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CHAPTER 2LECTURE OUTLINE
SEE POWERPOINT IMAGE SLIDESFOR ALL FIGURES AND TABLES PRE-
INSERTED INTOPOWERPOINT WITHOUT NOTES.
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Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Reading Assignment 1
Read pages 44-55 in Chapter 2
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The Chemical Elements2-3
_________ = 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 Structure2-6
______ = 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 Elements2-7
p+ represents protons, no represents neutrons
Electron Energy Levels2-8
Each energy level can hold certain maximum number of __________
Maximum number determined by formula
X=2(n squared)
Isotopes and Radioactivity2-9
_____________ 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 Radioactivity2-10
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 Ionization2-11
_______ = transfer of electrons from one atom to another ( stability of valence shell)
• Ions - carry a charge due to an unequal number of ________________
Anions and Cations2-12• _________
– 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 Chemical Bonds2-15
_________ 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 IsomersHow are molecular and structural
formulas different?
2-16
Chemical Bonds2-17
What are the 4 types?
Describe each.
Chemical Bonds Song2-18
http://www.youtube.com/watch?v=BCYrNU-7SfA&feature=related
_________ Bonds2-19
Attraction of oppositely charged ions No sharing of electronsWeak bond (easily dissociates in water)
________Bonds2-20
Formed by sharing of valence electronsTypes 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 Bond2-21
One pair of electrons are ________
2-22
Double covalent bonds: Two pairs of electrons are _____ each C=O bond
Nonpolar /Polar Covalent Bonds2-23
electrons shared ____
electrons shared _____
Covalent means?Nonpolar/polar refers to?
________Bonds2-24
Weakest bond = no sharing of electronsAttraction 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 animation2-26
http://www.youtube.com/watch?v=KiZJOTt3Dl0&feature=related
_________ Forces2-27
Weak attractions between neutral atomsFluctuations in electron density create
polarityOnly 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 Solvent2-29
______ water molecules overpower the ionic bond in Na+Cl-
-forming _______ around each ion-water molecules: ____ pole faces Na+, ____ pole faces Cl-
Adhesion and Cohesion2-30
_________- 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 Water2-31
Participation in chemical reactions Water ionizes into H+ OH- Water ionizes other chemicals (acids and salts) Water involved in _________ and __________ reactions
Thermal Stability of Water2-32
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 Concentration2-33
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
waterMolarity
moles of solute/liter in solution physiologic effects based on number of
molecules in solution not on weight
Molarity2-34
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 Concentrations2-35
Percentage# of molecules
unequal weight of solute
equal
Molar # of molecules equal weight of solute
unequal
Electrolyte Concentrations2-36
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 pH2-37
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 Scale2-38
Strong vs weak acidStrong vs weak base
Practice
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?
2-39
________
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+] decreasesBase- 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 ionsWould a solution of hydrochloric acid be an
electrolyte?HCl H+ + Cl-
Chemical Reaction2-43
Process that forms or breaks an ionic or covalent bond
Symbolized by chemical ________reactants products
What are the 4 Classes of reactions?
_______ Reactions2-44
Two or more small molecules combine to form a larger one
A + B AB
_______ Reactions2-45
Large molecules broken down into smaller ones
AB A + B
_______ Reactions2-46Two molecules collide and exchange
atoms or group of atomsAB+CD ABCD AC + BD
ex.
Stomach acid (HCl) and sodium bicarbonate (NaHCO3) from the pancreas combine to form NaCl and H2CO3 (carbonic acid)
Exchange Reactions2-47
Single exchangeAB+C AC+B
Double exchangeAB+CD AD + CB
_____ Reactions2-48
Go in either direction (symbolized with double-headed arrow)
A + B AB
CO2 + H2O <-> H2CO3 <-> HCO3- + H+
carbonic acid bicarbonate Law of ______ determines direction
side of equation with greater quantity of reactants dominates
Reaction Rates2-49
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 Reactions2-51
_______ 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 Chemistry2-53
Study of compounds containing carbon4 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 Polymers2-56
_________ = very large molecules______= macromolecules formed from
monomers bonded together ______ = an identical or similar subunit
Polymerization2-57
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
_________ Synthesis2-58
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
Hydrolysis2-59
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 moleculeGeneral formula
________ n = number of _____ atomsfor 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
Disaccharides2-62
Sugar molecule composed of ______
Major disaccharides sucrose = __________
glucose + fructose Lactose = __________
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 Functions2-64
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: Lipids2-66
_________ organic moleculeLess oxidized and thus has more
calories/gramWhat are the five primary types in humans?
1)2)3)4)
Fatty Acids2-67
Chain of 4 to 24 carbon atoms Where is the carboxyl (acid) group? Where is the
methyl group? hydrogen bonded along the sidesClassified
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?
Phospholipids2-69Triglyceride with one fatty acid replaced
by a ________ groupAmphiphilic character
fatty acid “tails” are _________ Phosphate “head” is _________
Eicosanoids2-70
Derived from _________ (a fatty acid)_____-like chemical signals between
cellsIncludes ________ – produced in all
tissues
Steroids and Cholesterol2-71
_______= 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: Proteins2-73
• ______ = 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 Peptides2-74
_____ = 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 Synthesis2-75
•____________creates a peptide bond that joins amino acids
Protein Structure and Shape2-76
Primary structure
Secondary structure ___________ shape _____bonds between negative C=O and positive
N-H groupsTertiary structure
further folding and bending into _____ and ________shapes that contain both alpha helix and beta pleated sheet
Quaternary structure
2-77
In Class
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.
2-78
Conjugated Proteins2-79
What do we mean by conjugated protein?Give an example
Protein Conformation and Denaturation2-80
Conformation – unique 3-D shape crucial to function ability to ______ change their conformation
opening and closing of cell membrane pores
Denaturation
Protein Functions2-81
What are 7 ways proteins function in the body?
Protein Functions2-82
What are 7 functions of proteins?Structure
collagen, keratin
Communication some hormones, cell receptors
Membrane Transport channels, carriers
Catalysis enzymes
Protein Functions 22-83
Recognition and protection antigens, antibodies and clotting proteins
Movement molecular motor = molecules that can change
shape repeatedly
Cell adhesion proteins bind cells together
Enzymes2-84
_______ as biological catalysts promote rapid reaction rates
Substrate - substance an enzyme acts uponNaming Convention
named for substrate with -ase as the suffix amylase enzyme digests starch (amylose)
Lowers ____________= energy needed to get reaction started
2-85
Enzymes and Activation Energy
Steps of an Enzyme Reaction2-86
Substrate approaches enzyme moleculeSubstrate binds to active site forming
enzyme-substrate complex highly specific
Enzyme breaks bonds in substrateReaction products releasedEnzyme repeats process over and over
Can an enzyme be reused?Can an enzyme facilitate any type of
reaction?
2-87
Enzymatic Reaction Steps
Enzymatic Action2-88
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 Coenzymes2-89
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 Pathways2-91
Chain of reactions, each catalyzed by an enzyme
A B C DA is initial reactant, B+C are intermediates
and D is the end productRegulation 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
ATP2-94
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
ATP consumed within 60 secondsContinually replenished
2-95
Other Nucleotides2-96
___________________(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 Acids2-97
______ (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