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Chemistry SM-1131 Week 7 Lesson 1

Chemistry SM-1131 Week 7 Lesson 1. Dr. Jesse Reich Assistant Professor of Chemistry Massachusetts Maritime Academy Fall 2008. Class Today. Polyatomic anions, Molecular Compounds, Acid Names, Formula Mass Grams, atoms, mols , avogadro’s number Take home quiz for Friday. Review.

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Chemistry SM-1131 Week 7 Lesson 1

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  1. Chemistry SM-1131Week 7 Lesson 1 Dr. Jesse Reich Assistant Professor of Chemistry Massachusetts Maritime Academy Fall 2008

  2. Class Today • Polyatomic anions, Molecular Compounds, Acid Names, Formula Mass • Grams, atoms, mols, avogadro’s number • Take home quiz for Friday

  3. Review • Polyatomic Ions • Ionic Compounds are between metals and non-metals, AND metals and polyatomic atoms • Poly=Many • Atomic= Atoms • Polyatomic= many atoms

  4. Polyatomic Anions • Compounds still work basically the same way • 1- Symbols (keep the parenthesis) • 2- Charges • 3- Switcheroo • 4- Reduce

  5. Example • Sodium and Carbonate combine to make a compound. What’s the formula and charge? • Na & (CO3) • Na+1 and CO3-2 • Na2(CO3) • Metal First polyatomic ion second • Sodium Carbonate

  6. Example 2 • Magnesium and Phosphate come together to form a compound. Formula and charge? • Mg & (PO4) • Mg+2 & (PO4)-3 • Mg3(PO4)2 • Metal first polyatomic ion second • Magnesium Phosphate

  7. Example 2 cont. • Mg3(PO4)2 • There are 3 Magnesium atoms • There are 2 PO4 groups • Each PO4 group has 1 P and 4 O • So, we have to multiply: • 2x 1P = 2P • 2x 4O = 8O • Total: Mg3P2O8

  8. Example 3 • Iron (III) and Nitrate form a compound. What’s the formula and name? • Fe(III) & (NO3) • Fe(III)+3 & (NO3)-1 • Fe(III)1(NO3)3 • Iron (III) nitrate • Formula = Fe(III)1N3O9

  9. Example 4 • Ammonium and Permanganate form a compound. Formula and Name? • (NH4) & (MnO4) • (NH4)+1 & (MnO4)-1 • (NH4)1(MnO4)1 • Ammonium Permanganate • This guy is a rarity because the non-metal thing is the cation and the metal thing is the anion. Polyatomics can act a little differerntly than metals or non-metals that are just by themselves.

  10. Polyatomics to Memorize • Table 5.6 page 138 • Make note cards. They are all fair game.

  11. Molecular Compounds • Ionic compounds are between metals and non-metals (or polyatomic ions) • Molecular compounds are between 2 or more non-metals

  12. Molecular Compounds • Two different naming systems. DON’T CONFUSE THEM! • This system is just for molecular compounds. • Molecular compounds have 2 or more non-metals in them

  13. Molecular Nomenclature • The naming systems for the simple ones works like this: • 1-Prefix • 2-First element (somewhat alphabetical) • 3-Prefix • 4-Second element • 5-change the ending of the second element to -ide.

  14. What are the prefixes • MEMORIZE THESE! • Mono-1 • Di-2 • Tri-3 • Tetra-4 • Penta-5 • Hexa-6 • Hepta-7 • Octa-8

  15. Example • Here’s a formula: N2O4. What’s the name? • Di • Nitrogen • Tetra • Oxygen • Oxide • Dinitrogentetraoxide

  16. Example 2 • SF6 • Mono (If mono is the very first one you don’t have to use it). • Sulfur • Hexa • Fluorine • Fluoride • Sulfur Hexafluoride

  17. Example 3 • CO2 • Mono (drop it) • Carbon • Di • Oxygen • Oxide • Carbon Dioxide

  18. Acids • Acids are things that create H+ ions when dissolved in water. They are typically bitter and sour tasting. Most acids can dissolve metals. • They are combinations of H+ atoms with anions

  19. Acid Types • Binary Acids • Oxyacids

  20. Binary Acid Names • Binary Acids are a combination of 2 things. Hydrogen and one other non-metal • Naming them is simple • 1-Hydro • 2-Base name of non-metal • 3-change the ending of the non-metal to –ic • 4-Add the word acid at the end

  21. Binary Acid names • HBr • 1-Hydro • 2-Brom • 3-ic • 4-Acid • Name= Hydrobromic acid

  22. Binary Acid Names • HCl • 1-Hydro • 2-Chlor • 3-ic • 4- Acid • Name= Hydrochloric Acid

  23. Oxyacid Names • Oxy Acids are built around compounds that have oxygen containing polyatomic anions in them.

  24. What polyatomic anions make sense? • Phosphate (PO4) • Phosphite (PO3) • Chlorate (ClO3) • Chlorite (ClO2) • Nitrate (NO3) • Sulfate (SO4) • Sulfite (SO3)

  25. Oxyacid naming with-ate • 1-Name of the polyatomic acid • 2-change the ending to –ic (sometimes needs a fudge factor) • 3-add the word acid

  26. Oxyacid Naming • Phosphate makes an acid. What is the name and formula? • 1-Phosphate • 2-turns into Phosphoric • 3- add acid • Name= Phosphoric Acid • 1-H (PO4) • 2-H+1(PO4)-3 • 3-H3(PO4)1 • Can’t reduce

