2. 1 - 1 © Chemeketa Community College: CH117 CH117 Consumer Chemistry: Chemistry of Food and Cooking Unit 2 Chemistry Basics Periodic Table Ionic and Covalent Compounds Utensils in Cooking Functional Groups in Flavor Molecules

3. 1 - 2 © Chemeketa Community College: CH117 stuff The stuff things are made of. Mass Volume Has Mass and Volume (takes up space). (Air, water, rocks, etc..) Matter What is Chemistry? Mass amount Mass = The amount of stuff (in g’s) ( Bowling Ball > Balloon) Weight Weight = Pull of Gravity on matter. “The study of Matter and its Changes.”

4. 1 - 3 © Chemeketa Community College: CH117 Pure Substance Pure Substance - something of uniform composition that can’t be sorted further by differences. A model of matter ie. Table of known elements Element Element - Pure substance composed of only one kind of atom. Chemical Compound Chemical Compound - A pure substance that is a combination of different elements. ie. Carbon Dioxide (CO 2 ) ie. Water (H 2 O) ie. Salt (NaCl)

5. 1 - 4 © Chemeketa Community College: CH117 Mixture Mixture - NOT of uniform composition and CAN be sorted further by differences. A model of matter ie. Homogenized Milk Homogeneous Homogeneous – Looks pure but is not. Heterogeneous Heterogeneous - Visibly a combination of different substances. ie. Chocolate Chip Cookies ie. Salt or Sugar Water (H 2 O + NaCl) ie. Pizza ie. Granite

6. 1 - 5 © Chemeketa Community College: CH117 A model of matter ie. Aluminum (Al) Atom Atom - The smallest unit of an element that is still that element. ie. Carbon Dioxide (CO 2 ) ie. Water (H 2 O) Molecule Molecule -The smallest unit of bonded atoms that is still that substance. Contains > 1 atom or element Contains > 1 atom or element. ie. Oxygen (O 2 ) ie. Not Salt (NaCl)

7. 1 - 6 © Chemeketa Community College: CH117 Classification of matter Matter Pure Substance MixtureElementCompound Fe FeS MgMgO Mg + O 2 Fe + S Homogeneous Heterogeneous

8. 1 - 7 © Chemeketa Community College: CH117 Pizza Mixture Homogeneous (Solution) (Solution)Heterogeneous Mixtures Non-uniform compositionNon-uniform compositionNon-uniform compositionNon-uniform composition Uniform composition Air Urine Gasoline Sand Tea w/ice Milk

9. 1 - 8 © Chemeketa Community College: CH117 Each element is assigned a unique symbol 1-2 letters; 1st is capitalized Elements & Symbols Hydrogen Nitrogen Aluminum Chlorine Calcium Carbon Copper (Cu) The original name is often of Latin or Greek origin Potassium (Kalium) Sodium (Natrium) Iron (Ferrum) Gold (Aurum)

10. 1 - 9 © Chemeketa Community College: CH117 Modern periodic table H Li Na Cs Rb K TlHgAuHfLsBa Fr PtIrOsReWTa He RnAtPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNiCoFeMnCrV InXeITeSbSn GaKrBrSeAsGe AlArClSPSi BNeFONC I A II A III A IV A V A VI A VIIA VIIIA III B IVB V B VIB VIIB VIII B IB IIB 12345671234567 Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es The periodic table helps us understand behavior,behavior, reactionsreactions propertiesproperties of the elements. Mendeleev, 1871 “Properties of the elements vary in a periodic manner.”

