2-1 CHAPTER 2 LECTURE OUTLINE SEE POWERPOINT IMAGE SLIDES FOR ALL FIGURES AND TABLES PRE-INSERTED INTO POWERPOINT WITHOUT NOTES. Copyright (c) The McGraw-Hill Companies, Inc.
Download ReportTranscript 2-1 CHAPTER 2 LECTURE OUTLINE SEE POWERPOINT IMAGE SLIDES FOR ALL FIGURES AND TABLES PRE-INSERTED INTO POWERPOINT WITHOUT NOTES. Copyright (c) The McGraw-Hill Companies, Inc.
2-1 CHAPTER 2 LECTURE OUTLINE SEE POWERPOINT IMAGE SLIDES FOR ALL FIGURES AND TABLES PRE-INSERTED INTO POWERPOINT WITHOUT NOTES. Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Reading Assignment 1 2-2 Read pages 44-55 in Chapter 2 The Chemical Elements 2-3 _________ = simplest form of matter with unique chemical properties 24 elements have biological role 6 elements = 98.5% of body weight trace elements in minute amounts _________ = # of protons in nucleus periodic table elements arranged by _________ 2-4 ______________ Number of protons and neutrons in nucleus Atomic mass units (amu) Number of neutrons determined by subtracting the atomic number from the mass number 2-5 Atomic Structure 2-6 ______ = center of atom _____ : single + charge, mass = 1 amu ______: no charge, mass = 1 amu Electron shells surround the nucleus ________: single negative charge, little mass electrons swarm about the nucleus in electron shells (energy levels) _________ in the outermost shell interact with other atoms determine chemical behavior Planetary Models of Elements 2-7 p+ represents protons, no represents neutrons Electron Energy Levels 2-8 Each energy level can hold certain maximum number of __________ Maximum number determined by formula X=2(n squared) Isotopes and2-9Radioactivity _____________ differ in # of neutrons extra neutrons increase atomic weight isotopes of an element are chemically similar have same valence electrons Atomic _____ average atomic mass of the isotopes Radioisotopes and Radioactivity 2-10 Isotopes same chemical behavior, differ in physical behavior breakdown gives off radiation ___________ unstable isotopes every element has at least one radioisotope Radioactivity radioisotopes decay to stable isotopes releasing radiation we are all mildly radioactive Ions and Ionization 2-11 • Ions - carry a charge due to an unequal number of ________________ _______ = transfer of electrons from one atom to another ( stability of valence shell) Anions and Cations • _________ 2-12 – atom that gained electrons (net negative charge) • ________ – atom that lost an electron (net positive charge) • Ions with opposite charges are _______ to each other ___________ 2-13 Salts that ionize in water to form body fluids Form solutions capable of conducting electricity Importance chemical reactivity osmotic effects (influence water movement) electrical effects on nerve and muscle tissue Imbalances cause muscle cramps, brittle bones, coma and death 2-14 Molecules and 2-15 Chemical Bonds _________ two or more atoms covalently bonded _________ two or more atoms of different elements covalently bonded ________ formula elements and how many atoms of each _________formula location of each atom structural isomers revealed Structural Formula of Isomers 2-16 How are molecular and structural formulas different? Chemical 2-17 Bonds What are the 4 types? Describe each. Chemical Bonds Song 2-18 http://www.youtube.com/watch?v=BCYrNU- 7SfA&feature=related _________ Bonds 2-19 Attraction of oppositely charged ions No sharing of electrons Weak bond (easily dissociates in water) ________Bonds 2-20 Formed by sharing of valence electrons Types of covalent bonds single = sharing of single pair electrons double = sharing of 2 pairs nonpolar shared electrons (equal time around each nucleus) strongest of all bonds polar negative charge where electrons spend most time Single Covalent Bond 2-21 One pair of electrons are ________ Double covalent bonds: Two pairs of electrons are _____ each C=O bond 2-22 Nonpolar /Polar Covalent Bonds 2-23 electrons shared ____ electrons shared _____ Covalent means? Nonpolar/polar refers to? ________Bonds 2-24 Weakest bond = no sharing of electrons Attraction between polar molecules positive hydrogen atoms to negative oxygen atoms in a 2nd molecule Physiological importance properties of water created by shapes of large complex molecules determined by folding due to hydrogen bonds Hydrogen Bonding in Water 2-25 1 2 Water animation 2-26 http://www.youtube.com/watch?v=KiZJOTt3Dl0&f eature=related _________ Forces 2-27 Weak attractions between neutral