(NO 2 ) 2  Ti 3 (PO 4 ) 2  Magnesium Nitrate  Aluminum Carbonate  Hydrogen Sulfate

22. Day 2

23. Transition Metals  use the same steps for naming the compound Name the cation using the elements name and then the anion using the root and adding -ide Name the cation using the elements name and then the anion using the root and adding -ide  Because transition metals can have multiple charges, put the charge after the cation’s name in parentheses

24. Example-FeCl 3  1 st : identify the cation and anion  Fe 3+ Cl 1- From the criss cross, method we know that the charge on Fe is +3 and Cl is -1 From the criss cross, method we know that the charge on Fe is +3 and Cl is -1  Cation: Iron (III) Place the charge in parentheses Place the charge in parentheses  Anion: Chlorine  root: chlor Add ide Add ide  Name: Iron (III) chloride

25. Transition Metals Continued…  If you are not given a specific charge, stick to the rule that all transition metals have 2 valence electrons so they have a +2 charge  If you are given the compounds name and you are trying to determine the formula but there is no number in parentheses, the transition metal’s charge is the same as the charge on the anion  Ex. Iron Sulfide: Fe 2+ and S 2-

26. Practice- Name or determine the chemical formula for the following compounds  CuBr 2  FeN  Ti 2 Se 3  Copper Fluoride  Nickel (II) Arsenide  Lead (I) Sulfide

27. Extra Credit  Using 50 of the vocabulary terms we have had thus far, make a crossword puzzle. Needs to have the definitions as the clues Needs to have the definitions as the clues  Turn in the blank crossword puzzle as well as the key  Replace your lowest test grade  Due Monday March 22, 2010

28. Complete the chart below FormulaIonic, Cov or both? Transitional Metal? Name CaBr 2 N2ON2O Fe 2 O 3 Cu 3 (PO 4 ) 2 Nitrogen Trioxide

29. Naming Acids  All acids start with H criss cross H with polyatomic ion to get the acid it makes criss cross H with polyatomic ion to get the acid it makes  Ex. Hydrogen and Phosphate H 3 PO 4 H 3 PO 4

30. 3 categories of acids  Binary acids – only 2 elements make up the acid hydro____ic acid hydro____ic acid Ex. HF  Hydrofluoric AcidEx. HF  Hydrofluoric Acid  Polyatomics with –ate ending Replace –ate with ic Replace –ate with ic Ex. HCO 3 - Carbonic AcidEx. HCO 3 - Carbonic Acid  Polyatomics with –ite ending Replace ite with ous Replace ite with ous Ex. HNO 2 - Nitrous AcidEx. HNO 2 - Nitrous Acid  If I ATE it, I said IC!! If I bITE it, I say deliciOUS

31. Name or determine the formula for the following acids:  HCl  HBrO 3  HIO 3  H 2 CrO 4  Hydrobromic Acid  Perchloric Acid  Dichromic Acid  Sulfurous Acid

32. Midterm Review Day 1

33. 4 th Block ONLY  Agenda Catalyst (15) Catalyst (15) Midterm Review Quiz (40) Midterm Review Quiz (40) Molar Conversions Review (30) Molar Conversions Review (30) Questions (5) Questions (5) Closing (1) Closing (1)  Essential Question What objectives do you need additional practice with before the midterm?  Objective (s) Exhibit mastery on all objectives covered thus far in the semester  Homework Molar conversions review

34. Day 4

35. Complete the following:  Calculate the molar mass of the following: PbSO 3 PbSO 3 C 2 H 5 OH C 2 H 5 OH  How many grams are in 3.45 moles of AlBr 3 ?  What is the mass of 2.55 moles of potassium permanganate?

36. Prerequisites for Understanding Percent Composition  You must be able to: Calculate molar mass Calculate molar mass Convert moles to grams Convert moles to grams Convert grams to moles Convert grams to moles Determine chemical formulas when given the name Determine chemical formulas when given the name

37. Percent Composition The percent by mass of each element in a compound

38. Percent by mass Mass of element Mass of element ---------------------------- X 100 Mass of Compound Mass of Compound

39. Percent composition of compound XYZ Percent mass of X Percent mass of Y Percent mass of Z

40. Example- What is the percent composition of NaCl?  Step 1: calculate the molar mass  Step 2: Calculate the percent by mass of each element  Step 3: percent composition of the compound