11. 1 - 10 © Chemeketa Community College: CH117 A row or period He Rn XeI KrBrSe ArClS NeFO P NC H Li Na Cs Rb K TlHgAuHfLsBa Fr PtIrOsReWTaPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNiCoFeMnCrV InSbSn GaGe Al Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es At Te As Si B 12345671234567 Periods are assigned numbers Periods are assigned numbers

12. 1 - 11 © Chemeketa Community College: CH117 Common group names H Li Na Cs Rb K TlHgAuHfLaBa Fr PtIrOsReWTa He RnAtPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNiCoFeMnCrV InXeITeSbSn GaKrBrSeAsGe AlArClSPSi BNeFONC I A III B IVB V B VIB VIIB VIII B IB IIB Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es Alkali Metals Alkaline Earth Metals HalogensHalogens Noble gases III A IV A V A VI A VIIA VIIIA II A Transition Metals LanthanidesLanthanides ActinidesActinides

13. 1 - 12 © Chemeketa Community College: CH117 Why do we have those rows on the bottom? H Li Na Cs Rb K LsBa Fr Be Mg Sr Ca Y AcRa Sc TlHgAuHfPtIrOsReWTa He RnAtPoBiPb CdAgZrPdRhRuTcMoNb ZnCuTiNiCoFeMnCrV InXeITeSbSn GaKrBrSeAsGe AlArClSPSi BNeFONC Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es This arrangement takes too much space and is hard to read.

14. 1 - 13 © Chemeketa Community College: CH117 Names & Symbols He Rn XeI KrBrSe ArClS NeFO P NC H Li Na Cs Rb K TlHgAuHfLsBa Fr PtIrOsReWTaPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNiCoFeMnCrV InSbSn GaGe Al Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es At Te As Si B 12345671234567 Know the names & symbols Know the names & symbols

15. 1 - 14 © Chemeketa Community College: CH117 At Te As Si B He Rn Xe I KrBrSe ArClS NeFO P NC H Li Na Cs Rb K TlHgAuHfLsBa Fr PtIrOsReWTaPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNi Co FeMnCrV InSbSn GaGe Al Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es MetalsMetals Lustrous, malleable and ductile. Solids at room temp (except Hg) Conductors (heat & electricity); electrons loose so can move freely (flow) and spread energy so make good cooking pans (ie. Al, Fe, Cu) Give electrons to nonmetals (Form (+) ions ). Lustrous, malleable and ductile. Solids at room temp (except Hg) Conductors (heat & electricity); electrons loose so can move freely (flow) and spread energy so make good cooking pans (ie. Al, Fe, Cu) Give electrons to nonmetals (Form (+) ions ).

16. 1 - 15 © Chemeketa Community College: CH117 High SpHt; Resists change Remember Specific Heat Fe0.11 Cu 0.093 Ag 0.057 Au 0.031 Sand 0.19 Al 0.22 H 2 O 1.00 1o1o 10 o 30 o 20 o Low SpHt; Heats quickly Cast Iron skillets (Fe/C) have more mass compared to normal Al or Stainless steel pans which is why they heat & cool slowly and hold heat longer than an Al or Fe pan of lower mass. Stainless steel (Fe/Cr/Ni all ~0.1) heats fast. Cu on bottom heats faster.

17. 1 - 16 © Chemeketa Community College: CH117 He Rn XeI KrBrSe ArClS NeFO P NC H Li Na Cs Rb K TlHgAuHfLsBa Fr PtIrOsReWTaPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNiCoFeMnCrV InSbSn GaGe Al Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es At Te As Si B Non-metalsNon-metals Gasliquidsolid (dull, brittle); Gas, liquid, solid (dull, brittle); Many are diatomic Poor conductors (Insulators); electrons held rigid in covalent bonds so can’t flow. Glass, SiO 2, heats slower than metal; Baking (hot air) is slower than Frying or boiling. Convection ovens make faster. Take electrons from metals (Form (-) ions); Share electrons (covalent) with other non- metals Gasliquidsolid (dull, brittle); Gas, liquid, solid (dull, brittle); Many are diatomic Poor conductors (Insulators); electrons held rigid in covalent bonds so can’t flow. Glass, SiO 2, heats slower than metal; Baking (hot air) is slower than Frying or boiling. Convection ovens make faster. Take electrons from metals (Form (-) ions); Share electrons (covalent) with other non- metals