atoms Fluctuations in electron density create polarity Only 1% as strong as a covalent bond folding of large molecules significant when 2 large surfaces meet ______= ability to dissolve other chemicals 2-28 ______(charged substances) dissolve easily in water ______ (neutral substances) do not easily dissolve in water Water= Metabolic reactions and transport of substances Water as a Solvent 2-29 ______ water molecules overpower the ionic bond in Na+Cl-forming _______ around each ion -water molecules: ____ pole faces Na+, ____ pole faces Cl- Adhesion and Cohesion 2-30 _________- tendency of one substance to cling to another _________-tendency of like molecules to cling to each other water is very cohesive due to its ______ bonds surface film on water formed by __________ Chemical Reactivity of Water 2-31 Participation in chemical reactions Water ionizes into H+ OH Water ionizes other chemicals (acids and salts) Water involved in _________ and __________ reactions Thermal Stability of Water 2-32 Water stabilizes internal temperature Has high _______ ______ Hydrogen bonds inhibit temperature increases by inhibiting molecular motion Water absorbs heat without changing temperatures Effective ________ 1 ml of perspiration removes 500 calories _______: amount of heat required to raise temperature of 1 g of water by 1 degree C Measures of Concentration 2-33 Weight per Volume weight of solute in given volume of solution IV saline: 8.5 grams NaCl/liter of solution Percentages Weight/volume of solute in solution IV D5W (5% w/v dextrose in distilled water) 5 grams of dextrose and fill to 100 ml water Molarity moles of solute/liter in solution physiologic effects based on number of molecules in solution not on weight Molarity 2-34 Molecular weight in grams = 1 mole of molecules 1 mole = Avogadro’s number of molecules Molarity is the number of moles of solute/ liter of solution MW of glucose is 180 one-molar (1.0M) glucose solution contains 180g/L Percentage vs. Molar Concentrations 2-35 Percentage # of molecules unequal weight of solute equal Molar # of molecules equal weight of solute unequal Electrolyte Concentrations 2-36 Effect the body chemically, physically and electrically depends on charge and concentration Measured in equivalents 1 Eq will electrically neutralize 1 mole of H+ or OH- ions multiply molar concentration x valence of the ion 1 M Na+ = 1 Eq/L 1 M Ca2+ = 2 Eq/L Acids, Bases and pH 2 3 7 An acid is a ____ ____ (releases H+ ions) A base is a _____ _____ (accepts H+ ions) pH = the concentration of _________ a pH of less than 7 is _____ solution a pH of greater than 7 is _____ solution a pH of 7.0 is _____ pH pH= -log [H+] pH Scale 2-38 Strong vs weak acid Strong vs weak base Practice 2-39 1) Regarding changes in pH, if pH changes from 7 to 5 will the [H+] increase or decrease? 2) By how much? 3) Will the solution become more acidic or more basic? ________ Maintains a constant pH upon the addition of small amounts of either acid or base 2 parts to a buffer: weak acid and a weak base Acid- can donate H+ ion if [H+] decreases Base- can accept H+ ion if [H+] increases Salts Mixing an acid and a base results in water and____ A compound that yields ions other than hydrogen ions is called a salt Electrolytes Acids, bases, and salts are called ________ Solutions of electrolytes conduct electricity because of the presence of ions Would a solution of hydrochloric acid be an electrolyte? HCl H+ + Cl- Chemical Reaction 2-43 Process that forms or breaks an ionic or covalent bond Symbolized by chemical ________ reactants products What are the 4 Classes of reactions? _______ Reactions 2-44 Two or more small molecules combine to form a larger one A + B AB _______ Reactions 2-45 Large molecules broken down into smaller ones AB A + B _______ Reactions Two molecules collide and exchange atoms or 2-46 group of atoms AB+CD ABCD ex. Stomach acid (HCl) and sodium bicarbonate (NaHCO3) from the pancreas combine to form NaCl and H2CO3 (carbonic acid) AC + BD Exchange Reactions 2-47 Single exchange AB+C AC+B Double exchange AB+CD AD + CB _____ Reactions 2-48 Go in either direction (symbolized with double-headed arrow) A + B AB CO2 + H2O <-> H2CO3 <-> carbonic acid HCO3- + H+ bicarbonate Law of ______ determines direction side of equation with greater quantity of reactants dominates Reaction Rates 2-49 Basis for reactions is _________ and collisions Reaction Rates affected by: 1) 2) 3) ________= all the chemical reactions