41. Example- NaCl  Molar mass: Na: 23g/molNa: 23g/mol Cl: 35.5g/molCl: 35.5g/mol Total: 58.5g/molTotal: 58.5g/mol  Percent mass of each element: Na: (23/58.5) X 100 = 39% Na: (23/58.5) X 100 = 39% Cl: (35.5/58.5) X 100 = 61% Cl: (35.5/58.5) X 100 = 61%  Percent composition of the compound: 39% Na 39% Na 61% Cl 61% Cl

42. Practice Example  Determine the percent composition of water (H 2 O) Step 1: Determine the Molar Mass Step 1: Determine the Molar Mass Step 2: Determine the percent mass of each element Step 2: Determine the percent mass of each element Step 3: Determine the percent composition of the compound Step 3: Determine the percent composition of the compound

43. Practice Problems

44. Determine the percent composition of HClO 3

45. Determine the percent composition of KMnO 4

46. Determine the percent composition of HCl

47. Determine the percent composition of Mg(NO 3 ) 2

48. Agenda  HOMEWORK 10 percent composition problems on the handout 10 percent composition problems on the handout

49. Day 5

50. 4 th Block ONLY  Agenda Catalyst (5) Catalyst (5) Molar Conversions Gallery Walk (10) Molar Conversions Gallery Walk (10) Midterm Review Quiz 1 (15) Midterm Review Quiz 1 (15) Midterm Review Quiz 2 (45) Midterm Review Quiz 2 (45) Questions (10) Questions (10) Closing (5) Closing (5)  Essential Question What units do you need to spend additional time reviewing tonight for tomorrow’s midterm?  Objectives Exhibit mastery on all objectives covered thus far in the semester  Homework Study for the midterm

51. Catalyst  Determine the percent composition of the following: (NH 4 ) 3 PO 4 (NH 4 ) 3 PO 4 Al 2 (SO 4 ) 3 Al 2 (SO 4 ) 3

52. Empirical Formula The formula with the smallest whole-number mole ratio of the elements

53. Molecular Formula The formula that specifies the actual number of moles in the compound

54. Determine the chemical formula for Dinitrogen Tetroxide

55. Example  Chemical Formula: N 2 O 4 N 2 O 4 Molecular FormulaMolecular Formula  Have the subscripts been reduced? NO NO  Reduce the subscripts NO 2 NO 2 Empirical FormulaEmpirical Formula

56. Practice  Determine the empirical and molecular formulas for the following compounds: Aluminum Bromide Aluminum Bromide Copper (II) Oxide Copper (II) Oxide Magnesium Nitride Magnesium Nitride Carbon Tetrafluoride Carbon Tetrafluoride

57. How do you determine the empirical formula when given the percent composition?

58. Example- What is the empirical formula for a blue solid that has a molar mass of 152g/mol and contains 36.84% nitrogen and 63.16% oxygen?

59. Step 1:  Use the percent as the number of grams of that element  Example: N: 36.84g N: 36.84g O: 63.16g O: 63.16g

60. Step 2: Convert your grams from step 1 to moles

61. Step 3: Divide each mole value by the smallest value

62. Step 4: Multiply the numbers of moles in the ratio by the smallest number that will produce a ratio of whole numbers

63. Empirical Formula N2O3N2O3N2O3N2O3

64. How do you determine the molecular formula when given the percent composition?

65. Step 1:  Find the empirical formula  Example: N 2 O 3 N 2 O 3

66. Step 2: Calculate the molar mass of the empirical formula

67. Step 3: Divide the molar mass of the compound as given in the original problem by the molar mass of the empirical formula

68. Step 4:  Multiply the subscripts in the empirical formula by answer in step 3 to determine the actual subscripts in the molecular formula  Example: N: 2 x 2 =4 N: 2 x 2 =4 O: 3 x 2 = 6 O: 3 x 2 = 6

69. Molecular Formula N4O6N4O6N4O6N4O6

70. Practice Problems

71. A colorless liquid composed of 46.68% N and 53.32% O has a molar mass of 60.01 g/mol. What is the empirical and molecular formula of this liquid?

72. Determine the empirical and molecular formula of a compound containing 65.45% C, 5.45% H, and 29.09% O with a molar mass of 110g/mol

73. A compound is found to contain 49.98g carbon and 10.47g hydrogen. The molar mass of the compound is 58.12g/mol. Determine the empirical and molecular formula of this compound.

74. Agenda  Homework Pg. 349: 143-150 Pg. 349: 143-150