18. 1 - 17 © Chemeketa Community College: CH117 He Rn Xe I KrBrSe ArClS NeFO P NC H Li Na Cs Rb K TlHgAuHfLsBa Fr PtIrOsReWTaPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNiCoFeMnCrV InSbSn GaGe Al Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es At Te As Si B 3 - 11 MetaloidsMetaloids Intermediate properties Semi conductors Intermediate properties Semi conductors

19. 1 - 18 © Chemeketa Community College: CH117 H Li Na Cs Rb K TlHgAuHfLsBa Fr PtIrOsReWTaPoBiPb Be Mg Sr Ca CdAgZrYPdRhRuTcMoNb AcRa ZnCuTiScNi Co FeMnCrV InSn Ga Al Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es He Rn XeI KrBrSe ArClS NeFO P NC Sb Ge At Te As Si B MetaloidsMetaloids MetalsMetals Non-metalsNon-metals

20. 1 - 19 © Chemeketa Community College: CH117 A model of matter Atom Atom - The smallest unit of an element that is still that element. Molecule Molecule -The smallest unit of a pure substance that is still that substance. May contain > 1 atom or element May contain > 1 atom or element. ie. Aluminum (Al) ie. Water (H 2 O)

21. 1 - 20 © Chemeketa Community College: CH117 Structure of the atom Nucleus + Small, dense, + charge in the center of an atom. containsprotons & neutrons + + + + ++

22. 1 - 21 © Chemeketa Community College: CH117 Structure of the atom Nucleus (+) Electrons - - charged particles that surround the nucleus. Electrons nucleusorbitals Electrons move around nucleus in orbitals.

23. 1 - 22 © Chemeketa Community College: CH117 Structure of the atom nucleus The nucleus is a small part of an atom. If the nucleus was the size of a marble, the atom would fill a football stadium. The nucleus would weigh over 10,000 tons.  Atoms are mostly empty space.  Atoms have a small, dense nucleus with + charge.

24. 1 - 23 © Chemeketa Community College: CH117 A A = Atomic mass The atomic symbol X A Z C # C C = Charge = + or - values # # = Number of atoms in a formula. Z = Atomic number = # protons = # electrons

25. 1 - 24 © Chemeketa Community College: CH117 A A = Atomic mass The atomic symbol O 16 8 2- C C = Charge = + or - values # # = Number of atoms in a formula. Z = Atomic number = # protons = # electrons

26. 1 - 25 © Chemeketa Community College: CH117 Electron arrangement 2 8 18 32 Electrons fill layers around nucleus Low  High Shells = Energy levels 2412 Mg A new layer is added for each row or period in the table.

27. 1 - 26 © Chemeketa Community College: CH11711H 73Li 42He IA II A 94Be 2, 1 2, 2

28. 1 - 27 © Chemeketa Community College: CH117115B 11H 73Li IA II A IIIA 94Be 2, 1 2, 2 2, 3

29. 1 - 28 © Chemeketa Community College: CH117115B 126C 137N IIIA IVA VA 2, 3 2, 4 2, 5

30. 1 - 29 © Chemeketa Community College: CH11794Be 11H 73Li 42He 2010Ne 2311 Na 2412 Mg 4018 Ar IA IIA VIIIA 2, 1 2, 2 2, 8, 1 2, 8, 2 2, 8 2, 8, 8

31. 1 - 30 © Chemeketa Community College: CH11711H 73Li 42He 94Be 2010Ne 2311 Na 2412 Mg 4018 Ar 881122 2, 1 2, 2 2, 8 2, 8, 1 2, 8, 2 2, 8, 8 Octet Rule

32. 1 - 31 © Chemeketa Community College: CH117 33 2412 Mg 11H 73Li 2311 Na 94Be 115B 2713 Al Valence electrons Where most chemical Reactions occur. 11 22 2, 1 2, 2 2, 8, 1 2, 8, 2 2, 3 2, 8, 3

33. 1 - 32 © Chemeketa Community College: CH11711H 73Li 2311 Na Electron Dot Structures Show only Valence Electrons H Li Na K

34. 1 - 33 © Chemeketa Community College: CH117 H Li Na K He Be B C O F Ne N Mg Ca Al Ga Si Ge P As S Se ClBrArKr 1 234567 8

