Chemistry of Life: Organic Compounds and Inorganic Substances Explained

1. Need a quiet place to do your work?1. Use MAP time! (except Wed) OR2. Go to the LIBRARY!New morning hours start Mon, Nov 11 at 6:45 AM (except Wed)

2. OrganicCompounds& Inorganic Substances in Living Thingsksuweb.kennesaw.edu/~vking2/Chemistry%20of%20Life%20Post.ppt www.wyalusingrams.com/53942041017952357/lib/53942041017952357/UNIT_2_chemistry.ppt faculty.sgc.edu/asafer/BIOL1107/chapt02_lecture.ppt

3. Introduction a) Organic compounds are carbon-based and are the key substances that make up living things. b) Inorganic substances also are important to organisms, but do NOT contain carbon

4. c) Organic (Carbon) Compounds • All living things are made MOSTLY of organic compounds! • Yes, you’re organic! 

5. The 4 Types of Organic (C) Compounds

6. Organic compounds are made of repeating units called monomers • Organic compounds FORM by dehydration synthesis (condensation) • Organic compounds are BROKEN DOWN by hydrolysis (decomposition)

7. Part 1: Types of Organic (C) Compounds 1) Carbohydrates Main Use: immediate energy • contain C, H, and O • polysaccharide is a long chains of monomers

8. Examples of carbohydrates: sugars & starches a) Monosaccharides: • glucose (main source of energy for cells) • fructose (in fruit) b) Disaccharides • sucrose (table sugar) • lactose (in milk)

9. c) Polysaccharides (starches) • glycogen starch stored in liver • cellulose fibers in plants

10. 2) Lipids (fats; triglycerides) Main Use: long term energy storage • contains C, H, and O • composed of glycerol + long fatty acid chains

11. a) Saturated fats – contain single bonds - solid fats (related to heart disease) e.g. butter, lard, coconut oil, palm oil

12. b) Unsaturated fats – contain double bonds • liquid oils (healthier) e.g. peanut, corn, olive oils

13. c) Steroids – have a four ring structure Examples: • cholesterol (LDL, HDL) • sex hormones (testosterone, estrogen), • cell membrane • bile

14. 3) Proteins Main Uses: Structural –muscle protein fibers Enzymes – catalysts to speed up chemical reactions Energy– only if starvation occurs • contains C, H, O, N • monomer = amino acids • polypeptide is a long chain of amino acids linked by peptide bonds

15. Examples of proteins • hemoglobin (in red blood cells) • digestive enzymes

16. Enzymes speed up chemical reactions! hydrolysis or decomposition (e.g. digestion)

17. dehydration synthesis - assembles larger organic compounds

18. 4) Nucleic Acids Main Use: store and carry genetic information • C, H, O, N and P • monomer = nucleotide

19. Examples of nucleic acids • DNA(deoxyribonucleic acid) is double stranded • RNA(ribonucleic acid) is single stranded

20. MATCHING MonomerOrganic compound 1. nucleotides carbohydrates 2. monosaccharides lipids 3. amino acids proteins 4. glycerol + fatty nucleic acids acid chains

21. Part 2: Inorganic Substances in Living Things(no carbon)

22. I. Water & Organisms • about two-thirds (2/3) of the human body is water!!! • Water is essential for cell function; it is required in chemical reactions to sustain life • Water is the only common substance in nature in all 3 physical states of matter– solid, liquid and gas

23. A) Polarity of Water • Water is a polar molecule with positive (+) and negative (-) ends • this leads to easy formation of hydrogen (H) bonds between water molecules

24. Water is a polar molecule Oxygen H H

25. H H Hydrogen (H) bonds form between water molecules Oxygen H bond H H bond H H H

26. B) Properties of Water 1. cohesion--water molecules H bond to one another easily and “cling” together

27. cohesion  surface tension water strider (or skater)

28. 2. adhesion--water molecules easily form H bonds to other non-water substances e.g. water travels UP through plant stems & tree trunks

29. adhesion  capillary action

30. 3. high specific heat! Water has high specific heat and resists changes in temperature e.g. sweat absorbs some of the heat of your body

31. 4. high heat of vaporization * It takes a significant temperature increase for water to evaporate!

33. 5. Water is less dense as a solid! • water E X P A N D S when it freezes • Therefore, ice FLOATS in water!! • and cells die when the cytoplasm (fluid) inside freezes! e.g. frostbite

34. Euphausid shrimp under ice

35. Ice fishing

36. 6. High solubility • water molecules surround molecules • water is practically a universal solvent

38. Many substances are dissolved in biological fluids (vitamins, glucose, oxygen, salts, carbon dioxide, wastes) • Detection by blood & urine tests

39. II. Acids & Bases • Acids are substances that form hydrogen ions (H+) in water 2. Bases are substances that form hydroxide ions (OH-) in water 3. The pH scale measures the acidity & alkalinity.

40. pH scale _________________________________________ 0 7 14 acids bases pH < 7 pH > 7 neutral pH = 7

42. III. Oxygen (O2) • cells use O2 to breakdown food into ATP energy molecules during cellular aerobic respiration • You need to breathe O2for energy! • No O2, no energy, no life!

43. IV. Salts • dissolve easily in water • form ions (electrolytes) for metabolism (chemical reactions for cell activities) e.g. Na+, Mg2+, Ca2+, K+, Cl-

45. Assignment #27: Create a thinking map entitled, “Chemicals in Living Things”

46. Enzymes • Enzymes are proteins that function as catalysts for chemical reactions • they speed up the rate of reactions by lowering the activation energy needed for a chemical reaction to happen • Lock and Key Model • Each enzyme has a specific shape (lock) • Substrate (key) • the reactant that must fit into active site of enzyme for reaction to occur • One enzyme  one specific reaction • Enzymes are not changed during the reaction; “re-usable”

47. Coenzymes – smaller organic molecules that are needed for a proper fit of an enzyme to substrate e.g. vitamins • Cofactors – ions needed for proper fit of enzyme/substrate e.g. Minerals • Denaturation – the change of a protein’s shape • Change the shape, change (usually ruin) the function • possible causes: high temperatures, wrong pH or salt concentration