of the body 2-50 _______: energy releasing (exergonic) decomposition reactions breaks covalent bonds, produces smaller molecules, releases ______ _______: energy storing (endergonic) synthesis reactions requires _____ input Oxidation-Reduction Reactions 2-51 _______ molecule gives up electrons and releases energy accepting molecule is the oxidizing agent oxygen is often the electron acceptor ________ molecule gains electrons and energy donating molecule is the reducing agent Oxidation-reduction (redox) reactions Electrons are often transferred as hydrogen atoms OIL-RIG 2-52 Organic Chemistry 2-53 Study of compounds containing carbon 4 categories of carbon compounds carbohydrates lipids proteins nucleotides and nucleic acids Organic Molecules and _____ 2-54 Only __ valence electrons bonds readily to gain more valence electrons Forms long chains, branched molecules and rings serve as the backbone for organic molecules Carries a variety of ____________ groups Functional Groups 2-55 Atoms attached to carbon backbone Determines __________ Monomers and Polymers 2-56 _________ = very large molecules ______= macromolecules formed from monomers bonded together ______ = an identical or similar subunit Polymerization 2-57 Bonding of monomers together to form a ________ Formed by _______ synthesis ________ molecules are a polymer of 3000 glucose monomers ______ molecules are a polymer of amino acids _________ Synthesis 2-58 Monomers covalently bond together to form a ________ with the removal of a _____ molecule A ______ group is removed from one monomer and a _______ from the next Hydrolysis 2-59 Splitting a polymer (____) by the addition of a water molecule (____) a covalent bond is broken All digestion reactions consists of ________ reactions Organic Molecules: _________ 2-60 Hydrophilic organic molecule General formula ________ n = number of _____ atoms for glucose, n = 6, so formula is C6H12O6 _______ of hydrogen to oxygen Names of carbohydrates word root sacchar- or the suffix -ose often used monosaccharide or glucose _____________ 2-61 Simple sugars General formula is C6H12O6 structural isomers • Major monosaccharides – ____________________ – produced by digestion of complex carbohydrates • glucose is blood sugar Disaccharides 2-62 Sugar molecule composed of ______ Major disaccharides sucrose = __________ Lactose = __________ glucose + fructose glucose + galactose Maltose = __________ glucose + glucose ___________ 2-63 Chains of _______ subunits _______: energy storage in plants _______: structural molecule of plant cell walls Glycogen: energy storage in animals Carbohydrate Functions 2-64 All digested carbohydrates converted to glucose and oxidized to make _______ What are conjugated carbohydrates? Give 3 types with examples of each? 2-65 Organic Molecules: Lipids 2-66 _________ organic molecule Less oxidized and thus has more calories/gram What are the five primary types in humans? 1) 2) 3) 4) Fatty Acids 2-67 Chain of 4 to 24 carbon atoms Where is the carboxyl (acid) group? Where is the methyl group? hydrogen bonded along the sides Classified saturated - carbon atoms saturated with hydrogen unsaturated - contains C=C bonds without hydrogen Is this saturated or unsaturated? Triglycerides (Neutral Fats) 2-68 3 fatty acids bonded to _______ molecule (________ synthesis) At room temperature when liquid called _____ often polyunsaturated fats from _______ when solid called _____ saturated fats from _______ Function? Phospholipids 2-69 Triglyceride with one fatty acid replaced by a ________ group Amphiphilic character fatty acid “tails” are _________ Phosphate “head” is _________ Eicosanoids 2-70 Derived from _________ (a fatty acid) _____-like chemical signals between cells Includes ________ – produced in all tissues Steroids and Cholesterol 2-71 _______= lipid with carbon atoms in four rings all steroids are derived from _________ Examples: Cholesterol important component of _________ produced only in animal _______ naturally produced by our body 2-72 Organic Molecules: Proteins 2-73 • ______ = polymer of amino acids • ______ = carbon with 3 attachments – Amino (NH2), carboxy (COOH) and radical group (R group) • 20 unique amino acids ____groups differ ______ determined by -R group Naming of Peptides 2-74 _____ = polymer of 2 or more amino acids Named for the number of amino acids _______ have 2, tripeptides have 3 _______ have fewer than 10 to 15 ________ have more than 15 _________ have more than 100 Dipeptide Synthesis 2-75 •____________creates a peptide bond that joins amino acids Protein Structure and Shape 2-76 Primary structure Secondary structure ___________ shape _____bonds between negative C=O and positive NH groups Tertiary structure further folding and bending into _____ and ________shapes that contain both alpha helix and beta pleated sheet Quaternary structure 2-77 In Class 2-78 1) Describe the secondary level of protein structure. 