35. 1 - 34 © Chemeketa Community College: CH117 Electron Affinity At I Br Cl Po Te Se S Bi Sb As P Pb Sn Ge Si FON Tl Na Cs Rb K Ba Mg Sr Ca In Ga Al H LiBeBC 4 - 50 Relative ability of atoms to attract electrons Oxidation: When electrons are grabbed by a “hungry” element like Oxygen (O) or Chlorine (Cl)

36. 1 - 35 © Chemeketa Community College: CH117 2311 Na Ions Metals give e - s to make (+) ions ( Cations) Na 11 +’s 11 -’s 0 11 +’s 11 -’s 0 11 +’s 10 -’s 1 + 1 + 11 +’s 10 -’s 1 + 1 + Na 1+ 2, 8 = [Ne] Now has e - s like Ne 2, 8 = [Ne] Now has e - s like Ne

37. 1 - 36 © Chemeketa Community College: CH117 Ions Nonmetals take e - s to make (–) ions (anions) 17 +’s 17 -’s 0 17 +’s 17 -’s 0 17 +’s 18 -’s 1 - 1 - 17 +’s 18 -’s 1 - 1 - Cl 1- 3517 Cl = Cl 1- 2, 8, 8 = [Ar]

38. 1 - 37 © Chemeketa Community College: CH117 Formation of NaCl Na + Cl Na + + Cl + and - ions attract to form an ionic bond. _ e- moves from Metal  Nonmetal Metal Cation Nonmetal Anion Stable octets Chemical Equation = expression of a reaction Na + Cl  NaCl

39. 1 - 38 © Chemeketa Community College: CH117 Properties of Ionic compounds Not individual molecules Form crystal arrays Ions touch many others Formula represents the average ion ratio NaCl sodium chloride NaCl sodium chloride Na Cl

40. 1 - 39 © Chemeketa Community College: CH117 Common ions H Li Na Cs Rb K TlBa Fr He RnAtPoBiPb Be Mg Sr Ca Ra InXeITeSbSn GaKrBrSeAsGe AlArClSPSi BNeFONC HgAuHfLsPtIrOsReWTa CdAgZrYPdRhRuTcMoNb Ac ZnCuTiScNiCoFeMnCrV Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es 1+ 2+2+3+3+ 4+4-4+4- 3-3-2-2-1-1- Transition Elements VariableVariable Representative Elements

41. 1 - 40 © Chemeketa Community College: CH117 Ionic Formulas Metal Cations + Nonmetal Anions Na 1+ Cl 1- NaCl Sodium Chloride Mg 2+ Cl 1- MgCl 2 Magnesium Chloride Cl 1- In Sea Salt; tastes bitter Table Salt Used for taste & preserving Mined from earth & from Sea

42. 1 - 41 © Chemeketa Community College: CH117 Polyatomic Ions Ca 2+ CO 3 2- CaCO 3 Calcium Carbonate Mg 2+ SO 4 2- MgSO 4 Magnesium Sulphate Sea shells, egg shells, Limestone, Marble; Used to remove Ca from sea salt In Sea Salt

43. 1 - 42 © Chemeketa Community College: CH117 Naming Practice Potassium Iodide (to iodize salt) CuO TiO 2 SiO 2 Fe 2 SO 4 NaHCO 3 Ca 3 (PO 4 ) 2 KNO 3 KI Copper (II) Oxide or Cupric Oxide Titanium oxide (white paint pigment) Silicon Dioxide (anti-caking agent) Potassium Nitrate (in fertilizer) Ferric Sulfate (Iron in vitamins) Sodium bicarbonate (baking soda) Calcium Phosphate (in milk) Common ingredients

44. 1 - 43 © Chemeketa Community College: CH117 H Li Na K He Be B C O F Ne N Mg Ca Al Ga Si Ge P As S Se ClBrArKr 1 234567 8 Metals give e-s to nonmetals Nonmetals Share e-s with other nonmetals Nonmetals Share e-s with other nonmetals

