Chem 115 1nd Edition Lecture 3Outline of Last LectureI. DensityII. TemperaturesIII. Significant FiguresOutline of Current LectureI. ErrorsII. ElementsIII. LawsIV. Dalton’s Atomic TheoryV. ExperimentsVI. Atomic PictureCurrent LecturePrecision: how close the measurements in a series are to each otherAccuracy: how close the measurement is to the actual valueSystematic Error: all numbers are either all higher or all lower to the actual value each timeElement: Simplest type of substance with unique physical and chemical propertiesMolecule: a structure that consists of two or more atomsCompound: a substance that consists of two or more elements which are chemically combinedMixture: a substance that consists of two or more elements and/or compounds that are physically intermingledIsotopes: atoms of an element with the same number of protons but different number of neutrons- Total mass of substances doesn’t change during a chemical reactionLaw of Definite Composition: no matter the source, a particular compound is composed of the same elements and the same partsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Law of Multiple Proportions: whole number compound ratiosDalton’s Atomic Theory – 1. All matter consists of atoms2. Atoms of one element cannot be converted into atoms of another element3. Atoms of an element are identical in mass and other properties andare different from the atoms of any other element4. Compounds result from the chemical composition of a specific ratioof atoms of different elements- Atoms cannot be destroyed or createdMilikan’s Oil Drop Experiment- Measured electron charge- Mass of electron = (mass/charge) X chargeRutherford’s Scattering Experiment- Discovered atomic nucleusA- Mass Number (protons + neutrons) Z- Atomic Number (protons) X- Atomic
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