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Prentice-Hall 2007General Chemistry: Chapter 1Slide 1 of 28

Philip Dutton

University of Windsor, CanadaPrentice-Hall 2007

Chapter 1: MatterIts Properties andMeasurement

CHEMISTRY

Ninth

EditionGENERAL

Principles and Modern Applications

Petrucci Harwood Herring Madura


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Contents

1-1 The Scientific Method1-2 Properties of Matter1-3 Classification of Matter

1-4 Measurement of Matter: SI (Metric) System1-5 Density and Percent Composition:Their Use in Problem Solving

1-6 Uncertainties in Scientific Measurements

1-7 Significant Figures Focus On The Scientific

Method at Work: Polywater


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1-1 The Scientific Method

Louis Pasteur (1822-1895) Developer of Germ Theory

Pasteurization

Rabies Vaccination Called the greatest physician

of all time by some.

He was a chemist by training

and profession.


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Figure 1-1 The Scientific Method Illustrated


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1-2 Properties of Matter

Matter: Occupies space, has mass and inertia

Composition: Parts or componentsex. H2O, 11.19% H and 88.81% O

Properties: Distinguishing featuresphysical and chemical properties


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1-2 Classification of Matter

Matter is made of atoms. 114 elements.

About 90% available from natural sources

Compoundsare comprised of two or more elements.

Moleculesare the smallest units of compounds.


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Separating Mixtures


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Separating Mixtures

General Chemistry: Chapter 1


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Decomposing Compounds



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States of Matter



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1-4 The Measurement of Matter


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Prentice-Hall 2007General Chemistry: Chapter 1Slide 12 of 28 General Chemistry: Chapter 1 Prentice-Hall 2007Slide 12 of 19


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Mass

Mass is the quantityof matter in an object.

Weight is the force of

gravity on an object

W m W =gm


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Temperature

General Chemistry: Chapter 1 Prentice-Hall 2007Slide 14 of 28


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Volume


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SI and non-SI Units Compared

1 kg 1 lb1 in 1 cm

1 US qt

0.936 L1 L

1 Imperial qt

1.136 L


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Units

S.I. Units

Length meter, m

Mass Kilogram, kg

Time second, s

Temperature Kelvin, K

Quantity Mole, 6.0221023 mol-1

Derived Quantities

Force Newton, kg m s-2

Pressure Pascal, kg m-1s-2

Energy Joule, kg m2s-2

Other Common Units

Length Angstrom, , 10-8cm

Volume Liter, L, 10-3m3

Energy Calorie, cal, 4.184 J

Pressure

1 Atm = 1.064 102 kPa

1 Atm = 760 mm Hg


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1-5 Density and Percent Composition

= m/V

m=V V=m/

g/mL

Mass and volume are extensivepropertiesDensity is an intensiveproperty


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Density in Conversion Pathways

What is the mass of a cube of osmium that is 1.25

inches on each side?

Have volume, need density = 22.48g/cm3


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Relating Mass, Volume and Density

The stainless steel in the solid cylindrical rod pictured below hasa density of 7.75 g/cm3. If we want a 1.00 kg mass of this rod,how long a section must we cut off?

EXAMPLE 1-2

Calculate the Length V = hr2 h =Vr2

V = m

d

= m d

1Calculate the Volume needed


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(3.1415){(0.5)(1.000 in)(2.54 cm/in)}2

EXAMPLE 1-2

Calculate the Length V = hr2 h = Vr2

V =m

d= m

d

1Calculate the Volume needed

= (1.00kg)(1000g/kg) 7.75 g1 cm3

= 129 cm3

= 25.5 cmh =Vr2

= 129 cm3

V =


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Measuring Volume of an Irregular Object


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1-6 Uncertainties in Scientific Measurements

Systematic errors. Thermometer constantly 2C too low.

Random errors

Limitation in reading a scale. Precision

Reproducibility of a measurement.

Accuracy How close to the real value.


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Precision

Reproducibility 0.1 g 0.0001 g

Precision low high


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1-7 Significant Figures


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Significant Figures

The calculators show the effect of the change in a low precision

number in a calculation 14.79 12.11 5.05

5.04 5.05 5.06


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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 examples

where the approach to the question must be identified.

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