45. 1 - 44 © Chemeketa Community College: CH117 Covalent compounds Discrete molecular units Atoms held together by bonds Covalent compounds exist in all states (CO 2 - gas, H 2 O - liquid, SiO 2 - solid) Formula represents atoms in a molecule Properties of covalent compounds O=O

46. 1 - 45 © Chemeketa Community College: CH117 Covalent Bonds HH + HHClO + O + + N N N NO O

47. 1 - 46 © Chemeketa Community College: CH117 Covalent Bonds HH Cl N NO O H 2 H-H H 2 Cl 2 Cl-Cl Cl 2 O 2 O=O O 2 N N2N2N2N2

48. 1 - 47 © Chemeketa Community College: CH117 OC OC Covalent Bonds O=C=O C O O Carbon monoxide Carbon dioxide CO 2 May modify rules to improve sound. iemonmono ie - monoxide not monooxide.

49. 1 - 48 © Chemeketa Community College: CH117 CO CO 2 SiO 2 CH 4 CH 3 CH 2 CH 3 CH 3 CH 2 OH CH 3 CO 2 H Common Covalent compounds Methane (Natural gas) carbon monoxide carbon dioxide silicon dioxide (in sand, glass) Propane (cooking gas) Ethanol (drinking alcohol) Acetic Acid (vinegar)

50. 1 - 49 © Chemeketa Community College: CH117 Tetrahedral electron-pair Geometries Tetrahedral Pyramidal Bent

51. 1 - 50 © Chemeketa Community College: CH117 Bond Polarity, Electron pull Cl H Electrons in covalent bonds rarely get shared equally. polar This unequal sharing results in polar bonds. H Cl Slight positive side Smaller electron pull Slight positive side Smaller electron pull Slight negative Larger electron pull Slight negative Larger electron pull ++ --

52. 1 - 51 © Chemeketa Community College: CH117 Electronegativity At I Br Cl Po Te Se S Bi Sb As P Pb Sn Ge Si FON Tl Na Cs Rb K Ba Mg Sr Ca In Ga Al H LiBeBC 4 - 50 3.983.443.04 3.16 2.96 2.55 2.20 2.192.58 Relative ability of atoms to attract electrons when they form bonds.

53. 1 - 52 © Chemeketa Community College: CH117 Ionic vs Covalent Strong attractions: Ionic High mp (1474F,801C) High bp (2575F, 1413C) Moderate attractions: Polar; H-bonds Low mp H 2 O (0C), Low bp H 2 O 100C; EtOH 78C Weak attractions: Vander Waals Lowest mp/bp Ionic Polar Covalent Nonpolar covalent Like NaClLike sugar, water, ethanol, Vit C Like oil, gasoline, hexane, Vit C

54. 1 - 53 © Chemeketa Community College: CH117 Attractive Forces Ionic Bonds 150 - 3000 kcal mol 150 - 3000 kcal mol Melting Point NaCl 801 o C Na 2 S 920 o C MgF 2 1248 o C Melting Point NaCl 801 o C Na 2 S 920 o C MgF 2 1248 o C

55. 1 - 54 © Chemeketa Community College: CH117 HCl ++++ ---- HCl ++++ ---- Attractive Forces Dipole-Dipole 0.1 - 1 kcal mol 0.1 - 1 kcal mol Melting Point HCl -114 o C CH 3 F -142 o C Melting Point HCl -114 o C CH 3 F -142 o C HCl ++++ ---- HCl ++++ ----

56. 1 - 55 © Chemeketa Community College: CH117 ClCl ++++ ---- Cl ++++ ---- Cl Attractive Forces Van der Waals (Dispersion Forces) 0.01 kcal mol 0.01 kcal mol Melting Point Cl 2 -102 o C CH 4 -183 o C Melting Point Cl 2 -102 o C CH 4 -183 o C Cl ++++ ----Cl Cl ++++ ---- Cl

