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Chemistry 140 Fall 2002

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General Chemistry: Chapter 1Slide 1 of 25

Burak ESATFATIH UNIVERSITY

DEPARTMENT OF CHEMISTRY

TENTH EDITIONGENERAL CHEMISTRYPrinciples and Modern Applications

PETRUCCI HERRING MADURA BISSONNETTE

Copyright © 2011 Pearson Canada Inc.

Matter: Its Propertiesand Measurement 1

IntroductionChemistry and chemicals is an integral part of lifeAll material objects-whether living or inanimate-are made up of chemicalsChemistry is a science of manipulating chemical

compounds which deals with the composition andproperties of the matterChemists decompose materials into their smallestcomponents (atoms or molecules) and reassembleto obtain materials that do not exist naturally andthat often exhibit desired or unusual properties

Copyright © 2011 Pearson Canada Inc.General Chemistry: Chapter 1Slide 2 of 25




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Matter: Its Propertiesand Measurement

CONTENTSCONTENTSCONTENTSCONTENTS

1-1 The Scientific Method

1-2 Properties of Matter

1-3 Classification of Matter

1-4 Measurement of Matter: SI(Metric) Units

1-5Density and PercentComposition: Their Use inProblem Solving

1-6 Uncertainties in ScientificMeasurements

1-7 Significant Figures


1-1 The Scientific Method

Louis Pasteur (1822-1895)developer of germ theorypasteurizationrabies vaccination

Called the greatest physician ofall time by some.

He was a chemist by trainingand profession.




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The Scientific Method

Originated in 17th century with Galileo, FrancisBacon, Robert Boyle, Isaac NewtonObservations→ Pattern→ Generalization(Natural Law)→ Test by experiment→ Theory (Model)→ Experiment→ TheoryestablishedWhen differing or conflicting theories are

proposed, the most successful one is chosen. Alsothe theory with the smallest number ofassumptions-- the simplest theory-- is preferred.


FIGURE 1-1

The Scientific Method Illustrated





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The Scientific Method

TheScientificScientific MethodMethod is a combination ofobservations , experimentation , and theformulation of laws, hypotheses andtheories



1-2 Properties of Matter

Matter: Occupies space, has mass and inertia

Composition: Parts or components &their relative proportions

ex. H2O, 11.19% H and 88.81% O

Properties: Distinguishing featuresphysicalandchemicalproperties




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1-3 Classification of Matter

Matter is made ofatoms .114elements .About 90% available from natural sourcesCompounds are comprised of two or more elements.Molecules are the smallest units of compounds (the

smallest entity that has the same composition as thecompound as a whole)

FIGURE 1-4A classification scheme for matter





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Separating Mixtures: a physical processCopyright © 2011 Pearson Canada Inc.General Chemistry: Chapter 1Slide 11 of 25

FIGURE 1-5

A chemical change: decomposition of ammonium dichromate


FIGURE 1-6




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Macroscopic and microscopic views of matterFigure 1-7



1-4 The Measurement of Matter



Slide 14

PD4 This table needs to be replaced with table in the new colour scheme.Philip Dutton, 3/3/2010




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Copyright © 2011 Pearson Canada Inc.Slide 15 of 25General Chemistry: Chapter 1

Mass


Mass is thequantity ofmatter in an object.

Weight is the force of

gravity on an object

W m W =g × m



Slide 15

PD5 This table needs to be replaced with the one in the new colour schemePhilip Dutton, 3/3/2010




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Temperature


Volume




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SI and non-SI Units Compared

1 kg 1 lb1 in 1 cm

1 US qt0.936 L

1 L

1 Imperial qt1.136 L


SI UnitsLength meter, mMass Kilogram, kgTime second, sTemperature Kelvin, KQuantity Mole, 6.022× 1023mol-

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Derived UnitsForce Newton, kg m s-2

Pressure Pascal, kg m-1 s-2

Energy Joule, kg m2 s-2

Non-SI UnitsLength Angstrom, Å, 10-8 cmVolume Liter, L, 10-3 m3

Energy Calorie, cal, 4.184 JPressure

1 Atm = 1.064× 102 kPa

1 Atm = 760 mm Hg




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1-5 Density and Percent Composition

δ = m/Vm=Vδ V=m/ δ

g/mLMass and volume areextensive properties

Density is anintensive property


Density in Conversion PathwaysWhat is the mass of a cube of osmium that is 1.25inches on each side?

Have volume, need density =22.59g/cm3



Slide 22

PD1 Replace figure, density value is wrongPhilip Dutton, 3/3/2010




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Measuring Volume of an Irregular Object


FIGURE 1-10


1-6 Uncertainties in Scientific Measurements

Systematic errors.Thermometer constantly 2° C too low.

Random errorsLimitation in reading a scale.

PrecisionReproducibility of a measurement.

AccuracyHow close to the real value.




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Precision

Reproducibility ∼ 0.1 g ∼ 0.0001 g

Precision low high


1-7 Significant Figures

Determining the number of significant figures in a quantityFigure 1-11





Significant FiguresThe calculators show the effect of the change in a low precisionnumber (N) in a calculation 14.79× 12.11× N

N = 5.04 5.05 5.06


End of Chapter Questions

Instructors may provide lists of questions thatreinforce topics they feel are particularly pertinent inthe chapter. If no list is given students should attemptquestions from each section of the chapter.

Build from the easier questions where the topic isidentified, to the more difficult integrative exampleswhere the approach to the question must be identified.

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