1. Chapter 7- Chemical Formulas and Chemical Compounds

2. Ban Dihydrogen Monoxide! Colorless, odorless, tasteless Colorless, odorless, tasteless Kills uncounted thousands of people every year. Kills uncounted thousands of people every year. Most deaths caused by accidental inhalation Most deaths caused by accidental inhalation Prolonged exposure to its solid form causes severe tissue damage. Prolonged exposure to its solid form causes severe tissue damage. Symptoms of ingestion can include Symptoms of ingestion can include excessive sweating and urination, excessive sweating and urination, a bloated feeling, a bloated feeling, nausea, nausea, vomiting vomiting body electrolyte imbalance. body electrolyte imbalance. For those who have become dependent, withdrawal means certain death. For those who have become dependent, withdrawal means certain death.

3. Ban Dihydrogen Monoxide! Also known as hydroxl acid Also known as hydroxl acid Major component of acid rain Major component of acid rain Contributes to the "greenhouse effect." Contributes to the "greenhouse effect." May cause severe burns. May cause severe burns. Contributes to the erosion of our natural landscape. Contributes to the erosion of our natural landscape. Accelerates corrosion and rusting of many metals. Accelerates corrosion and rusting of many metals. May cause electrical failures and decreased effectiveness of automobile brakes. May cause electrical failures and decreased effectiveness of automobile brakes. Been found in excised tumors of terminal cancer patients. Been found in excised tumors of terminal cancer patients. Is now an ingredient in most foods and beverages Is now an ingredient in most foods and beverages

4. Ban Dihydrogen Monoxide! Based on the evidence presented in the previous two slides, do you support the banning of dihydrogen monoxide? Based on the evidence presented in the previous two slides, do you support the banning of dihydrogen monoxide? Write at least two sentences stating your reasoning. Write at least two sentences stating your reasoning. Please sign the petition! Please sign the petition!

5. What is Dihydrogen Monoxide?

6. Chemical Formulas Indicate the relative number of atoms or ions of each kind in a chemical compound Indicate the relative number of atoms or ions of each kind in a chemical compound C 8 H 18 MgCl 2 Ca(OH) 2 8 C atoms18 H atoms 2 OH - ions 2 Cl - ions 1 Ca 2+ ion 1 Mg 2+ ion

7. Monatomic Ions Ions formed from a single atom Ions formed from a single atom Usually have noble gas configurations Usually have noble gas configurations That’s how we determine its charge That’s how we determine its charge Example: Example: Li: 1s 2 2s 1 Li: 1s 2 2s 1 Li + : 1s 2 or [He] Li + : 1s 2 or [He] Table on p.221 on monatomic ions Table on p.221 on monatomic ions

8. Naming Monatomic Cations Use the element’s name! Use the element’s name! Yes, it’s that simple! Yes, it’s that simple! Example: Example: Cs + = cesium Cs + = cesium Al 3+ = aluminum Al 3+ = aluminum

9. Naming Monatomic Anions Drop the ending of the element’s name Drop the ending of the element’s name Add the ending –ide Add the ending –ide Examples: Examples: Cl - = chloride Cl - = chloride N 3- = nitride N 3- = nitride

10. Naming Monatomic Ions K + K + S 2- S 2- Rb + Rb + O 2- O 2- I - I - Ba 2+ Ba 2+ Cu + Cu + potassium potassium sulfide sulfide rubidium rubidium oxide oxide iodide iodide barium barium copper copper

11. Binary Ionic Compounds Compounds composed of two ions Compounds composed of two ions Total numbers of positive charges and negative charges must be equal Total numbers of positive charges and negative charges must be equal Examples: Examples: NaCl NaCl KBr KBr CaF 2 CaF 2

12. Writing Binary Ionic Compounds Write the symbols for the ions side by side. Write the cation first. Write the symbols for the ions side by side. Write the cation first. Al 3+ O 2- Cross over the charges to use as the subscript for the other ion. Cross over the charges to use as the subscript for the other ion. Al 3+ O 2- Al 2 O 3

