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Chapter 7- Chemical Formulas and Chemical Compounds

Chapter 7- Chemical Formulas and Chemical Compounds. Ban Dihydrogen Monoxide!. Colorless, odorless, tasteless Kills uncounted thousands of people every year. Most deaths caused by accidental inhalation Prolonged exposure to its solid form causes severe tissue damage.

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Chapter 7- Chemical Formulas and Chemical Compounds

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  1. Chapter 7- Chemical Formulas and Chemical Compounds

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

  3. Ban Dihydrogen Monoxide! • Also known as hydroxl acid • Major component of acid rain • Contributes to the "greenhouse effect." • May cause severe burns. • Contributes to the erosion of our natural landscape. • Accelerates corrosion and rusting of many metals. • May cause electrical failures and decreased effectiveness of automobile brakes. • Been found in excised tumors of terminal cancer patients. • 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? • Write at least two sentences stating your reasoning. • 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 C8H18 MgCl2 Ca(OH)2 8 C atoms 18 H atoms 1 Mg2+ ion 2 Cl- ions 1 Ca2+ ion 2 OH- ions

  7. Monatomic Ions • Ions formed from a single atom • Usually have noble gas configurations • That’s how we determine its charge • Example: • Li: 1s22s1 • Li+: 1s2 or [He] • Table on p.221 on monatomic ions

  8. Naming Monatomic Cations • Use the element’s name! • Yes, it’s that simple! • Example: • Cs+ = cesium • Al3+ = aluminum

  9. Naming Monatomic Anions • Drop the ending of the element’s name • Add the ending –ide • Examples: • Cl- = chloride • N3- = nitride

  10. Naming Monatomic Ions • K+ • S2- • Rb+ • O2- • I- • Ba2+ • Cu+ • potassium • sulfide • rubidium • oxide • iodide • barium • copper

  11. Binary Ionic Compounds • Compounds composed of two ions • Total numbers of positive charges and negative charges must be equal • Examples: • NaCl • KBr • CaF2

  12. Writing Binary Ionic Compounds • Write the symbols for the ions side by side. Write the cation first. Al3+ O2- • Cross over the charges to use as the subscript for the other ion. Al3+ O2- Al2 O3

  13. Writing Binary Ionic Compounds • Check the subscripts and divide them to give the smallest whole number ratio of ions. Al2O3 • Write the formula! Al2O3

  14. Writing Binary Ionic Compounds • Zinc iodide • Barium fluoride • Lithium oxide • Calcium oxide • Magnesium bromide • ZnI2 • BaF2 • Li2O • CaO • MgBr2

  15. Naming Binary Ionic Compounds • Give name of cation first • Then name the anion • Al2O3 • Name of cation: aluminum • Name of anion: oxide • Name of compound: aluminum oxide

  16. Naming Binary Ionic Compounds • BaI2 • ZnF2 • K2O • MgO • CaBr2 • Barium iodide • Zinc fluoride • Potassium oxide • Magnesium oxide • Calcium bromide

  17. Cations With Different Charges • Some elements form two or more cations with different charges • Fe2+ and Fe3+ • Iron (II) and Iron (III) • Naming compounds • FeO and Fe2O3 • Iron (II) oxide and Iron (III) oxide

  18. Name the Following Compounds • CuO • CoF3 • SnI4 • FeS • Copper (II) oxide • Cobalt (III) fluoride • Tin (IV) iodide • Iron (II) sulfide

  19. Quiz- Name the Following Compounds • K2S • AgBr • Na2O • FeCl2 • BaS Lithium fluoride Silver iodide Iron (III) oxide Magnesium iodide Gold chloride

  20. Polyatomic Ions • Ions that contain two or more atoms • Most are negatively charged • List of polyatomic ions is on handout • **MEMORIZE THEM!!!** • Examples: • CN- cyanide • HCO3- hydrogen carbonate (bicarbonate) • NH4+ ammonium