57. 1 - 56 © Chemeketa Community College: CH117 HH O ++++ ++++ ---- HH O ++++ ++++ ---- HH O ++++ ++++ ---- HH O ++++ ++++ ---- Polar Attraction Attractive Forces Hydrogen Bonds

58. 1 - 57 © Chemeketa Community College: CH117 Hydrogen Bonding of Water Hydrogen Bonds 5 - 10 kcal mol 5 - 10 kcal mol Melting Point H 2 O 0 o C NH 3 -78 o C Melting Point H 2 O 0 o C NH 3 -78 o C Boiling Point H 2 O100 o C NH 3 -33 o C Boiling Point H 2 O100 o C NH 3 -33 o C

59. 1 - 58 © Chemeketa Community College: CH117 Ionic vs Covalent Strong attractions: Ionic High mp (1474F,801C) High bp (2575F, 1413C) Moderate attractions: Polar; H-bonds Low mp H 2 O (0C), Low bp H 2 O 100C; EtOH 78C Weak attractions: Vander Waals Lowest mp/bp Many water solubleSoluble in waterInsoluble in water Form ions in water (electrolytes) Don’t ionize in water Ionic Polar Covalent Nonpolar covalent Like NaClLike sugar, water, ethanol, Vit C Like oil, gasoline, hexane, Vit C

60. 1 - 59 © Chemeketa Community College: CH117 Dissoving of Ionic Compounds “Like Dissolves Like” Polar water attracts to Na + and Cl - ions Polar water attracts to Na + and Cl - ions When an ionic solid dissolves in water, the polar solvent removes ions from the crystal lattice.

61. 1 - 60 © Chemeketa Community College: CH117 H H O - + H H O - + H - H O + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + H H O - + “Like Dissolves Like” Dissoving of Ionic Compounds

62. 1 - 61 © Chemeketa Community College: CH117 Dissolving covalent compounds Covalent compounds do not break into ions.

63. 1 - 62 © Chemeketa Community College: CH117 Electrolytes Na + NaCl Na + Cl - C 6 H 12 O 6 Ionic (Salt) Covalent (sugar) Dissolved Ions in solution No Ions in solution NaCl  Na + + Cl -

64. 1 - 63 © Chemeketa Community College: CH117 Ionic vs Covalent Ionic Polar Covalent Nonpolar covalent Like NaClLike sugar, water, ethanol, Vit C Like oil, gasoline, hexane, Vit C Strong attractions: Ionic High mp (1474F,801C) High bp (2575F, 1413C) Moderate attractions: Polar; H-bonds Low mp H 2 O (0C), Low bp H 2 O 100C; EtOH 78C Weak attractions: Vander Waals Lowest mp/bp Many water solubleSoluble in waterInsoluble in water Form ions in water (electrolytes) Don’t ionize in water Not flammableFlammable

65. 1 - 64 © Chemeketa Community College: CH117 Organic Functional Groups Hydrocarbons

66. 1 - 65 © Chemeketa Community College: CH117 Drawing Covalent Compounds Practice building: Build with models Hexane Ethylene Ethanol (an alcohol) Isopropyl alcohol Cinnamaldehyde (an aldehyde) Acetone (a ketone) Acetic Acid (a carboxylic acid) Butyric Acid Phenol

67. 1 - 66 © Chemeketa Community College: CH117 Flavors: Terpenes Limonene Orange/lemons Citronellol Roses/geraniums

68. 1 - 67 © Chemeketa Community College: CH117 67 Smell: S-(+)-carvone Caraway (Dill) (Manderine Orange Peel) Caraway (Dill) (Manderine Orange Peel) R-(-)-carvone Spearmint

69. 1 - 68 © Chemeketa Community College: CH117 Flavors: Phenols Compounds of phenol are the active ingredients in the essential oils of cloves, vanilla, nutmeg, and mint. Nutmeg Thyme Cloves Vanilla Rosemary

70. 1 - 69 © Chemeketa Community College: CH117 Pungent Flavors Allyl isothiocyanate Thiocyanates: in Mustards and Horseradish Alkylamides: in chilli’s, & pepper CapsaicinPiperine GingerolShogoal