13. Writing Binary Ionic Compounds Check the subscripts and divide them to give the smallest whole number ratio of ions. Check the subscripts and divide them to give the smallest whole number ratio of ions. Al 2 O 3 Write the formula! Write the formula! Al 2 O 3

14. Writing Binary Ionic Compounds Zinc iodide Zinc iodide Barium fluoride Barium fluoride Lithium oxide Lithium oxide Calcium oxide Calcium oxide Magnesium bromide Magnesium bromide ZnI 2 ZnI 2 BaF 2 BaF 2 Li 2 O Li 2 O CaO CaO MgBr 2 MgBr 2

15. Naming Binary Ionic Compounds Give name of cation first Give name of cation first Then name the anion Then name the anion Al 2 O 3 Al 2 O 3 Name of cation: aluminum Name of cation: aluminum Name of anion: oxide Name of anion: oxide Name of compound: aluminum oxide Name of compound: aluminum oxide

16. Naming Binary Ionic Compounds BaI 2 BaI 2 ZnF 2 ZnF 2 K 2 O K 2 O MgO MgO CaBr 2 CaBr 2 Barium iodide Barium iodide Zinc fluoride Zinc fluoride Potassium oxide Potassium oxide Magnesium oxide Magnesium oxide Calcium bromide Calcium bromide

17. Cations With Different Charges Some elements form two or more cations with different charges Some elements form two or more cations with different charges Fe 2+ and Fe 3+ Fe 2+ and Fe 3+ Iron (II) and Iron (III) Iron (II) and Iron (III) Naming compounds Naming compounds FeO and Fe 2 O 3 FeO and Fe 2 O 3 Iron (II) oxide and Iron (III) oxide Iron (II) oxide and Iron (III) oxide

18. Name the Following Compounds CuO CuO CoF 3 CoF 3 SnI 4 SnI 4 FeS FeS Copper (II) oxide Copper (II) oxide Cobalt (III) fluoride Cobalt (III) fluoride Tin (IV) iodide Tin (IV) iodide Iron (II) sulfide Iron (II) sulfide

19. Quiz- Name the Following Compounds 1. K 2 S 2. AgBr 3. Na 2 O 4. FeCl 2 5. BaS 6. Lithium fluoride 7. Silver iodide 8. Iron (III) oxide 9. Magnesium iodide 10. Gold chloride

20. Polyatomic Ions Ions that contain two or more atoms Ions that contain two or more atoms Most are negatively charged Most are negatively charged List of polyatomic ions is on handout List of polyatomic ions is on handout **MEMORIZE THEM!!!** **MEMORIZE THEM!!!** Examples: Examples: CN - cyanide CN - cyanide HCO 3 - hydrogen carbonate (bicarbonate) HCO 3 - hydrogen carbonate (bicarbonate) NH 4 + ammonium NH 4 + ammonium

21. Polyatomic Ions You will need to memorize the following: You will need to memorize the following: AmmoniumNH 4 +1 AmmoniumNH 4 +1 AcetateC 2 H 3 O 2 -1 AcetateC 2 H 3 O 2 -1 HydroxideOH -1 HydroxideOH -1 NitriteNO 2 -1 NitriteNO 2 -1 NitrateNO 3 -1 NitrateNO 3 -1 BicarbonateHCO 3 -1 BicarbonateHCO 3 -1 CarbonateCO 3 -2 CarbonateCO 3 -2 ChromateCrO 4 -2 ChromateCrO 4 -2 SulfateSO 4 -2 SulfateSO 4 -2 PhosphatePO 4 -3 PhosphatePO 4 -3

22. Oxyanions Polyatomic ions that contain oxygen Polyatomic ions that contain oxygen Name depends on number of oxygen atoms Name depends on number of oxygen atoms

23. Oxyanions (cont.) If two oxyanions- If two oxyanions- Most oxygens: -ate Most oxygens: -ate Least oxygens: -ite Least oxygens: -ite Example Example NO 3 - : nitrate NO 3 - : nitrate NO 2 - : nitrite NO 2 - : nitrite

