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Do Now

Do Now. Draw an atom of oxygen Draw two atoms of hydrogen bonded to one atom of oxygen What type of bond do O and H form? What is a covalent bond? What is an ionic bond? What is an isotope?. Chapter 4. Organic Chemistry. 4-1 Water. 75% of earth’s surface

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Do Now

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  1. Do Now • Draw an atom of oxygen • Draw two atoms of hydrogen bonded to one atom of oxygen • What type of bond do O and H form? • What is a covalent bond? • What is an ionic bond? • What is an isotope?

  2. Chapter 4 Organic Chemistry

  3. 4-1 Water • 75% of earth’s surface • Most abundant compound in living things • Liquid at room temperature • Expands when freezes • Necessary for life

  4. Charged molecule – polar • E- unevenly distributed • “little magnet” • Polarity allows water to stick to others and go in between other molecules

  5. Water Molecule

  6. Cohension – water sticking to water • Adhesion – water sticking to other things

  7. Hydrogen Bonding

  8. Mixtures • Substances are physically mixed but have not formed new chemical bonds • Different substances in a mixture retain their usual properties

  9. Ex. Table salt and iron filings, sugar and sand • Homogeneous – spread evenly throughout

  10. Solutions • Solutions - Mixtures that are liquid • Solvent - the liquid substance that makes up the bulk of the solution • Water is the universal solvent. • Solute – other substances that are dissolved in the solvent

  11. Concentration – the measurement of the amount of solute dissolved in a fixed amount of solution • Aqueous solutions – solutions in which water is the solvent

  12. Solutions • When ionically bonded compounds dissolved in water they dissociate or break apart into individual ions • NaCl  Na+ + Cl- • HCl  H+ + Cl-

  13. H+ • Most chemically reactive ion • Single proton – no e- • Attacks chemical bonds • Acids release H+

  14. Bases • NaOH  Na+ + OH- • Bases release OH-

  15. Strong acids and bases are highly reactive – attack and break chemical bonds – dangerous to living tissues

  16. Neutralization Reaction • Mixing an acid and a base OH- cancels H+ • H+ + OH-  H2O

  17. Acids and Bases

  18. pH – a measure of the relative amounts of hydronium (H3O or H+) and hydroxide ions (OH-) • pH = power of hydrogen • In water these ions form naturally • Pure water contains equal numbers of H+ and OH- ions • Neutral – OH- = H+

  19. pH Scale • Ranges from 0 to 14 • 0 is very acidic – H+ • 7 is neutral OH- = H+ • 14 is very basic (alkaline) OH-

  20. A difference of 1 on the pH scale is actually a difference of 10 times the strength of acids or bases

  21. Acids • Acid solution – contains many more H+ ions that OH- ions • Ex. HCl (hydrochloric acid) or H2SO4 (sulfuric acid) • Have a sour taste, produce a tingling or burning sensation if they come in contact with skin, highly corrosive when concentrated • Ex. Citric acid – oranges, lemons and grapefruits

  22. Bases • Base solution – a solution that contains many more hydroxide ions (OH-) than hydronium ions (H3O+) • Ex. NaOH • Alkaline refers to bases • Have a bitter taste, feel slippery

  23. Importance of pH • certain pH’s are needed for different reactions in the body • Certain organisms need a certain pH to live • Ex. Fish

  24. Suspensions • A mixture in which particles spread through a liquid or gas but settle overtime

  25. 4-2 Chemical Compounds in Living Things • Elements • 90 naturally occurring • 11 common in organisms • 20 trace • 96.3% of the body – C, N, O, H

  26. In varying combinations the elements C, H, N, O make up practically all the chemical compounds in living things

  27. Inorganic Compounds • No C • Exception – CO2 • Ex. Water, minerals, salts

  28. Organic Compounds • Have C • “organic chemistry” • C makes about 2 million compounds

  29. Carbon is unique – remarkable ability to form stable and strong covalent bonds • Carbon can form 4 single covalent bonds • Methane – CH4 – chemical formula • Structural Formula

  30. Carbon can bond with O, N, P, S • Carbon can form chains of C atoms – unlimited length • C atoms can bond either single, double or triple • Carbon needs 4 bonds to be “happy”

  31. Carbon Atoms FormCovalent Bonds

  32. Carbon Formations • Chains • Rings • Mixes of single, double, triple bonds

  33. Polymerization • Taking smaller C compounds and joining them to form larger compounds

  34. Monomers • Small compounds • Ex. sugar

  35. Polymers • Many monomers joined together

  36. Macromolecule • A large polymer • Macro = giant • Polymerization allows us to join monomers together to get complex molecules • Ex. Alphabet – 26 letters – many combinations make many words

  37. 4.3 Compounds of Life • 4 groups of organic compounds • Carbohydrates – pasta, bread • Lipids – fats, oils, waxes • Proteins – meat • Nucleic acids – DNA and RNA

  38. Carbohydrates • Ex. Sugars and starches made of C, H, O • O to H ratio 1:2 like water, C varies • 1C:2H:1O

  39. Monosaccharides • Simplest carbohydrate • One sugar • Ex. Glucose – sugar – green plants make Fructose – in fruits Galactose – in milk

  40. All three – C6H12O6 • The 3 differ on how the atoms are arranged • Isomer - have the same number of atoms but they are arranged differently

  41. Importance of Sugars • Contain a lot of energy • Energy stored in the bonds • Break bonds  release energy

  42. Dehydration Synthesis • Complex carbohydrates made by the process of polymerization • Chemical bonds linked • Bond formed between OH-’s • Dehydration synthesis – removes a water, two monomers join • Fig. 4-12

  43. Dissacharide • Made of 2 monomers • Ex. Sucrose – table sugar • Maltose – malt sugar • Lactose – milk sugar

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