BIOL 213 1st Edition Lecture 3 Outline of Last Lecture I. Review of Pasteurization vs sterilizationII. DNA replicationA. Common goal of cellsB. Compartmentalization in cells III. The AtomA. Bonds – covalent and ionicIV. WaterA. Properties B. What if these properties weren’t true?V. Weaker bondsA. Hydrogen bondsB. Hydrophobic interactionsC. Van der Waals interactionsVI. pHVII. The MoleOutline of Current Lecture II. MolarityA. DefinitionB. Tips on how to do the molarity problems III. Acids, Bases and pHA.Definitions of acid and baseB.Ionization of water; Kw C.Tips on how to do problems involving pHD.BuffersIV. Review of the most common chemical groups in biological moleculesA. A list, their formulas, a unique characteristic, and where they’re commonly foundV. MacromoleculesA. “Monomers” of allB. Condensation reactionVI. PolysaccharidesA. Descriptioni. Major functionsB. StructureThese 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. How the flipping of an –O and –OH can change the sugarC. Glucose i. Alpha and betaVII. LipidsA. Descriptioni. Ester linkageB. Basic structurei. Hydrophobic and hydrophilic partsii. Saturated vs UnsaturatedC. PropertiesD. Two main different kinds covered in lecturei. Triacylglycerolii. Phospholipid1. PhosphatidylserineVIII. CholesterolA. Basic structureB. Main functionsi. Hormones IX. ProteinsA. Descriptioni. Major functionsB. Amino Acidsi. Structureii. Classification (nonpolar, charged, or uncharged polar)iii. We need to be able toCurrent LectureII. MolarityA. The concentration of a solution in moles/liter represented by ‘M’B. Commonly denoted by brackets: [X]i. So, if a problem says: [H+] = 0.2M that means:ii. The molarity of hydrogen ions is 0.2 mol/LC. Tips on how to do the molarity problemsi. List what you have and what you wantii. Use the “railroad” method (AKA stoichiometry) to find the answer1. Ex: 5.0 g x 2 mol = 10 g 1 moliii. When filling in the answer for how much water is needed, never put the total volume that the problem asks for. “Fill to (final volume)” is always correct.1. If the problem asks how many grams of something are in 1 liter of a (#) M solution, the answer for water would be “fill to 1 liter”iv. If the problem asks for a dilution1. (want) * (final volume) = (amount to add)(have)III. Acids, Bases and pHA. An acid is a molecule that donates a hydrogen ion H+ (proton)B. A base is a molecule that takes up (accepts) a hydrogen ion H+ (proton)C. pH is the concentration of hydrogen ions (H+) in a solutionD. water always has a neutral pH because it ionizesi. two water molecules are constantly switching back and forth between 2H2O and H3O+ + OH- ii. Kw is the water ionization constant and is equal to 1 x 10-141. Kw = [H+] [OH-] = 1 x 10-142. [H+] = [OH-] = 1 x 10-73. Using properties of log, it’s determined that:4. pH = -log [H+] = 7a. –log10 [H+] = 7 log10[H+] = -7b. 10-7 = [H+] = pHE. Tips on how to do problems involving pHi. TIP: the professor will always use strong acids and bases that completely dissociate on the examii. THEREFORE, the molarity of each ion of the acid/base will always equal to the molarity of the acid/base times the subscript on that specific atomF. Buffersi. All cells need buffers!!ii. Buffers (almost completely) neutralize the effect of the addition of an acid/baseiii. A buffer is a conjugate acid and a conjugate base that exist in equilibriumiv. If an acid is added to a solution containing a buffer:1. The conjugate base will take up H+ ions, causing the pH to go backupv. If a base is added to a solution containing a buffer:1. The conjugate acid will release H+ ions (because the added base took some that were already in the solution), causing the pH to go back downvi. But buffers aren’t perfect – they only work over a specific pH range because eventually the conjugate acid/base will be all used up after the addition of a certain amount of acid/baseIV. Review of the most common chemical groups in biological moleculesChemical Group Formula Characteristic Commonly foundMethyl -CH3Nonpolar hydrocarbonSome amino acids(part of side chain)Hydroxyl -OH Alcohols Carbs, lipidsCarboxyl -COOH Weak acid Amino acidsCarbonyl -Ketone -Aldehyde-C=O-in the middle of a molecule-at the end of a moleculeCarbohydratesAmino -NH2Weak base Amino acidsAmide O=C-NH2Carboxyl + aminePhosphate -PO3Ester and anhydridesPhospholipid bilayerSulfhydryl -SH Forms disulfide bondsAmino acid CysteineV. MacromoleculesA. There are four major classes of macromolecules in biology (only covered first 3 in lecture): i. Polysaccharides – 2% of bacterial cell chemicalsii. Lipids – 2% of bacterial cell chemicalsiii. Proteins – 15% of bacterial cell chemicalsiv. Nucleic acids – 7% of bacterial cell chemicalsB. Each macromolecule is made up of smaller building blocks (monomers):Building block (monomer) macromoleculeSugars PolysaccharidesFatty acids & glycerol chains LipidsAmino acids ProteinsNucleotides Nucleic acidsi. The fatty acids and glycerol chains of lipids technically are not monomers1. A monomer is something that can be added indefinitely to itself to create a polymer2. This cannot be done with the fatty acids or glycerol chains because only 3 fatty acids and one glycerol chain are used to make a lipidii. Therefore lipids are technically not polymers, but the other three are!C. All of these building blocks join together to form the macromolecules via condensation reactioni. The hydroxyl group (-OH) of one molecule joins with a hydrogen atom (-H) of another molecule to form water1. OH- + H+ = H2Oii. The formation of the H2O molecule causes the two building block molecules to bond to the same oxygen atom (O)iii. This bond is now reactiveD. All of these macromolecules break apart into the building blocks via hydrolysisi. Water is consumed by the reactive bond ii. The water molecule is then split to replace the hydroxyl (-OH) and hydrogen atom (H) that were originally given up to create the bondE. Condensation reaction and hydrolysis are oppositesi. Each reverses the effect of the otherVI. PolysaccharidesA. Also known as sugars and carbohydratesB. 1 saccharide = monosaccharideC. 2 saccharides = disaccharideD. Multiple saccharides = polysaccharideE. Thy have the general formula of (CH2O)n i. This is where the name carbohydrate comes from because the