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APPALACHIAN BIO 1201 - Reductionist View of Biology; Chemistry of Life; Water
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BIO 1201 1st Edition Lecture 4 Outline of Last Lecture I.How Science WorksII.Model SystemsIII.The Importance of Peer ReviewOutline of Current Lecture I.Reductionist View of BiologyII.Chemistry of Lifea.Chemical BondsIII.WaterCurrent LectureI. Reductionist View of Biology: one can understand the macromolecular by understanding the atoms/molecules that make it upa. Organisms tend to use a small number of atoms/elementsi. The main elements are oxygen (65%), carbon (18%), hydrogen (10%), and nitrogen (3%)II. Chemistry of Lifea. Atoms need to be joined together to form molecules—accomplished by chemicalbondsi. Atoms don’t always share electrons equally1. Electronegativity is a measure of the affinity for e- in a covalent bond by a particular atoma. Higher electronegativity=greater affinity for e- (example: oxygen)b. Carbon and hydrogen have medium electronegativityc. This is important for understanding how molecules are put together and is the basis for strength of bonds (covalent > ionic > H-bonds)ii. Covalent Bonds: when adjacent atoms share electrons (e-); specific atomsare most stable when forming a certain number of covalent bonds.1. Share 2e-: single bond2. Share 4e-: double bond3. Share 6e-: triple bond4. Example: hydrocarbons – C – Ha. Carbon and hydrogen both have similar electronegativity, so they share electrons equallyThese 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.iii. Ionic Bond: an association of two ions that have opposing charges—opposites attract; weaker than covalent bonds1. Example: NaCl --salta. Sodium (Na) has low electronegativity, so it becomes positive when it loses an electron to Chlorineb. Chlorine (Cl) has high electronegativity, so it becomes negative when it takes an electron from Sodiumiv. Hydrogen Bonds (H-bonds): weak chemical bond formed when a partially positive hydrogen atom in a molecule is attracted to the partially negativeatom of a neighboring molecule1. Example: H-Oa. Oxygen has high electronegativity, but hydrogen has medium electronegativity, so electrons cannot be stolen b. Instead, electrons are pulled closer to oxygen, giving it a slightly negative charge and hydrogen a slightly positive chargeIII. Water: a major component of all organismsa. It is a polar molecule because oxygen is slightly negative and hydrogen is slightly positiveb. Adjacent water molecules can interact with each other via Hydrogen bondsi. One water molecule can interact with as many as 4 adjacent water moleculesii. The number of interacting adjacent water molecules reflects the water’s state of matter1. Gas state: few H-bonds2. Liquid state: more H-bonds3. Solid State (ice): maximum number of H-bondsc. How other molecules interact with wateri. “like dissolves like”: molecules that have similar properties can interact with each otherii. Hydrophilic: water-loving; molecules that are polar or charged can interact with water1. Example: NaCliii. Hydrophobic: nonpolar molecules that cannot interact with water1. Example: oil, made of carbon and hydrogeniv. Amphipathic: molecules that have hydrophilic regions and hydrophobic regions1. Example:


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APPALACHIAN BIO 1201 - Reductionist View of Biology; Chemistry of Life; Water

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