MCB 100 1st Edition Lecture 5Outline of Last Lecture I. Study of fermentationII. Vaccination against viral infectionIII. Fighting infectious disease with cleanlinessIV. Four eras in the history of microbiologyOutline of Current Lecture I. Properties of living matter II. Common elements that are common in living matter III. Important chemistry terms IV. Differences between ionic and covalent bonds V. Organic compoundsVI. Organic functional groups (important!) Current LectureI. Properties of Living MatterA. Living matter contains carbonB. The atoms in an organic molecule are held together by covalent bonds C. Living organisms are mostly made of about 20 different elementsD. Six elements make up most of the mass of organic compounds and can form covalent bonds:i. C- Carbon (4 valence e-)ii. H- Hydrogen (1 valence e-)iii. O- Oxygen (6 valence e-)iv. N- Nitrogen (5 valence e-)v. P- Phosphorous (5 valence e-)vi. S- Sulfur (6 valence e-) E. Proteins, nucleic acids, lipids, and carbohydrates that form living matter are large complicated molecules (macromolecules). Macromolecules stick to each other due to non-covalent attractions so there's a higher level of order for structure. Enzyme subunits can stick and work together. Regulatory proteins can bind to specific DNA sequences. II. Important chemistry terms A. Mixture: a substance (or sample) that can be broken down into different parts by physical manipulations that don't necessarily involve chemical changesThese 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.B. Compound: a pure substance that can be broken down into different parts only by chemical reactions C. Element: a pure substance that can't be broken down into different parts by chemical reactionsD. Molecule: the smallest particle possible for a compoundE. Atom: the smallest particle possible for an elementIII. Ionic vs. covalent bonds A. Ionic bonds: formed when one or more electrons are transferred from one atom to another resulting in a charge imbalance in both atoms. Atom that loses electron becomes positively charged (cation). Atom that gains electron becomes negatively charged.i. Compounds held together by ionic bonds are usually simple (sodium chloride-NaCl, calcium bromide- CaBr2, potassium iodide- KI)ii. Oxidation/redox reactions B. Covalent bonds: formed when two atoms share a pair of electrons. Atoms must touch each other in order to share. A double bond forms when two atoms share two electron pairs and a triple bond forms when two atoms share three electron pairs. Quadruple bonds are not possible between two atoms. i. Compounds held together by covalent bonds can be large and complex (methane-CH4, water- H2O, ammonia- NH3, formaldehyde- CH2O, ATP, glucose, lactose, alanine, human chromosomes, etc.)IV. Organic compoundsA. Alkanes (methane- 1 carbon; ethane- 2 carbons; propane- 3 carbons; butane- 4 carbons; pentane, hexane, heptane, octane, nonane, decane)i. Hydrocarbon: composed of just carbon and hydrogenii. Saturated hydrocarbon: all C-C bonds are single bonds B. Louis Pasteur- figured out the 3D shapes of compounds (methane has a tetrahedral shape) V. Organic Functional groups (need to memorize everything on the chart!) A. Hydroxyl group (alcohol)i. -ol ii. R-O-H iii. Found in alcohols and sugars (very hydrophilic) B. Amino group (deprotonated)i. -amine ii. R-N-H-H iii. Basic, can act as a proton acceptorC. Aldehyde group (terminal carbonyl)i. -alii. R-C-O-Hiii. Found in sugars D. Ketone group (internal carbonyl)i. -oneii. R-C-O-Riii. Found in some sugarsE. Carboxylic acid group (protonated)i. -ic acid ii. R-C-O-O-Hiii. Acidic, acts as a proton donorF. Sulfhydryl groupi. Mercaptanii. R-S-Hiii. nonpolar-Organic phosphate groupi. Phospho- ii. R-O-P-O-O-Oiii. Seen in nucleic
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