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Macromolecules 1 Carbon (C) • Carbon has 4 valence electrons (bonding e- in highest energy level) • Carbon can form covalent bonds with as many as 4 other atoms. – 4 Bonds may be single bonds, usually with C, H, O or N. – Carbon can also form double and triple bonds – Phosphorus and Sulfur will also be in the bonds to the Oxygen and Carbons2 Macromolecules • ORGANIC Compounds are carbon based. • Macromolecules are LARGE organic molecules. • Are also called POLYMERS made from smaller “building blocks” called MONOMERS 3 Question: How Are Macromolecules Formed? 4 ANSWER: Remove WATER • This process is called dehydration synthesis which means to put together by removing water. • Remove the hydroxyl ( –OH) group off of one monomer • Remove a hydrogen off of the second monomer • H with the OH makes H2O Chemical Reactions • Chemical Bonds are broken and new Bonds are formed to form the Macromolecules 6 http://cnx.org/content/m47185/latest/ + H 2O 7 Question: How are Macromolecules separated and digested? 8 Answer: Hydrolysis • Hydro “Water”, Lyse “to break” – To break apart using water • Separates polymers by “adding water” HO HO H H H2O HO H 9 Carbohydrates 10 Carbohydrates • Small and large sugar molecules. • Function: The main source of energy for cellular work • Format: Composed of C, H, and O where Hydrogen to Oxygen Ratio is 2:1 • Suffix “ose” Examples: monosaccharides (simplest sugars), disaccharides, polysaccharides 11 Carbohydrates Monosaccharides these are one sugar unit Example: glucose glucose Disaccharide: two sugar unit Example: glucose glucose Sucrose (glucose+fructose) Maltose (glucose + glucose) 12 Carbohydrates Polysaccharides: many sugar units Examples:starch (plant’s energy storage) glycogen (in liver & muscles) cellulose (plant walls) glucose glucose glucose glucose cellulose glucose glucose glucose glucose 13 Example Forming Sucrose • Balanced Equation C6H12O6 + C6H12O6 | glucose C12H22O11 + H2O | fructose 14 ISOMERS – Same Formula, Different structures due to bonding locations http://www.elmhurst.edu/~chm/vchembook 15 Lipids 16 Lipids • Are nonpolar fats and oils that are not soluble in water. • Lipids are soluble in nonpolar solvents which are hydrophobic solvents which are“water fearing” • Format: Composed of C, H, and O but formula has a greater than 2:1 hydrogen to oxygen ratio • Example: C18H36O2 17 Major Function of a Lipid • Major Function: stores energy for long term • Examples: Fats, Phospholipids, Oils, Waxes, Steroid hormones, Triglycerides 18 Lipids Other Functions of lipids: 1. Long term energy storage 2. insulation 3. cushions organs 4. Chemical messengers (hormones) 5. Major component of membranes (phospholipids) 19 Lipids Triglycerides: composed of 1 glycerol and 3 fatty acids. H O H-C----O C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 O H-C----O C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 O fatty acids H-C----O C-CH -CH -CH -CH 2 2 2 H glycerol 20 Omega-3 Fatty Acid Fatty Acids There are two kinds of fatty acids. (You have seen these on food labels) 1. Saturated fatty acids: no Carbon to Carbon double bonds (C=C), carbon is saturated with hydrogens (bad – solids at room temp come from ANIMALS) 2. Unsaturated fatty acids: double bonds between the carbons, so less hydrogens in the structure (better for your health, liquids at room temp come from PLANTS) 22 Check out the Single vs. Double bonds… http://biology.clc.uc.edu/courses/bio104/lipids.htm 23 http://biology.clc.uc.edu/courses/bio104/lipids.htm 24 Proteins 25 Proteins • Monomer of Proteins are the Amino Acids (20 different kinds of AA) • AA bond together by peptide bonds – Attachment is a Carbon to Nitrogen single bond. • Format: All Contain C, H, O, N some have S. Contain amino (-NH2) and carboxyl (–COOH) functional groups. • Dehydration synthesis removes the H from the amino group and the OH from the carboxyl group. 26 http://hyperphysics.phy-astr.gsu.edu 27 Functions of Proteins Functions of proteins: Enzymes: speed up reactions Aid in Transportation in and out of cell. Regulates hormones (For example: insulin) Aid in Movement (controls actions in muscles) Defense: antibodies of the immune system Structures of membranes, hair, nails 28 Proteins • Common suffix -ase • Amylase, protease, isomerase, ligase, others: trypsin, pepsin • Optimal temperature and pH required for proper enzyme (protein) function 29 Enzymes Speed Up Reactions http://www.cikguhafiz.com/v1/webcikguhafiz /images/kuiz/enzyme2.png 30 Denaturing Destroys the Protein • Too hot, too acidic, too basic ruins the active site for the protein. • Activity graph show a drop off in rate. • Go back to previous graph, where does the enzyme denature? • http://highered.mheducation.com/sites/ 0072943696/student_view0/chapter2/an imation__protein_denaturation.html 31 Nucleic Acids 32 Nucleic acids • Two types: a. Deoxyribonucleic acid (DNAdouble helix) b. Ribonucleic acid (RNA-single strand) • Nucleic acids are composed of long chains of nucleotides linked by dehydration synthesis. • Function: genetic programming • Formula Format: C, H, N, O, and now P (Phosphorus) 33 Nucleic acids • Monomer is a Nucleotide – Which includes the following three things: phosphate group pentose sugar (5-carbon) Deoxyribose in DNA Ribose in RNA nitrogenous bases: adenine (A), thymine (T) DNA only, cytosine (C) guanine (G) uracil (U) RNA only 34 Nucleotide Phosphate Group O O=P-O O 5 CH2 O N C1 C4 Nitrogenous base (A, G, C, or T) Sugar (deoxyribose) C3 C2 35 5 DNA double helix O 3 3 O P 5 O C G 1 P 5 3 2 4 4 2 3 1 P T 5 A P 3 O O P 5 O 3 5 P 36 Two DNA Strands Connect Together… • Cytosine bonds to Guanine • Adenine bonds to Thymine • Notice that a purine will connect with a pyrimidine • Double helix bonds at nitrogenous bases by a HYDROGEN BOND – Not a true “bond”, but an attraction of one molecule’s slight Positive charge (due to polar bonding) to a lone pair of electrons on the opposing molecule. 37 Powerpoint Revised from www.biologycorner.com 38