Basic ChemistryWhy do I care?Matter and EnergySlide 4Forms of Energy the Body UsesComposition of Matter Elements and AtomsAtomic StructurePlanetary and Orbital Models of AtomIdentifying ElementsAtomic WeightPeriodic Table of ElementsMolecules and CompoundsChemical BondsElectron ShellsTypes of Chemical Bonds IonicTypes of Chemical Bonds CovalentPolar vs. NonpolarTypes of Chemical Bonds Hydrogen BondsChemical ReactionsFactors that Affect Rate of Chemical RxnsBiochemistry: Inorganic vs. OrganicInorganic Compounds WaterInorganic Compounds SaltsInorganic Compounds Acids and BasespH: Acid-Base ConcentrationsOrganic Compounds CarbohydratesOrganic Compounds LipidsSlide 28Slide 29Organic Compounds ProteinsSlide 31Enzymes and Enzyme ActivityOrganic Compounds Nucleic AcidsOrganic Compounds Nucleic Acids - DNAOrganic Compounds Nucleic Acids - RNAOrganic Compounds Nucleic Acids Adenosine Triphosphate - ATPThe EndBasic ChemistryChapter 2Why do I care?What about your food?Medicines?Reactions in your body?Matter and EnergyMatter = anything that takes up space and has massSolids – bones, teeth – definite shape and volumeLiquids – blood plasma – definite volumeGas – Air we breathe – changes volume and shapeChanges to MatterPhysical changes – do not change basic nature of substanceChemical changes – do alter basic nature of substanceMatter and EnergyEnergy = massless and doesn’t take up spaceAbility to do work or put matter into motionKinetic vs. Potential Energy, all forms exhibit bothForms of Energy the Body UsesChemical – stored in bonds, when broken potential energy converted to kinetic – ATPElectrical Energy – Movement of charged particles, electrical current generated when ions move across cell membranes – nerve impulsesMechanical Energy – Directly involved in moving matter – muscle contraction, pulls on bones, limbs moveRadiant Energy – Electromagnetic spectrum, travels in waves – visible light stimulated retina, visionEnergy easily converted from one type to anotherComposition of MatterElements and AtomsAll matter composed of elements (can’t be broken down further)Elements made of atoms, differ for each element96% of body made of C, O, H, N See Table 2.1 for other trace elementsAtomic StructureMade of 3 subatomic particlesProton (p+) – positive charge, found in nucleusNeutron (n0) – neutral, found in nucleusElectron (e-) – negative charge, found in nucleus, mass = 0Overall charge of atom = 0What does this mean? p+ = e-Atoms with a charge are called ionsFigure 2.1Planetary and Orbital Models of AtomPlanetary Model – heavy elements in charged nucleus, electrons orbit aroundProblem – we can never locate e-, jump aroundOrbital Model – more recent, electron cloud, shading shows where e- likely to be foundIdentifying Elements# of protons, neutrons, and electronsAtomic Number - # of protonsAtomic Mass – sum of neutrons and protonsH is uniqueAtomic Weight – Is it the same as Atomic Mass?Figure 2.2Atomic WeightIsotopes – Same # of protons and electrons, but different # of neutronsSame atomic #, different atomic massesAll will have same chemical propertiesAtomic Weight is most abundant isotopeFor Hydrogen AW=1.0079Figure 2.3Periodic Table of Elementshttp://www.astro.virginia.edu/class/oconnell/astr121/cosmic-history-narrative.htmlMolecules and CompoundsMolecule = 2+ atoms combine chemicallyExamples?Molecule of an element = atoms of same elements H2, O2, N2Molecule of Compound = atoms of different elements H20, CO2, NaClMolecules of compounds have properties very different than that of it’s componentsNa – silvery metalCl2 – poisonous gasNaCl – makes my food taste betterChemical BondsNot physical structure, energy relationship between electrons of reacting atomsElectron shells or energy levels – 1-7, held more strongly at 1.Figure 2.5Electron ShellsShell 1 = 2 electronsShell 2 = 8 electronsShell 3 = 18 electronsEtc. Shells filled 1 upValence Shell – Outermost shell, most important for chemical behavior of atom. Why?Rule of 8s – outermost shell has 8 electrons, inertException is Shell 1Types of Chemical BondsIonicComplete transfer of electronsIons – charged atomsLoss or gain of electrons completes valence shell, stabilityOverall charge – like magnets NaCl, mostly saltsFigure 2.6Types of Chemical BondsCovalentElectrons shared by atoms, valence shell filled part of timeSingle, double, or triple bondsShared equally = nonpolar moleculesShare unequally = polar molecules, H20Polar vs. NonpolarWhich is polar?Figure 2.8Types of Chemical BondsHydrogen BondsMost important bond in BiologyVery weak, but often numerousH bound to O or N, forms bridge with another electron-hungry atomSurface Tension of waterIntramolecular bondsDNAProteinsFigure 2.9Chemical ReactionsSynthesis Rxn – 2+ atoms come together form larger, bond formation, energy absorbing, anabolic rxns in bodyDecomposition Rxn – molecule broken down, energy released, catabolic rxns in bodyExchange Rxn – Both synthesis and decomposition, transfer or switchFigure 2.10Factors that Affect Rate of Chemical RxnsBiochemistry: Inorganic vs. OrganicAll molecules of body are either:Inorganic compounds: small molecules that lack C Exceptions: CO2, COExamples: H2O, salts, most acids and basesOrganic compounds: contain C, large, covalently bondedCarbohydrates - sugarsLipids - phospholipidsProteins – HemoglobinNucleic Acids – DNA, RNAInorganic CompoundsWaterHeat Capacity – high heat capacity, absorbs and releases large amounts of heat before temp changes.Polarity/solvent Properties – because of polarity, excellent solvent. Solvent vs. solute.Salts, acids, bases dissolve easily in waterNutrients, gases, waste dissolve easily in water, acts as transportChemical Reactivity – Important reactant, digest food or break down of molecules = hydrolysis rxn, water addedCushioning – Protective functionCerebrospinal fluid – cushions brainInorganic CompoundsSaltsCompound w/ cation and anion (not H+ or OH-)Dissociate into ions easily in bodily fluidsAll salts electrolytes = conduct electrical current in solutionSalts of many metals found in body Ca2+ and P3-Na, K in nerve impulsesFe in