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Ch 100: Fundamentals for ChemistryWhat is Chemistry?Scientific MethodThe Scientific AttitudeMajor Developments in Chemistry ISlide 6Slide 7Types of ObservationsMeasurementsScientific NotationWriting Numbers in Scientific NotationWriting Numbers in Standard FormMeasurement SystemsRelated Units in the Metric SystemUnits & MeasurementMeasurement & UncertaintyMeasurements & Significant FiguresRules for Counting Significant FiguresRules for Rounding OffExact NumbersConverting between Unit SystemsMetric PrefixesWeight vs. MassVolumeDensitySlide 26Using Density in CalculationsSlide 28Aristotle (384-322 BC)Physical & Chemical PropertiesPhysical & Chemical ChangesStates of MatterClassification of MatterSeparation of MixturesMethods of SeparationEnergyHeat & TemperatureTemperature ScalesTemperature of ice water and boiling water.HeatHeat (cont.)Specific Heat Capacity (s)Slide 43Table of Specific Heat for various substances @ 20oCSlide 45Dmitri Mendeleev (1834-1907)Chemical Symbols & FormulasDalton’s Atomic TheoryThe AtomStructure of the AtomElectric ChargeWhat holds the atom together?Atomic BookkeepingMass # vs. Atomic MassExamples of IsotopesThe Periodic TableElements and the Periodic TableIonsIons (cont.)Slide 60Antoine Lavoisier (1743-1794)Types of CompoundsTypes of Compounds (cont.)Naming CompoundsNaming Simple CompoundsIonic Charges & the Periodic TableGreek Prefixes for Compound NamesIonic Compounds containing Polyatomic ionsAcidsNaming AcidsNaming Acids (cont.)Slide 72Chemical Reactions (Intro)Chemical Reactions (cont.)Rates of Chemical ReactionsEnergy in Chemical ReactionsEnergy in Reactions (cont.)CatalystsCatalysts & Energy in ReactionsEndothermic or Exothermic? (that is the question…)Balancing Chemical ReactionsBalancing Chemical Reactions (example)Balancing Chemical Reactions (Hint)Slide 84Driving Forces & Chemical ReactionsSolubilityPrecipitation ReactionsDissociationDissociation (examples)Dissociation (example)Process for Predicting the Products of a Precipitation ReactionSolubility RulesIonic EquationsElectrolytesReactions that Form Water: Acids + BasesAcid-Base ReactionsReactions of Metals with Nonmetals (Oxidation-Reduction)Oxidation-Reduction ReactionsPredicting Products of Metal + Nonmetal ReactionsAnother Kind of Oxidation-Reduction ReactionWays to Classify ReactionsDouble Displacement ReactionsSlide 103Slide 104Other Ways to Classify ReactionsSlide 106Slide 107Slide 108Amadeo Avogadro (1743-1794)The MoleGot mole problems?Molar MassMole Calculations (1)Mole Calculations (2)Percent CompositionPercent Composition CalculationsSlide 117Slide 118Chemical Equations: What do they tell us?Information Given by the Chemical EquationSlide 121Slide 122Slide 123Example:Example (cont.)Slide 126SolutionsConcentrationMass Percent (%)MolarityThe pH ScalepH Concept QuestionsCh 100: Fundamentals for ChemistryChapter 1: Introduction Lecture NotesWhat is Chemistry?•Chemistry is considered to be the central science•Chemistry is the study of matter•Matter is the “stuff” that makes up the universe•The fundamental questions of Chemistry are:•How can matter be described?•How does one type of matter interact with other types of matter?•How does matter transform into other forms of matter?Scientific Method1. Recognize a problemMake observation Ask a question2. Make an educated guess - a hypothesisPredict the consequences of the hypothesis3. Perform experiments to test the predictionsDoes experiment support or dispute hypothesis?4. Formulate the simplest rule that organizes the 3 main ingredients - develop a theoryThe Scientific Attitude•All hypotheses must be testable (i.e. there must be a way to prove them wrong!!)•Scientific: “Matter is made up of tiny particles called atoms”•Non-Scientific: “There are tiny particles of matter in the universe that will never be detected”Major Developments in Chemistry I~400 BC: Democritus proposed the concept of the “atom”~300 BC: Aristotle developed 1st comprehensive model of matter~700 AD: Chinese alchemists invent gunpowder1661: Robert Boyle proposed the concept of elements1770-1790: Lavoisier proposed the concept of compounds & the Law of Mass Conservation1774: Priestly isolates oxygen1797: Proust proposed the Law of Definite Proportions1803: Dalton re-introduces the concept of the atom and establishes Dalton’s Laws1869: Mendeleev creates the 1st Periodic Table1910: Rutherford proposes the “nuclear” model of the atom1915: Bohr proposes a “planetary” model of the hydrogen atom1920: Schroedinger publishes his wave equation for hydrogen1969: Murray Gell-Mann proposes the theory of QCD (proposing the existence of quarks)Discovery of subatomic particles:1886: Proton (first observed by Eugene Goldstein)1897: Electron (JJ Thompson)1920: Proton (named by Ernest Rutherford)1932: Neutron (James Chadwick)Other Important Discoveries:1896: Antoine Henri Becquerel discovers radioactivity1911: H. Kamerlingh Onnes discovers superconductivity in low temperature mercury1947: William Shockley and colleagues invent the first transistor1996: Cornell, Wieman, and Ketterle observe the 5th state of matter (the Bose-Einstein condensate) in the laboratoryMajor Developments in Chemistry IICh 100: Fundamentals for ChemistryChapter 2: Measurements & CalculationsLecture NotesTypes of Observations•QualitativeDescriptive/subjective in natureDetail qualities such as color, taste, etc.Example: “It is really warm outside today”•QuantitativeDescribed by a number and a unit (an accepted reference scale)Also known as measurementsExample: “The temperature is 85oF outside today”Measurements•Described with a value (number) & a unit (reference scale)•Both the value and unit are of equal importance!! •The value indicates a measurement’s size (based on its unit)•The unit indicates a measurement’s relationship to other physical quantitiesScientific Notation•Technique Used to Express Very Large or Very Small Numbers•Based on Powers of 10•To Compare Numbers Written in Scientific NotationFirst Compare Exponents of 10 (order of magnitude)Then Compare NumbersWriting Numbers in Scientific Notation1Locate the Decimal Point2Move the decimal point to the right of the non-zero digit in the largest placeThe new number is now between 1 and 103Multiply the new number by 10nwhere n is the number of places you moved the decimal point4Determine the sign on the exponent, nIf the decimal
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