2) What makes up the primary structure of a protein? 3) Association of two or more polypeptide chains with one another refers to what level of protein structure? 4) The level of protein structure that includes both alpha helix and beta pleated sheets and results from interactions between R groups 5) The bonds between amino acids are _________ bonds. 6) The bonds between areas of an alpha helix are _________ bonds. Conjugated Proteins 2-79 What do we mean by conjugated protein? Give an example Protein Conformation and Denaturation 2-80 Conformation – unique 3-D shape crucial to function ability to ______ change their conformation opening and closing of cell membrane pores Denaturation Protein Functions 2-81 What are 7 ways proteins function in the body? Protein Functions 2-82 What are 7 functions of proteins? Structure collagen, keratin Communication some hormones, cell receptors Membrane Transport channels, carriers Catalysis enzymes Protein Functions 2 2-83 Recognition and protection antigens, antibodies and clotting proteins Movement molecular motor = molecules that can change shape repeatedly Cell adhesion proteins bind cells together Enzymes 2-84 _______ as biological catalysts promote rapid reaction rates Substrate - substance an enzyme acts upon Naming Convention named for substrate with -ase as the suffix amylase enzyme digests starch (amylose) Lowers ____________= energy needed to get reaction started Enzymes and Activation Energy 2-85 Steps of an Enzyme Reaction 2-86 Substrate approaches enzyme molecule Substrate binds to active site forming enzyme- substrate complex highly specific Enzyme breaks bonds in substrate Reaction products released Enzyme repeats process over and over Can an enzyme be reused? Can an enzyme facilitate any type of reaction? Enzymatic Reaction Steps 2-87 Enzymatic Action 2-88 Reusability of enzymes enzymes are unchanged by the reactions Astonishing speed millions of molecules per minute Temperature and pH change shape of enzyme and alter its ability to bind enzymes vary in optimum pH salivary amylase works best at pH 7.0 pepsin works best at pH 2.0 temperature optimum for human enzymes = __________ Cofactors and Coenzymes 2-89 Cofactors _________ (iron, copper, zinc, magnesium or calcium ions) bind to enzyme and change its ______ _______to function Coenzymes ______ cofactors derived from water-soluble vitamins (niacin, riboflavin) transfer ______ between enzymes NAD+ (Cofactor or Coenzyme??) 2-90 NAD+ transports ______from one metabolic pathway to another Metabolic Pathways 2-91 Chain of reactions, each catalyzed by an enzyme ABCD A is initial reactant, B+C are intermediates and D is the end product Regulation of metabolic pathways activation or deactivation of the _________ cells can turn on or off pathways Organic Molecules: ________ 2-92 3 components nitrogenous base sugar (monosaccharide) one or more phosphate groups Physiological important nucleotides ATP = energy carrying molecule cAMP = activates metabolic pathways DNA = carries genetic code RNA = assists with protein synthesis ATP (Adenosine Triphosphate) 2-93 ATP contains adenine, ribose and 3 phosphate groups ATP 2-94 Holds energy in covalent bonds 2nd and 3rd phosphate groups have high energy bonds ~ ATPases hydrolyze the 3rd high energy phosphate bond separates into ADP + Pi + energy _____________ addition of free phosphate group to another molecule Overview of ATP Production 2-95 ATP consumed within 60 seconds Continually replenished Other Nucleotides 2-96 ___________________(cAMP) formed by removal of both high energy Pi’s from ATP formation triggered by hormone binding to cell surface cAMP becomes “___________” within cell activates effects inside cell Nucleic Acids 2-97 ______ (deoxyribonucleic acid) 100 million to 1 billion nucleotides long contains genetic code cell division, sexual reproduction, protein synthesis _____(ribonucleic acid) – 3 types transfer RNA, messenger RNA, ribosomal RNA 70 to 10,000 nucleotides long involved in protein synthesis coded for by DNA