CHEM 1120 1nd Edition Lecture 11Outline of Last Lecture I. Detection of Radioactivitya. Scintillation counterb. Radiotracersc. PET imagingd. Applications of Ionizing RadiationII. Energy Changes in Nuclear Reactionsa. Radioactive decayb. Nuclear fissionc. Nuclear fusiond. The mass defecte. Nuclear binding energiesf. Fission and Fusiong. MeVIII. Nuclear Power: Fissiona. Subcriticalb. Critical massc. SupercriticalThese 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.d. Controlled vs uncontrolledIV. Nuclear Power FusionV. Radiation in the Environment and Living Systemsa. Excitationb. IonizationOutline of Current Lecture I. Radiation Units and Dosesa. Gray (Gy)b. Radc. Sievert (Sv)d. Reme. Radon (Rn)II. Begin Chapter 16 (Acids and Bases)-Not on Exam 1III. Acids and Bases: A brief reviewa. Arrhenius acid and base definitionIV. Bronsted-Lowry Acid Base Definitiona. Conjugate Base Pairsb. Strong Acids and BasesCurrent LectureI. Radiation Units and Dosesa. 1 gray (Gy) = 1 J/kg of tissue (SI)b. 1 rad = 1 x 10^-2 J/kg of tissuec. Not all forms of radiation cause equivalent harm, multiplication by relative biological effectiveness (RBE)i. 1 sievert (Sv) = (1 gray)(RBE)ii. 1 rem = (1 rad)(RBE)d. Radon (Rn)i. Product of nuclear disintegration series of Uranium-238ii. Continually produced as uranium in rocks and soil decaysiii. Radon is a noble gas-unreactiveiv. Has short half-life and alpha-particles have a high RBE, inhaled radon has been linked to lung cancerv. US EPA recommends that radon-222 levels not exceed 4pCi per liter of air in homesII. Begin Chapter 16 (Acids and Bases)-Not on exam 1 III. Acids and Bases: A Brief Reviewa. 3 Levels: Arrhenius, Bronsted, Lewis goes from narrowest to broadest theoryb. Arrhenius acid: substance that directly yields H+ ions when dissolved in waterc. Arrhenius base: a substance that directly yields OH- ions when dissolved in waterd. Missing the role of water look to Bronsted-Lowry theoryIV. Bronsted-Lowry Acid Base Definitiona. Acid: proton donor, any species which donates a H+b. Base: proton acceptor, any species which accepts a H+c. Conjugate acid base pair: 2 species whose formulas differ by a single H+i. Conjugate acid: a species with one more H+ than its conjugate baseii. Conjugate base: a species with on fewer H+ than its conjugate acidd. Strong acids are strong electrolytes: disassociate 100% in wateri. Weak acids are weak electrolytes: do not completely disassociate in waterii. Some substances have negligible acidity in water: negligible acidity, conjugate bases are exceedingly strongiii. The stronger an acid, the weaker its conjugate base (and vise versa)e. Common strong acids: HCl, HBr, HI, HClO3, HClO4, HNO3, H2SO4f. Common strong bases: hydroxides of Group 1A metals and Heavy Group 2A metalsg. How do you know which is stronger?i. Strong acid=weak conjugate
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