BIOL 101 1st Edition Lecture 4Outline of Last Lecture I. Importance of WaterII. Causes of Unusual Behaviors of WaterIII. Unusual Properties of WaterIV. Aqueous Solutions and Their PropertiesV. Acids, Bases, and pHVI. Solute Concentration EXTRA CREDIT HW Problems VII. Solute Concentration EXTRA CREDIT HW SolutionsVIII. pH EXTRA CREDIT HW ProblemsIX. pH EXTRA CREDIT HW SolutionsX. QUIZ THURSDAY IN CLASSOutline of Current Lecture I. Why Carbon?II. IsomersIII. HydrocarbonsIV. Functional GroupsV. Chart of 6 Functional GroupsVI. Introduction to Macromolecules (Chapter 5)Current LectureChapter 4 - Carbon and Molecular DiversityThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.I. Why Carbona. Atoms are small and form strong bonds (valence of Carbon is 4)b. Versatility in bonding  bond to other Carbons or elementsc. Good Transport Formi. CO2 easily crosses membranesd. Carbon can form large complex and diverse molecules that have different functionse. Organic molecules – molecules that contain Carbonf. Carbon Skeleton – refers to the arrangement of carbon atoms in the moleculei. Length – how many atomsii. Shape – straight chain, branched chain, ringiii. Location and number of double bondsiv. What other elements are covalently bonded to the skeletonII. Isomersa. These are compounds that have the same molecular formula, but DIFFERENT structuresb. 3 kinds:i. Structural Isomers – different in the covalent arrangement of atoms (C4H10)ii. Geometric Isomers – same covalent bonds, but differ in spatial arrangement (C2O2H4)1. Because of the rigid double bond, there is no rotation2. Subtle difference affects biological activityiii. Optical Isomers (Sterioisomers) – Isomers that are mirror images of each other1. Occurs when there are 4 different atoms or groups of atoms bonded to the same carbon atom2. Asymmetric Carbon - a carbon atom with 4 different atoms bonded to it3. The 4 different groups can be arranged in space in 2 different ways that are mirror images of each other  they cant superimpose4. Speak of left or right-handed as isomers (hands are mirror images of each other) (D and L isomers)5. Usually only one of the forms is biologically active6. Examples:a. Amino Acids – only the L isomer is used to make proteinsb. Sugars – only the D isomer is recognizedIII. Hydrocarbons a. Molecules containing only Carbon and Hydrogen b. Major components in fossil fuelsc. Hydrocarbons are nonpolar (hydrophobic – lecture 2), so they don’t dissolve in H2O because water is polar (lecture 3)d. Nonpolar because the bonds between C and H are nonpolar covalent bonds (electronegativity of C is 2.55 and H is 2.2  share electrons equally, lecture 2)IV. Functional Groupsa. Specific groups of atoms bonded to the carbon skeletonb. Each functional group has specific chemical and physical propertiesc. They behave consistently from one molecule to the nextd. Usually involved in chemical reactionse. Can be thought of as “molecular accessories”  change them and change the behaviorV. Functional Group Charta. Know:i. The names of the groups ii. Their structuresiii. How they are attached to the carbon skeleton (except phosphate)iv. Characteristics conferred by the groupName of the Group Structural Formula CharacteristicsHydroxyl R ⟷ O ⟷ H Polarity, solubility in H2OCarbonyl R ↔C ⟺ O↕HPolarity, solubility in H2OCarboxyl or Carboxylic Acid O↗↗R ⟷ C ↘ O↘ HDissociates H+ (acidity), adds H+(decreases pH)Amine H↗R ↔ N ↘ HAccepts H+ to become NH3(basic), removes H+ (increasespH)Sulfhydryl R ↔ S ↔ H Forms cross links, stabilizesmoleculesPhosphate R ↔ O ↔ PO3H2Used in energy transferChapter 5 – MacromoleculesVI. Macromoleculesa. 4 Major Types:i. Proteinsii. Carbohydratesiii. Nucleic Acidsiv. Lipidsb. Large organic polymers – large molecules made from many identical or similar subunits connected by covalent bondsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.c. Subunit = monomer = building blocksd. Example of unity in life (lecture 1) – only 40-50 common monomers in all living thingse. Example of diversity in life (lecture 1) – hooking them in different ways creates many kinds of molecules utilizing the same small set of monomersf. Polymers are formed from monomers by:i. Dehydration Synthesis  the loss of H2Oii. One monomer loses a hydroxyl group (-OH)iii. Other monomer loses a hydrogen atom (-H)iv. Those then bond to form H2O, and the two monomers are bonded to each otherv. Dehydration Synthesis REQUIRES energyg. Polymers are broken down into monomers by the opposite process:i. Hydrolysis  adding H2Oii. One monomer adds an -OH groupiii. Other monomer adds an H atomiv. The two monomers are now separatev. Hydrolysis RELEASES energyThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a