  27. Naming Oxyacids with -ite polyatomic anions • 1-Write the anion name • 2-Change the ending to –ous (might need a fudge factor) • 3- add the word acid

  28. Oxyacid Naming with -ite polyatomic anions • The polyatomic anion sulfite forms an oxyacid. What is the name and formula? • 1-Sulfite • 2- Change to Sulferous • 3- add Acid • Name= Sulferous Acid • H (SO3) • H+1 (SO3)-2 • H2(SO3)1 • Can’t reduce

  29. Molecular Mass • To figure out molecular mass you have to know the atomic mass. • Let’s start easily • Ne- it exists by itself and doesn’t form molecules. It’s mass is just the atomic mass of Ne, which is 20.18

  30. Simple Molecule Mass • The mass of N2 is going to be twice the mass of 1 atom of N • So, if N has an atomic mass of 14.01, then N2 must have a mass of 2x14.01 or 28.02

  31. Molecular Mass • Ozone has the formula O3, what is it’s molecular mass • 1 Oxygen has a mass of 16.00 • 3x(16.00) has a mass of 48.00 amu

  32. More Complex Masses • Water has the formula H2O • The molecular mass is going to be from 2H atoms and 1 O atom, so • 2x(1.0079) + 1x(16.00)= 18.0158amu

  33. Sugar • C6H12O6 • 6(12.01) + 12(1.0079) + 6(16.00)= ???

  34. New Material • Moles, Atoms, Molecules, grams • IT’S MATH HEAVY TODAY! PAY ATTENTION YOU SCURVEY DOGS!

  35. Moles • Dozen: 12 somethings • Baker’s Dozen: 13 Somethings • A Score: 20 Somethings • Avogadro’s number: 1 mol= 6.022e23 somethings

  36. See how it works • A dozen atoms = 12 atoms • A baker’s dozen atoms = 13 atoms • A score of atoms = 20 atoms • A mole of atoms = 6.022e23 atoms

  37. Moles • 1 mole of atoms = 6.022e23 atoms • 2 moles of atoms= 2(6.022e23)atoms= 1.2044e24 atoms • 3 moles of atoms = 3(6.022e23)atoms= 1.8066e24

  38. Moles • 1 mole of kittens = 6.022e23 kittens • 2 moles of kittens= 2(6.022e23)kittens= 1.2044e24 kittens • 3 moles of kittens = 3(6.022e23)kittens= 1.8066e24

  39. Moles • It just means a big number. • 602,200,000,000,000,000,000,000,000 • But we do this because it converts amu to grams

  40. Why a 6.022e23 • 1 amu = 1.66e-24 grams • So, 1.66e-24gx6.022e23= 0.99652g which is very similar to 1g. • The point is that if you multiply the mass of something in amu you can convert amu into a mass in grams • We don’t weigh anything in amu, but we do in grams so this is useful. • So, if we multiply the atomic mass of something by 1 mol it turns from amu into grams.

  41. If you have 1 mole of N2 how much would it weigh? • Atomic Mass of N= 14.01 amu • Molecular Mass of N2= 28.02 amu • 6.022e23 atoms of N2 x 28.02 amu x 1.66e-24g = 1 atom 1 amu Which equals 28.02g. So, 1 mol x molecular mass = # of grams

  42. What do we do with this? • Chemists generally convert moles into atoms. • Atoms into Moles • Moles into grams • Grams into Moles

  43. Moles into atoms • 1 mole has 6.022e23 atoms in it • 5 moles of Ne x 6.022e23 atoms = 3.011e24 atoms 1 mole • 24.00 moles of He 6.022e23 atoms = 1.445e25 atoms 1 mole

  44. Atoms into Moles • You have 18.066 e23 atoms of Cu many many moles of Cu do you have? 18.066e23 atoms x 1 mol = 3.0000 mol 6.022e23 atoms

  45. So • Atoms x 1 mole = moles 6.022e23 atoms • Moles x 6.022e23 atoms = atoms 1 mole

  46. Moles to grams • We also convert moles into grams • You can’t weigh a mole, you weigh a gram • Moles x molecular mass in grams = grams 1 mole

  47. Moles to Grams Example 1 • 5 moles of N2 is how many grams? Copy the given 5.000 moles x grams = grams 1 moles How many grams in 1 mole? Use the atomic mass. N= 14.01amu, so N2= 28.02amu 5.000 moles x 28.02 g = 140.1 g 1 mole

  48. Moles to Grams Example 2 • 8 moles of O3 is how many grams? Copy the given 8.000 moles x atomic mass in grams = grams 1 moles How many grams in 1 mole? Use the atomic mass. O= 16.00 amu, so O3= 48.00amu 8.000 moles x 48.00 g = 384.0 g 1 mole

  49. Moles to Grams Example 3 • 10 moles of H2O is how many grams? Copy the given 10.0 moles H2O x molecular mass in grams = grams 1 moles How many grams in 1 mole? Use the atomic mass. O= 16.00 amu, H = 1.0079 so H2O= 18.0158amu 10.0 moles H2O x 18.00158 g = 180.0158 g = 180g 1 mole

  50. Grams to Moles • Grams -> Moles • Xgrams x moles = moles Atomic mass

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