1. Biochemistry Chapter 2

2. Background Organic molecules contain both the elements carbon and hydrogen –Glucose  C 6 H 12 O 6 Inorganic molecules do not contain both carbon and hydrogen –Water  H 2 O –Carbon Dioxide  CO 2

3. Background Dehydration Synthesis Reaction –A reaction that builds larger molecules from smaller molecules –A water molecule is released during the process –Small + Small  Large + H 2 O (water)

4. Background Hydrolysis Reaction –A reaction that breaks down larger molecules into smaller molecules –A water molecule is used up during the process. –Large + H 2 O (water)  Small + Small

5. Background Dehydration Synthesis Reaction Small + Small  Large + H 2 0 Large + H 2 0  Small + Small Hydrolysis Reaction

6. Chemistry Review- THE ATOM Atom is the basic unit of matter –Remember Proton = positive charge Electron = negative charge Neutron = neutral charge Compound-combo of 2 or more elements Molecule- formed when atoms joined together; smallest unit of most compounds

7. Chemical Bonds Ionic bond –1 or more electrons transferred Covalent Bond –electrons shared -Van der Walls Forces –weak intermolecular forces –Can develop when molecules are close together

8. Water is Essential to Life Water Polarity –polar molecule-the charges are unevenly distributed –like a magnet with poles A water molecule is polar because there is an uneven distribution between the O and H atoms –negative near O positive between H

9. Polarity allows water mo Polarity allows water molecules to attract each other Hydrogen bonds- bonds between H molecules -weak -allow for special properties of water

10. Mixtures: Solution and Suspensions Mixture- 2 or more elements or compounds –-physically mixed together but not chemically combined –-can be separated –ex: salt and pepper, sugar and sand Solutions- mixture of 2 or more substances in which the molecules are evenly distributed –ex: table salt in water –table salt= solute- substance that is dissolved –water= solvent- does dissolving Suspension-mixtures with non- dissolved material –ex: -water and sand

11. Acids, Bases and pH Remember: ion = charged particle –pH= “potential of Hydrogen” –indicates the concentration of H + ions­­­­ pH scale- ranges from 0 – 14 pH 7 = concentration of H + ions and OH - equal Below 7 = acidic = more H + ions Above 7 = basic = more OH - ions Controlling pH= buffers buffers= weak acids or bases –-can react w/strong acids or bases –prevent sudden changes in pH

12. Chemistry of Carbon I. The Chemistry of Carbon A. Characteristics of Carbon 4 valence electrons allows C to form strong covalent bonds 2. Can form C to C bonds a. Types of bonds i. single C-C ii. double C=C ii. triple C=C 3. Very versatile (can make many different compounds)

13. Macromolecules A. Formed by polymerization –1. Process of joining many monomers B. Types of Biological macromolecules 1. Carbohydrates 2. Lipids 3. Nucleic Acids 4. Protein

14. The Macromolecules of Life 1.Carbohydrates 2.Lipids (Fats) 3.Proteins 4.Nucleic Acids

15. Carbohydrates Function: molecules that contain energy and give structure Composed of which 3 elements? –Carbon, Hydrogen, and Oxygen The ratio of hydrogen to oxygen is 2:1

16. Carbohydrates Basic Building block is a Monosaccharide, which is a simple sugar –Example: C 6 H 12 O 6 (Glucose) Glucose - made during photosynthesis; main source of energy for plants and animals

17. Carbohydrates Diagram of Glucose

18. Carbohydrates Fructose - in fruits, sweetest of the simple sugars Galactose - in milk

19. Carbohydrates Disaccharides are formed when 2 monosaccharides combine in a dehydration synthesis reaction: –Examples of disaccharides Lactose = glucose + galactose Sucrose (table sugar) = glucose + fructose

20. Carbohydrates

21. Polysaccharides are 3 or more monosaccharides joined together 3 biologically important examples: –Glycogen in animals –Starch in plants –Cellulose in plants These molecules have a lot of energy stored in them repeating glucose units

22. Carbohydrates Polysaccharide

23. Lipids (Fats) Function: these molecules store long-term energy and make up the cell membrane of cells (phospholipids) Lipids are made of which elements? –Carbon, Hydrogen, and Oxygen There are many carbon and hydrogen atoms but only a few oxygen atoms Do lipids dissolve well in water? –No - they are therefore considered hydrophobic (water-fearing) Some examples of lipids: oils, fats, waxes, steroids, phospholipids

24. Lipids (Fats)

25. Lipids Examples of lipids 1. Steriods- act as chemical messengers 2. Fatty acids i. Saturated- all single bond ii. unsaturated (olive oil)- one C=C iii. polyunsaturated (cooking oils: corn, peanut, sesame, canola) – many C=C

26. Proteins Function: control the rate of reactions, transport materials, form bone and muscle, transport materials. Fight disease, act as enzymes Composed of which 4 elements? –Carbon, Hydrogen, Oxygen, Nitrogen and sulfur Basic building block: amino acid (AA)

27. Proteins Basic building block: amino acid (AA) Question: How many different amino acids are there? –20

28. Proteins Dipeptide –2 amino acids bonded together with a peptide bond. They are joined by dehydration synthesis reactions Polypeptide –long chain of AA bonded together Proteins are composed of 2 or more polypeptide chains

29. Proteins Enzymes are biological catalyst made of protein What is a catalyst? –A substance that speeds up a chemical reaction without being altered How does an enzyme speed up a reaction? –It lowers the activation energy needed to start the reaction Substrate - the molecule(s) that are acted upon by the enzyme Active site - the spot on the enzyme where the substrate fits

30. Proteins - Enzymes Lock and Key Model:

31. Proteins - Enzymes Lock and Key Model:

32. Proteins - Enzymes Lock and Key Model: http://waynesword.palomar.edu/molecu1.htm#lock

33. Proteins How many times can a single enzyme be used? –Thousands Enzymes work at specific pH values and temperatures. If the pH or temperature goes too high or too low, the enzyme won’t work properly –ex. Lactase catalyzes (speed up) the breakdown of lactose into glucose and galactose –ex. Catalase speeds up the breakdown of hydrogen peroxide

34. Nucleic Acids Nucleic Acids are composed of Carbon, Hydrogen, Oxygen, and Nitrogen, Phosophorous Nucleic Acids function in living things as the structure of DNA and RNA –The blueprint of life Monomers- Nucleotides –Composed of a 5-Carbon Sugar, Phosphate group, and Nitrogen Base –Store genetic information –Held together by covalent bonds Polymers- Nucleic Acids –A string of nucleotides –DNA or RNA

35. Nucleic Acids There are four nitrogen bases, meaning there are four “types” of nucleotides –Adenine, Thymine, Guanine, Cytosine RNA is a single strand nucleic acid In DNA, two strands of nucleic acid bond –Double Helix –Adenine always bonds with Thymine –Guanine always bonds with Cytosine

36. Nucleic Acids NUCLEOTIDE RNA DNA

37. Biochemistry THE END