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HONORS BIOLOGY Chapter 2 Quiz Review Name ____________ Chemistry and Radioisotopes These are topics and vocabulary terms covered in this chapter which may appear on the chapter test. Also see pp. 18-23, 30-31 in text for more review. Elements, Atoms, and Molecules Why is chemistry important to biology? Elements (all same atoms); compounds (different elements, in a ratio) Major elements in biology – C, H, O, N, Some minor elements – ex. Cl, Na, P, S – cell parts and chem. reactions Some trace elements – iodine- thyroid; iron– oxygen in blood; fluorine-teeth Atomic Structure Matter, Atomic Theory, Law of Conservation Nucleus – particles, charges, most mass of atom Electrons – electron cloud, charge, most volume of atom Energy levels, valence electrons determine chemical activity Octet Rule- to fill valence 2-8-8, atom then stable Atomic number, mass number (protons + neutrons) Isotopes and average atomic mass – same element, different # neutrons Radioisotopes Unstable – decay to different element, but now stable Half-life, be able to calculate amount remaining or age of fossil Uses: date fossils – use carbon 14 o research “tracers” – use carbon and other isotopes o medical tests - PET scans, iodine goes to thyroid, technetium to bone o radiation therapy - internal pellets or external (use cobalt) o nuclear energy – use uranium; kill bacteria Compounds and chemical bonding ions: electrons gained or lost (+) and (-) charges ionic bonding - opposite charges attract each other o forms a crystal, dissociates in water individual ions Covalent bonding – form molecules, share valence electron pair o Bonds do not break in water but molecules separate Chemical formula, structural formula Chemical Reactions – reactants and products; same atoms, different combinations 1 HONORS BIOLOGY Chapter 2 Quiz Review Water and its Properties Name ____________ These are topics and vocabulary terms covered in Chapter 2 which may appear on the chapter test or quizzes. Also see pp. 24-31 in text for more review. The Water Molecule Why is water necessary for life? Polar covalent bonds – electrons shared unevenly around molecule Water molecule – more electrons on oxygen end (-) Shape is bent, has (+) and (-) poles Hydrogen bonds – H on one molecule oxygen on another Properties of water What are they? Why are they important in living things? Cohesion – hydrogen bonds hold water molecules together o Surface tension – acts like a membrane for cells o High specific heat – stores heat without changing temp o Temperature moderation – keeps temp stable in organisms, constant ocean temp, slow season changes, mild coastal climate o High heat of vaporization – surface water molecules take heat away Evaporative cooling o Why ice floats –less dense than liquid water, molecules farther apart Ice insulates ponds, so water below stays liquid o Capillary action/capillarity – water climbs up narrow tube, small spaces o Transpiration in plants – water climbs against gravity through pull from evaporation on leaves; roots stem leaves air Adhesion – water forms hydrogen bonds to other substances o Universal solvent – polar and ionic, but not nonpolar o Dissolve in water – ions dissociate; molecules stay intact o Capillary action – uses both cohesion and adhesion Blood vessels in animals, veins in plants Solutions and Mixtures Solvent and solute – solvent= main part of a mixture Aqueous solution – solvent is water; fluids in all living things Suspension – too big to dissolve; ex. Blood - cells in watery fluid Acids and bases pH : [H+] ion concentration acid – higher H+, pH below 7; base- higher OH- (lower H+), pH above 7 neutralization reaction: acid + base salt (ionic) + water buffers – weak acid or base, minimizes pH change in humans: mostly pH 7; stomach –acid, pancreas – base, intestine - neutral 2