  21. Polyatomic Ions • You will need to memorize the following: • Ammonium NH4+1 • Acetate C2H3O2-1 • Hydroxide OH-1 • Nitrite NO2-1 • Nitrate NO3-1 • Bicarbonate HCO3-1 • Carbonate CO3-2 • Chromate CrO4-2 • Sulfate SO4-2 • Phosphate PO4-3

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

  23. Oxyanions (cont.) • If two oxyanions- • Most oxygens: -ate • Least oxygens: -ite • Example • NO3- : nitrate • NO2- : nitrite

  24. Oxyanions (cont.) • If more than two oxyanions • Most oxygens: “Per- …. –ate” • “-ate” • “-ite” • Least oxygens: “Hypo- …. –ite” • Example • ClO4- : perchlorate • ClO3- : chlorate • ClO2- : chlorite • ClO- : hypochlorite

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

  26. Polyatomic Ion Quiz • Bicarbonate • Acetate • Bisulfite • Permanganate • Nitrite • Cyanide • Hydroxide • Bisulfate • Nitrate • What’s your favorite polyatomic ion?

  27. Binary Molecular Compounds • Composed of molecules (covalently bonded!) • A nonmetal bonded to another nonmetal • Examples: • SO3 • ICl3 • CH4 • H2O

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

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

  30. Naming Binary Molecular Compounds • Examples: • SO3 – sulfur trioxide • BrCl3 – bromine trichloride • PBr5 – phosphorus pentabromide • N2O5 – dinitrogen pentoxide

  31. Naming Binary Molecular Compounds • N2O • CCl4 • NO • CO2 • N2O3 • P4O10 • Dinitrogen monoxide • Carbon tetrachloride • Nitrogen monoxide • Carbon dioxide • Dinitrogen trioxide • Tetraphosphorus decoxide

  32. Naming Binary Molecular Compounds- More Practice! • Disulfur dioxide • Silicon tetrafluoride • Sulfur monoxide • Phosphorus trioxide • Boron trifluoride • Diphosphorus pentoxide • S2O2 • SiF4 • SO • PO3 • BF3 • P2O5

  33. Acids • Acid- a type of molecular compound • Two types • 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 • Examples • Binary acids: • HCl- hydrochloric acid; HF- hydrofluoric acid • Oxyacids: • H2SO4: sulfuric acid • HNO3: nitric acid

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

  35. Formula Mass • Find the formula mass of the following: • KClO3 • H2SO4 • Mg(NO3)2 • C12H22O11

  36. Molar Mass • The mass in grams of one mole of a substance • If we have 1 mole of H2O, we have • 2 moles of H atoms • 1 mole of O atoms

  37. Molar Mass (cont.) • How many moles of each atom are in the following? • CaCl2 • NaOH • KMnO4 • NH4OH • Mg(NO3)2

  38. Molar Mass (cont.) • Once we know the number of moles of each atom, we can calculate the molar mass. • In H2O: • 2 moles H x 1.01 g H = 2.02 g H 1 mole H • 1 mole O x 16.00 g O = 16.00 g O 1 mole O

  39. Molar Mass (cont.) • Total mass of 1 mole H2O • 2.02 g + 16.00 g = 18.02 g/mol

  40. Molar Mass (cont.) • Determine the molar mass of the following: • CaCl2 • NaOH • KMnO4 • NH4OH • Mg(NO3)2

  41. Molar Mass as a Conversion Factor • Can use molar mass as a conversion factor to determine number of moles • How many moles of H2O 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?

  43. Molar Mass as a Conversion Factor • How many carbon atoms are in a 23.43 g sample of CO2?

  44. Fun With Conversions! • Ibuprofen, C13H18O2, is the active ingredient in Advil. • 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? • How many molecules of ibuprofen are in the bottle? • What is the total mass in grams of carbon in 33 g of ibuprofen?

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