24. Oxyanions (cont.) If more than two oxyanions If more than two oxyanions Most oxygens: “Per- …. –ate” Most oxygens: “Per- …. –ate” “-ate” “-ate” “-ite” “-ite” Least oxygens: “Hypo- …. –ite” Least oxygens: “Hypo- …. –ite” Example Example ClO 4 - : perchlorate ClO 4 - : perchlorate ClO 3 - : chlorate ClO 3 - : chlorate ClO 2 - : chlorite ClO 2 - : chlorite ClO - : hypochlorite ClO - : hypochlorite

25. Polyatomic Ion Quiz Sodium hypochlorite Sodium hypochlorite Potassium sulfate Potassium sulfate Magnesium peroxide Magnesium peroxide Ammonium chloride Ammonium chloride Lithium nitrate Lithium nitrate Potassium phosphate Potassium phosphate NaClO K2SO4 MgO2 NH4Cl LiNO3 K3PO4

26. Polyatomic Ion Quiz 1. Bicarbonate 2. Acetate 3. Bisulfite 4. Permanganate 5. Nitrite 6. Cyanide 7. Hydroxide 8. Bisulfate 9. Nitrate 10. What’s your favorite polyatomic ion?

27. Binary Molecular Compounds Composed of molecules (covalently bonded!) Composed of molecules (covalently bonded!) A nonmetal bonded to another nonmetal A nonmetal bonded to another nonmetal Examples: Examples: SO 3 SO 3 ICl 3 ICl 3 CH 4 CH 4 H 2 O H 2 O

28. Prefixes for Naming Binary Molecular Compounds 1mono- 1mono- 2di- 2di- 3tri- 3tri- 4tetra- 4tetra- 5penta- 5penta- 6hexa- 6hexa- 7hepta- 7hepta- 8octa- 8octa- 9nona- 9nona- 10deca 10deca

29. Naming Binary Molecular Compounds Which element goes first? Which element goes first? Smaller group number Smaller group number If same group- greater period number If same group- greater period number Use prefix only if there is more than one atom Use prefix only if there is more than one atom Second element Second element Prefix indicating number of atoms + root of the name of the element + -ide Prefix indicating number of atoms + root of the name of the element + -ide General order of elements in binary compounds: General order of elements in binary compounds: C, P, N, H, S, I, Br, Cl, O, F C, P, N, H, S, I, Br, Cl, O, F

30. Naming Binary Molecular Compounds Examples: Examples: SO 3 – sulfur trioxide SO 3 – sulfur trioxide BrCl 3 – bromine trichloride BrCl 3 – bromine trichloride PBr 5 – phosphorus pentabromide PBr 5 – phosphorus pentabromide N 2 O 5 – dinitrogen pentoxide N 2 O 5 – dinitrogen pentoxide

31. Naming Binary Molecular Compounds N 2 O N 2 O CCl 4 CCl 4 NO NO CO 2 CO 2 N 2 O 3 N 2 O 3 P 4 O 10 P 4 O 10 Dinitrogen monoxide Dinitrogen monoxide Carbon tetrachloride Carbon tetrachloride Nitrogen monoxide Nitrogen monoxide Carbon dioxide Carbon dioxide Dinitrogen trioxide Dinitrogen trioxide Tetraphosphorus decoxide Tetraphosphorus decoxide

32. Naming Binary Molecular Compounds- More Practice! Disulfur dioxide Disulfur dioxide Silicon tetrafluoride Silicon tetrafluoride Sulfur monoxide Sulfur monoxide Phosphorus trioxide Phosphorus trioxide Boron trifluoride Boron trifluoride Diphosphorus pentoxide Diphosphorus pentoxide S 2 O 2 S 2 O 2 SiF 4 SiF 4 SO SO PO 3 PO 3 BF 3 BF 3 P 2 O 5 P 2 O 5

33. Acids Acid- a type of molecular compound Acid- a type of molecular compound Two types Two types Binary acids- made up of two elements- hydrogen, and one of the halogens (F, Cl, Br, I) Binary acids- made up of two elements- hydrogen, and one of the halogens (F, Cl, Br, I) Oxyacids- contain hydrogen, oxygen, and a third element Oxyacids- contain hydrogen, oxygen, and a third element Examples Examples Binary acids: Binary acids: HCl- hydrochloric acid; HF- hydrofluoric acid HCl- hydrochloric acid; HF- hydrofluoric acid Oxyacids: Oxyacids: H 2 SO 4 : sulfuric acid H 2 SO 4 : sulfuric acid HNO 3 : nitric acid HNO 3 : nitric acid

