Slide 1Slide 2Slide 3Slide 4Slide 5Slide 6Classification of MatterSlide 8Slide 9The Metric System of UnitsSlide 11Slide 12Slide 13Slide 14Slide 15Slide 16Slide 17Slide 18Slide 19Slide 20Slide 21Slide 22Slide 23Slide 24Practice:Slide 26Problem Solving Using Conversion FactorsSlide 28Slide 29Slide 30Slide 31Slide 32Slide 33Solving a Problem Using Two or More Conversion FactorsSlide 35Density and Specific GravitySolving Problems with DensitySlide 38Specific GravityJohn Dalton, 1766-1844Marie Curie, 1867-1934Antoine Lavoisier, 1743-1794Joseph Priestly, 1733-1804Dmitri Mendeleev, 1834-1907What is Matter?Matter: Anything that occupies space and has mass Physical States of MatterGas: Indefinite volume, indefinite shape, particles far away from each otherLiquid: Definite volume, indefinite shape, particles closer together than in gasSolid: Definite volume, definite shape, particles close to each otherProperties of MatterProperty: Characteristic of a substancePhysical Properties: Properties of matter that can be observed without changing the composition or identity of a substanceExample: Size, physical stateChemical Properties: Properties that matter demonstrates when attempts are made to change it into new substances, as a result of chemical reactionsExample: Burning, rustingChanges in MatterPhysical Changes: Changes matter undergoes without changing compositionExample: Melting ice; crushing rockChemical Changes: Changes matter undergoes that involve changes in composition; a conversion of reactants to productsExample: Burning match; fruit ripeningClassifying MatterPure substance: Matter that has only 1 component; constant composition and fixed propertiesExample: water, sugar •Element: Pure substance consisting of only 1 kind of atom (homoatomic molecule) Example: O2•Compound: Pure substance consisting of 2 or more kinds of atoms (heteroatomic molecules)Example: CO2Mixture: A combination of 2 or more pure substances, with each retaining its own identity; variable composition and variable propertiesExample: sugar-water•Homogenous matter: Matter that has the same properties throughout the sample•Heterogenous matter: Matter with properties that differ throughout the sampleSolution: A homogenous mixture of 2 or more substances (sugar-water, air)Classification of MatterMeasurement SystemsMeasurement: Determination of dimensions, capacity, quantity or extent of something; represented by both a number and a unitExamples: Mass, length, volume, energy, density, specific gravity, temperatureMass vs. WeightMass: A measurement of the amount of matter in an objectWeight: A measurement of the gravitational force acting on an objectEnglish System Units: Inch, foot, pound, quartEach type of measurement has a base unit.The Metric System of Units• Other units are related to the base unit by a power of 10.• The prefix of the unit name indicates if the unit is larger or smaller than the base unit.Unit of LengthMeter = basic unit of length, approximately 1 yard 1 meter = 1.09 yardsKilometer = 1000 larger than a meterCentimeter = 1/100 of a meter 100 cm = 1 meterMillimeter = 1/1000 of a meter1000 mm = 1 meterUnit of MassGram: basic unit of mass454 grams = 1 poundKilogram: 1000 times larger than a gram1 Kg = 2.2 poundsMilligram: 1/1000 of a gramUnit of VolumeLiter: basic unit of volume1 Liter = 1.06 quarts1 Liter = 10 cm x 10 cm x 10 cm1 liter = 1000 cm31 ml = 1 cm3 (1 cc)Units of TemperatureFahrenheit: -459oF (absolute zero) - 212oF (water boils)Celsius: -273oC (absolute zero) - 100oC (water boils)Kelvin: 0K (absolute zero) - 373 K (water boils)Different Temperature ScalesConverting Celsius and Fahrenheit:oC = 5/9 (Fo - 32)oF = 9/5 (oC) +32Converting Celsius and Kelvin:oC = K - 273 K = oC + 273Scientific Notation and Significant FiguresScientific notation: a shorthand way of representing very small or very large numbersExamples: 3 x 102, 2.5 x 10-4The exponent is the number of places the decimal must be moved from its original position in the number to its position when the number is written in scientific notationIf the exponent is positive, move the decimal to the right of the standard positionExample: 4.50 x 102  450 3.72 x 105  372,000If the exponent is negative, move the decimal to the left of the standard positionExample: 9.2 x 10-3  .0092Practice with Scientific Notation50,000 = 5.0 x 104300 =.00045 = 4.5 x 10-4.0005 =3.00 x 1025 x 10-4Significant FiguresSignificant Figures: Numbers in a measurement that reflect the certainty of the measurement, plus one number representing an estimateExample: 3.27cmRules for Determining Significance:-All nonzero digits are significant-Zeroes between significant digits are significantExample: 205 has 3 significant digits1,006 has 10,004 has 4 sig. figs.5 sig. figs.-Leading zeroes are not significantExample: 0.025 has 2 significant digits 0.000459 has 3 significant digits 0.0000003645 -Trailing zeroes are significant only if there is a decimal point in the numberExamples: 1.00 has 3 significant figures 2.0 has 2 significant digits 20 has 1500 1.5004 sig. figs.1 sig. fig.2 sig. figs.4 sig. figs.Calculations and Significant FiguresAnswers obtained by calculations cannot contain more certainty (significant figures) than the least certain measurement used in the calculationMultiplication/Division: The answers from these calculations must contain the same number of significant figures as the quantity with the fewest significant figures used in the calculationExample: 4.95 x 12.10 = 59.895 Round to how many sig. figs.? Final answer:359.9Addition/Subtraction: The answers from these calculations must contain the same number of places to the right of the decimal point as the quantity in the calculation that has the fewest number of places to the right of the decimalExample: 1.9 + 18.65 = 20.55How many sig. figs. required?Final answer: Rounding OffRounding off: a way reducing the number of significant digits to follow the above rules120.6Rules of Rounding Off:Determine the appropriate number of significant figures; any and all digits after this one will be dropped.If the number to be dropped is 5 or greater, all the nonsignificant figures are dropped and the last significant figure is increased by 1If the number to be dropped is less than 5, all nonsignificant figures are dropped and the last