34. Formula Mass The sum of the atomic masses of all atoms represented in its formula The sum of the atomic masses of all atoms represented in its formula Units = amu (atomic mass units) Units = amu (atomic mass units) Example: What is the formula mass of water? Example: What is the formula mass of water? 2 H atoms @ 1.01 amu each = 2.02 amu 2 H atoms @ 1.01 amu each = 2.02 amu 1 O atom @ 16.00 amu each = 16.00 amu 1 O atom @ 16.00 amu each = 16.00 amu Total mass of water = 16.00 + 2.02 = 18.02 Total mass of water = 16.00 + 2.02 = 18.02

35. Formula Mass Find the formula mass of the following: Find the formula mass of the following: KClO 3 KClO 3 H 2 SO 4 H 2 SO 4 Mg(NO 3 ) 2 Mg(NO 3 ) 2 C 12 H 22 O 11 C 12 H 22 O 11

36. Molar Mass The mass in grams of one mole of a substance The mass in grams of one mole of a substance If we have 1 mole of H 2 O, we have If we have 1 mole of H 2 O, we have 2 moles of H atoms 2 moles of H atoms 1 mole of O atoms 1 mole of O atoms

37. Molar Mass (cont.) How many moles of each atom are in the following? How many moles of each atom are in the following? CaCl 2 CaCl 2 NaOH NaOH KMnO 4 KMnO 4 NH 4 OH NH 4 OH Mg(NO 3 ) 2 Mg(NO 3 ) 2

38. Molar Mass (cont.) Once we know the number of moles of each atom, we can calculate the molar mass. Once we know the number of moles of each atom, we can calculate the molar mass. In H 2 O: In H 2 O: 2 moles H x 1.01 g H = 2.02 g H 2 moles H x 1.01 g H = 2.02 g H 1 mole H 1 mole H 1 mole O x 16.00 g O = 16.00 g O 1 mole O x 16.00 g O = 16.00 g O 1 mole O 1 mole O

39. Molar Mass (cont.) Total mass of 1 mole H 2 O Total mass of 1 mole H 2 O 2.02 g + 16.00 g = 18.02 g/mol 2.02 g + 16.00 g = 18.02 g/mol

40. Molar Mass (cont.) Determine the molar mass of the following: Determine the molar mass of the following: CaCl 2 CaCl 2 NaOH NaOH KMnO 4 KMnO 4 NH 4 OH NH 4 OH Mg(NO 3 ) 2 Mg(NO 3 ) 2

41. Molar Mass as a Conversion Factor Can use molar mass as a conversion factor to determine number of moles Can use molar mass as a conversion factor to determine number of moles How many moles of H 2 O are in 34.32 g? How many moles of H 2 O are in 34.32 g?

42. Molar Mass as a Conversion Factor How many molecules of NaCl can be found in a sample containing 45.43 g? How many molecules of NaCl can be found in a sample containing 45.43 g?

43. Molar Mass as a Conversion Factor How many carbon atoms are in a 23.43 g sample of CO 2 ? How many carbon atoms are in a 23.43 g sample of CO 2 ?

44. Fun With Conversions! Ibuprofen, C 13 H 18 O 2, is the active ingredient in Advil. Ibuprofen, C 13 H 18 O 2, is the active ingredient in Advil. Find its molar mass Find its molar mass If the tablets in the bottle contain a total of 33 g of ibuprofen, how many moles of ibuprofen are in the bottle? If the tablets in the bottle contain a total of 33 g of ibuprofen, how many moles of ibuprofen are in the bottle? How many molecules of ibuprofen are in the bottle? How many molecules of ibuprofen are in the bottle? What is the total mass in grams of carbon in 33 g of ibuprofen? What is the total mass in grams of carbon in 33 g of ibuprofen?